warning - Smithsonian Store

Transcription

WARNING:
Additional SupplyNeeds(to be suppliedby you)
Your Microchemistry set includes all of the special chemicals and materials to provide you with the reagent chemicals and equipmentto
perform experiments and provide you with hours of educational fun. Since there are so manyexperiments and procedures, you are
asked to supply manyof the common
household items and household chemicals which would be impractical to supply and ship in your
chemistry set.
THISSETCONTAINS
CHEMICALS
& APPARATUS
THAT
MAY
BEHARMFUL
IF MISUSED.
READ
ITEM #2835
AGES 10 AND UP
CAUTIONS
ONINDIVIDUAL
CONTAINERS
CAREFULLY.
NOTTOBEUSED
BYCHILDREN
EXCEPT
UNDER
ADULT
SUPERVISION.
Youwill need to gather various items listed in each experiment so that you can perform the experiments. Always read through your
experimentbeforehandand gather all of the materials you will needat the beginning.
Thefollowing list of outside items and materials is listed below for your convenience.YouDONOTneedto collect ALLitems on the list
at one time, only as you plan aheadto perform a particular experimentor series of experiments.
Plastic sheeting for workarea
paper towels for cleanup
Cotton or cotton balls
Scissors
Distilled water
Isopropyl RubbingAlcohol or Ethyl RubbingAlcohol
Cardstock (3" x 5" filing card)
Pencils (red and black)
Ball point pen
Kitchen paring knife
Fine sandpaper
Sheet of white paper
Liquid dishwashing soap
Hair shampoo
Dishwasher Jet-Dry @soap
Liquid hand soap
Baby powder or talcum powderor flour
SodiumChloride (table salt)
Iron nails
Copper tacks
Aluminumnails
Styrofoamballs
Modeling clay
Toothpicks
P!pe c!ea~ers
Straws
Gum drops
9 volt battery
D-cell battery
Vinegar
Cornstarch
Several heavy books
Crushed ice
Cellophane tape
Transparent tape
Household ammonia
Plastic sandwich bags
Lemonjuice
3%solution hydrogen peroxide
Fine steel wool
Rawliver
Rawpotato
Grassclippings and/or plant leaf
Sunlight and/or strong artificial light source
Sodiumbicarbonate (baking soda)
Alka Seltzer~ tablet
Teaspoon
Toothbrush
Window pane
Woodenruler
Set of colored pencils
Flower petals
Plant fruit skins i.e. blueberries, blackberries,cherries, red cabbage leaves
Householdtea from tea bags
Householdsoap solution
Liquid laundry detergent
Pet shampoo
Clear soda (sparkling water)
Toothpaste
Milk
Grapefruit juice
Rain water
Plastic wrap
Fine line marker
Individual brand samplesof different vinegars i.e. apple cider
vinegar, white vinegar, ambervinegar, pineapple vinegar, tarragon vinegar
Various brands of Antacid tablets
C~eanseror scouring powder
Kleenex
Various nickels and pennies (15 each)
Model paint or fingernail enamel
SMITHSONIAN
,®
Chem-Works
MicroChemistry
~"
2
3
4
5
6
7 __~.__~
10
11
1 2D
O0 0000
O0 0000
O0 0000
00"" "-"
© MM
NATURAL SCIENCE INDUSTRIES, LTD.
¯ WESTHEMPSTEAD,
910 ORLANDO
AVENUE
NY 11552-3942° (516) 678-1700
®
© 2000SmithsonianInstitution
PART#2835-08
PRINTEDIN HONGKONG
PLEASE KEEP A NOTE OF OUR NAME AND ADDRESSDETAILS FOR FUTURE REFERENCE.
IN U.S.A. CONTACT."
NATURALSCIENCEINDUSTRIES, LTD.
910 Orlando Avenue
West Hempstead, NY 11552-3942
516-678-1700
Chem-Works
List of Set Contents
IN EUROPECONTACT:
NSI SIMM GmbH
D 76162 KARLSRUHE
GERMANY
49- 0721-9584-116
WARNING!
ONLY FOR USE
BY CHILDREN OVER 10 YEARS OLD. TO BE USED SOLELY UNDER THE STRICT
SUPERVISION OF ADULTS THAT HAVE STUDIED THE PRECAUTIONSGIVEN IN THE EXPERIMENTALSET.
CAUTION!
CONTAINS SOME CHEMICALS WHICH ARE CLASSIFIED AS A SAFETY HAZARD. READ THE INSTRUCTIONS BEFORE USE, FOLLOWTHEM AND KEEP FOR REFERENCE. DO NOT ALLOW CHEMICALS TO COME
INTO CONTACTWITH ANY PART OF THE BODY, PARTICULARLY THE MOUTHAND EYES. KEEP SMALL CHILDREN
AND ANIMALS AWAYFROMEXPERIMENTS. STORE THIS SET OUT OF REACHFROMSMALL CHILDREN. EYE PROTECTION FOR SUPERVISING ADULTS IS NOT PROVIDED.
ENTER THE DETAILS AND TELEPHONE NUMBEROF THE LOCAL POISON CENTER QR HOSPITAL IN THE BOX
BELOW:
IN CASE OF ACCIDENTALINTAKE OF A CHEMICALCONTACT:
#8
#11
#18
#40
#41
#42
#44
#47
#49
#53
#57
#58
#64
#65
#67
#70
#63
#54
#38
#61
1 Well
.............. Cobalt
Chloride
...................... China
1 Bottle.......... Copper
Sulfate
........................ England
1 Bottle.......... Sodium
Silicate...................... Sweden
1 Bottle.......... Calcium
Hydroxide
.................. Germany
1 Well
.............. Calcium
Nitrate...................... Japan
1 Bottle.......... CitricAcid
................................ China
1 Well
.............. Ferrous
Sulfate
...................... Taiwan
1 Well
.............. Methylene
Blue...................... England
1 Bottle.......... Potassium
Iodide.................... Japan
Sulfate
........................ Germany
1 Bottle.......... AluminumAmmonium
Sulfate China
1 Bottle.......... Ammonium
Japan
Chloride..............
1 Bottle.......... Magnesium
Sulfate................ Germany
1 Well
.............. Phenolphthalein
...................... U.S.A.
Carbonate
.................. Germany
1 Well
.............. Universal
Indicator
.................. U.S.A.
1 Package
...... IronWire
................................ China
1 Package
...... ZincWire
................................ China
1 Package
...... Aluminum
Wire........................ China
1 Package
...... Copper
Wire
............................ China
1 Each
.............. 6"Plastic
Ruler
............................ China
1 Each
.............. FilterPaper
.................................. England
1 Package
........ Molecule
Kit.................................. China
1 Each
.............. Safety
Goggles
............................ China
1 Package
........ Galvanometer
Kit .......................... China
1 Pair................ Spring
Clips
.................................. China
1 Each
.............. Soda
Straw
.................................. Hong Kong
1 Each
.............. Magnifier
...................................... China
1 Each
.............. Battery
Clip9V............................. China
...................................... U.S.A.
2 Each
.............. 1oz.Cup
1 Each
.............. Atom
Sheet
.................................. China
t Each
.............. Red
LED
...................................... China
1 Each
.............. Microplate
.................................... China
8 Each
.............. Pipette
..........................................U.S.A.
1 Each
.............. Resistor
1KOhm
.......................... Taiwan
Each
.............. PlasticTube
withCap.................. China
...................................... China
2 Each
............ Toothpick
Each
.............. PVC
Coated
Wire........................
China
Each
.............. Instruction
Manual
........................ Hong Kong
GENERALFIRST AID INFORMATION:
IN CASE OF EYE CONTACT: WASHOUT WITH PLENTY OF WATER, HOLDING EYE OPENIF NECESSARY.SEEK IMMEDIATE MEDICAL ADVICE. IF SWALLOWED:WASHOUT MOUTHWITH PLENTY OF WATER, DRINK SOME FRESH
WATER. DO NOT INDUCE VOMITING. SEEK IMMEDIATE MEDICAL ADVICE. IN CASE OF INHALATION: REMOVE
PERSONTO FRESH AIR. IN CASE OF CONTACTAND BURNS: WASHAFFECTED AREA WITH PLENTY OF WATER
FOR 5 MINUTES. IN CASE OF INJURY OR DOUBT, SEEK MEDICAL ADVICE WITHOUT DELAY. TAKE THE CHEMICAL WITH THE CONTAINERWITH YOU. NOTE: FIRST AID INFORMATIONMAY ALSO BE FOUNDIN THE INSTRUCTIONS FOR CARRYING OUT THE EXPERIMENTS OR ON THE CONTAINERS.
ADVICE FOR SUPERVISING ADULTS:
¯ READ AND FOLLOWTHESE SAFETY INSTRUCTIONS, THE SAFETY RULES AND THE FIRST AID INFORMATION
AND KEEP THEM FOR REFERENCE. ¯ THE INCORRECT USE OF CHEMICALS CAN CAUSE INJURY AND DAMAGE
TO HEALTH. ¯ ONLY CARRYOUT THOSEEXPERIMENTSWHICHARE LISTED IN THE INSTRUCTIONS.¯ THIS SET IS
FOR USE BY CHILDREN OVER 10 YEARS OF AGE. ¯ BECAUSECHILDREN’S ABILITIES VARY SQ MUCH, EVEN
WITHIN AGE GROUPS, SUPERVISING ADULTS SHOULD EXERCISE DISCRETION AS TO WHICH EXPERIMENTS
ARE SUITABLE AND SAFE FOR THEM. THE INSTRUCTIONS SHOULDENABLE SUPERVISORSTO ASSESS ANY EXPERIMENTTO ESTABLISH ITS SUITABILITY FOR A PARTICULARCHILD. ¯ THE SUPERVISINGADULT SHOULDDISCUSS THE WARNINGSAND SAFETY INFORMATION WITH THE CHILD OR CHILDREN BEFORE COMMENCINGTHE
EXPERIMENTS. PARTICULARATTENTION SHOULDBE PAID TO THE SAFE HANDLINGOF HOT LIQUIDS. THE AREA
SURROUNDINGTHE ACTIVITY SHOULD BE KEPT CLEAR OF ANY OBSTRUCTIONS AND AWAY FROM STORAGE
OF FOOD, IT SHOULDBE WELL LIT AND VENTILATEDAND CLOSETO A WATERSUPPLY. ¯ A SOLID TABLE WITH A
HEAT RESISTANT TOP SHOULD BE PROVIDED.
If wemade
anerror andleft something
out of this set, or if
something
is damaged,
weare sorry and wish to correct our
error. Pleasedo not return the set to the store whereyou
purchased
it, as the store doesnot havereplacement
parts.
Instead,write us a letter givingus:
1. Date of Purchase
2. WherePurchased
3. Price Paid
4. Model Number
5. Nameof Set
6. Brief Descriptionof Problem
7. SalesReceipt
Wewill do our best to satisfy you.
SAFETY RULES:
° DO READ THESE INSTRUCTIONS BEFORE USE, FOLLOWTHEM AND KEEP THEM FORREFERENCE. ¯ DO KEEP
YOUNG CHILDREN AND ANIMALS AND THOSE NOT WEARING EYE PROTECTION AWAYFROM THE EXPERIMENTAL AREA. ¯ DO ALWAYSWEAREYE PROTECTION.¯ DO STORE CHEMICALSETS OUT OF REACHOF YOUNGCHILDREN. ¯ DO CLEAN ALL EQUIPMENTAND WASHAFTER CARRYINGOUT THE EXPERIMENTS.¯ DO NOT EAT, DRINK
OR SMOKEIN THE ACTIVITY OR EXPERIMENTALAREA. ¯ DO NOT USE EQUIPMENTWHICH HAS NOT BEEN SUPPLIED QR RECOMMENDED
IN THE SET. ¯ DO NOT ALLOWCHEMICALS TO COMEINTO CONTACTWITH THE EYES
OR MOUTH. ¯ DO NOT REPLACEFOODSTUFFSIN ORIGINAL CONTAINER. DISPOSE OF IMMEDIATELY. ¯ DO MAKE
SURE THAT ALL CONTAINERS ARE FULLY CLOSED AND PROPERLYSTORED AFTER USE.
Quality Control Department
Natural ScienceIndustries, Ltd.
910 Orlando Avenue
West Hempstead, NY 11552-3942
(516) 678-1700
~
VIAL
UMBEF
SIZE OF NAME OF CONTENTS
VIAL OR
CONTAINER (CHEMICAL NAME)
CHEMICAL
FORMULA
WARNING
ON LABEL
WARNING
#53
#57
SODIUM
SULFATE
6 ml
ALUMINUM
AMMONIUM
SULFATE
Na2SO4 o10H20
READ SIDE PANEL BEFORE
USING CAUSES EYE AND
SKIN IRRITATION MAY BE
HARMFUL IF SWALLOWED,
INHAI ED OR ABSORBED
f HROUGH
SKIN.
DANGER
°12H20
AINH4(SO4)2
R[AD SIDE PANEL. BEFORE
(/,=;INC. CAUSESBURNS
CORROSIVE HARMFUL IF
SWALLOWED, INHALED OR
ABSORBED
THROUGH
SKIN
WARNING
#58
6 ml
AMMONIUM
CHLORIDE
NH4C1
USING CAUSES SKIN. MUCOUS MEMBRANEAND SEVERE EYE
IR RITA’IION.
MAY BE HARMFULIF SWALLOWED, INHALED OR ABSORBED THROUGHSKIN.
WARNING
#64
6 ml
MAGNESIUM
SULFATE
MgSO4°7H20
USING.
CAUSES IRRITAT/ON
MAYBE HARMFULIF
SWALLOWED, iNHALED OR
ABSORBED
THROUGH
SKIN.
WARNING
#65
6 ml
PHENOLPHTHALEIN
C20H1404
USING CAUSES EYE. SKIN
AND MUCOUS MEMBRANE
IRRITATION. MAY BE HARMFUL ~F SWALLOWED, INHALED OR A R£CIRFCFI3
THROUGHSKIN.
DANGER
#67
6 ml
SODIUM
CARBONATE
Na2CO3ol0H20
READ SIDE PANFL BEFORE
USING. CAUSES BURNS _
CORROSIVE HARMFUL IF
,SWALLOWED. INHALED OR
ABSORBED
]HROUGH
SKIN
FIRST AID
FIRST AID: ¯ IN CASEOF EYE CONTACT,IMMEDIATELYFLUSH
EYES FREELY WITH WATER
¯ IN CASE OF SKIN CONTACT. IMMEDIATELY WASHSKIN WITH
SOAP AND LARGE AMOUNTSOF WATER
¯ IF INHALED. GETTO FRESHAIR
¯ IF SWALLOWED
GET MEDICAL HELP IMMEDIATELY
IN ALL CASES. CONTACT A POISON CONTROL CENTER
AND/OR SEEK MEDICAL AT-rENTION. KEEP OUT OF REACH
OF CHILDREN.
FIRST AID: ¯ IN CASE OF EYE CONTACT,IMMEDIATELYFLUSH
¯ IN CASEOFSKIN CONTAC
1. IMMEuIAIELY I- LUSHSKIN l- HEELY WITH WATER
¯ IF INHALED, GET10 FRESHA R
I " IF SWALLOWED
AND PERSONIS CONSCIOUS, GIVE WATER
AND GET MEDICAL HELP
AND/OR SEEK MEDICAL ATTENTION. KEEP OUT OF REACH
OF CHILDREN.
FIRST AID: ¯ IN CASE OF EYE CONTACT.IMMEDIATELYFLUSH
¯ IN CASE OF SKIN CONTACT, IMMEDIATELY WASHSKIN WlrH
SOAP AND LARGE AMOUNTSOF WAFER
¯ IF INHALED,GET 1O FFIESH AIR
¯ IF SWALLOWEDAND PERSON IS CONSCIOUS. WASHOUT
MOUTHWITH WATER.
AND/OR SEEK MEDICAL ATrENTION. KEEP OUT OF REACH
OF CHILDREN.
I
FIRST AID: ¯ IN CASEOF EYE CONTAC~"IMMF
DIAIELY FI.USH
¯ IN CASE OF SKiN CONTACT. IMMEDIATELYWASHSKIN WITH
J SOAP AND LARGE AMOUNTSOF WATER
¯ IF INHALED, GET TO FRESHAIR
¯ IF SWALLOWEDAND PERSON IS CONSCIOUS, WASH OUT
~ MOUTHW TH WATER¯
IN ALL CASES, CONTACT A POISON CONTROL CENTER
AND/OR SEEK MEDICAL A’VrENTION. KEEP OUT OF REACH
OF CHILDREN.
¯ IN CASE OF SKIN CONTACT, IMMEDIATELYFLUSH SKIN WITH
WATER, THEN WASHTHOROUGHLYwITH SOAP AND WATER
¯ IF INHALED, GET TO FRESHAIR
¯ IF SWALLOWED
AND PERSONIS CONSCIOUS, GIVE WATER
AND GET MEDICAL HELP IMMEDIATELY¯
AND~OR SEEK MEDICAL ATTENTION. KEEP OUT OF REACH
)F CHILDREN.
¯ IN CASE OF SKIN CONTACT.IMMEDIATELY WASHSKIN WITH
SOAP AND LARGE AMOUNTSOF WATER
IF INHALED. GET TO FRESHAIR
IF SWALLOWED
AND PERSON IS CONSCIOUS. IMMEDIATELY
JVE WATERAND GET MEDICAL HELP.
OF CHILDREN.
Methyl Red-
C15H15N302
WARNING
USING. CAUSES EYE AND
SKIN IRRITATION. HARMFUL IF
SWALLOWED,
INHALED
OR
ABSORBED
THROUGHSKIN.
FIRST AID: ¯ IN CASEOF EYE CONTACT.IMMEDIATELYFLUSH
¯ IN CASEOF SKIN CONTACT,IMMEDIAFELYFLUSH SKIN FREELY WITH WATER
¯ IF INHALED. GET TO FRESHAIR
¯ IF SWALLOWEDAND PERSON IS CONSCIOUS. WASH OUT
MOUTHWITH WATER.
AND/OR SEEK MEDICAL ATTENTION. KEEP OUT OF REACH
OF CHILDREN.
6 ml
UNIVERSAL
INDICATOR
onpaperstrips
polybag
IRON
WIRE
Fe
#54
polybag
ZINC
WIRE
Zn
CAUTION
KEEP OUT OF REACHOF CHILDREN.
#38
polybag
ALUMINUM
WIRE
AI
CAUTION
KEEP OUT OF REACH OF CHILDREN.
#61
polybag
COPPER
WIRE
#70
Phenolphthalein
Bromthymol Blue
Thymol Blue
Methy~ Yellow
CAUTION
THE SMITHSONIAN INSTITUTION FACT SHEET
The SmithsonianInstitution is a museum,education and research complexof 17
museums
and galleries, and the National Zoological Park. Fifteen museums
and galleries
are located in Washington,D.C., two are in NewYork City, and the National Zoois in
Washington.Ten of the museums
and galleries are situated on the National Mall between
the U.S. Capitol and WashingtonMonument.
Oneof the world’sleadingscientific researchcenters,the Institution hasfacilities in
eight states andthe Republicof Panama.
Research
projectsin the arts, history, andscience
are carried out by the Smithsonian
atf over the world.
The newNational Museum
of the AmericanIndian is scheduledto openonthe National
Mall in 2002. The centerpieceof the museum
is the priceless collection of Native American
artifacts transferred to the Smithsonianfrom the Museum
ot the AmericanIndian, Heye
Foundation
(NewYork). The NewYork exhibition facility - the HeyeCenterof the National
Museurnof the AmericanIndian openedOctober30, 1994 in lower Manhattan.
Anothernewmuseum,
the National Postal Museum,
is located near UnionStation on
Capitol Hill. Devotedto the history of the U.S. mail service, the museum
housesthe world’s
largest and mostcomprehensive
collection of its kind, with morethan 16 million stamps,
covers,andartifacts.
HISTORY
JamesSmithson
(1765-1829), a British scientist, drewup his will in 1826 naminghis
nephew,HenryJamesHungerford,as beneficiary. Smithsonstipulated that, shouldthe
nephew
die withoutheirs (as he did in 1835), the estate wouldgo the UnitedStatesto found
"at Washington,underthe nameof the Smithsonian
Institution, an establishmentfor the
increase and diffusion of knowledge..."
On July 1, 1836, Congressacceptedthe legacy bequeathedto the nation by James
Smithsor~,~nd,nh=clo#dth~ faith nf the United States to the charitable trust. In 1838,
following approval of the bequest by the British courts, the United States received
Smithson’sestate- bagsof gold sovereigns- then the equivalent of $515,169. Eight years
later, on August10, 1846, an Act of Congresssigned by President JamesK. Polk,
establishedthe Smithsonian
Institution in its presentformandprovidedfor the administration of the trust, independent
of the government
itself, by a Boardof RegentsandSecretary
of the Smithsonian.
SMITHSONIAN
Cu
CAUTION
Page 57
MUSEUMS, GALLERIES
AND ZOO
SmithsonianInstitution Building ("Castle")
Anacostia Museum
Arthur M. Sackler Gallery
Arts and Industries Building
Cooper-Hew/It, National Design Museum
Freer Gallery of Art
Hirshhorn Museumand Sculpture Garden
National Museumof American Art
National Museumof American History
National Museumof the American Indian
National Museumof Natural History
National Portrait Gallery
National Postal Museum
National Zoological Park
National Air andSpaceMuseum
Renwiek
Gallery
National Museumof African Art
S. Dillon Ripley Center
SIZE OF NAMEOF CONTENTS
VIAL
NUMBER VIAL OR
(CHEMICALNAME)
3ONTAINER
Chem-Works
CHEMICAL
FORMULA
INDEX
Introduction
..........................................................................................................................
AWord
toThe
"Chemist".
...............................................................................................................
TheMicroChemistry
System
..........................................................................................................
Section1 - Preparation
of Laboratory
Equipment
................................................................
Section2 - Properties
of theMicrochemistry
System
..........................................................
Section3 - How
to Destroy
Surface
Tension
......................................................................
Section4 - Alcohol
andSurface
Tension
............................................................................
Section5 - AVisible
Illustration
of Surface
Tension
............................................................
FIRSTAID: ¯ IN CASEOF EYECONTACT,
IMMEDIATELY
FLUSH
EYES FREELYWITHWATER
¯ IN CASEOF SKIN CONTACT,
IMMEDIATELY
FLUSHSKINFREEREADSIDE PANELBEFORE
US- LY WITHWATER
AIR
ING. CAUSES
EYE, SKIN, AND ¯ IF INHALED,GETTOFRESH
¯ IF SWALLOWED
AND PERSON
IS CONSCIOUS,
IMMEDIATELY
MUCOUSMEMBRANEIRRITAGIVE
WATER
.
TION, HARMFUL
IF INHALEDOR
IN ALL CASES, CONTACTA POISON CONTROLCENTER
ABSORBEDTHROUGHSKIN.
MAYBE FATALIF SWALLOWED.AND/ORSEEKMEDICALATTENTION.KEEPOUT OF REACH
OF CHILDREN.
page 1
page 2
page 2
page 3
page 8
page 8
page 9
page 9
6 ml
COBALT
CHLORIDE
CoC12¯ 6H20
WARNING
#11
6 ml
COPPER
SULFATE
CuSO
4 ¯ 5H20
READSIDE PANELBEFORE
USING.CAUSES
SKIN, MUCOUSMEMBRANE
AND SEVERE EYE IRRITATION.
HARMFULIF SWALLOWED.
INHALED OR ABSORBED
THROUGH
SKIN.
DANGER
Chapter4
Chapter5
Chapter6
Chemical ModelsandChemical
Reactions
..................................................................................
Section1 - Paper
Chemistry
LabI ....................................................................................
Section2 - Paper
Chemistry
LabII ....................................................................................
Section3 - Synthesis
........................................................................................................
Section 3A- Synthesis
........................................................................................................
Section4 - Paper
Chemistry
Lab
III ..................................................................................
Section 4A- Using
Molecular
Models
..................................................................................
Section 4B- Using
Molecular
Models
II ..............................................................................
Section5 - Decomposition
of Water- A Chemical
Change
..............................................
Section6 - Paper
Chemistry
IV........................................................................................
Section 6A- Using
3-DModels
............................................................................................
Section7 - ElectricalSeparation
of Elements
froma Compound
....................................
Section8 - Another
Electrical
Separation
..........................................................................
Section9 - Electrolysis
of Ferrous
Sulfate
........................................................................
Section10- AChemical
Separation
....................................................................................
page 10
page 11
page 12
page 13
page 13
page 14
page 15
page 15
page 16
page 17
page 17
page 17
page 18
page 19
page 19
The Gaseous
Phases
ofMatter
....................................................................................................
Section
1 - TheEffectof Pressure
ontheVolume
of a Gas..............................................
ontheVolume
of a Gas........................................
Section2 - TheEffectof Temperature
Section3 - Gas
Diffusion
..................................................................................................
Section 3A- Gas
Diffusion
II ................................................................................................
Section4 - Preparation
of Oxygen
....................................................................................
Section5 - Does
AirContain
Oxygen?
..............................................................................
Section6 - NaturalOxygen
Production:
TheActionof Enzymes
......................................
Section7 - Methylene
BlueasanIndicator
......................................................................
Section8 - Plants
and
Oxygen
..........................................................................................
Section9 - Testing
a Gasfor Carbon
Dioxide
..................................................................
Section 10 - Preparation
ofCarbon
Dioxide
........................................................................
Section11 - AReaction
which
Produces
Carbon
Dioxide
..................................................
Section12 - Producing
Carbon
Dioxide
in Another
Way
....................................................
Section13 - TheProduction
of Ammonia
............................................................................
Section 14- Neutralization
of Gases
..................................................................................
Section15 - A Reactionof Ammonium
ChlorideandCalciumHydroxide
..........................
page 19
page 19
page 20
page 21
page 21
page 21
page 22
page 22
page 23
page 23
page 23
page 24
page 24
page 25
page 25
page 25
page 26
Experimentswith
Section1 Section2 Section3 Section4 Section5 Section6 -
page 26
page 27
page 27
page 28
page 29
page 30
page 31
Solutions
..........................................................................................................
AnElectrolyte
Detector
....................................................................................
Electrolytes
andNon-Electrolytes
....................................................................
Another
Usefor theElectrolyte
Detector
........................................................
Reactions
of Solutions
....................................................................................
Testing
theProducts
of a Reaction
..................................................................
TestingtheRemaining
Solutionof a Chemical
Reaction
................................
FIRSTAID
POISON
DANGER
#8
Chapter1
Chapter2
Chapter 3
WARNING
ON LABEL
#18
6 ml
SODIUM
SILICATE
Na2SiO
3 ° 5H20
USING.CAUSES
SKIN, MUCOUSMEMBRANE
AND SEVERE EYE IRRITATION.
HARMFULIF SWALLOWED.
INHALED OR ABSORBED
THROUGH
SKIN.
DANGER
#40
6 ml
CALCIUM
HYDROXIDE
Ca(OH)
2
USING. CAUSESBURNS.
ESPECIAL
I "V ONWET
SK!NCORROSIVE.HARMFULIF
SWALLOWED OR ABSORBEDTHROUGHSKIN.
MAYBE FATALIF INHALED.
WARNING
#41
#42
6 ml
6 ml
CALCIUM
NITRATE
CITRICAcID-t-
Ca(NO3)
2 ¯ H20
C6H807° H20
USING.CAUSES
EYE,SKIN,
AND MUCOUSMEMBRANE
IRRITATION.MAYBE HARMFUL ~F SWALLOWED,
INHALED OR ABSORBED
THROUGH
SKIN.
FERROUS
SULFATE
FeSO
4 ¯ 7H20
H18C1N3S°3H20
C16
CAUSESEYE AND
SKINIRRITATION.
AND/ORSEEKMEDICALATTENTION.KEEPOUT OF REACH
OF CHILDREN.
READS~DEPANELBEFORE
USING.CAUSES
EYE. SKIN,
AND MUCOUSMEMBRANE
IRRITATION.MAYBE HARMFUL IF SWALLOWED,
INHALED OR ABSORBED
THROUGH
SKIN.
READS~DEPANELBEFORE
USING. CAUSESEYE AND
SKIN IRRITATION. HARMFUL IF SWALLOWED.
INHALED OR ABSORBED
THROUGH
SKIN.
WARNING
POTASSIUM
IODIDE
KI
FIRST AID: ¯ IN CASEOF EYECONTACT,
IMMEDIATELY
FL~H
IMMEDIATELY
FLUSHSKIN FREELY WITHWATER
¯ IF INHALED.GETTO
FRESH
AIR
¯ IF SWALLOWED
AND PERSON
IS CONSCIOUS.WASHOUT
MOUTH
WITHWATER.
AND/ORSEEKMEDICALA’I-rENTION. KEEPOUTOF REACH
OF CHILDREN.
FIRSTAID: ¯ IN CASEOF EYECONTACT.
IMMEDIATELY
FLUSH
¯ IN CASEOF SKiN CONTACT,
IMMEDIATELY
WASH
SKIN WITH
SOAPAND LARGEAMOUNTS
OF WATER
¯ IF INHALED.GETTOFRESH
AIR
WARNING
METHYLENE
BLUE
FIRST AID: ¯ IN CASEOF EYECONTACT,
IMMEDIATELY
FLUSH
¯ IN CASEOF SKINCONTACT.
IMMEDIATELY
¯ IF INHALED,GETTOFRESH
AIR
¯ IF SWALLOWED
ANDPERSON
IS CONSCIOUS,
GIVE LARGE
QUANTITIESOF WATER
ORMILK. DO NOTINDUCEVOMITING,
OF CHILDREN.
IMMEDIATELY
FLUSH
EYESFREELYWITHWATER
¯ IN CASEOF SKIN CONTACT.
IMMEDIATELY
FLUSH
SKIN FREELY WITHWATER
¯ IF INHALED.GETTO FRESH
AIR
¯ IF SWALLOWED
AND PERSONIS CONSCIOUS,WASHOUT
MOUTH
WITHWATER.
OF CHILDREN.
WARNING
READSIDE PANEL
BEFORE
USING.
WARNING
6 ml
IMMEDIATELY
FLUSH
EYESFREELYWITHWATER
¯ IN CASEOF SKINCONTACT.
IMMEDIATELY
¯ IF INHALED.GETTO FRESH
AIR
¯ IF SWALLOWED
ANDPERSON
IS CONSCIOUS,
IMMEDIATELY
GIVEWATER
..
AND/ORSEEKMEDICALAI-rENTION. KEEPOUTOF REACH
OF CHILDREN.
USING.CAUSES
EYE, SKIN,
AND MUCOUSMEMBRANE
IRRITATION. HARMFUL
IF
INHALED OR ABSORBED
THROUGH
SKIN.
Page 56
IMMEDIATELY
FLUSH
EYESFREELYWITHWATER
IMMEDIATELY
FLUSH
SKIN FREELY WITHWATER
¯ IF INHALED,GETTO
FRESH
AIR
¯ IF SWALLOWED
ANDPERSON
IS CONSCIOUS.
IMMEDIATELY
GIVEWATER..
IN ALL CASES. CONTACTA POISON CONTROLCENTER
AND/ORSEEKMEDICALA’ITENTION. KEEPOUT OF REACH
OF CHILDREN.
FIRSTAID: ¯ IN CASEOF EYECONTACT.
IMMEDIATELY
FLUSH
EYESFREELYWITHWATER
IMMEDIATELY
WASH
SKIN WITH
SOAPAND LARGEAMOUNTS
OF WATER
¯ IF INHALED.GETTO
FRESH
AIR
¯ IF SWALLOWED
AND PERSON
IS CONSCIOUS.WASHOUT
MOUTH
WITH WATER.
OF CHILDREN.
IMMEDIATELY
FLUSH
EYESFREELYWITHWATER
¯ IN CASEOFSKIN CONTACT,
IMMEDIATELY
FLUSHSKINFREELY WITHWATER
¯ IF INHALED,GETTOFRESH
AIR
¯ IF SWALLOWED
ANDPERSON
IS CONSCIOUS.
IMMEDIATELY
GIVE WATER.
OF CHILDREN.
APPENDIX C
Chapter 7
AcidandBase
Solutions
..............................................................................................................
Section
1 - ThepHScaleandIndicators
..........................................................................
Section 1A- Dilution
of anAcid............................................................................................
Section 2 - Natural
Indicators
............................................................................................
Section 3 - Natural
Indicators
............................................................................................
Section 4 - Other
Natural
Indicators
..................................................................................
Section 5 - Testing
for Acids
andBases
............................................................................
Section 6 - Testing
RainWater
for pHValue
....................................................................
Section 7 - Testing
thepHof Other
Chemicals
..................................................................
page 32
page 32
page 33
page 34
page 34
page 35
page 35
page 35
page 36
Chapter 8
Titration,A Quantitative
Method
....................................................................................................
Section 1 - Preparation
of a Standard
BaseSolution
........................................................
Section 2 - Testing
Vinegar
Solutions
................................................................................
Section 3 - How
Much
AceticAcidis in Vinegar?
..............................................................
Section 4 - Comparing
DifferentBrands
of Vinegar
..........................................................
Section 5 - How
Much
Base
is in AntacidTablets?
..........................................................
Section 6 - Different
Brands
of Antacid
..............................................................................
page 37
page 37
page 37
page 38
page 39
page 40
page 40
Chapter 9
Electrochemistry
Section 1 Section 1 ASection 2 Section 3 Section 4 Section 5 Section 6 Section 7 Section 8 -
Appendix A
Answers
to Experiment
Questions
..............................................................................................
page 49
Appendix B
ThePeriodic
Table
of Elements
....................................................................................................
page 53
Appendix C
ANote
to AdultsandParents
......................................................................................................
page 55
A NOTE TO ADULTS AND PARENTS
Youhave wisely chosento purchasethe NSI XM4000chemistry set. With this set, you have started your child on the path
of learning about SCIENCE
and the wondersfound in the world of chemistry, biology and physics. But rememberalso, too
little knowledgecan be a dangerousthing. Real scientists use powerful tools, substanceswhich can be poisons and may
cause harm if misused or misapplied. Becauseof this, the WARNINGS
on this set are REAL.They apply to the materials
WHEN
USEDIN LARGER
QUAN]I! IES! BUT, that is not the case here! HERE’SWHY!The amounts are deliberately
madesmall and dilute. They are less LIKELYto cause harmbecauseof the limited quantity and form. BUT,westill want
YOUANDYOURCHILDto READ,HEEDANDUNDERSTAND
the instructions given you in the set. In this way, we trust
that POWERFUL
chemicals may be SAFELYUSED,in many fun experiments. Remember,too, if you have any questions
about CHEMICAL
HEALTHANDSAFETYcontact your local physician or Poison Control Center, or Natural Science
Industries.
Chemicalssupplied in your microplate are:
Well B-l: Cobalt Chloride
Well B-2: CalciumNitrate
Well B-3: Ferrous Sulfate
Well B-4: MethyleneBlue
Well B-5: Phenolphthalein
Well B-6: Universal Indicator
Page 55
........................................................................................................................ page
42
page
42
Detecting
..........................................................................................................
page 43
Detecting
theFlowof Electrons
......................................................................
page 44
ASimple
Cell..................................................................................................
page 44
ASimple
Battery
..............................................................................................
page
45
Another
Battery
................................................................................................
page
45
Activityof Metals
..............................................................................................
page
46
OtherElectrochemical
Reactions
....................................................................
page
47
Corrosion
of Different
Metals
..........................................................................
page
48
ACorrosion
Pair..............................................................................................
II
Thesafest wayto handleANYchemicalis to treat it as if it were
CHAPTER1
’1’!!!~
)lOS’r
l)i~tl)l.¥
APPENDIX B
THE PERIODIC TABLE OF ELEMENTS
I~OISON
NOBEL
Introduction
_A_W~O_RD
TO PARENTS
This laboratory manualis prepared with one main concern:
/
1) NEVER ALLOW A CHILD TO EAT ANY CHEMICAL OR
THE PRODUCTSOF THEIR EXPERIMENT!
In recent years the ecological and health sciences have
stated that exposure to certain chemicals, either in work,
school, or at home, can cause serious health problems. Yet
youngscientists needthe "handson" experience,the thrill of ex*
perimentation, and the satisfaction of discovery which is possible only through labs.
mA
10.81
0.083
2.34
NEVER ALLOW THEM TO EAT FOOD WHEN YOU ARE
EXPERIMENTING. DO NOT ALLOW ANY LIQUID TO BE
DRUNK WHILE EXPERIMENTATION IS BEING CONDUCTED.
2)
CAUTION A CHILD NEVERTO HANDLEA CHEMICAL
WITH THEIR BARE HANDS. USE A SCOOP OR FOLLOW
DIRECTIONS FOR MAKING A PLASTIC SCOOP TO MEASURE OUT SOLID CHEMICALS.
The MicroChemistry approach has been adopted by high
schools and colleges throughout the United States. The use of
small amounts of chemicals to investigate the workings of
chemistry in no way lessens the excitement of experimentation.
Yet, this approachreducesthe possibility of exposureof the experimenter to harm from chemicals necessary for the experimentitself.
3) LIQUID CHEMICALS ARE ALWAYSDISPENSED WITH A
SPECIAL PIPETTE.
USE ONLY DROPS OF CHEMICAL
FROMTHIS PIPETTE. DO NOT USE THIS PIPETTE OR ANY
OTHER EQUIPMENTIN THIS SET FOR OTHER PURPOSES!
This is not to say that ALL CHEMICALS
and CHEMICAL
PROCESSES
in the MicroChemistry approach are absolutely
safe.
__.ALL CH.~MICALS AND PROCEDURES
HAVE A POTENTIAL TO CAUSE HARM.
MicroChemistrylessens that possibility by reducing, considerably, the amountof materials used. By using plasticware,
minimal amountsof glassware, by eliminating the use of fire or
burners andrestricting the use of heat, an additional safety factor is provided. MicroChemistryequipmentis safe and easy to
use.
Fromthe scientific viewpoint, for the first time in ANY
chemistry set, young experimenters will be able to tell HOW
MUCH
of a substancereacts or is present rather than only looking at generalproperties.
Someof the experiments in this manualare:
for example,be able
20~
0~.7
IB
QUANTITATIVE
This meansthat youngchemistswill be able to tell, for example,
HOW
MUCH
starch there is in a sample of food.
Prior to the MicroChemistry approach, QUANTITATIVE
experiments by youngscientists were not possible.
Even though MicroChemistry is safer than the chemistry
whichrequires morematerial, it is important to realize that you
are STILL handling somepotentially harmful materials.
iV A
V A
~-12.011
I 2[0.077
I 210.070
BH2.267
I
]
] 130.974
~
I ~n~5
~+~+:~
29 COPPER
0.125
8.90
63.546
0.!28
8.96 Cu
.
65.38
z8 0.133
7.13
0.00018
H.
WA
~
VI~ A
~5
9;9--~~.998-~
I ;10.066
I z10.072
ALWAYS WORKWITH GOGGLES.
46 PALLA01U
M
47
5) CHILDREN SHOULD WORKUNDER THE SUPERVISION
OF AN ADULTAT ALL TIMES.
106.4
0.138
12.02 Pd
107.868
0.144
18 0.149
10 50 ~g
8.65
6) IF THERE IS A SPILL OF ANY CHEMICAL, THE AREA
SHOULD BE CLEANED THOROUGHLY.
2+.3+4+
7) WASTE CHEMICALS FROM EXPERIMENTS AND MATERIALS USED TO CLEAN AN AREA OF SPILL OR ACCIDENT
SHOULD BE DISPOSED OF IN AN ENVIRONMENTALLY
SAFE MANNER.
79
t95.o9I
0.138
~÷"......
SILVER
"~
GOLD
] I 35 453
I 39948
I~ 0.191
~-"~"
I I
~
I I
I -
°.°°4
"I"I
~A~
J~l
Cdl;~
80 MERCURY
196.967
; 200.59
28
1,810.!44
0~~
19.3 Au ’8 13.546 Hg
~~
~
0.~
o~.1
1’1
¯ NOTE. Symbols&narnesusedare assignedby IUPAC
O, fferent names
& symbols
arefrequentlyused/nthe U.S.& C.I.S. (fom~erlyU.S.S.R.)
8) IT IS IMPORTANTTO COVERCLOTHINGWITH A PROTECTIVE LAYER OF CLOTH, PLASTIC OR RUBBER. YOU
SHOULDOBTAIN AN APRON (LIKE A WORKSHOP
APRON)
AND WEAR IT WHILE YOU WORKWITH YOUR CHEMISTRY
SET. A PROTECTIVE PIECE OF PLASTIC SHEET SHOULD
BE USED UNDER YOUR WORK AREA TO PROTECT THE
SURFACE YOU ARE WORKING ON.
Whileit is fitting that your child learns someideas andprinciples about chemistry while experimenting with his/her new
set, it is important that he/she have FUNwhile exploring and
discovering! Throughout this Laboratory Manual, questions
have been provided to help the experimenter "HOME
IN" on the
principles of chemistry. Someanswersare given right in the
experiment, while other answerscan be found in the Appendix
at the end of the Laboratory Manual.
~
I ~ 0.~0
I ~10.~04 I q0099
1+2+
4)
--
I . 132.06
J2
I
I 8l
ZnJ ~!J
ELECTRON
O,STR,BUT,O
KEY
ELEMENT NAME
162.50
0.177
8.550 Dy
3+
2
2
14
ERBIUM
69 THULIUM
Cf 28
FERMIUM
3+
70 YTTERBIUM
8
2 --
2 2+3+
2
101 MENDELEVIUM
102 NOBELIUM
~ 257.095
18 _
Es3229
--
2
3+
EINSTEINIUM100
254.088
--
--
2
3+
98 CALIFORNIUM 99
251.08
68
2 164.930
z8 167.26
z 168.934
~
2
8
8
8 17304
8
’8 0.176
18 0.194
,8
0.177
~8 0.175
~
~o
HO
;~1
8.795
8 9.066 Er 8 9.321 Tm 8 6.965 Yb 328
~ 258
Fm 32
)8 __
8
2 --
8 255.093
18
32
Md 3~
-8
2 --
82
No 32
32
8
2
It is hopedthat by providing interesting questions along
with the experiments, the young chemist will develop a basic
knowledgeof chemistry along with the workings of chemistry.
Page 1
4.003
\ 0.122
el.J0.001Nl~10.00,
0l~10002 FJ,0.001
~
lib
66 DYSPROSIUM 67 HOLMIUM
Someof the experimentsin this manualare:
NONMETALS
- ...................................
"
SafetyRules
SAFETY!
QUALITATIVE
This meansthat if a test is doneyou will,
to tell if starch is presentin a food.
GASES
Follow these simple rules to insure that your interest in
chemistry will not be stoppedby an injury or sickness causedby
mishandling your experiment.
ATOMIC
NUMBER
-,’-29
COPPER
"ATOMIC MASS
(AMU)
’63.546
"ATOMIC RADIUS
(NM), .,.-0.128
"DENSITY
~) -(GiCM
..-8.96
-.,~-’- K SHELL
Cu
18
OUTERMOST
~SHEI.L
MAJOR -OXIDATION
STATES
ELEMENT SYMBOL
¯ Values
for atomic mass, etc.
rounded to the nearest lO00th.
Page 54
are
APPENDIX B
THE PERIODIC
TABLE OF ELEMENTS
CHAPTER2
A Word to
IA
You live
1 HYDROGEN
1 008
0 053
0.0001 H
IIA
METALS
¯
6.941
2 0.152
9 012
0 111
I 21
i~848
U
Li
Be
0.5341+
11
TRANSITION ELEMENTS
SODIUM 1_~2 MAGNESIUM
J
I
1,124.3°5
0.192
I 10 160
] 1
Iv B
J~’~S~U-M
’ t
l
0.227
0.862
VB
V~ B
VIIIB
V, B
SC~.=UM
I el0 197
KI e/,.S5
C
0 16
~.989
47.90 I ;I 50.942
I 2151._~96
I 2154938I ;I 55847I ;I 58933
Sc
4540145
874°~1"1
"1’01 I1’ =’1"1Mn{"~
8.92
co
~ ST.0.TIUM ] 3~ YTTNIUM
1.532
R"
2.54
91.22
0 160
Srl ~14469
55.......
CESIUM
~
132 905
0.265
1 873 Cs
137 33
0.217
~92.906
I ,~1 0 ;43
~9594
I ,~1 0 136
~
96906
I ,~1 0.136
~101.07
I ,;I 0 133
~102906
I ,~1 0 135
~’~$-~Ei~-6 ......
;8 174 967
~8 0 173
;
lib
~2849I ;I 180.948
II ~1 0.137
0n56
I~1 0.143
I;I
I
I ~ 0.137
I
1,*
87
FRANCIUM
223 02
0.27
~
226 025
0.220
256099
I ~
SAFETY
A WORDTO
THE "CHEMIST"
No matter what the experiment, equipment, or procedure,
one thing should be the first to think about:
SAFETY
The "Chemist"
Follow these simple rules to insure that your interest in
chemistry will not be stopped by an injury or sickness
caused by mishandling your experiment.
in an EXCITINGworld.
It is a world full of the latest in TECHNOLOGY
(the use of
scientific
knowhowin every day life) and invention. Many of the
things in today’s world were never considered to be possible a
few years ago. The advancements in technology could only be
possible by advancement in the basic sciences. For example,
scientists
found that by treating silicon wafers with certain
chemicals that the electrical
conducting ability of the silicon
wafers was changed in certain ways. This discovery opened up
a whole world of "electronic micro chips" which helped in the
development of computers and other electronic devices.
Your chemistry set is an excellent starting point to advance
your skills as a scientist.
The world of science is a world of questions.
While you are working on your experiments in this manual,
a series of questions will help you understand the hows and
whys of what you are seeing. The answers to some questions
will be given right after the questions in the experiments. The
answers to other questions will be given in the Appendix section
at the end of the Laboratory Manual.
The world of SCIENCE is the world of OBSERVATION.
Scientific
Observation means that the experimenter looks for
and writes down (records) all the changes which happen that
can be seen, and records how much these changes can be
measured (quantifies).
Everything that scientists
do depends on their ability
to
make careful observations and measurements about their experiences. We call these experiences EXPERIMENTS.An experiment is a carefully controlled set of situations which allows a
scientist to see what effects a change in a single VARIABLEwill
have on the rest of the experiment. A variable is a single part of
the experiment.
SAFETY RULES
NEVER
EAT ANY CHEMICAL OR THE PRODUCTSOF
YOUR EXPERIMENT!
NEVER EAT FOOD WHEN YOU ARE EXPERIMENTING.
DO NOT DRINK ANY LIQUID WHILE YOU ARE EXPERIMENTING.
2)
NEVER HANDLE A CHEMICAL WITH YOUR BARE HANDS.
USE A CHEMICAL SCOOP.
FOLLOWDIRECTIONS ON
PAGE 4 FOR MAKING A PLASTIC SCOOP TQ MEASURE
OUT SOLID CHEMICALS.
3)
DISPENSE LIQUID CHEMICALS WITH CARE. USE ONLY
DROPS OF CHEMICAL FROM A SPECIAL MEDICINE
DROPPER CALLED A PIPETTE.
THESE PLASTIC PIPETTES ARE PROVIDEDIN YOUR CHEMISTRYSET.
4)
USE CHEMISTRY SET EQUIPMENT FOR EXPERIMENTS
IN YOURCHEMISTRYLAB MANUALONLY.
5)
ALWAYSWORKWITH GOGGLES, IN PLACE, OVER YOUR
EYES.
6)
YOU SHOULD WORKUNDER THE SUPERVISION OF AN
ADULTAT ALL TIMES.
7)
IF THERE IS A SPILL OF ANY CHEMICAL, THE AREA
SHOULD BE CLEANED THOROUGHLY.
MATERIALS
USED TO CLEAN THE AREA SHOULD BE DISPOSED OF
IN A SAFE MANNER.
IT (S 1~4P(~F~TANT
T~ ~C’)\II=R Y(")l IR WORK
ARFA
PROTECTIVE NEWSPAPER,LAYER OF CLOTH OR PLASTIC.
and the effects of a change of things important to a plant.
We would start with two sets of plants. The two sets of
RAREEARTH ELEMENTS
57 LANTHANUM58 CERIUM
138.906
LANTHANIDE 0.188
SERIES
6 145
3+
89
140 12
0.183
6.657 Ce
3+ ~+
59PRASEODYMIUM
60 NEOOYMIUM
61 PROMETHIUM
62 SAMARIUM
2
2
;
140.908
144 913
8 144.24
8
8 150.4
~e 0.182
0.183
0.181
~ 0.180
Pr ;~ 6.90
Nd 8’
6.64
7.22 Pm ~ 7.520 Sm 8
63 EURDPIUM 64 GADOLINIUM65 TERBIUM
2
151 96
8 157.25
0. 204
~8 0 180
5.243 Eu 25 7.900 Gd
2 3+
2+.3+
2
2
34.
2+ 3+
PROACTINIUM
92 URANIUM 93 NEPTUNIUM 94 PLUTONIUM N5 AMERICIUM 96 CURIUM
ACTINIUM 90 THORIUM 91
~ 232038
227.028
;8 231 036
8
ACTINIDE 0 188
~ 0.180
0.161
SERIES 10.07 AC
Th 3;:8 1537
~z~8
11.7
2 4+
3+
2 4. 5*
~! 238.029
~8~0.139
32I
Pa ;’~1
1895U
~ 3+4+5+6*
237048
~ 244.064
~ 243.061
~ 0.157
~8
0.131
32
~
PU ~! 13.67 Am
9 20.25 Np ~9 19.816
3+4+64-
Page53
2 3÷4~6~
2
3..4.~
82
247.070
13.51
2
158.925
0.178
18.23
Tb
13+
: 97 BERKELIUM
247.070
C~
14.78
Bk
plants have to be identical to each other. They must be of the
same species, size, age, etc. One set would be a CONTROL,
or standard. The control set would be compared with an EXPERIMENTALgroup. The control plants would be treated in a
normal manner. An experimental set of plants would have the
same treatment as the control,
EXCEPTFOR ONE PART. This
is the VARIABLE. In our experiment, let’s select temperature
as the variable.
In the experiment, the control and the experimental plants
would have the identical soil, receive the sameamount of water,
and have the same lighting.
The temperature surrounding the
experimental plants, however, would be different
than the control plants. By making careful observations, the scientist would
be able to see what effect temperature has on the growth of
plants. He could do this by comparing the experimental plants
to the control plants.
In this laboratory manual you will always be asked to compare an EXPERIMENTAL to a CONTROL.
9)
DISPOSE OF USED CHEMICALS IN A MANNERWHICH IS
ENVIRONMENTALLYSAFE. TALK TO YOUR PARENTS OR
SCHOOL SCIENCE TEACHER ABOUT THE BEST WAY TO
DISPOSE OF CHEMICALS.
CHAPTER 3
THE MICROCHEMISTRY
SYSTEM
The MicroChemistrySystem
Your
chemistry
setis different!
It usesthe latest methods
in experimental
chemistry.
These
methods
weredeveloped
to make
chemistry
a saferscience.
Page 2
The MicroChemistrySystemuses smaller amountsof chemicals than other chemistrysets. Thehazardsof glass havebeen
minimizedby the useof plastic labware.If a chemicalreaction
mustbe heated, hot water will provide the neededheat. Open
flames or burners are NEVER
used in MicroChemistry.
By usingMicroChemistry
youwill be able to do moreexperiments,get better results in a shorter amount
of time andhave
a safer environment
in whichto work. Yourworkin the laboratory will bemoreefficient. Thatmeans
youwill be ableto have
moretime to explorechemistryandhavemorefun doing it!
Youwill needthe followingmaterialsto complete
this series
of experiments.
Chapter 8 - TITRATION:A QUANTITATIVE
METHOD
~000000000
~000000000
cO00000000
o O00000000
0
0 O~
0 0 O~
0 0 Oc
0 0 Oo
SECTION1 - PREPARATION
OF LABORATORY
EQUIPMENT
Figure #1A
BE SURE TO WEARGOGGLESWHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
Thetray is divided into two parts. Eachhasa series of
rowsand columns.This makesthe microplatevery orderly. It
also makes
a groupof experimentalchemicalreactions easyto
compareto a control group. Changes
in color, or any other
changesin a reaction can be easily seenwhencompared
to the
control.
Thebottom row of the microplate contains the various
chemicalsyouwill be using in your experiments.Thesechemicals are permanently
kept in this rowof large microwells.
Thechemicalssuppliedin the B wells of your microplate
are:
B-1: CobaltChloride
B-2: CalciumNitrate
B-3: FerrousSulfate
B-4: MethyleneBlue
B-5: Phenolphthalein
B-6: UniversalIndicator
LIST OF MATERIALS
[]
-I
Microplate(from your chemistryset)
Threeplastic pipettes(from your chemistryset)
[] Smallpieceof cotton (obtain at groceryor drugstore)
fl
Pair of scissors(from home)
Measuring
cup(from your chemistryset)
[] Distilled water(fromgrocery)
--1 Rubbing
alcohol or isopropylalcohol (from grocery
or drugstore)
[] Goggles
~ Storage case
YOUR WORKSPACE
MicroChemistry
usestwo basic tools:
the microplateandthe plastic pipette.
Theremainderof your chemicalsare supplied in plastic
vials (small plastic bottles) contained
in yourchemistry
set.
There are 48 "small wells" or depressions in the
MICROPLATE.
These are numberedas columns #1 through
#12. Theseare also lettered as rowsA,B, C, D. Duringtesting
of reactions,youcanidentify individual reaction"wells" by using
the rowand column.For example,"Smallwell A-7 or Smallwell
C-10".
There are 12 "large wells" or depressions in the
MICROPLATE.
Theselarge wells are located directly down
from the small well section. Thelarge wells are numbered
as
columns
1, 2, 3, 4, 5, 6.
Thesecolumnnumbersfor the large wells appearat the
base of the MICROPLATE
near the bottom edge. The deep
wells are lettered as rowsA andB. Youcanidentify individual
large wells by the samemethodyouidentified the small wells,
for example,
"Largewell A-6or Largewell B-2".
Figure#1
MicroplateUnit
PLASTICPIPETTE
(medicinedropper)
MicroChemistry
usesa plastic pipette, suchas in Figure#2.
THE MICROPLATE
Thefirst is a plastic tray called a microplate.Thistray is
very sturdy. Thetray hasshallow wells arrangedin order of
rows (running across) and columns(running up and down).
Thesewells are usedinsteadof test tubes, flasks andbeakers.
SeeFigure #1A.
STEM
"-,
Figure #2
Page 3
_
10) Theactivity of a metalpair canbe determined
by the size
of the movement
of the compass
needle. Thegreater the
swingof the needle,the moreactive the metalpair.
SECTION1
5)
A solution of sodiumbicarbonateconductselectricity becausesodiumbicarbonateionizes in water. If a drop of
UniversalIndicator is addedto sodiumbicarbonate,the indicator turns blue to indicate the presenceof a base.
Sodiumhydroxide, ammonium
hydroxide, calcium hydroxide and potassium carbonate are commonbases.
Individual tests with UniversalIndicator will showwhichof
the salt solutionsin the chemistryset are bases.
11) Inactive metalsare useful in applications wherea resistanceto corrosionis important.Inactive metalswouldhave
a longeruseful life thanactive metals.
SECTION6
7)
SECTION2
2)
Sodiumacetateis the nameof the salt formedwhensodiumbicarbonatereacts with acetic acid. Thegasformedis
carbondioxide.
The metals which were not coated would be expectedto
corrode.Metal whichwaswrapped
in zinc wire did not corrode becausethe moreactive zinc metal corrodedbefore
the metalwith whichthe zinc wasin contact.Thezinc functioned as a SACRIFICIAL
METAL.
SECTION8
SECTION4
4)
5)
Household
productswhichtest positive with UniversalIndicator are acids. Common
acids are citrus juices, vinegar
and soda water. The amountof base in a substancecan
bedetermined
by the processof titration.
SECTION5
8)
ThepHof a solution will varywith the substance
beingtested. ThepHcanbe estimatedby comparing
the color in the
test solution with the indicator with the standardcolors of
the indicator as determined
in the previousseries of experiments.
SECTION6
Basescommonlyfound in the homeare milk of magnesia,
householdammonia,and milk.
Chapter 9 - ELECTROCHEMISTRY
SECTION1
7) Thecompass
needlemovesto the left or to the right. The
movement
indicates that a current is flowing throughthe
wire fromoneendof the battery to the other.
10) When
the connectionsare reversed, the needle movesin
the oppositedirection. As electrons movethrougha wire
they createa magneticfield whichaffects the compass.
SECTION2
6)
BULB
SECTION5
Theneedle of the galvanometermovesin responseto a
flow of electrons. By comparingthe movement
noted in
this experimentto the movement
in the previous experiment,the direction of electron flow can be determined
in
SECTION
3.
Electrons flow from the NEGATIVE
TERMINAL
of the battery or cell to the POSITIVE
TERMINAL
of the battery or
cell.
Page 52
Themetals corrodedin the expectedmanner.Changes
in
the solutions wouldalso be noteddue to a changein the
pH of the solution as indicated by the changein the
Universal Indicator color change.Evidenceof corrosion
wouldbe seenon the nail similar to previousexperiments
onthe activity of metals.
SECTION 13
SECTION 4
chloride with calcium hydroxide
5) The reaction of ammonium
3)
will produce ammoniagas. The ammoniagas dissolves in
the moistened filter
paper and causes the Universal
Indicator to changecolor.
Electrolytes causethe indicator to glow while non-electrolytes do not causethe indicator to showconductivity.
9) The combinations of chemicals which produce a precipitate
or gas gives an indication that a chemical reaction has
taken place.
SECTION 14
The chemicals in your chemistry set will most often be in
SOLUTION. This means that the chemical has been DISSOLVED
in water. Solutions of chemicals react faster and more
evenly than if the chemical were in the powderedor solid form.
In fact, manyof the experimentswhich will be donein this manual would not be possible if the chemicalswere not in solution.
Your pipettes are kept in the receptacles provided in your lab
station stand.
The pipette is madeof POLYETHYLENE.
This form of plastic
is soft andis very DUCTILE
(flexible).
Examineone of the pipettes provided in your chemistry set.
Youwill observe that it has an enlarged area called a BULB,a
long tubelike section called a STEM.You maywish to form a
microtip on one of your pipettes. This can be done by pulling
the tubelike portion of the microtip until it stretches into a thinner diameterandthen cutting the lower portion off with scissors,
allowing only the very thin tip to be the endof the stem.
Making a Chemical Scoop
4) & 5)
The filter
paper which had been soaked in Universal
Indicator will changecolor as the ammonia
is reacted with
the vaporsof vinegar.
Whenit is necessaryfor you to use a solid in an experiment, the chemical solid can be transferred by the use of a
CHEMICALSCOOP. We can very easily make a CHEMICAL
SCOOP
out of another pipette.
1) Hold a plastic pipette by the stem.
2) With scissors, cut through both sides of the pipette at
an angle. SeeFigure #3 for a picture of the procedure.
The cut pipette makesan excellent chemical scoopfor
any solids whichwill be usedin the rest of the experimentsin the laboratory manual.
SECTION 5
7) & 8)
The reactants would be electrolytes since their solutions
showedconduction with the conductivity tester. Oneof the
productsof the reaction is a precipitate. Precipitates do not
dissolve or ionize in water. If no ionization takes place, a
solution of a chemical doesnot showconductivity.
6) Thevinegar will eventually tint the Universal Indicator back
to greenand finally to orangeor red. The side of the paper
closest to the vinegar vaporswilt changecolor first.
The reaction of householdvinegar (acid) with calcium hydroxide (a base) and ammonium
chloride would produce
solution which would cause the Universal Indicator to
return to its greencolor.
Chapter 7 - ACID AND BASESOLUTIONS
SECTION 1
SECTION 15
Figure #2A
3) By diluting the acid by a factor of 10, the amountof acid per
unit volumeis decreasedby an equal amount.
7) The Universal Indicator paper would showthat the reaction
would produce a basic gas, ammonia. You would know a
reaction occurred by the changein the color of the paper.
7) By diluting the base by a factor of 10, the amountof acid
per unit volumeis decreasedby an equal amount.
10) TheUniversal Indicator will turn different colors dependent
on the amountof acid or basein the solution in eachwell.
Chapter 6 - EXPERIMENTSWITH SOLUTIONS
11) Phenolphthalein
is different than Universal Indicator since it
has only one changeof color. Phenolphthalein is a single
chemicalindicator. Universal Indicator is a mixture of several indicators.
PRE-LAB:
1)
Any metallic alloy is an example of a solid solution.
Stainless steel, carbonsteel, gold jewelry, etc., is a solid
solution.
2)
Air is a goodexampleof a solution of a gas in a gas. In the
case ef a!r, nitrogen is the so!vent since it !s in greater
amountin the air.
The plastic PIPETTEwill be used to dispense drops of
chemical liquids to the microplate wells where your chemical
reactions will take place. The use of the PIPETTE
is just the
sameas the use of a conventional medicine dropper or eye
dropper. Whenthe tip is placed below the surface of a liquid
and the bulb squeezed BETWEENTHUMBAND FOREFINGER,and then released, the PIPETTE
will draw up liquid into
the bulb. The pipette can then be used to deliver drops of liquid or chemicals to your MICROPLATE
wells.
/
Figure #3
Makinga Filter Funnel
Wecan makea filter
1) Hold a plastic pipette by the stem.
2) With scissors, cut through the entire pipette straight across
the bulb of the pipette.
3) Place a small piece of cotton from a cotton swabor cotton
ball in the bottomof bulb. SeeFigure #4 for a picture of the
procedure.
SECTION 4
Eachindicator changescolor at only one concentration of acid
or base. Often, a single chemical indicators maybe found in
more than one source.
SECTION 2
4) Pure water is not an electrolyte.
Tap water is not pure
water. Try to detect conduction with distilled water. There
should be little or no conductivity. Tap water contains some
salts and chemicals addedto prevent bacterial contamination.
SECTION 5
4) Youwill be able to tell if eachproductis acid or baseby the
SOLUTION
TO BE
CUT ~
Slowlyrelease
bulb anddrawliquid
upinto pipette
To deliver drops,
gently squeeze
bulb.
color of the Universal Indicator. It is very unusualto find a
product which is neutral.
7) Non-electrolytes are solutions of either compoundswhich
TrON
Figure #2B
have carbon in the molecule or are precipitates.
Electrolytes are solutions of inorganic compoundswhich
dissolve and ionize in water to form chargedparticles.
CUT -:
SECTION 6
8)
SECTION 3
Conductorsconduct electricity.
electricity.
funnel from another pipette.
Non-conductorsdo not conduct
Page..51
An indicator which turns color near the range of pure water
would be most useful. Ask your teacher about the normal
pHof rain.
The pipette can be used over again by simply rinsing the
stem and bulb between chemicals. Water and chemical solutions do not "stick" to the plastic inside the pipette the waythey
might if the pipette wasmadeof glass or rubber. The plastic
surface of the pipette is NON-WETTING.
This meansthat all
the contents of the pipette can be dispensed with none of the
chemicalleft behind.
Figure #4
Delicatefiltering of liquids into test tubesor into wells of the
MICROPLATE
can be accomplished using the microfunnel.
Figure #4B shows how a funnel stand is made from a small
piece of folded card stock.
Page 4
Noticehowit opensto allow the pipette to enter the chemical
vial. Noticehowit closesbackup after youtakethe pipette out.
Youmayhaveto usea pencilor ball point pen’spoint to initially openandwidenthe "H" cuts in the seals so that your
pipettecaneasily be insertedinto the vial well.
Thechemicalin eachvial well is either on small strips of
special paperor as solids in precisely measured
amounts.
Lookat oneof the plastic vials (small plastic bottles).
Notice that eachhas a screw-on,screw-off cap. Thecap is a
safety cap. To get it off, simply pushdownon the plastic cap
and unscrewthe cap. If you turn the cap clockwise it gets
tighter. If youturn the capcounter-clockwise
it comes
off.
\.._../"
SECTION4
7) & 8)
TheUniversalIndicatorturns two different colors in the two
wells. Thepositive electrode well producesoxygengas
(whichis soluble) andan orangeor red color is seenwhen
the indicator is present. Thenegativeelectrodeproduces
hydrogen
and is coloredblue.
oxygengas is
9) As the hydrogenperoxide is decomposed,
generated.As the oxygengas bubblesthrough the methyleneblue solution the methylene
blue is decolorized.
SECTION5
8) As air goes into the methyleneblue solution, a small
SECTION10
amountof oxygenin the air causesthe methyleneblue to
de-color in the samewayas in SECTION
4, part 9. Oxygen
gas is the only gaswhichdecolorizesmethylene
blue.
1) Thelast or control well is left aloneto showthe original
Push Down
Figure #4A& 4B
SECTION9
Push Down
A Measuring Cup
color of the coppersulfate solution beforethe reactionhas
occurred.
SECTION6
2) & 3)
Thecoppersolution did not changein the control or copper
wire well. Thewell which containedthe zinc wire faded
whenthe zinc wasleft in the solution.
Oftensolid material will be requiredin your experimentation. In order to weighout correct amounts
of solid materials,
youwill needto usethe plastic measuring
cup. SeeFigure#5.
aids in the decomposition
of hydrogenperoxideto water
and oxygen.Thegas, oxygen,can be identified by oxygen’sability to decolorizemethylene
blue.
4) & 5)
Asthe zinc wire reactedwith the copperion in solution, the
zinc metal in the wire became
zinc ion and dissolvedinto
the solution. Zinc in aqueous
solution is colorless. The
copperwire in the coppersolution showed
no change.
Turn
To Open
3) Liver andpotatocontainthe natural catalyst catalasewhich
To Close
SECTION8
6) Whenthe leaf is exposedto light, photosynthesisoccurs.
Photosynthesisproducesoxygenas one of its products.
Theoxygendecolorizesthe methylene
blue solution.
SECTION9
Chapter 5 - THEGASEOUS
PHASEOF MATTER
5) Thecarbondioxidereacts with the calciumhydroxidesolu-
Figure #6
tion to formcalciumcarbonate,
a whiteprecipitate. Theformationof a white precipitate whena gasis bubbledthrough
calciumhydroxidesolution provesthe presenceof carbon
dioxide.
SECTION1
Figure #5 - Plastic MeasuringCup
Thesemeasuringcupsare providedin your chemistryset
andare printed on their sides with different lines andmeasurements. Thereare measurement
lines for teaspoons(tsp) and
tablespoons(tbs) andalso measurement
lines for fluid ounces
(fl. oz.). Thereare measurement
lines for cubiccentimeters
(cc)
andfor milliliters (ml).
Alwayskeepthe plastic measuring
cupscleanand dry.
PART TWO
Preparingthe ChemicalVial Well
When
a solvent is addedto the vial, the chemicalsdissolve
uponshakingthe microplate, and formsthe chemicalsolution
whichyouwill usein your experiments.
Thechemical’sname
is printed on the label on the exterior
portion of eachvial well. Specialreceptaclesare providedin
yourlab station standto holdthe microplateandits contents.
IMPORTANT NOTE: READ THESE DIRECTIONS BEFOREADDINGANYLIQUID TO YOURCHEMICALS!
ADDING SOLVENT
EXPERIMENTS
IN THIS CHEMISTRY
SECTION!
All of the chemicalvial wells andchemicalvials in this
chemistryset will produce
the chemical
solutionsyouwill usein
your experiments.
Thesespecial vial wells are actually the large microplate
wells in the "B" rowof your microplate. Eachof the chemical
wells is cappedwith an "H" seal, and is labeled as to what
chemical
it contains.
Theother separatevials in your chemistryset will produce
other chemicalswhich you will needin experiments.Eachof
the chemicalvials are also cappedwith an "H" seal. Eachvial
is labeledas to whatchemical
it contains.
Affixedto the top of the vial well is the vial sealingdisk.
Lookclosely at the sealingdisk. Youwill observethat thereis
a small"H" shaped
cut in the top of the seal. Thisis the "H" septurn sealingdisk.
The"H" cut in the seal is a specialopeningfor the stemand
tip of your pipette. Try pushingthe tip end of your pipette
throughthe "H" cut in the seal.
Page 5
Youare nowreadyto activate your chemicalvial wells and
your separatechemicalvials with either wateror alcohol. Be
sureto follow the directionsexactlyso that youwill put the correct liquid into thecorrectchemical
vial.
Youwill needto gatherthe followingmaterialsto complete
this procedure:
MATERIALS
--I Observethat someof the chemicalvial wells in your
microplate and your separate vials have YELLOW
TOPS.
Observethat someof the chemical vials wells in your
microplate and your separatevials have BLUETOPS
Twoplastic pipettes (medicinedroppers)fromyour set.
Oneplastic measuringcupfrom your set
Sharppointedpencil or ball point pen
Alcohol- either isopropylalcohol(rubbingalcohol)or ethyl
alcohol, fromyour local pharmacy
or grocerystore.
Distilled waterfrom your local supermarket
or pharmacy.
8) Asthe pressureon the gasis increased,the volumeof the
gas trapped in the columndecreases.Pressureand volumeare INVERSELY
related. Thehigher the pressure, the
smaller the volume.
SECTION10
9) Thereaction of the calciumcarbonatewith an acid producescarbondioxide gas.
SECTION2
6) Asthe gasin the bulbof the pipette is decreased,
the vol-
10) Calciumhydroxidereacts with carbondioxide to producea
whiteprecipitate of calciumcarbonate.
umeof the gas decreases. Weknow that the volume
decreases
because
the liquid level goesup into the pipette.
Thevolumeof a gas is DIRECTLY
related to the temperature of the gas.
10) As the air in the bulb is warmed,the volumeof the gas
increases. Theair whichis heatedexpandsandis forced
out into the well of water. Asthe temperature
on the gasis
increased,the volumeof the gasincreases.
11) Theprecipitation reaction hasbeenthe methodof testing
for carbondioxide in SECTION
9 andalso this section.
SECTION11
5) The reaction of an acid with sodiumhydrogencarbonate
producescarbondioxide. Precipitation of calciumhydroxide solution is a goodtest for the presence
of carbondioxide.
SECTION3
7) Asthe ammonia
vaporsleavethe well, the UniversalIndicator changesfrom green to blue. As the vinegar vapors
leavethe well, the UniversalIndicator changes
fromgreen
to orangeor red.
SECTION12
~ is a solid mixtureof anacid anda carbonate.
3) Alka-Seltzer
vaportravels faster than the vinegar vapor.
8) Theammonia
Theammonia
moleculeis smaller and travels faster than
the vinegar(acetic acid) molecule.
When
the Alka-Seltzer® dissolves, the acid and the carbonateproducescarbondioxide. Thereaction of this gas
with calcium hydroxide wouldshowthe gas to be carbon
dioxide.
Page 50
APPENDIX A
12) The nail which showsthe most changeis the nail which is
in a salt solution. In order for nails to changeinto rust, the
iron mustbe able to react with oxygenin the water or oxygenin the air.
Answers to Experiment Questions
Chapter 3 - BASICS
SECTION 3A
SECTION 2
10) The liquid which has beenaddedto the well remainsin the
well. The force of cohesionof water (surface tension) and
adhesionto the plastic is greater than the force of gravity.
Waterin the large welts has greater massand a larger surface area. Thewaterin the large wells falls out of the wells.
The surface tension of the water is not great enoughto
keepthe water in the wells.
DIRECTIONS
(1) II,~ing the point of a pencil or ball point pen. pokethroughthe
plastic inner seal of all the chemicalvial wells which havethe
small "H" cut on the inner seals.
This will allow you to insert the pipette into these vials and
will makeit easier to fill anduselater.
Dish detergent destroys the surface tension of water. The
water falls out of the wells. The "wetting" powerof detergent is what makesdetergent a valuable cleaning agent.
The water once again falls out of the wells. Alcohol also
destroys the surface tension of water. The results of this
part are similar to SECTION
2.
The baby powderor flour coated the surface of the water.
Whenthe detergent was addedthe surface tension of the
water was destroyed and the powder or flour was forced
toward the walls of the well. The flour or powdersunk to
the bottomof the well.
MICROPLATE
- A plastic plate containing a series of small
and large wells in which chemicalsare tested and reactions
observed. The wells are arranged in numberedcolumns
and lettered rows.
10) The hydrogenion has a positive (+) charge.
11) The possible products formed at the positive wire of the
battery are: gaseous hydrogen and gaseous oxygen. The
gas released is gaseousoxygen.
12) The positive electrode is producing oxygen gas. Hydrogen
gas is being producedat the negative electrode.
17) The formula for water gives us the clue. H20tells us that
a molecule of water has two hydrogen atoms for every one
oxygen. Whenwe decompose water, two times as much
hydrogen is produced than oxygen. This is why twice as
manybubbles of hydrogencomeout of the solution at the
cathode as do oxygenbubbles comeout of the solution at
the anode.
PLASTICPIPETTE- A plastic one-piece dropper. The
microtip endof the pipette is used1o deliver small droplets
of liquids for reactions in the microplate.
Enlarge"H" sealswith ball point penso pipette canbeused.
Chapter 4 - MODELS
SECTION1
A 3-D modelis better than a paper or 2-D model since the
3-D modelgives a clearer, moreuseful picture of what the
actual moleculeis believed to look like. The 3-13 modellets
you look at the structure of the molecule.
The electrolysis of aqueouspotassiumiodine produceselementaliodine (12) at the positive electrode. Hydrogen
nroducedat the neaative electrode,
7)
Iodine is producedat the red electrode. Hydrogenis producedat the black electrode.
11) & 12)
The positive electrode producedthe iodine whichtests positive with starch or paperas the indicator. A black color indicates iodine.
SECTION 2
4)
SECTION 8
The combinatioq of iron and oxygenrequires that the iron
and oxygenform an alternating structure of oxygen-ironoxygen-iron-oxygen. The paper model may show this but
the 3-D model is moreinformative.
SECTION 3
11) The nails which were covered with solution showgreater
rusting than nails which were only covered with water. The
nails tend to be rusty ABOVE
the line of the solution. The
red-browncolor of the nail is due to the formation of iron
oxide or rust.
Page 49
"H" CUTIN
RED SEAL
2) Find the plastic measuringcup in your set. Youwill see it is
marked with various measurements.Using the "ML" measurementscale ("ML" stands for milliliter),
fill the cup to the 5
markwith distilled water.
L~SERTED
~ / "HIROUGH
],-J’H"
CUT
"H" CUT
RESEALS/
/
Figure #9
6)
A chargedatom is Called an ion.
//~
Figure #7
SECTION 7
6)
IMPORTANT:
After activation of the chemicals, always keep
the microplate flat on its base. Donot store it on edgeor on its
side, as the chemicalsmayleak out over time. Be sure to keep
the microplate in its pouchwhennot using.
Reviewof Terms
SECTION 5
5)
3) Youare nowready to fill someof the other vials with alcohol.
You may use Isopropyl (rubbing) alcohol or Ethyl alcohol.
(Obtain the alcohol from the local pharmacyor grocery store.)
Using the sametechnique as you did in step 2, place 5 ML(live
milliliters)
of alcohol into the measuringcup. Thenusing your
pipette, draw up the 5 MLof alcohol into a pipette and then
insert the pipette into ONLYthe following vials. PUTTHE
ALCOHOL ONLY INTO THE VIALS WHICH HAVE YELLOW
COLORED SEALS:
Phenolphthalein (#65)
Universal Indicator (#70)
9) The oxygenion has a negative (-) charge.
SECTION 4
5)
12) Copper and aluminum nails are resistant to chemical
change. A discoloration shows which chemicals tend to
change copper and aluminum.
SECTION 5
SECTION 3
7)
11) The nails which were covered with solution showgreater
changethan the nails which were only coveredwith water.
NOTE:In the top of each of the YELLOW
or BLUEcaps of
the chemical vial wells or separate chemical vials, there
can be seen an "H" shaped letter. This "H" is the place
where you will puncture, or makea hole, in the chemical
vial well. Youshoulduse a pencil point or a ball point pen
to break through this "H", and thereby open up the chemical vial so that you mayadd liquid or take out liquid. The
"H" cut will actually seal itself betweenuses. For now,
however, go ahead and proceed with the steps outlined
next.
7) & 8)
The Universal Indicator turns two different colors in the two
wells. The positive electrode well produces oxygen gas
(which is soluble) and an orange or red color is seen when
the indicator is present. The negative electrode produces
hydrogenand is colored blue.
Addingwaterto the chemicalvial wells.
Figure #8
Using your plastic pipettes, and your measuringcup with
distilled water in it, drawup (sucking up into the pipette) 5
(five milliliters)
of DISTILLED
WATER.
Nowpushthe tip of the pipette through the inner seals with
the "H" cut on themand squeezeout 5 MLof distilled water into
only the vial wells with the BLUEtops. ADDTHEDISTILLED
WATER ONLY TO THE VIAL WELLS WHICH HAVE BLUE
COLORED
SEALS!These vials which will get the 5 ML of distilled waterare listed below:
MethyleneBlue(#47)
CobaltChloride(#8)
FerrousSulfate(#44)
CalciumNitrate (#41)
Copper
Sulfate (#11)
Sodium
Silicate (#18)
CalciumHydroxide(#40)
Youmayhaveto use a pencil or ball point pen’s point to initially open and widen the "H" cuts in the seals so that your
pipette can easily be inserted into the vials.
Each chemical vial contains a few small plastic "mixing
beads" which themselves do not dissolve. The "chemical" in
eachvial is either on small strips of special paperor as solids in
precisely measured amounts. The "miring beads" he~l~ the
chemicalsdissolve.
Whena solvent is addedto the vial, the chemicalsdissolve
upon shaking the vial, and form the chemical _solution which
you will use in your experiments.
The chemical’s nameis printed or~ the label on the exterior
of eachvial.
-- SAIq’.’TY
CAP
C){EMICALI~AI)ER
OR POWDER
(IN-~IDE VIAL)
Citric Acid(#42)
PotassiumIodide (#49)
Sodium
Sulfate (#53)
AluminumAmmonium
Sulfate (#57)
Ammonium
Chloride (#58)
Magnesium
Sulfate (#64)
SodiumCarbonate(#67)
CItEMICAL
MIXING BEADS
(INSIDE VIAL)
Figure #10
Page 6
REVIEW:
A_D__D_.!.N_G
SOLVEN_T_._T_O.
THEVIALS
IMPORTANT
READ THESE DIRECTIONS BEFORE ADDING ANY LIQUID TO YOUR CHEMICALS!
Youare nowreadyto activate your chemicalvials or vial wells with either wateror alcohol. Besure to follow the directionsexactly
so that youwill put the correctliquid into the correctchemical
vial.
Youwill needto gatherthe followingmaterialsto completethis procedure:
All of the YELLOW
TOPchemicalvial(s) from your chemistryset
All of the BLUE
TOPchemicalvials from your chemistryset
All of the plastic seal top envelopes
with wiresor othermaterial
Twoplastic pipettes (medicinedroppers)fromyour set
Oneplastic measuringcup (measuringcup with measurement
markson it) from your set
Sharppointedpencil or ball point pen
Alcohol- either isopropylalcohol(rubbingalcohol)or ethyl alcohol. (Obtainfromyourlocal pharmacy
or grocerystore)
Distilled water(Obtainfrom your local supermarket
or pharmacy)
NOTE:
Some
vials andinside inner tops maybe sealedwith clear tape for addedprotection. Remove
the tape on the inner top and
puncture"H" with pencil point or ball point penandproceed
with the instructions below.
STEP
1 - Usingthe point of a pencil or ball point pen,pokethroughthe plastic inner seal of all the chemicalvials whichhavethe
small"H" cut onthe innerseals. Thiswill allowyouto insert the pipetteinto thesevials andwill make
it easierto fill anduselater.
Makesure youput the safety screw-oncapbackonto eachvial after you puncturethe seal.
STEP
2 - Find the plastic measuringcup in your set. Youwil~ seeit is markedwith various measurements.
Usingthe "ML"measurement
scale("ML"standsof milliliter), fill thecupto the ML
_ ma
rk with distilled water.
Usingyourplastic pipettes,andyourmeasuring
cupwith distilled waterin it, drawup (suckup into the pipette) 5 ML(five milliliters)
of DISTILLED
WATER.
Nowpushthe tip of the pipette throughthe inner seals with the "H" cut on themand squeezeout 5 MLof
distilled water into only the vials with the BLUEtops. ADDTHEDISTILLEDWATER
ONLYTOTHEVIALSWHICH
HAVEBLUE
TOPS
ANDBLUE
COLORED
SEALS!
Thesevials whichwill get the 5 MLof distilled water are listed below:
¯ MethyleneBlue (#47)
¯ FerrousSulfate (#44)
¯ PotassiumIodide (#49)
¯ Citric Acid(#42)
¯ CalciumNitrate (#41)
¯ CalciumHydroxide(#40)
¯ Sodium
Silicate (#18)
¯ CopperSulfate (#11)
¯ CobaltChloride(#8)
¯ SodiumSulfate (#53)
¯ AluminumAmmonium
Sulfate (#57)
¯ Ammonium
Chloride (#58)
BE SURETO WEARGO.._G_GLES
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
Repeatthe experimentin SECTION
6 using aluminumor copper nails insteadof common
iron nails.
SECTION8 - A CORROSION
PAIR
In this experimentyoucanactually seethe changeoccur, just
overnight,whentwo different metalsare in close contactwith
oneanotherin a salt solution. By useof an indicatorwecansee
if a changehasoccurredin the solution,andalso if a change
hasoccurredto the different metals.
chloridesolution. Place1/2
1) Fill a plastic pipettewith sodium
Youwill needthe following materials to completethis experiment:
2)
Adda few dropsof UniversalIndicator to both wells with
thesodiumchloridesolution.
LIST OF MATERIALS
Aniron nail (or a 3 cm.lengthof iron wire)
Analuminum
nail (or a 3 cm.length of aluminum
wire)
Sodiumchloride solution. (Prepareyour ownsodium
chloridesolution by mixing1/2 teaspoon
of table salt
with10ml. of water.Stir until all salt is dissolved.)
UniversalIndicatorsolution
Wirewith springclips
Microplate
Plasticpipette
Goggles
3)
Join an aluminum
nail or wire and a common
iron nail or
iron wire at their endswith a springclip.
4)
Placethe joined nails or wire in oneof the wells with the
sodiumchloridesolution.
5)
Leavethe nails in the solutionovernight.
pipettefull of sodium
chloridesolutionin eachof twolarge
wells in the microplate.
Whathappens
to eachof the nails?
Whathappens
to the UniversalIndicator?
ls there evidenceof corrosion?
¯ Magnesium
Sulfate (#64)
¯ SodiumCarbonate(#67)
STEP
3 - Youare nowreadyto fill someof the other vials with alcohol. YoumayuseIsopropyl (rubbing)alcohol or Ethyl alcohol.
Obtainthe alcohol from the local pharmacy
or grocerystore. Usingthe sametechniqueas youdid in STEP
2, place5 ML(five milliliters) of alcohol into the measuring
cup. Thenusingyour pipette, suckupthe 5 MLof alcoholinto a pipette andtheninsert the
pipette into ._only the vials with the YELLOW
tops. PUTTHEALCOHOL
ONLYINTOTHEVIALSWHICH
HAVEYELLOW
COLORED
CAPSAND YELLOWCOLORED
SEALS:
¯ Phenolphthalein
(#65)
¯ UniversalIndicator(#70)
STEP4 - DONOTADDANYTHING
TOthe following plastic envelopes:
¯ CopperWire(#61)
¯ Iron Wire(#63)
¯ Aluminum
Wire (#38)
¯ ZincWire(#54)
NOTE:
Iron Wireusedin this set is pureandwill rust. Rustwill not affect your experiments.
Just wipeoff as much
rust as possible
with a cleanpapertowel andsandthe iron wire with a smallpieceof sandpaper
if needed.Thewire doeshavea light coatingof oil
to reducerusting.
STEP
5 - Nowreplace all of the capsbackon to the vials which they cameoff of. Screwthe capson securely. Makesure you
ALWAYS
put the SAME
capbackon the SAME
vial it cameoff of eachtime you use a chemical.Finally, placeall of the vials and
all of the plastic envelopes
backinto the properplacein your chemistryset.
................
R~view
of
Te~S
...............
MICFIOPLATE
- A plastic plate containinga series of small
tip endof the pipetteis usedto deliver smalldropletsof liquids for reactionsin the microplate.
andlarge wells in whichchemicalsare tested andreactions
FILTER
FUNNEL
- An altered pipette whichcontains cotton
observed.The wells are arrangedin numbered
columnsand
as thefilter element.
lettered rows.
CHEMICAL
SCOOP
- A pipette which has had its bulb end
PLASTIC
PIPEI-FE - A plastic one-piece dropper. The
cut off and is used as a chemicalspoonto deliver solid
microchemicals.
Page 7
Page 48
1)
Obtain 15 small iron nails (check with magnetto see that
they are iron). Makesure the 15 nails are the samesize.
Sandthe iron nails with fine sandpaperto removeany oxidation or coating. Youmayalso use 3 cm. lengths of iron
wire from your chemistry set.
7)
Add 7 drops of each of the following solutions in the
microplate columnas directed.
COLUMN
2)
Paint the "point half" of 5 nails or wire with oil paint, nail polish or modelpaint. Allow the coating time to dry.
3)
Cut 5 lengths of zinc wire (from your chemistry set) into
lengths of 3 cm. each. Wrapeachof the five nails with zinc
wire. See Figure #44.
1
2
3
4
5
8)
SECT!.ON2_.-. PROPERTIES
_OF THE__
MICROCHEMISTRY SYSTEM
Are you ready to do your first
CHEMICAL SOLUTION
WELLS USED
Sodium Chloride
Ferrous Sulfate
Citric Acid
Sodium Carbonate
Tap Water
A-l,
A-2,
A-3,
A-4,
A-5,
B-l,
B-2,
B-3,
B-4,
B-5,
C-1
C-2
C-3
C-4
C-5
Cover the microplate with a piece of plastic wrap. Leave
the nails in the solutions in a safe place overnight.
Normally, you would expect the solution to fall out of the
wells. This does not happenbecausethe solution holds onto
itself and the surface of the plastic well by SURFACE
TENSION. Surface tension is the force which binds water to itself
and the surface of the container in which it is stored. The surface tension of the water(a force) is greater than gravity (another force). Sothe water stays in the plate.
experiment?
It is a good thing to know the properties of your equipment
BEFOREYOU USE IT.
11) Nowplace someof the blue dye/water mixture in three of
the LARGEWELLS. Large well B-l, A-3 and B-6. Use
moreliquid since the large wells can hold moreliquid.
LIST OF MATERIALS
Plastic cup (from your chemistry set)
12) Lookat the color of the large wells w=ththe drops of coloring. Turn the plate and look at the drops from the side of
the plate.
Water
Methylene Blue Dye Solution
Which nails did you expect to be protected? Why?
Look up the word GALVANIZED
in your dictionary.
is associated with GALVANIZED
steel?
Whichmetal
Plastic pipette
PERFORMTHE NEXT STEP #13 OVER THE SINK!
DO NOT TRY THIS UPSIDE DOWNOVER YOUR HEAD!
Microplate
IJ Goggles
to the sink. Turn the
13) Carry the microplate CAREFULLY
microplate upside down over the sink. What happened?
BE SURETO WEARGOGGLES
WHEN.D_._OIN(~
EXPERIMENTS
IN THIS CHEMISTI~_Y_SET.!
14) Nowwashthe microplate out with water, being careful to
clean andrinse all of the wells of the water/dyemixture.
SECTION 7 - CORROSIONOF DIFFERENT METAL.$
Figure #44
4)
5)
6)
Place the 5 painted nails in the first five small wells of Row
1 in the microplate. Thepainted nails will be in small wells
A-l, A-2, A-3, A-4 and A-5. SeeFigure #45.
Place the 5 nails wrappedwith zinc wire in the first five
small wells of RowB in the microplate. The zinc wire
wrappednails will be in small wells B-l, B-2, B-3, B-4 and
B-5. See Figure #45.
Different metals often corrode whenthey comein contact with
each other. This is a problem if the two different metals are
used in ships or boats wheresalt water is present or sometimes
in plumbing systems in houses where water or steam makes
contact with both metals. Sometimesto prevent this corrosion
problem, one of the metals is coated to protect it. Sometimes
non-corrosive
metals must be used in certain
applications...such as stainless steel or platinum which do not
tend to corrode.
LIST OF MATERIALS
Fifteen (15) small copper nails OR15 lengths of copper
wire cut into 3 cm. lengths
Piece of fine sandpaper
Place the 5 other nails in the next row of small wells in the
microplate. Use small wells C-1, C-2, C-3, C-4 and C-5.
See Figure #45.
DIRECTIONS
1) Place your microplate on several pieces of white paper.
2)
Fill a small plastic cup about1/2 full of water.
3)
Add two drops of methylene blue dye to the water in the
cup. Be sure to use your MICROTIP
pipette for this experiment.
4)
Return the blue dye which you have not used back to its
original container.
Thewater/dyemixture acts differently in the large wells than it
did in the small wells. Why?
Answer: Waterin the large wells has greater massand a larger
surface area. The water in the large wells falls out of the wells.
Thesurface tension of the water is not great enoughto keep the
waterin the large wells.
SECTION 3 - HOWTO DESTROYSURFACE TENSION
Howto Destroy Surface Tension
5)
Stir the water with the stemof the pipette.
6)
Drawup someof the water/dye mixture into the MICROTIP
pipette.
7)
Place 7 or 8 drops of the water/dyemixture into small wells
A-l, A-2, A-3, A-12, B-12, C-12. SeeFigure #11.
Moaeipaint or [i~gu~,,aii puli~l~
Sodiumchloride solution
f
Ferroussulfate solution
2 3 4 5 6 7 .~
~~000000
~000000000
cO00000000
o:000000000
Citric acid solution
Wire
I1
Sodiumcarbonate solution
Tap water
Zinc wire cut into 3 cm. lengths (from your chemistry set)
9 ~ O
0
0
0
0
1 1 1 2~
0
0
0
0
There are chemicals which will destroy or lessen the effect of
surface tension. Just think how difficult it would be to wash
yourself or other things if the surface tension of the water was
so strong that it would not penetrate dirt or cloth or whatever
you are trying to wash!
~
Dc
Oo
~:OOOOOO
Microplate
Plastic wrap
Surface tension, as you have learned, is the property of a liquid’s surface to form a thin layer of particles or moleculesat the
surface of the liquid whichpull on oneanother so that a "surface
layer" is formed. This tends to "hold in" the liquid below. On
water, for instance, the surface tension is strong enoughto support the weight of small insects whichlive on the surface of the
water in ponds and lakes. You can see how surface tension
fnrm¢ m~.ha laver bv carefully "floatine" a needle on the top
surface of a container of water.
In this experimentwe will destroy or lessen the effect of surface
tension by the use of something that makeswater more wet. A
dishwashing soap has the property of a "wetting agent," or in
other words, it will makewater wetter!
Plastic Pipette
Goggles
Solutions
BE SURE TO WEAR. GOGGLESWHEN DOING
EXPERIMENTSIN THIS CHEMISTRYSET!
Figure #45
8)
9)
Figure #11
Lookat the color of the wells with the dropsof the coloring.
Turn the plate and look at the drops from the side of the
plate.
You will need the following materials to completethis experiment:
Hold the plate up to a light source. Observethe color of the
wells through the bottomof the plate.
Methylene Blue DyeSolution (from your chemistry set)
LIST OF MATERIALS
Plastic cup (from your chemistry set)
Liquid dishwashingsoap (obtain from grocery or kitchen)
Microplate (from your chemistry set)
10) Finally,
Page 47
turn the plate upside downover the white paper.
Does anything unexpected happen?
Goggles
Page 8
1) Throwawaythe water/dye/detergentmixturefrom the pre-
BE.SU_R_.E__T_O
WEARGOGGLES
WHEN
DOING
EXPERIMENTS
IN THIS CHEMISTRy
SET.!
blue dyesolution left in your cup
1) If youhaveanymethylene
fromthe last experiment,
youmayuseit here. If not, mixa
little moremethylene
blue dye solution with waterin the
plastic cup.(seeSection2, steps2 and3).
2)
3)
ACTIVITY CHART
vious experiment.
2)
Rinsethe plastic cupandadd40 dropsof waterto the cup.
3)
Adda few dropsof methylene
blue dye solution as youdid
previously.
Add one drop of dishwashing soap to the methylene
blue/watermixture.Stir andmix thoroughly.
4) Add20 dropsof ethyl or isopropylalcoholto the waterin
Drawup someof the water/dye/soapmixture into the
MICROTIP
pipette.
5) Repeatsteps6, 7, 8, 9 and10 fromSection2 Experiment.
ACTIVITYSERIESMETALSWHICHWILL TENDTO LOSE ELECTRONS
MOSTACTIVE METALS
(Thosewhich lose
electronsmosteasily)
the plastic cup.
How
is the result similar to either Section2 or Section3?
4) Place7 or 8 dropsof the water/dye/soap
mixtureinto small
Figure #42
wells of the microplate.Usethe samewells as before: A1, A-2, A-3, A-12,B-12andC-12.
SECTION
5 - A VISIBLE ILLUSTRATION
OF
SURFACETENSION
5) Lookat the color of the wells with the mixturein them.Turn
the plate and look at the wells from the side of the
microplate.
6)
Finally, carry the microplateCAREFULLY
to the sink. Turn
the microplateupsidedownover the sink.
7)
Whathappens?Whatdoes the dishwashingsoapdo to the
water?Whyis this propertyof detergentvaluable?
As in manyexperimentsin chemistry, eventhoughchanges
go on at the atomicor molecularlevel, weoften cannotseethe
effects with our eyes. Sometimes
weneedto usesomethingwe
CANsee to showus things wecannotsee. In this experiment
weare using fine powders, which wecan see, to help us
observethe changes
taking placewith the surfacetensionlayer
of a liquid.
Answer:Dishwashingsoap destroys the surface tension of
water. Thewaterfalls out of the wells. The"wetting" powerof
the detergentis whatmakes
it a valuablecleaningagent.
LIST OF MATERIALS
Microplate
Ethyl or isopropylalcohol(obtain fromdrugstore)
Water
Liquid dishwashing
detergent
Plasticpipette
Babypowder,talcumpowderor flour
Goggles
Extension:
Try this sameexperimentusing a drop of hair shampoo.
Try this sameexperiment
usingdishwasher
"Jet DryTM’’ liquid.
Try this sameexperimentusinga dropof liquid handsoap.
SECTION
4 - A_I,-COHOL._.AND..SURFACE
TENSION
Other chemicalsbesidessoapproductshave the property
of destroyingor lesseningsurfacetension. Thisexperiment
explores thesechemicals.
WARNING:
Ethyl alcohol, isopropyl alcohol and rubbingalcohol
are flammableliquids. Keepthese liquids and their vapors
awayfrom any openflame. Usethesechemicalsonly in a wellventilatedarea.
~000000000
~~000000000
~lO00000000
0 0
0
0 00c
der,
talcumpowder
or flour.
4) Add1 dropof dishwashing
detergentto onewell with alcohol (A-3) andonewell with water(A-l).
5)
Describethe result. Whatcausedthe change?
Notes:
In a previoussection youexperimented
with iron wire or nails
whichwereplacedin salt solutions. Thesesalt solutions helped
the processof corrosion. Someprocesseshelp PREVENT
corrosion.
~OOG!
,_
0,0,
Oil
8) Touchthe endsof the galvanometerto two metalsin the
3) Dust the surfaceof eachof the four wells with babypow-
Themost common
form of electrochemistryof metals does not
occur in a battery. Metalsgive up electronsto non-metalsand
other metals in chemicalreactions. Oneof the mostcommon
electrochemicalreactions is the processof CORROSION.
ooloo_~oo_.~o~xoo
o o oo
1) Fill two large wells of the microplatewith water.Uselarge
large wells A-3 andB-3.
solutions.
9) Repeatthe processof testing with eachcombinationof
metals. Whichmetal pair gave the greatest movement
of
the compassneedle? Whichmetal pair gave the least
movement
of the compassneedle? Whichpair of metals
wouldmakethe best battery or cell?
10) Whichmetal of the three is the mostactive? Howdo you
know?Whichmetalis the least active?
11) Whatwouldbe a gooduse for metals which are not very
active?
12) Compare
your results of the metals you tested with the
Activity Chartabove.
LIST OF MATERIALS
Fifteen (15) smalliron nails or 3 cmlengthsof iron w~re
Pieceof fine sandpaper
Modelpaint or fingernail polish
Sodium
chloride solution
Citric acidsolution
Sodiumcarbonatesolution
Tap water
Zinc wire (from your chemistryset)
Microplate
Plastic wrap
Plastic Pipette
Goggles
BESURETOWEAR
GOGGLES
W_H_E_N_._D_
OI._NG
EXPERIMENTS
IN .T__HI.S_
C__H__EMIS__T_R_Y_S_E_.T_.!
BE SURETO WEARGOGGLE_S
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
Page 9
PotassiumMetal
BariumMetal
CalciumMetal
SodiumMetal
MagnesiumMetal
AluminumMetal
Zinc Metal
ChromiumMetal
Iron Metal
CobaltMetal
Nickel Metal
Tin Metal
LeadMetal
HYDROGEN--CopperMetal
Silver Metal
PlatinumMetal
GoldMetal
SECTION6 - OTHERELECTROCHEMICAL
RE.A_C_]-IONS
Figure #43
2) Fill two other wells with ethyl or isopropyl alcohol. Use
LIST OF MATERIALS
Plastic cup
Water
MethyleneBlue DyeSolution
Isopropyl"rubbingalcohol,"or ethyl alcohol(from
the drugstore)
Plastic pipette
Microplate
Goggles
7) Insert the filter papercut out into thethreewells containing
the three different solutions. SeeFigure#43.
BE SURETO WEARGOGGLESWHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
wells A-1 andB-I.
6) Soakthe filter paperwith sodiumchloride solution. Make
your ownsodiumchloride solution by addingsometable
salt to waterin yourplastic measuring
cupanddissolvingit
thoroughly.
K
Ba
Ca
Na
Mg
AI
Zn
Cr
Fe
Co
Hydrogen
sometimes
acts like
Ni
a metalby giving off anelectron. Sn
Hydrogen
is shownhere in the
Pb
ACTIVITYSERIES.
H
Cu
LEAST ACTIVE METAL
Ag
(Those which DONOT
Pt
lose electronsveryeasily)
Au
Page 46
4)
5)
6)
7)
Attach the wires to the galvanometeryou built in SECTION
1.
SECTION
5 - _A.C_T_IylTY._O~"METALS
Thereare several different kinds of cells, but they all haveone
thing in common. Each cell converts STOREDCHEMICAL
ENERGYinto ELECTRICAL ENERGY.
Wetall the pieces of paper towel with a solution of sodium
chloride (salt water).
Test this electrolytic cell by touchingthe wires in an "off-onoff-on" method. Watch the needle on your galvanometer
moveback and forth.
What happens to the needle of the galvanometer? Which
direction does the needle move?Which metal gives up
electrons? Which metal receives them? Which electrode
was the NEGATIVEELECTRODE?
Which electrode was
the POSITIVE ELECTRODE?
As you may have guessed by now, chemists have a good idea
which metals on the Periodic Chart are best for cells or batteries. Their ideas about activity are based on experiments. The
experiment below is an example of how these activities were
determined.
You will needthe following materials to completethis experiment:
LIST OF MATERIALS
~J
Compassgalvanometer from SECTION1
i_~ Ferroussulfate solution
SECTION 4 - ANOTHERBATTERY
You can makea simple battery by connecting several cells
together. A battery is a series of cells.
~J
LIST OF MATERIALS
~,J Compass galvanometer
(ELECTRON FLOW DETECTOR) which you made in SECTION
10 nickels
I1
Iron nail or a 3 cm. length of iron wire from your
chemistry set
Aluminumammonium
sulfate solution
~1
Aluminumnail or a 3 cm. length of aluminumwire
ATOM
- The smallest particle of an element.
CHEMICAL
MEANS
- Methods of treating material which separate pure substances into new compounds
or elements.
COMPOUND
- A chemical combination of two or more elements. A compound
has different properties from the elements
which makeit up. Compounds
cannot be separated into their
elements by physical means.
ELECTRODE
- A wire which is placed in an electrolyte
through whichan electrical chargeflows.
ELECTROLYTE
- A solution which conducts an electric
and
current.
ELEMENT
- A substance which contains only ONEKIND of
atom. Example: iron, sulfur or carbon are each ELEMENTS.
Coppernail or a 3 cm. length of copper wire from your
Cleanser or scouring powder, or fine sandpaper
~.J
Insulated wire with spring clips
®
Papertowel or tissue like Kleenex
~
Plastic pipette
~J
Ruler
Sodiumchloride solution (salt water). Prepare your own
~J
Pencil
sodiumchloride solution by mixing 1/2 teaspoontable
salt with 10ml. of water. Stir until all salt is dissolved.
Goggles
[,.J
;I
Scissors
~J
Microplate
Goggles
BE SURETO WEARGO_GG_LE$__WHEN
_DOIN(~
EXPERIMEN_T$_.J.N
.T..HIS C_HEMISTRY
S..E~
1) Clean the coins with scouring powder or sandpaper.
EQUATION
- A statement showing the way chemicals combine
or break up. An equation shows how reactants becomeproducts in a chemicalreaction.
ION - An atom or a group of atoms which are NOTelectrically
neutral. Ions will either be POSITIVEcharged or NEGATIVE
charged.
METAL
- A chemical elementwhich tends to lose electrons in a
chemical reaction. Example: SodiumMetal (Na) will give off
one electron per atom during a chemical reaction. Sodium
metal atom will then becomea sodium metal ion (Na+).
It is important to knowhow chemicalsreact before you experiment. An explanation of the workings of chemical reactions
means that a MODELshould be used. Models are used
becausethe atoms and molecules which makea chemical reaction are far too small to be seen even with the most powerful
microscope.
A MODEL
is an imitation of the real thing. Modelsare useful in trying to understandhowthings work. Scientists often use
models to explain unseen forces, Weuse models to makean
idea easier to understand.
The advantageof a modelis in its ease of use. For example, it is certainly easier to showsomeone
a MODEL
of a plane,
rather than a full size one.
A MODEL
airplane is an imitation. A model plane is not a
real plane. It is a smaller representationof a real plane. It can
be used to imitate the workings of a real plane. A model can
help to picture somethingreal but unseenor unfamiliar.
In the samemanner, models of chemicals can be used to
scale down, represent or MODELthe functioning of REAL
chemicals.
Whenchemicals combine they are said to REACT.Reactions can be of several types involving few or manychemicals.
By using cut-out model ions you can see how different chemicals can combine to form the manycompoundswhich chemists
find so interesting.
In addition to the papercut-out atomsandions, your chemistry set contains three-dimen._sional (3-D) modelsof atoms.
Thesemodelsgive a 3-D view of the structure of someof the
chemical compounds
which you will use in your set.
It is interesting to see if you can build both the papermodel
and the 3-D model of molecules for comparison. The paper
model is useful only to showhow manyions combinewith others to form compounds.The method of telling how manyIONS
of one chemical reacts with howmanyions of another is called
STOICHIOMETRY
(sto ’key ah ma tree). The 3-D models give
you a better picture of what chemists think these molecules
would look like if we could see them. The 3-D modelsstill can
showthe stoichiometry of a reaction.
Experiments with Model Elements and Ions
An ELEMENT
is a chemical which has only one kind of
MODEL
- A representation of something else.
~tnrn
2) Attach a copperwire to one of eachkind of coin with spring
4)
TERMS TO KNOW
[...J Sodiumchloride solution (salt water)
~J
Insulated wire
BE SURE TO WEAR GOGGLES WHEN DOING
EXPERIMENTS
IN THIS CH_E.MIST_B.Y.,SET!
3)
Chemical Models and Chemical Reactions
ELECTRON
- The particle outside the nucleus of an atom which
carries a negative (--) charge.
chemistry set
Filter paper(from your chemistry set)
clips. These will
Figure #41.
CHEMICAL MODELS
CHEMICAL REACTIONS
from your chemistry set
~.~ Coppersulfate solution
~J
10 pennies
CHAPTER 4
be the TI=RMINALELECTROD~=$.
See
Place a piece of folded paper towel, alternating between
pennies and nickels. See Figure #41. Makesure that the
spring clips touch the coins at eachend of the stack.
Attach the wires to the galvanometeryou built in SECTION
1.
5)
Wetall the pieces of paper towel with a solution of sodium
chloride.
6)
What happens to the needle of the galvanometer? Which
direction does the needle move?Which metal gives up
electrons? Which metal receives them? Which electrode
was the NEGATIVEELECTRODE?
Which electrode was
the POSITIVE ELECTRODE?
How do you know?
Page 45
1)
Place1/2 pipette full of ferrous sulfate solution in large well
A-1. Rinse the pipette with rinse (tap) water.
2)
Place 1/2 pipette full of Aluminumammonium
sulfate solution in large well A-2. Rinse the pipette with rinse (tap)
water.
3)
Place1/2 pipette full of coppersulfate solution in large well
A-3. Rinsethe pipette with rinse (tap) water.
4)
Place a piece of metal wire or nail in each well which has
the sameion in solution. Put the iron nail or wire in the ferrous sulfate solution (large well A-l). Put the piece
Aluminumwire or nail in the Aluminumammonium
sulfate
solution (large well A-2). Put the piece of copper wire
nail in the coppersulfate solution (large well A-3).
5)
Mark the filter paper with ruler and pencil to the shape
shownin Figure #42. Eachleg of the filter paper should be
1 cm apart. See Figure #43. Fold the filter paper on the
dotted line.
becomea Chlorine Ion (CI-).
PERIODIC
TABLE
- A list
their properties.
of the different elements and someof
PRODUCT
- A substance which is produced in a chemical reaction.
PROTON
- The particle in the nucleus center of an atomwhich
carries a positive (+) charge.
REACTANT
- A substance which combines with another in a
chemicalreaction.
REACTION
- The chemical combination or change of two or
more elements or compounds.
STOICHIOMETRY
- The combining ratios
chemical reaction.
Th~a ~tr~m~ ~r~ n~ltr~l
in nh~r~a~.
An IONis an atomor group ol atoms which is NOTelectrically neutral. Someions are positive in charge. Other ions are
negative in charge.
A MOLECULE
is a chemically combined unit of two or
more atoms. The atoms maybe of the sameelements (such as
two hydrogens) in order to makea molecule of hydrogen gas,
H20or the molecule maybe of two or more different elements,
such as NaCL, or table salt, which is made of an atom of
Sodium(Na) and an atomof Chlorine (Cl). A moleculeis of
tral charge.
Chemists experiment with elements, ions, and molecules.
Atoms, though very small, are madeup of parts. These
parts makethe atom what it is. Atomsare the basic building
blocks of all chemicals.
In order to talk about the atom, scientists have devised a
MODEL
of what an atom looks like. This model is called the
PLANETARY
or BOHRmodel of the atom. The model is named
after a scientist, Niels Bohr, who cameup with the idea.
Further, based on the reactions of atoms, they have an idea
(MODEL)of what the molecules of chemical compoundslook
like.
NON-METAL
- A chemical element which tends to gain electrons. Example: A Chlorine atom will accept an electron to
of chemicals in a
Page 10
Thenucleusis the centerof the atomandhasalmostall the
WEIGHT
or MASSof the atom. Eachelement has a DIFFERENTNUMBER
of positive chargesin the center of the atom.
Thesecharges are called PROTONS.
Thenumberof positive
chargesin the center of the atomis called the ATOMIC
NUMBER.Eachelementhas a distinct atomic number.
Thepositive particles or protons,alongwith neutral particles, called NEUTRONS,
makeup the NUCLEUS
of an atom.
SeeFigure #12.
Theatomalso contains negative charges, called ELECTRONS,
whichare locatedat different distancesfromthe nucleus in ORBITSor ENERGY
LEVELS.
Thenumberof electrons in an elementis the sameas the
numberof protons in the sameelement. Thenumberof electrons (-) mustequalthe number
of protons(+) in a neutral atom.
Theelectrons are NOTlocatedin the nucleus.
Whatwe, as chemists,can"see" in our mind’seye, are the
representations, or MODELS,
of atomsand molecules!
Youare urgedto completethis experimentfully because
eachof the models
youwill seeandstudy, will representfor you
the "picture" of unseenatomsand moleculesand howthese
very small building blocks of our world combineand form new
substances!
LIST OF MATERIALS
I,~ Paperions and atoms(pink and blue sheet of cardboard
ions fromyour chemistryset)
Pair of scissors
3-Dplastic models(from your chemistryset)
Goggles
+2.
EXPERIMENTS
IN THIS CHEMISTRY
SET!
1)
Figure #12
Cut out or separateall the paperatomswhichare metals.
Noticethat the metalatomshavelittle triangles on oneside.
Thesetriangles represent(are MODELS
of) the electrons which
metals lose whenthey form compounds.EachELEMENT
has
a SYMBOL.
A SYMBOL
is like a special initial or name(model)
whichis written insteadof usingthe wholewordfor the element.
Figure #13
The SYMBOL
is used by chemistsas a shorthandwayof talking aboutchemicalelementsor chemicalions.
If the numberof electrons DOES
NOTEQUAL
the number
of protons, the atomhas a charge. Whatis a chargedatom
called? SeeFigure #13. Figure #13 is an exampleof a positively charged
ion.
Eventhoughthe electrons are located at a distance from
the nucleus, ELECTRONS
MAKECHEMICALREACTIONS
HAPPEN.
Chemistshaveorganizedall the knownatomsinto an organized list they call the PERIODIC
TABLE.SeeAppendixB at
the end of your manual.
Each ELEMENT
has only the sametype of atoms. By
organizingthe knownatoms,or elementsinto a table, chemists
havebeenable to predict the propertiesof manyother elements
and the chemical compounds
they form. The most important
organizationof all elements
is the division of the elements
into
two generalclasses.
For example,sodiumis a metal element. Sodiumhas a SYMBOL.Thesymbolfor sodiumis Na. TheNastandsfor the original namefor sodiumwhich wasNATRIUM.
The symbolNa is
still used today. Sodiumacts alone as a chemicalelement.
Manyof the elementson the Periodic Tablehavesymbolstaken
fromtheir original names
in Greekor Latin. Iron wasoriginally
called ferrum. Thesymbolfor iron is Fe. Gold wascalled
aurum.Thesymbolfor gold is Au.
Usually,thesymbol
for the element
is thefirst letter or first two
letters in its Englishname.Oxygen’ssymbolis O, hydrogen’s
is H, nitrogen’sis N, helium’sis He,etc.
2)
Thetwo generalclassesof elementsare:
Metals and Non-Metals
Cutout or...s_._e..garate
all the paperatoms
whichare
non-metals.
Noticethat the non-metal
atomshavelittle notcheson oneside.
Thesenotchesrepresent(are MODELS
of) the sites whichnonmetals use whenthey form compounds.
Metals tend to GIVEUPor release electrons. Non-metals
tend to GAINor take on electrons.
The paper and plastic modelsof atomshave beenorganizedinto thesetwo groups.
Thereis a set of 3-Dmodelsof the elementsin your chemistry
set. Thesemodelsgive you another wayof seeing howchemicals combine.Theplastic modelsare also color coded.(See
Table#1 on page12.)
3) Chlorineis a non-metal.Thesymbolfor an atomof chloSECTION
1 - PAPER
CHE._MI_.S~_R__Y.
LAmB
1
Most of the time chemistsnever actually SEEthe atomsand
moleculeswhich makeup the chemical reactions they study
and experimentwith.
Page11
rine is CI. Chlorineexists in natureas a gasmade
of two
atomsjoined together. Chlorine is DIATOMIC
(die’ ah tom
ik). This means
two atomsof a particular elementjoined
togetherto forma molecule.
8) Detachonewire going to the "D" cell. Wh~thappens
to the
needle?Whichdirection did the needlemove?Note the
movement
of the needleon a piece of paper. BESURE
TO
NOTEBOTHTHE MOVEMENT
AND TH~ WIRE ATTACHMENT.
SpringClip
9) Touchthe wires to the OPPOSITE
ENDS
of the "D" cell.
10) What happens to the needle? NOTE_THE NEEDLE
MOVEMENT
ANDTHE WIRE ATTACHM!~NT.
This deviceis called a GALVANOMETER.
It detects the flow of
electricity throughwires. It also tells the DIRECTION
of the flow
of electrons! How?
Figure #40
DO NOTDISASSEMBLE
THIS DEVICE!! IT WILL BE USED
IN THE FOLLOWING
SERIES OF EXPERIMENTS.
SECTION2 - A SIMPLECELL
ELECTRONSALWAYSFLOWFROM
NEGATIVE
TOPOS.._TJ._VE!
7)
Thefirst electrical cell ever made
wasthe voltaic cell. It was
first made
by the Italian scientist Alessandro
Volta. Wecanperforma similar experiment
whichVolta did backin the 18th century.
Disassemble
your cell. Rinseoff the coins. Discardthe
papertowel.
SECTION3 - A SIMPLE BATTERY
Youcan makea simple battery by connecting several cells
together.A batteryis a seriesof cells.
Youwill needthe following materialsto completethis experiment:
LISTOF MATERIALS
Compassgalvanometer (ELECTRON
FLOW
DETECTOR)
which you madein SECTION
A nickel
A penny
SpringClips
Cleanseror scouringpowder,or fine sandpaper
Insulatedwire
®
Salt water(’sodiumchloride solution) Prepareyour
ownsodiumchloride solution by mixing1/2 teaspoon
of table salt with10ml. of water.Stir until all salt
is dissolved.
Go gles
B~: SURETO WEARGOGGLES
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
LIST OF MATERIALS
[~
Compass
galvanometer(from SECTION
1)
~
5 nickels
I-I 5 pennies
~,1 SpringClips
~1 Cleanseror scouringpowder,or fine sandpaper
~
Insulatedwire
®
~
I--I Sodium
chloride solution (salt water)
~
Goggles
WHENDOING
EXPERIMENTS
IN -[HIS CHEMISTRY
SET!
1) Clean the pennies and nickels with scouring powderor
sandpaper.
1) Cleana pennyanda nickel with scouringpowderor sandpaper.Theseare the two different metals.
2) Attach a copper wire to one pennyandone nickel with
spring clips. Thesewill be the TERMINAL
ELECTRODES.
2) Attacha springclip andwire to the penny.Attachthe other
springclip andwireto the nickel.
3) Placea piece of folded papertowel, alternating between
penniesand nickels. SeeFigure #41. Makesure that the
coinswith the wires are locatedat the endsof the stack.
3) Placea pieceof folded papertowel betweenthe two coins.
SeeFigure #40.
4) Attach the wires to the galvanometer
you built in SECTION
1.
SpringClip
5) Wetthe papertowelwith a solution of sodiumchloride(salt
water). Sodiumchloride solution is the electrolyte. (Remember
to use the "off-on-off" techniquefor testing this
"electrolyticcell").
Nickel
Towel
~
Sprin,~lip
Penny
I
6) Whathappensto the galvanometer?Whichwaydid the
needlemove?Whichmetal do you think is giving up the
electrons?Whichis taking the electrons?
Figure#41
Page44
4)
If you wish, you maytape the compassface into its round
depressionwith a loop of transparent cellophane tape just
to secure it from turning in the round depression. See
Figure #38.
Youwill needthe following materials to complete this experiment:
4) Select two paper atomsof chlorine.
10) Makea 3-D model of sodium chloride. Use the colorcode
given in Table #1 to identify the different atoms.SeeFigure
#16.
5) Slide the two atomstogether in such a waythat the side tab
LIST OF MATERIALS
IJ
Compass assembly
andnotch of one chlorine fill
other. SeeFigure #14.
the side notch and tab of the
SODIUM
D-Cell battery
CO~VIPASS
NEEDLE
Permanentfine tip marker
[J
COMPASS
FACE
[J
TAPE
~
PLASTIC
B~
Insul~a_te~dwire (the clear lacqueron the outsideof the
wire acts as insulation)
Goggles
CHLORINE
Figure #16
BE SURE TO WEARGOGGLESW_H..EN DOING_
EXPERIMENTS
IN THIS CHEMISTRY
SE..T..!
Figure #14
~UMB
¯ TACK
CARDBOARD
RECTA~E
1)
Locate the magnetic compasspacked in your chemistry
set, whichyou built in the previous section.
This is a MODELof a MOLECULE
OF CHLORINE.A chlorine
molecule
would
have
the
symbol
CI
2.
2)
Measureout about 2 ft.
wire.
6)
3)
Strip the insulation awayfrom about 1" (2.5 cm.) of each
end of a wire. Label one end of the wire negative (-) and
the other endof the wire positive (+). Useyour transparent
tape to label the ends of the wire. (The wire is insulated
with clear lacquer. This coat of lacquer is whatyou "strip"
awayat the ends of the wire.)
Figure #38
5)
Press thumbtackup through the bottom of the black plastic
base and up through the very center of the compassface
so that the sharp point of the tack comesout right in the
center of the 8-pointed star of the compass
face.
4)
6) Tape a small length of plastic cellophane tape over the
headof the thumbtackunderneathso that the tack doesn’t
fall out. SeeFigure #38.
(60 cm.) of #24 insulated copper
Using your plastic molecule models now makea 3-D model
of chlorine. Usethe following color codeto identify the different atoms. See Figure #15.
TABLE #1
Color code for plastic molecule models
COLOR
Black
White
Red
Green
Gray
Orange
Orange
Silver
Yellow
Blue
Wrapthe wire around the compassas shownin Figure #39.
BE SURE TO HAVE THE COMPASS NEEDLE AT AN
ANGLE WITH THE WRAPPEDWIRE.
7) Gently sit the compassneedle with its one end dyed blue
onto the sharp, pointed end of the thumbtack.
8)
Sodiummetal is a silvery substance.It is an active element
whichwill react violently with water. Chlorine is a green-yellow
gas. Chlorine wasused in war as a poison. Sodiumchloride is
a substancewhich is essential to life. Sodiumchloride is also
kr~owr~ as table sa(t. Weuse tab(e sa{t to seasonour food.
Sodiumchloride is a simple compound
which has the properties
of neither sodiumnor chlorine.
THE REACTION OF TWO OR MORE SUBSTANCES
PRODUCESA NEW SET OF SUBSTANCESWHICH ARE DIFFERENT THAN THE ORIGINAL CHEMICALS.
Twoor more elements can react with each other to form a
new chemical called a COMPOUND.
The process of forming a compoundfrom the elements is
called SYNTHESIS
(sin’ the sis).
Youwill notice that the compassneedlewill movefreely on
top of the thumbtackand the needle will eventually become
still andpoint to magneticNorth.
Number
of Arms
Atomthis represents
4 arms
1 arm
2 arms
1 arm
1 arm
2 arms
3 arms
3 arms
4 & 6 arms
4 arms
Carbon
Hydrogen
Oxygen
Chlorine, Fluorine
Sodium, potassium
Iron +2
Iron +3
Aluminum
Sulfur
Nitrogen
SECTION.2__-..PAPER CHEMISTRY
LAB II
Iron is a metal. Iron can combinewith manynon-metals.
The most commoncompoundformed by iron is iron oxide. The
oxide of iron is knownas RUST.
Some elements, you may remember, are diatomic.
Oxygenis diatomic like chlorine. Iron is not diatomic.
You will needthe following materials to complete this experiment:
LIST OF MATERIALS
Papermodelso1 iron (Fe+2) and Ch(orir~e {C(-1)
9) Makesure that neither of the points of the compassneedle
scrape on the cardboard compassface.
3-D modelsof the atomsof Iron (Fe+2) and Chlorine (C1-1)
10) Youmayturn the whole compassunit so that the blue end
of the compassneedle and the "N" printed on the compass
face line up. This particular orientation of the compass
unit
will tell you whichwayis North (N), or South (S), or
(E), or West (W). You can even read off the "degrees"
the compass,like 90° for EAST,or 180° °for SOUTH
or 270
for WEST,
or, finally, Zero, or 360° for NORTH.
_RF,£URETOWEAR
GOGGLES
.W..H__E_N__D_O!.N~G
E .X.PE_RIMENTS
IN THISCHE__M._.,.,STRY
,,SET!
11) The white piece of cardboard with the notches on each end
is the base of your compass. You should tape the cardboard onto the underside of the compassplastic frame.
Tapeif to the long sides of the plastic base. This will give
your compassassemblymore rigidity.
See Figure #38.
Goggles
CHLORINE
Figure #15
Figure #39
5)
Lay the compassand wire on a flat surface. Be sure that
the needle can movefreely.
6)
Touchthe ends of the wire to the ends of a "D" cell. (The
best methodfor using your electron flow detector is to just
touch the wire ends to whatever you are testing. An "onoff-on-off" techniqueis best. Whenyou touch wire for "on,"
quickly look for movementof compassneedle. Then take
wire "off" and observe compassneedle return to normal
direction.)
_SECTION1A_-. D._E._T.ECTING THE FLOWOF ELECTRONS
Whenelectrons flow through a wire, a magneticfield is formed.
Wecan detect the flow of electrons through a wire by detecting
the magneticfield which is formed.
Page 43
7)
What happens to the compassneedle? Which way did the
needle move?
1)
Select two paper iron atoms.
2)
Select three oxygenions.
Select a sodiummetal atom and a chlorine non-metal molecule from your supply.
3)
8)
Slide the sodiummetal atom’s triangles into the notch in the
chlorine atom.
Rearrangethe atomsto form a molecules of iron oxide, or
rust. Rust has ’the formula Fe20
3.
4)
9)
Oncethe sodiummetal has been placed into contact with
the chlorine, the side tie to the other chlorine is broken.
Pull awaythe combinedchlorine with the attached sodium
from the uncombinedchlorine.
Try to makea 3-D model of iron oxide. Howdo the atoms
arrange themselves? Does the paper model show this?
See Figure #17.
7)
What do you think happens to the uncombinedchlorine
atom?
The combination of sodium, a metal, with chlorine, a
non-metal, has formed a new substance, a compound. This
compoundis sodium chloride. The FORMULA
(model) for sodiumchloride is NaCI.
OXYGENATOMS
/ ,,,
~.ON ATOMS
Figure #17
This is another synthesis reaction.
Page 12
4) Place1 cmlengthof iron wire in eachof the wells contain-
SECTION3 - SYNTHESIS
ing a solution.
Synthesisis oneof the mostimportantandinteresting areasof
chemistry.You,as a chemist,are putting together, perhapsfor the
FIRSTTIMEEVER,chemicalswhich have never beenput together
before!
Eventhoughthe reactionsyouare doingare "known"...you
will be making"brand new"chemicalsand compounds
which were
not presentin the materialsyouare workingwith beforeyoustarted
your experiment!
As a goodchemist,you mustobserveclosely and you must
recordor write downyour results. Thechart andtables are provided for your NEW
data!
emptywell. This is a control.
E/ectrochemistry
6)
Fill a smalltest tubewithwater.
7)
Ptacea 1 cmlengthof iron wire in the test tubeso that the
wire is totally UNDER
the water’s surface.
8) Standthe smalltest tubein a large well in the microplate.
SeeFigure #19.
A battery is composed
of CELLS.A cell contains two metals
and an electrolyte. Onemetal in the battery GIVESUPelectrons, the other metalTAKES
ONelectrons. If the flow of electrons goesthrougha wire, the electrons can do work! This is
the waya cell provides electrical power. TWODIFFERENT
METALS,
in an ELECTROLYTE,
form a cell. A battery is a
seriesof cells linkedtogether.
9) Let all the iron wiresremain,undisturbed,for twodays.
10) Observe
the iron wire over the next two days.
1) Using your MICROTIP
pipette, place ten drops of sodium
chloridesolutionto oneof the smallwells in the microplate.
Rinsethe plastic pipette. Placeten dropsof calciumnitrate
solutionin anothersmallwell. Repeat
this processwith ferrous sulfate, cobalt chloride andammonium
chloride solution. Be sure to rinse the pipette betweeneachchemical
solution.
Placefourteen microdropsof water in an adjacentwell.
SeeFigure #18.
SMALL WELLS
Figure #18
LARGE WELL
LIST OF MATERIALS
Compass
unit (from your chemistryset) whichcontains
the plastic base, compass
face, thumbtack,compass
needle,andcardboardbackplate with the notchescut
into its ends
~
Transparentcellophanetape
Goggles
Figure #19
BE SURETQ..WEAI~..GOGGLES
WHENDOING
EXPERIM_ENTS
IN THIS CHEMISTRY
SET!
3)
When
you turn on a portable radio, TVremotecontrol or any
other device which uses electrical energyawayfrom a wall
socket, you are using chemicalenergyprovidedby batteries.
BATTERIES
are simple machines, A battery is a simple
machinebecausea machinechangesone form of energy into
another.Batterieschangechemicalenergyinto electrical energy. Electrical energyis carriedby electronsin motion.
Thefollowing experimentshowsyou howto build a detector or
instrumentfor detectingthe "flow of electrons"througha wire.
This flow of electronshappens
whenan electrical currentis producedin a chemicalreaction andby using the instrumentthat
you will make,you can actually see evidenceof the electrons
producedin your chemicalreaction. Theelectron detector is a
compass
device which changesthe "deflection," or movement
of the compass
needle,whenelectronsflow in a series of loops
of wire near the compass.
IRON WIRES
LIST OF MATERIALS
Sodiumchloride solution (makeyour ownsodiumchloride
solutionby addingoneml. of table salt to 10 ml. of water)
Calcium
nitrate solution
Cobaltchloridesolution
Ammonium
chloride solution
Microplate
Plasticpipettes(6)
Short(1 cm)lengthsof iron wire (fromyour chemistryset)
Water
Smalltest tube
Goggles
Addfour dropsof waterto eachsolution.
ELECTROCHEMISTRY
5) Place another 1 cmlength of iron wire in an adjoining
this experiment:
2)
SECTION
1 - BUI_L_D.ING..__YOUR
DETECTO.R
CHAPTER9
BATTERY
- A series of cells connected
together.
12) Whichwire showedthe most change?Whichwire showed
no sign of change?Whatother chemicalis necessaryfor
iron wire to change
the wayit did?
CELL- A chemicaldevicecomposed
of two different metalsin
an electrolyte. Cells convertchemicalenergyinto electrical
energy.
SECTION3A- SYNTHESIS
CHEMICAL
ENERGY
- Energy stored in the bonds of chemicals.
LIST OF MATERIALS
~,] Sodiumchloride solution (makeyour ownsodiumchloride
solution by addingoneml. of table salt to 10 ml. of water)
~ Calcium
nitrate solution
F_.] Ferroussulfate solution
I~ Cobaltchloridesolution
~ Ammonium
chloride solution
~ Microplate
L.] Plasticpipettes(6)
~ Copperwire lengths (1 cm)from your chemistryset
[~] Aluminum
wire lengths (1 cm) from your chemistryset
Page 13
ACTIVITY
SERIES
- A list of elements
in orderof their ability to
give up or take onelectrons.
11) Howdid the iron wire change?Wherehaveyou seenthis
color before?Whatchemicaldo you think has formedfrom
the iron wire?
In this experiment
youwill go evenfurther in making"new
materials". Themaintasks of the chemistare (1) experimenting, (2) observing,and(3) recordingthe results so that the
thesis of newmaterials andnewsubstancescan be provenand
doneagain by anotherchemistin anotherlab! If a friend also
hasa chemistryset, compare
data andresults with your friend
as you eachdo the sameexperimentseparately!
BE SURE_..__TOWEAR
GOGGLES
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
TERMS TO KNOW
Layall of the materialsout in front of you andlook them
over carefully. Thethumbtack
is stuck into the top of the
plastic caseso it won’t get lost duringshipping.Takethe
thumbtack
out of whereit hasbeenstuck, and lay it with
yourotherparts in front of you.
BOND
- A force whichholds moleculestogether.
2) Youshouldhavethe following parts ready:
Thumbtack
Blackplastic casewith a rounddepressionin its center
Compass
needle, one end of which is dyedblue
Compass
face, or roundcardboarddisc with N, E, S and W
printedonit
Cardboard
backplatewhichgoes on the undersideof your
compass.
COMPASS
- A devicefor the detection of magneticfields.
CORROSION
- The chemical combination of a metal with
anotherchemicalusually resulting in the destruction of the
metal.
3) Place the cardboarddisc (compassface) into the round
depression
of the plastic base.Youwantthe Northor N letter of the compass
face to point towardthe endof the rectangular case. SeeFigure #37.
ELECTRICAL
ENERGY
- The energy carried by electrons in
motion.
ELECTRODE
- A piece of metal surroundedby an electrolyte.
ELECTROLYTE
- A solution which conductselectricity.
GALVANOMETER
- A device which detects the flow of electronsor electricity.
TERMINAL
- The part of a battery which provides or draws
electrons.
BUILDING_Y...O_UR
.CO_M__PASS/
E_L..ECTRO_N
_F__/_O_W..
_D..ET__EC~TO~R
In your next section (SECTION
1) you will use a compass
which
is wiredin a certain wayto detectthe flow of electronsthrougha
wire. You must first assembleyour COMPASS
- ELECTRON
FLOW
DETECTOR
from the materials provided in your chemistry set. First, find the plastic bagin yourchemistry
set containing the parts for your compass.
Pace42
Figure #37
1) Obtain as manysample tablets of different brands of
antacid as you can. Askfriends or relatives for one or two
tablets for youto test.
2) Place onetablet of each brandto be tested in each of your
plastic measuringcups. You maywant to crush the tablet
into smaller pieces just as you did in the previous experiment.
ANTACID SOLUBILITY COMPARISONCHART
Goggles
BE SURE TO WEAR GOGGLESWHEN DOING
EXPERIMENTS
IN THIS CHEMI$._T_RYSETI.
Antacid Tablet #1
Antacid Tablet #2
Antacid Tablet #3
Antacid Tablet #4
6) Place 20 drops of each sampleinto separate large wells of
the microplate. Uselarge wells B-l, B-2, B-3, etc.
7)
brand .............
Note on a piece of paperwhich brand of antacid is in large
well B-l, which is in large well B-2, etc. Washout your
pipette with water betweensamples.
8) Usingyour pipette, place 3 drops of Universal Indicator solution into eachwell containing the samples.
9) Stir each well with the toothpick and observe the color
change.
CHEMICALS
USED
SODIUM
CHLORIDE
brand
brand
.......................
5) Carefully draw up someof the liquid from the top of the
measuringcup into your pipette.
DATA TABLE #2
NOTE:Copper wire is copper colored (like a new penny) and
will NOTbe attracted by a magnet. Aluminumwire will seem
very light in weight and will be shiny silver in color. Aluminum
wire will NOTbe attracted by a magnet.
1)
4) Stir each samplewith a toothpick and then allow the cups
to sit undisturbedfor 30 minutes.
12) Comparingreactions of the iron wire from Section 3 and
the aluminumand copper wire from Section 3A, which wire
showed change? Which wire showed no change? What
can you predict about the use of copper and aluminumwire
instead of iron wire? Recordyour results on Data Table #2.
Small test tube
Color of Universal Indicator compared
with chart from Chapter7, Section 1
brand
3) Add enough water with your pipette to EACHmeasuring
cup to bring the level of the waterANDthe antacid tablet in
the, wate,r up to the 10 ml or 10 cc markon the side of the
cup.
Water
Antacid Tablet #5
brand
Antacid Tablet #6
Usingyour microtip pipette, place ten drops of sodiumchloride solution in small wells A-1 andA-12. Rinsethe pipette.
Place ten drops of sodiumchloride solution in small wells
A-1 and A-12. Rinse the pipette. Place ten drops of calciumnitrate solution in small well B-1 and B-12. Repeatthis
process placing ferrous sulfate solution in C-1 and C-12,
cobalt chloride in small wells D-1 and D-12, ammonium
chloride in D-3 and D-10. Be sure to rinse the pipette
betweeneach chemical solution.
2)
Addfour drops of water to eachsolution.
3)
Place fourteen drops of water in small wells D-4 and D-9.
See Figure #20.
11) Which sample showed the stronger base? The sample
which showedthe stronger base will be the brand which
has the most soluble base. In other words, the moresoluble basewill go into the water solution moreeasily andproduce more base for use as an antacid.
brand
................
COLBALT
CHLORIDE
AMMONIUM
CHLORIDE
WATER
SECTION4 - PAPERCHEMISTRYLAB Ill
Youwill need the following materials to complete this experiment:
LIST OF MATERIALS
~ Paper models of atoms
Antacid Tablet #8
3-D models of atoms
A
B
LOW
MEDIUM
HIGH
concentrationconcentrationconcentration
of basethus of basethus of basethus
less soluble mediumsolu- high soluble
Now that you have seen the way chemicals can combine to
form a newsubstance, let’s take the samechemical apart. The
compound,sodium chloride can be separated into the original
elements by adding the correct amountof energy. The process
of makinga compoundreturn to the elements Tromwmcn~t was
formed is called DECOMPOSITION
(dee’ kom po zi shun)
ANALYSIS
(an al’ lee sis).
Figure #20
h~e in t=hlet
parison Chart.
tablet
What other household products do you think have base? Look
at the results of your experimentsin the part of this lab bookon
pH.
I, D-I,D-3andD-4.
5) Place 1 cmlength of aluminumwire in small wells A-12, B12, C-12, D-12, D-9 and D-10.
1)
Join one sodiumatomto one chlorine atom to form a sodium chloride molecule. Maketwo paper molecules of sodium chloride. This is the process of SYNTHESIS.
2)
DECOMPOSE
the two molecules of sodium chloride by
breaking the two chlorine atoms away from the sodium
atoms.
3)
The two atoms of chlorine combinewith each other to form
a MOLECULE
of chlorine. This molecule of chlorine has
the symbolCI
2.
4)
Each of the two atoms of sodium remain individual
of sodium.
5)
The compound sodium chloride has been DECOMPOSED
into the elements sodiumand chlorine.
6) Place 1
cmlength of copper wire in empty small well A-4.
Place 1 cmlength of aluminumwire in small empty well A9. Theseare control wells.
7) Fill two small test tubeswith water.
8) Place 1 cm length of
copper wire in one test tube so that
the wire is completely under water’s surface. Stand this
test tube in large well A-I.
9) Let the wire remain undisturbed for two days.
10) Observethe wire for the next two days.
11) Did the wire change?
Page 4 !
ALUMINUM
NAILS
FERROUS
SULFATE
Antacid Tablet #7
brand
COPPER
NAILS
CALCIUM
NITRA1~
brand
10) Comparethe color changeof the Universal Indicator solution with the comparisoncolor chart you preparedin CHAPTER 7, SECTION1.
IRON
NAILS
Page 14
atoms
SECTION4A -. U._S.ING MOLECULAR
MODELS
SECTION 5 - HOWMUCHBASE IS IN
ANTACID TABLETS
5)
Transfer the remaining solution in the large test tube for
storage.
Antacid tablets are sources of mild base. These tablets are
used to settle upset (sour or acid) stomachs. Whyshould the
base used to settle upset stomachs be a mild base? A mild
base does not dissolve completely in a water solution. A solution of householdvinegar is about 5%acetic acid. This acid can
be used as a standard (control) for the determination of the
amountof basein a solution of antacid tablets.
6)
Fill another microtip pipette with STANDARD
ACID SOLU®
TION(Heinz White Distilled Vinegar).
7)
Add2 drops of Universal Indicator to the acid solution in the
large well. Whatis the pH of the solution?
OXYGEN
Repeatthe building of the moleculeslisted in Section 4 by
using the 3-D molecular modelsprovided in your chemistry set.
Usethe color code found in SECTION
1:6 to identify the different atoms.
S__E.._C-[JO_N_4B__-__U_SING
_MOLECULAR
MODELS
II
8ULFUR~
CARBONOlOXlO[MOLECULE
Figure21-b
Figure21-c
¯ HYDROGEN
Lookat the labels on the vials of chemicalsprovidedin your
chemistry set. There is listed on each label the nameof the
chemical as well as the FORMULA
of the chemical compound
which that namerepresents.
Write down on the chad below the nameof the chemical compound,and next to it, the chemical FORMULA
of that
compound.The chad has started a few entries for you. Now
you completethe rest.
(~"
CHLORINE
(~ HYDROGEN
.~.
HYDROGEN
CHLORID~MOLECULE
Figure21-d
NYDROG[CN
PEROXIDE
MOLECULE
Figure 21-e
CARBON
HYDROGEN
HYDROGEN
CHLORNE MOLECLLE
DATA TABLE #3
Figure21-f
Chemical Name
onlabel o! vial
Chemical Formula of
the compund
CALCIUM NITRATE
Ca(NO3)2
SODIUM SILICATE
Na2SiO3.5 H20
SODIUM CARBONATE
Na2CO3
OXYGEN--~f~=~
METHANOL
MOLECUI
Figure 21-g
HYDROGFN
~
[]
[]
Antacid tablets (as manydifferent brands as you
want to sample)
Microplate
[]
Plastic pipette
[]
Toothpick
[]
IJ
Universal Indicator solution
[]
Metal teaspoon
Using a toothpick to constantly stir, add the standard acid
solution to the well with the antacid solution. SeeFigure
#35.
9)
Whenthe antacid solution has beenneutralized, (how will
you know?) enter the numberof drops of acid used in the
Data Table below.
ANTACID NEUTRALIZATION TABLE
Antacid Tablet #1
A) Mass(weight) of hydroxide
one antacid tablet
B) Numberof drops of vinegar used
Metal tablespoon
__
mg
dr
__
mg
dr
Small test tube
[]
Figure 21-h
WATER
{,~=~SHLO
NINE
CARBON
CARBCN
TETRACHLORIDE
MOLECULE
~.
1)
CARBON
METHANE
MOLECULE
Figure21-i
TEASPOON
~’,~.l
~
~
CRUSH
TABLET
EI"HANE
~4OLECULE
Figure21-k
mg
dr
TABLESPOON
Figure #36
YDROGEN
HYDROGE~~c~RBO~
2)
3)
The weight or mass amountin milligrams of the active
ingredient in antacid tablets is printed on the label of the
antacid containers. Readon your various antacid bottles
under the heading of ACTIVEINGREDIENTS:
Listed there
will be the amountin rag. (milligrams) chemicals which
have hydroxide as pad of their chemical name, such as
AluminumHydroxide or MagnesiumHydroxide. Add these
amountstogether to obtain the total numberof milligrams
(mg.) of the hydroxides listed, PERTABLET.Record this
weight on your data table provided.
Dissolve the crushed antacid tablet in 10 ml of distilled
water in a large plastic cup.
PROPYLENE
MOLECULE
Figure 21-m
®, etc.) to deterTest different brands of antacid (Rolaids®, Tums
mine which antacid has the most soluble base.
Figure21-a
Page 15
Antacid Tablet #3
A) Mass(weight) of hydroxide
one antacid tablet
SECTION 6 - DIFFERENT BRANDSOF ANTACID
Figure21-I
Youmight look around your housefor things like styrofoam
balls, modeling clay, toothpicks, pipe cleaners, and straws.
Thesemakeexcellent materials for building larger molecular
models. Gumdrop candies and toothpicks makegreat molecular models!
Using the large tablespoon as a base, place the antacid
tablet into the large tablespoon. Takethe smaller teaspoon
and use the teaspoonto crush the antacid tablet into powder in the large tablespoonby putting your thumbinto the
curved inside of the teaspoon. See Figure #36. Be sure
not to lose any of the particles of the antacid tablet.
Figure21-j
ETHYLENE
MOLECULE
OXYGEN
Antacid Tablet #2
A) Mass (weight) of hydroxide
one antacid tablet
Goggles
HYDROGEN
After you have listed all of the namesand formulas, and
using your paper models, construct as manyof the compounds
as you can with the papermodels. This will let you think of the
"making" (COMPOSITION)
of chemical compoundsin the same
waychemists think of them.
Nowtry to put together your plastic 3-D modelsof these
samechemical compoundswhich you were able to put together your paper models. Usethe proper color code for different
elements of your compoundsas shown in SECTION1:6.
SOMEFORMULAS
may be too long or complex to do with
your models, so don’t worry if you don’t get all of them. You
should, however,be careful with most of the chemicals.
At right are included someexamples of simple and complex molecular models.
As you do the various experimentsin this set, try building
modelsof the reactions. This will help you to understandwhat
is happeningin each reaction. For example, reacting hydrogen
with oxygenwill result in the formation of water. The reaction
lookslike this:
OXYC,[N
8)
LIST OF MATERIALS
Vinegar
~4YDROGEN
ACETONE
MOLECJLE
HYDROGFN
Be sure to COUNTTHE NUMBEROF DROPSOF ACID
USEDin the next steps below.
4)
LIST OF MATERIALS
® Samplesof different
IJ
brands of antacid (example: Rolaids
[]
®)
or Tums
Twoplastic measuring cups
[]
Water
[]
Toothpick
[]
Plastic pipette
[]
White paper
[]
Tablespoonand teaspoon for crushing tablets
[]
Color chart from CHAPTER
7, SECTION1
[]
[]
Goggles
Transfer 20 drops of antacid tablet solution to a large well
in the microplate.
Page 40
SECT_~ON
5- DECOM_P_._.O._SlTIQN__Q~-WAT~
A CHEMICAL CHANGE
Usingyour pipette, place 10 drops of each brand or type of
vinegar in a large well of the microplate. Start with large
ontinue putting 10 drops of EACHDIFFER_ a_n,?.c..
well A 1,
.... ~n ~. ch different large we~l. Keeptrack
a
ENTkind ~f v,-~u .....
o! whichtype of vinegar is in whichlarge well.
1)
ARIN-G I-~-E~-E-R
SECTION 4 - COMP
T~~L~
oE_W._N
E_5~_&~-
Try to collect samples of as manyDIFFERENT
brands of vinegar, both white vinegar and ambercolored vinegar, Apple Cider
Vinegar, Tarragon Vinegar, and yes, even vinegar madefrom
pineapple juice! You should try to get as manyDIFFERENT
brand makesof vinegar as you can. Ask neighbors and relatives for samplesof their vinegar and be sure to record the
nameand type of the vinegar collected.
3)
Fill another pipette
SECTION1.
4)
Add2 drops of Universal Indicator solution to each of the
large wells whereyou are testing the different vinegars.
5)
Using your pipette with the CONTROL
BASE, add the
Control Base, drop by drop, to the vinegar test wells. BE
~,.I
~
Microplate
~
Plastic pipette
Your color chart for Universal Indicator andvinegar
6)
7)
Microplate
A strip of filter paperandscissors
Vinegar(acetic acid) - obtain from your kitchen
Goggles
BE SURE TO WEAR GOGGLES _W~
EXPERIMENTS
IN THIS CHEM!T,~_T_~Y..~S-~.
Use the toothpick to constantly stir as you add the STANDARD(CONTROL
BASE) solution. See Figure #35.
1) Place1/4 pipette full of vinegar in a small plastic cup.
Whenthe acid (vinegar) solution has been neutralized,
enter the numberof drops of base used in the data table
provided below. Determinethe %acid of each of the diflerent types of vinegar tested.
(Chapter 7 - Sections 1, 1A)
Toothpick
Test different brands of vinegar to determinewhich vinegar has
Goggles
the most acid.
pipette by drawingthe solution up into the pipette and then
squirting it backin the cup. Dothis several times to insure
a goodmixing of the vinegar (acetic acid) andwater.
Place one pipette of the water-vinegar solution in each o!
three large wells of your microplate. Usewells A-l, A-2 and
A-3. Twoadjoining wells are lor the experiment. The third
3)
well is a control.
If the substanceis a base, howwould you find out _H_. WMO_~
~ is present?
4)
Cut a piece of filter paper 6 mmx60 ram. Wet the entire
strip of filter paperwith vinegarsolution.
5)
Place oneend of the filter paper in ~argewell A-1 and the
other endof the filter paperstrip in large well A-2.
6)
Connecta battery clip to a 9-V battery.
Percentageof Acetic Acid in Different Vinegars - DATATABLE
#11
% ACID IN THIS BRAND/
TYPE OF VINEGAR
/
COLUMN
~ No of Drops of Base |
(ColumnB divided by A)
~ for this brand/tyPe
of vinegar
%
Wh~eVinegar)
drops~
drops /
COLUMNA
No.of Dropsof Base
for 5%Acetic Ac{d
TYPE/BRAND
OF VINEGAR TESTED
(He~nZ~ D~$tfiled
White Vinegar
drop.~_
-- Amber Vinegar
Apple Cider Vinegar
drops
Pineapple Vinegar
drops
8) Observethe bubbling from each of the wells.
drops
9)
Whatcharge is on the oxygenion? (See your paper ion collection for the answer,if necessary).
10)
Whatcharge is on the hydrogen ion? (See your paper ion
collection for the answer,if necessary).
drops
Tarragon Vinegar
Brand
Vinegar
Vinegar
Place the red coated wire (+ charge) in one o! the wells
containing the paper and the black wire (- charge) in the
wull ~u,~,~i~&~u~i,~ ut’, ,e, endo; tt;c p~pcr.Ccc,rLGurc,,#22.
drops
drops
%
%
11) If unlike chargesattract eachother, what possible gaseous
elementsare being given off at the positive chargedwire?
%
12)
%
13)
drops
drops
Brand
drops
Vinegar
Brand
drops
Vinegar
Brand
drops
Vinegar
--Brand
Page 39
drops
drops
drops
~rop;
+)
15) Since hydrogen IONSare positive (H these will be attracted to the NEGATIVE
wire (negative electrode). Since
the oxygen(0") ions are negative, they will be attracted
the POSITIVE
wire (positive electrode).
16) The acetic acid (vinegar) was used only to makethe water
conductelectricity better. The vinegar helpedthe water be
an ELECTROLYTE.
1"7)
%
%
What gaseous products are given off at the negative
charged wire?
You are decomposingwater (H20) into its two basic elements. These two basic e~ementsare oxygen and hydro-
Look closely at the positive electrode and at the negative
electrode. Which electrode seems to be producing more
bubbles than the other?
2) Add3 pipettes of tap water to the vinegar andstir with the
Whatother household products do you think have acid?
W.H._E._N_ P.QI~LG
-T..-R-~’.-~
-~-T~
EXPERIMENTS
IN THISCHE--MI-~
Figure #22
9-volt battery clip
with CONTROL
BASEprepared in
SURE TO COUNTTHE DROPSOF BASE USED IN EACH
LARGE WELL.
Control base (prepared in SECTION
1)
~
LIST OF MATERIALS
Plastic pipette
9-volt battery
ferent types of vinegar.
UST OF MATERIALS
~ Samples of vinegar (as manyas possible)
’~
ment:
Add10 drops of water to each large well whichcontains dif-
2)
Youwill need the following materials to completethis experiment:
Youwill need the following materials to completethis experi-
Since water is madeup of t_wo_hydrogensfor every o__n__e
oxygen (H20), there will be twice as muchhydrogen gas
18)
produced as oxygen gas.
19)
More bubbles wil~ be produced at the negative electrode
(wherehydrogengas is produced)than at the positive electrode (where oxygen is produced).
20) The wet filter paper betweenthe we~ls not only conducts
electricity betweenthe wells but it also lets any ions go
back and forth to get to the electrode to which they are
attracted.
SECTION
6 - pAP_E__R
CH__~_EM_IST.F~¥_.I--V
~ja.~, yuu ,-j~, ,~’ ~’"~" ..... "~ .- ~._~ ~n~l moecu~arlevel
somethingthat is happeningon the atuH, ......
which you cannot actually see with your eye. Remember
the
"way" in which the hydrogen and oxygengo together and come
apart. This is an important reaction to knowabout.
Hydrogenand oxygenonly go together in a very certain wayto
makewater molecules. Water only decomposesin a very carrain way to produce hydrogen gas and oxygen gas. Can you
see the simple mathematica~way that this happens?
LIST OF MATERIALS
~3 Paper models of hydrogen
Paper models of oxygen
gen.
Since hydrogen and oxygen are both gaseous at normal
14)
conditions, you should see bubbles forming at the wires,
and bubbles movingup the wires to the surface of the liq- Page 16
uid.
3-D models of hydrogen
3-D models of oxygen
Onered pencil
Oneb~ackpencil
BE SURE TO WEARGOGGLES
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
A circle of filter paper
Smallamountof corn starch (obtain fromkitchen)
Goggles
1)
Build two papermodelsof water (H20).
2)
Place two pencils downon the table top. Thesetwo pencils representthe red andblack wires in the waterelectrolyte.
3) Breakthe moleculesof water up to form hydrogengas at
the negative wire (negative electrode). Remember
hydrogenis diatomicgas(H2).
Acidsreact with bases.Thereactionof an acid with a baseproducesa SALTand water. Common
salt, sodiumchloride (NaCI),
is the salt resulting froma reaction between
sodiumhydroxide
(NaOH)and hydrogenchloride (HCI). Thereaction which
ducessodiumchloride is:
BE SURE-EO W~E.A.RGO_GGLES
WHEN
DOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
4) Breakthe moleculesof water up to form oxygengas at the
positive wire (positive electrode). Remember
oxygen
diatomicgas(02).
1) Place1/2 pipette of potassium
iodide (KI) solution in each
5) Nowcan you see whytwice as manybubbles are formed
at the electrode wherehydrogengas is produced?
SECTION6A- USING 3-D MODELS
BE SURETO WEAR
GOGGLES
W .H.E.~N_ DOING
EXPERIMENTS
IN THIS CHEMIST_RY
SET!
of 3 large wells of the microplate.Usewells A-l, A-2 and
A-3. Remember
large well A-3 is a control.
NaOH+ HCI
(base) (acid)
Acetic acid ionizes to producea hydrogenion and an acetate
ion.
3) Placeoneendof the filter paperin onewell A-1 andthe
CHEMICALCOMPOUNDS
AND CHEMICALSEPARATIONS
otherendin the otherwell A-2. Bothwells containsolution
of potassium
iodide.
4) Connect
a 9-volt batteryto a batteryclip.
Isolation of Elementsfrom Compounds
Compounds
are NOTmixtures. A mixture can be separatedby
physical means.Examples
of physical means
include: boiling,
condensing,
melting, thawing,etc. Thesubstances
in a mixture
keep their ownphysical properties. Compounds
can only be
separated into elements by CHEMICAL
MEANS.
A compound
is a chemically DIFFERENT
SUBSTANCE
from the reactants
whichformedit.
5) Placethe red wire fromthe battery clip into onewell with
8) Cut a roundpieceof filter paperabout2 inchesin diameter. Wetthe filter paperwith tap waterand rub the corn
starchontothe wetpieceof roundfilter paper.
9) Cutthe roundstarchrubbedfilter papercircle in four parts.
Placeoneslice of the roundfilter paperin smallwell A-l,
placeanotherslice of the roundstarchfilter paperin small
well B-1.
someof the liquid fromthe well with the (-) elec11) Remove
trode. Placea few dropsof the liquid in two small wells.
Placea pieceof filter paperinto onewell. Theappearance
of a blackstainis a positivetest for iodine.
LIST OF MATERIALS
Solutionof potassium
iodide
Plasticpipette
Microplate
9-volt battery
9-volt batteryclip
Filter paperstrip (SeeSection5)
12) Using anotherpipette, removesomeliquid from the well
with the (+) electrode.Placea fewdropsof the liquid in two
small wells. Adda pieceof paperto onewell. Theappearanceof a black complex
on the paperis a positive test for
iodine.
Whichelectrode producedthe iodine? Howdo you know?
Page 17
2)
Add10 dropsof waterto the acetic acid solution.
3)
Fill another microtip pipette with CONTROL
BASEprepared in SECTION
1.
4) Add2 dropsof UniversalIndicatorto the acid solutionin the
Testa solutionof household
vinegarto seeif it is anacid.
Whatwouldyouuseto test it?
Be sure to COUNTTHE NUMBER
OF DROPSOF BASE
USED
in the next step (5).
Vinegarreacts with sodiumbicarbonateto producesodium
acetate, water and ???????.
do you observein eachwell?
Usinga microtip pipette, place10 dropsof oneindividual
brandof aceticacid in a large well of the microplate.
large well. Whatis the pHof the acid?(Consultthe chart
youcoloredin.)
6) Waitabout5 minutesfor the reaction to take place. What
(Likefourslicesof pie).
SECTION
7- ELEC’ERICA.L
SE_P_A...R_.ATION
OFELEMENTS
FROM....A...CQM
POU
N.D
Doesvinegar conductelectricity? Whatwouldyou use to
checkfor conductivity?
When
acetic acid (vinegar) reacts with sodiumbicarbonate,
a salt, waterand a gas is formed.Thereaction is given
below:
ed to the battery?Whatelementis produced
at the red (+)
electrode?Whatelementis produced
at the black (-) electrode?
Elementscan be isolated or separated from compounds
by
using electrical, chemicalor heat energy.Thecompound
containing the elementto be isolated mustreceive enoughenergy
to allow the splitting of the compound
into elements.For the
experiments
below,attention will be focusedon the isolation of
a single elementby the useof electrical energy.
1) Place7 dropsof vinegarin a smallwell of the microplate.
2)
1)
/ H+(aq) CH3COO-(aq)
the paperconnectorandthe blackfromthe battery clip into
the well whichis connected
to the other endof the paper.
SeeFigure #22.
7) Whatdo you think is producedat eachelectrode connect-
THE SEPARATIONOF ELEMENTSFROMTHEIR
COMPOUNDS
ALWAYSREQUIRESTHE USE OF
ENERGYFROMSOMEOUTSIDE SOURCE.
CH3COOH(aq)
BE SURETO WEAR.GOGGLES
WHE_NDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
A standard5%solution of acetic acid is a solution of household
whitedistilled vinegar!
Household
(salad) vinegar is acidic. Theacid in vinegar
acetic acid (CH3COOH).
Acetic acid dissolvesin waterandionizeslike this:
Wetthe strip of filter paperwith potassium
iodidesolution.
[]
~> NaCI + H20
(a salt) (water)
2) Cut a piece of filter paper6 mmx 60 mmwith scissors.
Repeatthe building of the molecules
listed aboveby usingthe
3-D molecularmodelsprovidedin your chemistryset. Usethe
color codefoundin SECTION
1:6 to identify the different atoms.
Yourcolor chart for UniversalIndicator andvinegar
(Chapter7 - Sections1, 1A)
UniversalIndicatorsolution
Microplate
Goggles
CH3COOH
+ NaHCO
CH3COONa
+ H20 + ????
3
(vinegar) (sodiumbicarbonate) (
) + ( ) +
Whatis the name
of the salt produced
in this reaction?Lookat
the SECTIONON NAMINGCOMPOUNDS
to check the name
of the salt. Whatgasis produced
in this reaction?Lookat the
SECTION
ONGASES
to check your guess.
If you use your CONTROL
BASE
to titrate householdvinegar,
you can determine howmuchacid is in commercialvinegar
preparations.
5)
Usinga toothpickto constantlystir, addthe standardbase
to the acid solution. SeeFigure#35.
the acid solution hasbeenneutralized, (howwill you
6) When
know?)enter the numberof dropsof baseusedin the Data
Tablebelow.Determine
the %acetic acid in vinegar.
PipettewithBase
Solution
\ acidsolution
SECTION3 - HOWMUCH__ACETIC
ACID IS IN VINEGAR?
Figure #35
Somehouseholdvinegars measureout to have a 3%solution
of acetic acid in them.Othervinegars, like Heinz® Distilled
WhiteVinegar,measure
out to have5%acetic acid in them.
DATATABLE#10
A) Numberof drops of base
(for 5%acetic acid)
drops
B) Numberof drops of base
LIST OF MATERIALS
[] Twoplastic pipettes
[] Toothpick
[] Water
Control base (prepared in SECTION
1)
(for anothervinegarsample)
C) %acetic acid in vinegarsample.
(B divided by A)
Page 38
drops
SECTION9 - ELECTR_O_L_Y_$1S
OF FERROUS
SULFATE
SECTION 8 - ANOTHERE_ E~_ICAL SEPARATION
Plastic scoop
CHAPTER
Titration:
TITRATION: A
QUANTITATIVE
METHOD
A Quantitative Method
Using your chemistry set, you have beenable to test manydifferent materials to see if they were ACIDICor BASIC. Chemists sometimes want to know HOWMUCH
acid or base is in a
substance. While pH tells the general amountof H+ in a solution, a more exacting methodused to determine the amountof
acid or base is the process called TITRATION.
Titration is the Odest method of QUANTIFYING
in chemistry.
By comparing a standard solution (a control) to an unknown
solution, we can determinethe exact amountof acid or base in
solution. This is the processof titration.
Titration is a very common
scientific procedure. Perhaps you
have seen advertisements which say something like...
"our
product contains 47 times as muchas BrandX." This statement
is basedon comparisonsmadeby using titration.
Plastic wrap (,Saran® wrap or other plastic wrap)
Transparent cellophane tape
Fine point marker (Sharpie® brand by Sanford or
iJ
onelike it)
Goggles
I,J
Again you are able to separate a compoundby using a small
amountof electrical energy. Andagain you can see if the separation has taken place by using an "individual," or in other
words, somethingthat will let your eye "see" a reaction which
otherwise you could not see!
BE SURE
TO WEAR
GOGGLES
~_H_.._E...N_...D_OLN_~
EXPERIMENTS
IN TH.!$..CHE_M._L~T__.R...Y.__.SE~TJ
NaHCO3(s)
1)
2)
~ Na+ (aq)
LIST OF MATERIALS
Sodiumsulfate solution
Sodiumbicarbonate is a base. In water, sodium bicarbonate
breaks up into sodium ions and hydrogen carbonate ions.
Universal Indicator
HC
) O-3(aq
Plastic pipette
LIST OF MATERIALS
I I Ferroussulfate solution
Microplate
id
9-volt battery
J
9-volt battery clip
Plastic pipette
(,J Microplate
Filter paperstrip (SeeSection5)
;_~ 9-volt battery
Addthree pipettes of water to the solid in the tube.
Goggles
’J
9-volt battery clip
IJ
Paperstrip (See Section 5)
J
Goggles
3)
4)
Cover the tube with a piece of plastic wrap and label the
tube "Control Base" with cellophane tape and your fine
point marker.
TERMS TO KNOW
ACIDIC- A solution which has a pH less than 7.
ALKALINE
- A solution which has a pH greater than 7.
P~ace7 drops of sodium bicarbonate solution which you
madein a small well of the microplate. What would you
use to seeif it conductselectricity?
BASE
- A chemical that ionizes in water to form OH"ions.
Doesa solution of sodiumbicarbonate conduct electricity?
NEUTRALIZATION
- The reaction of H+ ions with another ion
to form water. A BASENEUTRALIZES
A__N_..ACID TO FORM
WATER.
Whattest will showif sodiumbicarbonate is a base?
QUANTIFYING
- Telling b_o_YYmuchthere is.
What other compoundsin your chemistry set are bases?
(Refer to Chapter7 - Section 7.)
5)
TITRATION
- A process of determining the amountof acid or
base In a sample.
SECTION
1 .-...I~__R._.E_PARATION
O~-.._A._
STANDARD.I~A~E SOLUTION
It is important to always have a "standard" solution which can
be used to compareother solutions which you are testing. This
comparisonof a "known" (‘standard) to an "unknown"(thing
be tested) is what TITRATION
is all about. With a standard
base solution you can test acids. With a standard acid solution
you can test bases.
BE SURE TO WEAR GOG._G__L__ES
~
EXPERIMENTSIN THIS.CHEMISTRY SET!
1)
2)
4)
Plastic pipette
Control base (prepared previously in SECTION
1)
Microplate
Place one drop of Universal Indicator in eachof the wells.
Cut a piece of filter
Wetthe strip of filter
It maybe a surprise that not ALLvinegars which are sold have
the sameacid concentration. Manytimes the makers of the
vinegar will put on their label howmuchacid (the concentration
of acetic acid) is in their product.
LIST OF MATERIALS
Householdvinegar (white vinegar)
Place 1/2 pipette of sodiumsulfate (Na2S04)solution
each of 3 wells of the microplate. Be sure that the wells
selected are next to each other for comparison.
1)
Using your pipette, place 10 drops of ferrous sulfate solution in each of 3 large wells of the microplate. Uselarge
wells A-l, A-2 and A-3. Next, pipette 30 drops of water into
eachof the ferrous sulfate wel~s, A-l, A-2 and A-3.
2)
Place one drop of Universal Indicator in each of the wells.
(Remember
the third well is the control!).
SECTION
2 - TESTIN.G.V.!_N._E,G.,~R
,~O_.L_._~ONS
paper 6 mmx 60 mmwith scissors.
paperwith sodiumsulfate solution.
Wetthe strip of filter paperwith ferrous sulfate solution.
4)
P~aceone end of the filter paper in one large well A-1 and
place the other end of the paper in an adjoining large well
A-2 which also contains the ferrous sulfate solution.
5) Connecta 9-volt battery to a battery clip.
5)
Connecta 9-volt battery to a battery clip.
6) Place the red wire from the battery clip into onewell with
6)
Place the red wire from the battery clip into one well with
the paper connectorand the black wire from the battery clip
into the well which is connectedto the other end of the
paper connector.
Place one end of the filter paper in one well and place the
other end of the paper in an adjoining well which contains
the sodiumsulfate solution.
the paper connectorandthe black wire from the battery clip
into the well which is connected to the other end of the
paper connector.
7)
Wait for about 3 minutes for the reaction to take place.
Whatdo you observe in each well?
7)
Wait for about 3 minutes for the reaction to take place.
What do you observe in each well?
8)
Whatdo you think is produced at each electrode connected to the battery? Whatelementis producedat the red (+)
e~ectrode?Whatelementis producedat the black (-) electrode?
8)
Whatdo you think is producedat each electrode connected to the battery? Whatis produced at the red (+) electrode? Whatis producedat the black (-) electrode?
Universal Indicator Solution
LIST OF MATERIALS
[] Sodiumbicarbonate solid (baking soda) obtain from
[]
BE SURE TO WEARGOGGL_E.~ WHENDOING
EXPERIMENTS
IN THIS.C.H_E_MISTRYSET!
What other bases do you know?
SALT- The chemical produced whenan acid and a base react.
Place 1/2 scoopof sodiumbicarbonatesolid in a small test
tube.
Stir the solid in the liquid until the solid totally dissolves.
ACID- A chemical which ionizes in water to form H+ ions.
The secret in understanding this experiment and the
unseenreactions taking place at the molecular level is in the
positive andnegative chargeat the endsof the wire (electrodes)
which are in different wells. Also rememberthat when compoundsdissolve in water the molecules break up into positive
charged and negative charged ions (in this case Fe++and S04-). The negative electrodes attract the positive chemical ions.
The positive electrodes attract the negative chemicalions.
Toothpick
Electrolyte detector (‘from Chapter6)
kitchen or grocery
Test tube, small
9-volt battery
Water
Goggles
Electrolyte detector (from Chapter6)
[] 9-volt battery
Page 18
Page 37
SECTION
10 : A CH._E___M./CAL
SEPARATION
Sometimes
to makea separation of a compound
happen,
chemistsdo not needto rely on an outsideelectrical force, such
as a battery, but candepend
onthe "activity" of different metals
to do the job for us. In this experiment
wedependon the different "activity" of zinc andcoppermetalsto helpus in separating the coppersulfate molecule.
LIST OF MATERIALS
[]
Coppersulfate solution
Plastic pipette
Microplate
Zinc wire
[]
Copperwire
[]
Goggles
BE SUBE TO WEARGOGGLES
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
1)
Place1/2 pipette of coppersulfate solution into eachof 3
large wells in the microplate.
2) Cut a pieceof zinc wire (providedin your chemistryset)
CHAPTER5
The GaseousPhase of Matter
Gasmoleculesare free to moveabout. Theyare not limited by
other molecules.Sincegas moleculesare farther apart from
eachotherthanmolecules
in the solid state or the liquid state,
gasmoleculesfill the shapeof their container. Gaseschange
their volumewith temperaturechangesand pressurechanges.
Since most gasesare colorless, odorless and tasteless, we
tendto forgetthat:
A GASIS MATTER.
Sometimes
it is easyto forget that a gasis a formof matter.For
us the mostcommon
gasis air. Air is not a single gas. It is a
MIXTURE
of gases. Is there any wayto separatethe gasesin
air?
Mostof air is nitrogen. Animportant part of air is oxygen.
Withoutoxygen,life on earth wouldbe impossible. Canyou
think of any other gasesin the air whichare important?Can
youthink of other gaseswhichare important?
Gasesare not easily packedin your chemistryset. Some
of the
gaseswhichwewill use in experimentswill be madefrom the
chemicalsin the set. Gaseswhichwewill usefor our experimentswill be madeby chemicalreactions.
4) Donot addanymetalwire to the last well. Thisis the control well. Whatis the purposeof the control well? See
Figure#23.
2) Transferten dropsof the rain waterto eachof 4 smallwells
in the microplate.
3)
Adda dropof UniversalIndicator to ONE
of the wells with
rain water.
4)
Addphenolphthalein
indicator to the nextwell.
5)
Finally, test some
of yournatural indicatorswith your rain
sample.
EXPERIMENTS
IN THIS CHEMISTRY
SET!
the color of the indicator in the rain samplewell
6) Compare
1) Using the small well rows C-1 through C-12 and D-1
with the control UniversalIndicator wells youpreparedin
SECTION
1.
throughD-12,place9 dropsof waterinto eachsmallwell in
rowC and rowD of your microplate.
7)
Compare
the color of the indicator in the phenolphthalein
control with the rain sampleandphenolphthalein.
8)
Finally, compare
the "natural indicators" andrain sample
with the colors notedin SECTION
2.
Whichindicator wasthe best for telling the pHof rain
water?
Whichindicator wouldbe the worst?
2)
Place9 dropsof waterin large well A-1andlarge well B-I.
3)
Pipette one drop of eachsolution listed abovein small
wells C-1 throughC-12 and large well A-I. Againdo the
samefor small wells D-1throughD-12andlarge well B-I.
DONOTuse the phenolphthaleinor Universal Indicator
yet.
4) Pipette onedropof UniversalIndicator solution to small
wells C-1throughC-12and large well A-I.
Whatwould you expect the pH of rain to be? Are your
results different than whatyouexpected?
indicator to eachof the
5) Pipetteonedropof phenolphthalein
small wells D-1throughD-12andto large well B-I.
TERMSTO KNOW
with scissors or wire cutter. Cut the piece about1 inch
long. Placethis wire into the other ~argewe~whereyou
haveaddedthe coppersulfate solution.
Calciumhydroxidesolution (from your chemistryset)
Aluminumammonium
sulfate solution
(from yourchemistryset)
Magnesium
sulfate solution (from your chemistryset)
UniversalIndicatorsolution (as an indicator)
Phenolphthalein
solution (as an indicator)
Goggles
1) Obtaina sampleof rain waterin a plastic cup.
with scissors or wire cutter. Cut the piece about1 inch
long. Placethis wire into oneof the large wells whereyou
haveaddedthe coppersulfate solution.
3) Cut a pieceof copperwire (providedin your chemistryset)
[]
_BESURE_TO
WEAR
GOGGLES
..W_HE~..N_.DOING
EXPERIMENTS
IN TH_IS.CHEMISTRY
SET!
THE GASEOUS
PHASE OF MATTER
CATALYST
- A chemical which either speedsup or slows down
a reactionwithoutbeingusedupin the reaction.
DECOMPOSE
- Break up into parts.
INVERSELY
RELATED
- If one variable goes up in value,
anothergoesdown.Inversesare opposites.
PRECIPITATE
- A solid whichdoesnot dissolve in a solution.
5) Allowthe wire to remainin the wells for at least ten minutes. Observeany changein the wells. Which well
changes?Whydoes the other well NOTchange?Leave
the wire in solution for 3-4 hours. Whatchangesdo you
notice?
PhysicalPropertiesof Gases
Anexample
of this chemistryfact canbequite startling!
Whathappenedto the zinc wire? Whathappenedto the cop3er solution?Compare
the experimental
solution to the control
~nlI~tinn
Gasesrespondto changesin the temperatureand the pressure
which surroundthem. A gas changesits volumewhenthe temperature and/or the pressureon the gas changes.When
scientists talk aboutgases,they are alwayscareful to note the
temperatureand the pressuresurroundingthe gas.
SECTION1 - THE..EFFECTOF PRESSURE
ON
THE VOLUME__OF
A GAS
Did youever try to squeeze
a balloon without bursting it? Did
youwonderwhatwashappening
to the air inside the balloonas
you squeezed?
Scientists have very carefully measured
this
experimentwith all types of gasesand havefoundinteresting
things which happen to gases (like air) whenthey are
"squeezed"or put under pressure. Squeezedand expanded
gasesin the cylinder
Figure #23
Page 19
Extend the spaceson your RECORD
CHART
#8 to include
the rainwater sampleyou tested. Color in any changes
noticed.
SECTION7 - TESTINGTHE pH OF OTHERCHEMICALS
Nowthat you know that an INDICATOR
such as Universal
Indicator Solution or Phenolphthalein
Solution maybe usedto
tell thechemist
if a solutionis anacidor base,it is timeto determinethe acidity and basicity of the other chemicalsin your
chemistryset.
6) Observeany color changein all of the wells tested. (A
piece of white paperunderyour microplatemayhelp show
the colors.)
7) Usingyour coloredpencil set, record anycolor changeon
RECORD
CHART#9.
8) Someof your chemical solutions will showno change.
Some
will be acids. Some
will be bases.Witha black pen,
put an "A" by the oneswhichshowan acid color present.
Put a "B" by the oneswhichshowa basepresent. Put an
"N" (neutral) by the oneswhichappearto haveno change.
SOLUTIONS TESTED
LIST OF MATERIALS
[~ Microplate of indicators from SECTION
1 (with indicator
colors in small well rowsA andB)
[]
Plastic pipette
[]
Water
Coloredpencil set
Calciumnitrate solution (from yourchemistryset)
Ferroussulfate solution (fromyour chemistryset)
[]
Cobaltchloridesolution (fromyour chemistryset)
[]
Ammonium
chloride solution (from your chemistryset)
Potassium
iodide solution (from your chemistryset)
Sodium
sulfate solution (from yourchemistryset)
[]
Coppersulfate solution (from your chemistryset)
Sodiumcarbonatesolution (from your chemistryset)
[]
Citric acid solution(fromyourchemistryset)
[]
Sodium
silicate solution (fromyour chemistryset)
UNIVERSAL
INDICATOR
SOLUTION
TEST
MAGNESIUM
SULFATE
SOLUTION
ALUMINUM
AMMONIUM
SULFATE
SOLUTION
CALCIUM
HYDROXIDE
SOLUTION
SODIUM
SILICATE
SOLUTION
CITRICACIDSOLUTION
SODIUM
CARBONATE
SOLUTION
COPPER
SULFATE
SOLUTION
: SODIUM
SULFATE
~OLUTION
POTASSIUM
IODIDESOLUTION
~ ~-HI~ORIDE SOLI.)TION
COBALT
CHLORIDE
sOLUTION
-~RROUS
SULFATE
SOLUTION
CALCIUM
NITRATE
SOLUTI[~RECORDCHART#9
Page 36
PHENOLPHTHALEIN
INDICATOR
SOLUTION
TEST
1) Placea small sampleof eachof the liquids mentionedin
Put the correct name
at the endof the rowyou are recording as to whatindicator youusedandthe colors indicated.
the materials list
microplate.
Note: Youmayhaveto repeatedly clean out the wells in
rowsC andD and re-usethemafter eachrecordingandexperimentwith different indicators. Try to find as many
colored"natural indicators" possible.Alwaysrecordthe color
changes on RECORD
CHART#7.
separately in large wells of your
2) Addsomewater to eachlarge well containing your samples.
3) Adda fewdropsof UniversalIndicator to eachof the large
wells containingsamples.
SECTION4 - OTHERNATURALINDICATORS
the colors of the wells with samples
to the control
4) Compare
wells with UniversalIndicator youpreparedin SECTION
1.
Record the sululions yuu test un RECORD
CHA_RT
#8.
Useyour coloredpencils to showchanges.
Repeatthe procedurein SECTION
3 until youhavetested all of
yournatural indicators.
Whatcanyoutell aboutall the indicators?
Whichproductsare acids? Which are bases? Wereany
of the materials ,ou testedneutral?
Whatis similar or different abouteachof the indicators?
SOLUTIONS
TESTED
BE SURETO RECORD,
on RECORD
CHART#7
with your coloredpencils, all of the color changes
observed
fromthe testing
of yournaturalindicators.
COLORAFTER
UNIVERSAL
INDICATOR
AODED
Shampoo
Dishwashing
detergent
Laundry
detergent
Pet Shampoo
Vinegar
Clear Soda
Toothpaste
Milk
Lemon
juic~
Grapefruitjui¢~
Rain water
SECTION5 - TESTINGFORA(,31D$ ANDBASES
Nowby using the tests and the color changeswhichyou recorded in previousexperimentswhichtold you the color changesoccurring at specific acid or baseconcentrations,youcannowtest
for the acid and basechangesand concentrationswith someunknownsolutions. Againcompareany color changeswith whatyou
alreadyrecordedfrom previousexperimentsand color changes.
this experiment:
LIST OF MATERIALS
Microplateof indicators from SECTION
1 (small rowsA & B)
Household
soapsolution (example:Dial® liquid soapor
dishwashing
liquid soap)
Shampoo
solutions
Liquid laundrydetergent
Pet shampoo
Vinegar
Clearsoda(sparkling water)
Toothpaste
Milk
Lemonjuice
Grapefruitjuice
UniversalIndicator solution
Plastic pipettes
Coloredpencil set
Goggles
COLORBEFORE
UNIVERSAL
INDICATOR
ADDED
of an automobile engine is what makesthe engine run.
Scientistswhofill up large heliumweatherballoonsdo NOT
fill
themup all the waybecausethe heliumexpandsas the balloon
goeshigherandhigher. If the balloonswerefilled full at ground
level, it wouldburst at higheraltitudes wherethe atmospheric
pressureis less and the helium gas volumebecomes
so much
greater.
3) Graspthe pipette stemin onehandand the end of the
pipettestemin the other. Pull until the pipettetubestretches verythin. Tie a knotin the stretchedpart of the pipette
tube. SeeFigure #25.
bookor heavy
weight
knot In pipelts~
Thefollowingexperiment
lets youtest for the effect of pressure
onthe volumeof a gas. Theblue solution is usedin this experimentso that youcan"see"the changein the volumeof the gas
you are testing. Whenyou add weight (books) on top of the
bulb, youare exertingforce (pressure)on the gasto "reduce"its
volume..,just like squeezing
a balloon.
"stretch~
pipette
Gasesexpandand contract with changesin the pressure of
their surroundings.Gasesexpandwhenthe pressuredecreases. Theycontract whenthe pressuresurroundingthemincreases. Gasvolumeand pressure are INVERSELY
related.
Figure #25
4) Accuratelymeasure
the length of the trappedair columnin
the stemof the pipette usingyour metric ruler. SeeFigure
#25.
LIST OF MATERIALS
Metricruler
[-I A newplastic pipette
5)
Placea bookon top of the bulbof the pipette.
6)
Measure
the length of trappedair in the columnwith the
bookin place. Whathappened
to the length of the column?
Methylene
blue solution (from your chemistryset)
Plastic measuring
cup
.1 Water
7) Continueto stack bookson top of the bulb of the pipette.
Several heavybooks
[J Goggles
8) Whatstatement can you makeabout the way pressure
Measure
the length of the columnafter eachbookhasbeen
added.
effects the volumeof a gas?
WHENDOING
EXPERIMENTS.
IN THIS CHEMISTRY
SET!
RECORDCHART
SECTION6 - TESTINGRAIN WATERFORpH VALUE
Rainwateris not purewater.As rain falls fromthe sky, it picks
up particles and chemicals. Theparticles maybe pieces of
dust, dirt or smoke.Thechemicalsmaybe gaseswhich have
beenreleasedfroma factory or home.In any case, rain water
mayabsorbthis material andchangethe pHof rain water.
SECTION2 - THE EFFECTOF TEMPERATURE
ON A VOLUMEOF GAS
Temperature
also will "changethe volumeof a gas." This is
why,for instance,the tires ona carneedto beinflatedwith a little moreair than normalin very cold weather, and whyyou
shouldlet a little air out of the tires in veryhot weather
or ona
long trip on hot highwaysurfaces.
t) Place2 dropsof methylene
blue dyein a smallplastic cup.
Fill the cupabout1/2 full with water.
2) Fill ONLY
the bulb of a plastic pipette with methylene
blue
In this experiment
wewill cool a gas(air) andwatchas the volumeof a gas changes(is reduced). Againweuse the methyleneblue dyesolution just to be able to "see"the gasvolume
as
it changes.
solution. SeeFigure #24. After it is filled, DONOT
SQUEEZE
the bulb, but hold the pipette tube and bulb as
shownin Figure #24.
EXPERIMENTS
IN THIS CHEMISTRY
SET!
As stated above,manyof the productswhichare in your home
are acidsandbases.Youcantest home
products
for acid, base
or neutral pHin the followingway.
LIST OF MATERIALS
I_,1 Microplateof indicators from SECTION
1
F~ Rain water
I~1 Plastic cup
~
Plastic pipette
i~
[~
Goggles
Page 35
metric
ruler
LIST OF MATERIALS
Methylene
blue dyesolution (from your chemistryset)
A newplastic pipette
Crushedice
Microplate
Goggles
EXPERIMENTS
IN THIS CHEMISTRY
SET!
Figure #24
I’age 20
Gasesexpandand contract with changesin temperature. The
expansionor contraction of a gas varies DIRECTLY
with the
temperatureof a gas.
1)
LIST OF MATERIALS
Microplate
[]
Vinegar(from kitchen or grocerystore)
[]
Household
Ammonia
(from kitchen or grocerystore)
Id
UniversalIndicator Solution(from yourchemistryset)
[]
Plastic pipette
Plastic sandwichbag
Water
--I Goggles
Start with a newpipette.
2) Fill a large well of the microplatewith water. Adda few
dropsof methylene
blue dye solution. Thedye will allow
youto observe
the level of waterin the stemof the pipette.
3)
Placethe bulbof the plastic pipettein a plastic cup.
4) Direct the stemof the pipette into the waterin the well of
the microplate. Hold the stem of the pipette belowthe
water line by using sometape to securethe stemto the
plate. SeeFigure #26.
EXPERIMENTS
IN THIS CHEMISTRY
SET!
cru.shsd
~
_
tapestem
into deep
well
1)
Selectonerowof small wells in your microplate.
2)
Place10 drops of water in eachwell in the row, EXCEPT
for the first andlast well in therow.
3)
4)
Figure #26
5) Placean ice cubeor somecrushedice into a plastic cup
withthe pipette.
to the water/methylene
blue solution level in
6) Whathappens
the stem?As the temperatureof the air in the bulb decreased,what happened
to the volumeof the air? Howdo
you know?
Addonedropof UniversalIndicator to eachwell containing
waterin the row.
Place10 dropsof vinegarin oneof the emptywells.
5)
Place10 dropsof ammonia
in the other emptywell.
6)
QUICKLY
place the microplatein a plastic sandwichbag.
7)
Whathappensto the Universal Indicator? A changein
color is dueto the diffusion of vinegarandammonia.
A blue
color indicates ammonia;
a red color indicate vinegar.
8)
the pipette fromcontactwith the ice. Allowthe air
7) Remove
in the pipette to cometo roomtemperature.Whathappens
to volumeof air as the bulb warms?
8) Whenthe trappedair has returned to roomtemperature.
pour somewarmwaterinto the plastic cup.
9) Placethe bulb of the plastic pipette in contact with the
warmwater, by pouring warmwater into the plastic measuring cup.
SE~C.TtO_N_
3_.A.......:...G.A.,~...I~.!_EE~__S_.!ON
II
SECTION3 - GASDIFFUSION
Of all states of matter,gaseshavethe greatestability to move
from place to place and the greatest freedomof movement.
Theability of gasesto movethroughother gasesis called DIFFUSION.
Thelighter the gas (the smaller the molecule), the
faster its molecules
can move.
Youcan savethe UniversalIndicator and phenolphthaleinfor
use as CONTROLS
for experimentsyou will do later. Seal the
indicators in their wells by coveringthe wells with a pieceof
transparenttape. Covereachrow of wells with a long, single
piece of tape. Runyour finger over eachwell to seal the contents in thewell.
~ water and oxygen
1
Placea 5-6 gramsampleof the plant or flower into a test
tube.
2) Add1/2 pipette of ethyl or isopropyl alcohol. Mix well.
SECTION2 - NATURALINDICATORS
3) Allowthe plantmaterialto stay in the alcoholfor at least 5
Oneof the mostfascinatingdiscoveriesis that manyplants also
havenatural "indicators" included in the flowers, leavesor
stemsof the plant. Wecanusetheseas indicators for our acid
and base changeexperiments.
minutes.
4) Pouroff the liquid into a largewell of the microplate.
5) Savethis liquid as your"naturalindicatorsolution"in further
experiments.If youwish, youmayalso savethe indicator
in sameplastic pipette whichyouusedfor extracting or
drawingup the indicator solution out of the test tube. Be
sureto label yourplastic pipette, whichindicatorit holds.
SECTION3 - NATURALINDICATORS
LIST OF MATERIALS
~ Flowerpetals (obtain from plant flowers with colored
petals)
--I Plant fruit skin (example:cherries,blueberries,etc.)
[]
[]
[]
hydrogenperoxide
DO NOTMIX SKINS OR FLOWERS!
BE SURETO EXTRACTEACHPLANTOR
FLOWER
INDIVIDUALLY
Crushthe petals with a plastic sodastrawto squeeze
alcohol throughoutthe sample.
SECTION4 - PREPARATION
OF OXYGEN
(steel wool)
TO EXTRACTTHE INDICATOR, FOLLOWTHESEDIRECTIONS:
Besure to usea microtip pipette for this experiment.
DO NOTDISCARDYOURINDICATORS!!
[]
[]
Thesteel woolis the catalystfor the reaction.It is writtenabove
the arrowfor the equation.
Page21
12) OnRECORD
CHART
#7, using your colored pencils, fill in
the colors which the phenolphthaleinIndicator Solution
changedto in eachof the small wells B-2 throughB-11.
Markthis row on your RECORD
CHART
#7 (B-2 through B10) Phenolphthalein
Indicator Row.
Repeatthe previous SECTION
3 in exactly the sameway, but
this time insteadof usingvinegar(acetic acid) try usinglemon
juice(citric acid).
Theextra oxygenin peroxidecanbe freed by the reaction of
hydrogenperoxide with a CATALYST.
Thereaction looks like
this:
Almostall plant colors (pigments)are indicators. Usethe skin,
rind, or petal of a plant. Theindicatorwill be in the coloredor
tinted part of the plant. Greenleaves contain CHLOROPHYLL.
Chlorophyllis not an indicator. Thepetals of flowers,evenwhite
flowers, contain indicators. Thefollowing is a list of plant
sourcesof indicators. Redcabbage,
cherryskins, tea, blueberry skins, blackberryskins or flower petals are goodsourcesof
naturalindicators.
Compare
the results of your experiments.Howis phenolphthaleindifferent fromUniversalIndicator?
Whichdiffused faster? Whichis lighter?
Hydrogenperoxide (H202) is a common
householdantiseptic
which can be found as a 3%solution in manydrug or grocery
stores. Hydrogenperoxide can be DECOMPOSED
into water
the oxygen. The compound
has a formula similar to water
(H20).
10) Whathappened
to the level of water in the stem of the
pipette as the bulb of air is warmed?
Whathappensto a
gasif the temperature
of the gasincreases?
11) Addonedropof phenolphthalein
solution (anotherindicator) to eachof thewellsin this row.
[]
Redcabbage
leaves(obtain from your grocery)
Largetest tube with cap
Household
tea (from tea bag)
Isopropylalcohol (rubbingalcohol)(obtain fromdrugstore
or grocery)
Microplate
Household
vinegar(acetic acid)
Householdammonia(ammonium
hydroxide)
Plastic pipette
Plastic sodastraw
Scissors
Goggles
LIST OF MATERIALS
II Flowerpetals, plant skin, or red cabbage
extraction
(from previousexperiment)
Largetest tube
Isopropylalcohol(rubbingalcohol)
[]
Microplate
[,J Household
vinegar(acetic acid)
[]
Householdammonia(ammonium
hydroxide)
/
Plasticpipette
Coloredpencils
[]
Water
[]
Goggles
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
WARNING:
Ethyl or isopropylalcohol andtheir vaporsare highly flammable.Donot use alcohol in the presenceof an open
flame. Usealcohol in an areawith goodventilation.
1) RepeatSECTION
1 Steps1-9 in anotherrow of small wells
Some
naturally occurring chemicalsare indicators. Theymust
be separatedfrom natural sourcesin order to see themwork.
Wewill EXTRACT
the natural indicators with ethyl alcohol or
with isopropylalcohol(rubbingalcohol).
(RowsC and D).
2) Add6-8 dropsof your indicator to eachof the wells in the
row.
CHART
#7 by col3) Record the color changeon RECORD
oring in the correct well circles with yourcoloredpencils.
Page 34
1) Place 9 drops of water in each of the small wells A-3 and
A-10in the microplate.
2) Place 10 drops of vinegar (acetic acid) in well A-2.
3) Takeone drop out from small well A-2 and drop it into the
water in small well A-3.
You have just madethe acid in small well A-3 ten times
LESSTHANthe acid solution in small well A-2. Why?See
Figure #34.
4) lake onedrop out ot small well A-3 andm~x~t w~ththe water
in small well A-4.
5) Repeat the above process with well 5 and 6. DONOTADD
ANYTHING TO WELL 7. Why?
(Hint: small well A-7 will be used as neutral or just plain
water which is neutral pH.)
You have just madethe base in small well A-10 ten times
LESSTHAN(weaker than) the basic solution in small well
A-11. Why?
Why?
highest Ammonia
(Base
I concentration
-’=~
, , , , , , ,o-,.,, ,, r
¯
c~O00000000
o~O00000000
¯
0
0
0
0
RECORDCHART #7
In this experimentyou will see howto dilute an acid, moreand
more, and to showhow the dilution can be seen by the use of
an "indicator." The indicator usedin this experimentis Phenolphthalein which will changecolor in a basic solution and NOTin
an acid solution. Youwill needthe color changeinformation to
comparewith acid and base experiments later.
1) Place 9 drops of water in small wells B-3 and B-10 in the
microplate.
2) Place 10 drops of vinegar (acetic acid) in small well B-2.
11) Addone drop of Universal Indicator to all the wells. What
happensin each of the wells?
~0~~000~
°000
08888
~J
I1
Microplate
[,_]
~1
Water
2)
4) Take one drop out of small well B-3 and mix it with the
water in small well B-4.
5) Repeat the above process with small wells B-5 and Be6.
DO NOT DO ANYTHING TO WELL 7. Why?
0
0
6) Place 10 drops of household ammonia(ammoniumhydroxide) in small well B-11.
Plastic pipette
LIST OF MATERIALS
[]
A newplastic pipette
Goggles
[_.1 Methyleneblue solution
B_.E..SU__R_E
TO.W___E_A__R_...G.QGG.LE__S____W_HEN___POJ.NPa
._E__X_
..P.E_
RI ME_N~F
.S...
!..N_
...T_I~
I $,C_H__E_._M__!
_S.
_T..
_R_
_y
._~_.E
T!
:J
Microplate
II
Water
Cut the round end of a pipette off with scissors. (If you
"~
Goggles
have already madea filer funnel out of a pipette, you may
BE SUR_E_TO WEARG,OGGLESWHEN_D_.QIN~
use that.)
.I~X..I~E!~IMENT~
IN. THIS_..CHEMI
_S.T__R_Y.
SET.!.
Packsteel wool into the bulb of the pipette so that it will not
fall out the openend you just cut. Makesure the steel wool
1) Place 1/2 pipette of water in a large well in the microplate.
is close to the cut end but not sticking OUTof the openend
you have cut.
2) Addone drop of methyleneblue to the water in the well.
With anotherpipette, addonepipette full of water to a large
well of your microplate. Add1 drop of methyleneblue solution to the waterin this large well.
4)
Rinse out the pipette you have used with the water and the
methyleneblue solution.
5)
Nowplace 1/2 pipette full
into anotherlarge well.
6)
water in small well B-3. You have just madethe acid in
small well B-3 ten times LESSTHANsmall well B-2 by a
factor of 10. Why?See Figure #34.
0
"’000000
-~OOOOOO,
You probably have already heard that air contains oxygen.
Oxygenis a gas which we breathe and which sustains life. How
can we measurewhether air actually does contain oxygen?By
using methylene blue dye solution, we can measurefor the
presence of oxygen. Methylene blue dye solution will change
color if it is in contact with oxygen. Wecan use this changeof
color to test for the presenceof oxygen.
3)
EXPERIMENTSIN THIS CHEMISTRYSETI
9) Takeonedrop out of small well A-9 andmix it with the water
in small well A-8.
SECTION 5 - DOES AIR CONTAIN OXYGEN?
LIST OF MATERIALS
IJ
Fine steel wool (obtain from hardwarestore or grocery)
DONOTuse the steel wool with soap embedded
in it!
~
Hydrogen peroxide (3%) (obtain from drugstore or
cery)
Ij
Methyleneblue solution
Usea microtip pipette for these experiments.
8) Takeone drop out of small well A-IO and mix it with the
water in small well A-9.
HEU
.-rI:L&L
000000000
000000000
0000000©0
000000000
000000000
0
0000
QO0000000
000000000
1)
7) Takeone drop out of small well A-11 andadd it to the water
in small well A-10.
highest
Acetic
/v:~dconcentration
UNIVERSAL
INDICATOR
ROW
PHENOPHTHALEIN
INDICATOR
ROW
NATURAl
INDICATOR
ROW
NATURAL,
INDICATOR
ROW
NATURAL
INDIGATOR
ROW
NATURAL
INDICATOR
ROW
NATURAL
INDICATOR
ROW
NATURAL
INDICATOR
ROW
NATURAL
INDICATOR
ROW
$.EC_T.!_ON
1A - DILUT.I,O_N_,O_E_A.CJD
6) Place 10 drops of household ammonia(ammoniumhydroxide) in small well A-11.
10) DO NOT ADD ANYTHING TO SMALL WELL A-7.
~ we~Uw~i weUw~ weUwell we~wr.U
2 3 4 $ 6 ? 8 9 10
7)
8)
Direct the stem of a plastic pipette into the methyleneblue
solution.
4)
Squeeze
the air out of the plastic pipette into the watercontaining the methyleneblue solution.
5)
Withdrawthe tube from the methyleneblue solution.
6)
Allow the bulb to expandandfill
7)
Repeatthe bubbling of air into the well as often as necessary until a color changeis noted. Be sure to removethe
tube from the well before allowing the bulb to return to the
full position.
of hydrogenperoxide solution
3)
Takethe cut pipette with the steel wool and place the cut
end into the well containing the hydrogen peroxide. Hold
the pipette with the steel wool downward
all the wayto the
bottom of the well of hydrogenperoxide. Hold the cut end
of the pipette tightly against the bottomof the well containing hydrogenperoxide.
Oxygengas will now be producedby the action of the catalyst (steel wool) and the hydrogen peroxide. The oxygen
gas will go up the tube of the pipette.
Direct the stemof the pipette into the methyleneblue solution. See Figure #27.
pipette with steel
wool and peroxide
/ in large well
water in small well B-10. You have just madethe base in
small well B-10, ten times LESSTHANsmall well B-11.
Why?
10) DO NOT ADD ANYTHING TO SMALL WELL B-7.
Page 33
Why?
hh ~p ~ml, lfi~n9
Oxygenis produced all the time by natural processes. The
enzymesin the cells in liver will causeoxygento be produced.
Natural enzymesin raw potato will cause oxygen to be produced. In this experiment see if you can use the enzymesto
release the oxygenfrom the hydrogen peroxide.
LIST OF MATERIALS
I-I Hydrogen peroxide (3%) (obtain from drugstore or
h~t_n,_ngn £ tm thn rnr~th~,~l#n~
S~E_.C_.~E!.ON
.. 6 - NATURAL
OXYGEN
PRODUCTI,ON:
.T__H_.E ACTI,ONOF ENZYMES
Figure #34
12) On RECORD
CHART
#7, using your colored pencils, fill in
the colors whichthe Universal Indicator solution changedto
in each of the small wells A-2 through A-11. Markthis row
(A-2 through A-10) the UniversalIndicator
~^lh~t
with air.
cery)
Rawliver or raw potato (obtain from your kitchen)
’1 Microplate
methylene blue solution
9)
Figure #27
Observethe color of the methylene blue solution as the
hydrogen peroxide decomposes. What happens? What
gas is formed?
Plastic pipette
Page 22
[]
Water
[]
Goggles
3) Cut a small sample(about 1 g) of plant leaf into small
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
1)
2)
Placea smallpieceof rawliver or crushed
potatoin a large
well in the microplate.
4) Usinga chemicalscoop,transfer the cut leaf to oneof the
wells in the microplatecontainingthe methylene
blue solution.
Adda pipette full of hydrogen
peroxideto the liver or potato.
3) Whatgas is produced?Howcould you identify this gas?
SECTION7 - METHYLENE
BLUEAS AN.!NDICATOR
5)
Placethe plate in the sunlightor undera light for a fewminutes.
6)
What happens?
SECTION9 - TESTINGA GASFORCARBON
DIOXID~E
Using the materials listed above,andmethyleneblue, repeat
the experiment.
BE SURETOWEAR
GOGGLES
WHEN.
_D..E)J_N..G
EXPERIMENTS
IN THIS CHEMISTRY
SET!
A test for the presence
of carbondioxide in a gasis to bubble
the gas into a saturated solution of calcium hydroxide.
(Saturated calciumhydroxidesolution is also knownas lime
water.)
1)
Adda pipette of hydrogen
peroxideto two other large wells
in the microplate.
2)
Adda few dropsof methylene
blue to the hydrogenperoxide in bothwells.
3)
Placea smallpieceof liver or crushedpotatoin ONE
of the
wells.
LIST OF MATERIALS
[]
~1 Scissors
.7-1 Microplate
I~
Plasticpipette
[]
Goggles
SECTION8 - PLANTSAND OXYGEN
EXPERIMENTS
IN THIS CHEMISTI~YSET!
Plantsnaturally produceoxygen
whenthey are exposed
to light.
Plants take carbondioxide from the atmosphere
and produce
oxygen. The next time you have FRESH
spinach or a FRESH
leafy greenvegetablefor dinner, savea few leavesof the vegetable for this experiment.Youcanusea plant leaf or a blade
of grassinsteadof fresh spinach.
NOTE:
To obtainlime water(saturatedcalciumhydroxidesolution)
you mayhaveto see your pharmacistat your local drugstore, or use the calciumhydroxide solution from your
chemistryset.
1) Cut a plastic pipette as shownin Figure#28. Usethe cutoff stemas the blowstraw. Savethe bulbportion for another experiment.
LIST OF MATERIALS
[]
Source
of sunlightor bright light
Scissors
[]
Microplate
[]
Plasticpipette
[]
Plastic measuring
cup
Grassor plant leaf
[]
Methylene
blue solution
[]
Goggles
SAVE THIS STEMFORUSE IN OTHEREXPERIMENTS
savethisend
Figure #28
2) Fill anotherpipette with calciumhydroxidesolution (lime
water).
CUTTING LEAVESSHOULDBE DONEWITH
YOURPARENTS’ASSISTANCE
1)
3) Place1/2 the calciumhydroxidesolution in onelarge well
of the microplate.Placethe other1/2 of the solution in an
adjoiningwell.
Place 1/2 pipette of water into two large wells in the
microplate.
4)
2) Addonedropof methyleneblue to eachof the wells containing the water.
Page 23
Acid and Base Solutions
Placethe large endof the plastic straw into your mouth.
Direct a streamof breathgently into the solution.
Almost ALLsolutions are either ACIDICor ALKALINE.
Very
few solutionsare NEUTRAL.
Acidsandbasesare two types of chemicalswhich youhave
contactwith every day. Common
acids can be foundin many
man-made
and natural products. Acidswhichyoumayhave
seenincludeascorbic
acid(vitaminC), aceticacid(vinegar),
autobatteryacid(sulfuricacid),tea (tannicacid), andsour
andyogurt
(lactic acid).
Scientistsmeasure
theamount
of acidity or alkalinity by usinga
specialscale called the pHSCALE.
ThepHscale rates solutions from 1 to 14 basedon the amount
of H+ or OHion in the
solution.Asolutionwhich
hasa rating of between
1 to 6 is consideredACIDIC
(1 is the highestamount
of acid, 6 is the least).
A solution whichis rated 8 to 14 is ALKALINE
or BASIC
(a solution whichhas a 14 pHhas the highest amount
of base,while 8
is the least basic). A solution whichis exactly 7 is NEUTRAL.
Basesare also quite common.
Milk of magnesia
(magnesium
hydroxide), lye (sodium hydroxide) andhousehold
ammonia
(ammonium
hydroxide) are somecommon
bases.
The chart below mayhelp you to understandthis important
scale.
ACIDS AND BASESARE WATERSOLUTIONS.
TERMS TO KNOW
pH(1 - 2 . 3- 4 . 5 - 6) 7 (8.9.10 -11 -12 .13 .14)
<
-,
STRONGER
STRONGER
ACID
BASE
n
ACID- A chemicalwhichionizes in water to formH+ ions.
ACIDIC
- A solution whichhasa pHless than 7.
STRONGEST WEAKESTU
ACID
AC/D t
ALKALINE
- A solution whichhas a pHgreater than 7.
BASE
- A chemicalthat ionizes in waterto form OH-ions.
r
EXTRACT
- To use a solvent to isolate an individual chemical
from a source.
I
WEAKEST
STRONGEST
BASE
BASE
SECTION1 - THE pH SCALEANDINDICATORS
INDICATOR
- A chemicalwhichturns color at a particular pH.
ION- A chargedatomor groupof atoms.
IONIZATION
- Thebreakingapart of a moleculeinto parts which
havea positive (+) or negative(-) charge.
NEUTRAL
- Neither acid nor base.
pHSCALE
- A scale whichtells the relative amountof acid or
basein a solution.
SALT
- Thechemicalwhich results whenan acid reacts with a
base.
cut here
usethis end
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
When
calciumoxide,unslaked
lime, (CaO)is addedto water
form slaked lime, the amountof OH" increases while the
amount
of H+decreases.This solution is said to be BASIC
or
ALKALINE.
ACID AND BASE
SOLUTIONS
pieces with scissors. Usea plastic cup to collect the
pieces.
Water(H20)contains
twodifferent chemicalparts. Theseparts
are called IONS.Thehydrogenion (H+) whichhas a positive
charge and the hydroxide ion (OH) which has a negative
charge.Acids add extra H+ ions to water, basesadd extra OHionsto water.
LIST OF MATERIALS
[] Household
vinegar(acetic acid) obtain from kitchen
grocery
Householdammonia
(ammonium
hydroxide solution)
obtain fromkitchen or grocery
Microplate
[]
Plastic pipette
[]
Water
[]
UniversalIndicator solution (fromyour chemistryset)
Phenolphthalein
solution (from your chemistry
set)
[]
[]
Transparenttape
[]
Set of coloredpencils
Goggles
In pure water the amountof H+ ion exactly equalsthe amount
of OH"ion.
WH__ENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
Whenany chemical is addedto water the balanceof H+ and
OHin the solution changes.For example,whensulfuric acid is
addedto waterto makea solution for a car battery, the amount
of H+ increaseswhile the amountof OH"decreases.
This experiment
will showyouthe characteristicsof both the pH
scale and the wayINDICATORS
work.
This solution is said to be ACIDIC.
Page 32
Usea microtip pipette for theseexperiments.
7)
Is there any difference betweenthe products and the reactants which formed them? Whatdo you think happenedto
give the results you have noticed?
8)
Which combination of chemicals produced a reaction?
Which chemical product is a PRECIPITATE?
Which chemical productis a gas?
5)
LIST OF MATERIALS
Microplate with the solutions from SECTION
4
(wells A, B, C, D- 8-12)
I-I Electrolyte Detector
calcium hydroxide + carbon dioxide .... ~ calcium carbonate
+ water
Plastic pipettes
Goggles
SECTION 6 - TESTING THE REMAINING SOLUTION
OFA CHEMICAL REACTION
7) Direct the stem of the pipette into the calcium hydroxide
solution.
Thereactionfor this precipitation is:
6)
Water
draw up somevinegar into the pipette with the
6) QUICKLY
sodiumbicarbonate.
Watchthe solution carefully. A PRECIPITATE
should form.
A precipitate is a solid which is formed whena reaction
occurs in solution. A precipitate formedin this experiment
is an indication that carbon dioxide is in your exhaled
breath. Howcould you tell if air has carbon dioxide?
CaCO3 + H20
Ca(OH)2 +
2 CO
BE SURE TO WE__ARGOGGLESWHENDOING
EXPERIMENTSIN. THIS CHEMISTRYSET!
Just as you tested the precipitates (the wet and dry products of
a chemical reaction), you nowneedto test the solutions which
were formedin the chemical reactions. Manyof these solutions
carry dissolved in themthe salts from a chemicalreaction. Your
electrolyte detector will showthe ones whichconduct electrical
current, in other words, the solutions whichhavedissolved salts
and which are ELECTROLYTES!
Test the solutions saved from SECTION
5 in the small wells A,
B, C, D - 8 - 12, for conductivity using the ELECTROLYTE
DETECTOR.
Prepare another table like Table #6 and record which solutions
conduct electricity
(these are ELECTROLYTES).
SECTION 10 - PREPARATIONOF CARBONDIOXIDE
Carbon dioxide gas is produced when compoundscontaining
carbonate react with acids. Carbondioxide is also producedby
living things.
NATE
I ~~ Lu..M_ E! ’..C..A_~_~P_
~ .....
Figure #30
LIST OF MATERIALS
Calciumhydroxide solution (lime water)
8) Standthe plastic pipette combinationin the microplate next
to the well containing the calciumhydroxidesolution, allowing the pipette end to bubble CO2 gas into the calcium
hydroxidesolution.
Scissors
SampleElectrolyte Table
Column 1
Column 2
Column 3
Column 4
[]
Column 5
Column 6
Microplate
Plastic pipette
9) Whatcompoundis generated by this reaction?
[]
Cellophane tape
[]
--I
Sodiumbicarbonate (baking soda from your kitchen)
[]
ROW1
calcium hydroxide + carbon dioxide -
) ???? + H20
Vinegar (from your kitchen)
10) Whathappensto the calcium hydroxide solution when the
gas generated bubbles through the solution?
Goggles
EXPERIMENTS.
IN _T_HIS CHEMISTRY
SET!
ROW 2
~I~!D. VINEGAR
I~ HYDROXIDE
1)
Cut a plastic pipette with scissors as indicated in Figure
#29.
2)
Place a 1/4 scoop of sodium bicarbonate in the pipette
through the slit you havejust formed.
3)
Coverthe slit
tape.
11) Wherehave you seen this reaction of calcium hydroxide
before?
SECTION
11 - A REACTION
WH!.C_HPR_O__D.IJC..E_S
CARBON__DIOXIDE
with a piece of transparent tape or electrical
SAVE THIS PIPETTE FOR USE IN OTHER EXPERIMENTS
pipette
LIST OF MATERIALS
[J
Baking soda solution (Sodiumbicarbonate solution)
[1
Plastic pipette
ROW 3
Microplate
[]
Plastic pipette
Citric acid solution
scissorcut
Water
clear tape
Goggles
Figure #29
ROW 4
Page 31
4)
With anotherpipette, fill a large well of the microplate with
calcium hydroxide solution.
5)
With another clean pipette, fill
gar.
BE SURE 3"_0 WEARGOGGLESWHENDOING
an adjoining well with vinePage 24
Makeyour ownsodiumbicarbonate(baking soda) solution
placing 1/4 scoopof bakingsoda(obtain from your kitchen or
grocery) in your plastic measuring
cupandaddinga pipette of
water.Stir this mixtureuntil all bakingsodahasdissolved.
LIST OF MATERIALS
Ammonium
chloride solution (from your chemistryset)
Microplate
Plasticpipette
Filter paper
Q Goggles
1)
Place20 dropsof sodiumbicarbonatesolution in a large
well of the microplate.
2)
Add1/2 pipette of waterto the well.
3)
Add1/2 pipetteof citric acidto thewell.
4)
Watchwhathappensas acid is addedto the sodiumbicarbonate.
5)
Howcouldyoutell that the gasproduced
is carbondioxide?
BE SURETO WE&._RGOGGLES
WHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
SECTION
12.- PBO_DU.C_.!NG
CARBON
DIOXIDE
IN ANOTHERWAY
1)
Place1/2 of a pipette of ammonium
chloride solution into a
well of yourmicroplate.
2)
Moistena small(1 inch x 1 inch) pieceof filter paperwith
UniversalIndicatorsolution.
3)
Add1/2 plastic pipette of calciumhydroxidesolution to the
well containing ammonium
chloride.
4)
Holdthe moistened
filter paperover the well containingthe
mixture of ammonium
chloride and calciumhydroxide.
5)
Whatis the result? Whatgas causedthe color change,if
any?
LIST OF MATERIALS
@
-3
Alka Seltzer
-1
Scissors
Microplate
Plasticpipette
Cellophanetape
Vinegar
Goggles
A color changewith UniversalIndicator indicatesthe presence of ammoniavapor. Remember
that ammoniais a
base!
WHENDOING
EXPERIMI~NTS
IN THIS CHEMISTRY
SET!
Table #6 - REACTION
RECORDING
TABLE
ROW1
ROW2
ROW3
ROW4
Column1
Column2
Column3
Column4
Copper
Sulfate
Copper
Sulfate
+
Sodium
Chloride
Copper
Sulfate
+
Sodium
Sulfate
Copper
Sulfate
+
Sodium
Bicarbonate
Copper
Sulfate
+
Sodium
Carbonate
Copper
Sulfate
+
Ammonium
Chloride
Ferrous
Sulfate
Ferrous
Sulfate
Ferrous
Sulfate
Sodium
Carbonate
Ferrous
Sulfate
+
Ammonium
Chloride
+
Potassium
Iodide
Column5
Ferrous
Sulfate
+
Potassium
Iodide
Sodium
Chloride
Sodium
Sulfate
Ferrous
Sulfate
+
Sodium
Bicarbonate
Calcium
Nitrate
+
Potassium
Iodide
Calcium
Nitrate
+
Sodium
Chloride
Calcium
Nitrate
+
Sodium
Sulfate
Calcium
Nitrate
+
Sodium
Bicarbonate
Calcium
Nitrate
+
Sodium
Carbonate
Magnesium
Sulfate
+
Potassium
Iodide
Magnesium
Sulfate
+
Sodium
Chloride
Magnesium
Sulfate
+
Sodium
Sulfate
Magnesium
Sulfate
Magnesium
Sulfate
+
+
+
Sodium
Bicarbonate
+
+
Sodium
Carbonate
Column6
Calcium
Nitrate
+
Ammonium
Chloride
Magnesium
Sulfate
+
Ammonium
Chloride
SECTION14 - NEUTRALIZATION
OF GASES
1)
Clean,rinse and dry the pipette you preparedin SECTION
10, Figure#30.
2)
Breakoff a pieceof AIka Seltzer@whichwill fit into the
pipette.
3)
Repeatthe procedureof SECTION
10, Parts 3-11.
What gas was produced by this reaction? Howdo you
know?
Sometimes
gasesmaybe "acidic"... like the pollution gasesin
the atmosphere
whichdissolvein rainwaterto cause"acid rain."
Sometimes
gasesare "basic" or alkaline. And, as you might
expect, the acid gases and the base gases can be mixed to
neutralize oneanother.In the following experiment
youwill see
howsomegases are acidic by the waygaseswill changethe
color of a special "UniversalIndicator" test paper. Thetest
paperwill change
color to shownot only if an acid is presentbut
the color changecanalso give youan idea of "howstrong" the
acidis.
Whatchemicalsdo youthink causedthe productionof this
gas?
SECTION13 - TH_E PRODUCTION
OF AMMONIA
LIST OF MATERIALS
Microplate
Plastic pipette
[]
UniversalIndicatorsolutionona smallpieceof filter paper
[]
Vinegar
Goggles
Ammonia
(NH3)is a gaseouscompound
which, in water solution is foundin the householdpreparationcalled "household
ammonia."Ammonia
and its solutions have a piercing odor.
Ammonia
is also commonly
found in a medicinal preparation
called smellingsalts. Ammonia
is importantfor useas a fertilizer. Ammonia
is often a productof protein decay.
Page 25
BE SURETO WEAR_GO.GGLESWHENDOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
1) Allowall the reactionsto finish. (Waitabout15minutesfor
the reactionsto settle out.)
SECTION5 - TESTINGTHEPRODUCTS
OF A RE,~.CTION
Eventhoughyouhavealreadytested solutionsandsolids in the
previous experiments, nowyou can test the PRODUCTS
of a
reaction with your electrolyte detector. Remember:
in this experimentyou are testing to see whetherthe PRODUCTS
of a
chemicalreaction will behavedifferently than the chemicals
which wereusedto form them.Observecarefully, and you may
wantto test someof the productsafter youhavedried themout
to seeif the dry powder
productsreact differently thanthe "wet"
products.
pipette just belowthe liquid
2) Placethe tip of a MICROTIP
level in a well. Remove
the LIQUIDONLY
from eachof the
wells where a reaction has occurred. DONOTDISCARD
THESESOLUTIONS!
Place each solution removed in
anotherunusedwell on the right side of your microplate.
Example:solution fromA-1 shouldbe put in well A-7, and
so on. Rinsethe pipette with water betweeneach chemical solution. Theliquids whichyouare savingin microwells
A, B, C, D-7-12will be usedin SECTION
6 experiments.
3) Add10dropsof rinse water(tap water)to eachof the wells
LIST OF MATERIALS
~
Microplate with the completedreactions from SECTION
4
I~
Electrolyte Detector madein SECTION
1
[]
Water
[...] Plastic pipettes
-I
Goggles
whichshowed
a chemicalreaction and allow the precipitate
to settle to the bottomof the well.
4)
Remove
and discard the rinse water which is abovethe
precipitatein the well.
5)
Add8 dropsof fresh water to each of the wells wherea
reaction has occurred.
6) Testthe solution of the productsin eachof the wells where
BE SURETO WEAR_GO_GGL_ES_WHEN
QOING
EXPERIMENTS
IN THIS CHEMISTRY
SET!
a reaction has occurred with the ELECTROLYTE
DETECTOR.
Page 30
SECTION4.-__REACTIONS O.F SOLUT_IONS
[1
3
4
5
8
7
8
9
10
~000000000
0
~000000000
0
c OOOOOOOOO 0
~000000000
0
LIST OF MATERIALS
II Solutions of the chemicals listed below in Table #5
(Two Groups: Group 1 Chemicals and Group 2 Chemicals)
Electrolyte Detector
~000000
-~O0000O
Microplate
IJ
2
Plastic pipettes
Goggles
,.__L!.__
.W_H_E..N O.OING
EXPERIMENTS
IN THIS CHEMISTRY
S.E._T_!
Z
;]
4
1.1
121
0 0
0 0
0 0
0 0
-~
1)
Place 1/2 pipette of householdvinegar in a well.
2)
Place the filter paper which wasmadein SECTION
13, Part
4 over the well with the vinegar.
3)
Allow the paper to stay abovethe well for a few minutes.
4)
Whathappensto the color of the paper?Whichside of the
paperturns color first?
5)
Addhouseholdammoniato the well drop by drop. Mix after
each addition. Cover with the paper again after each addition.
EXPERIMENTS
WITH SOLUTIONS
~
8 I ~
Experiments with Solutions
TERMS TO KNOW
AQUEOUS
- A water solution.
ANION
- A negatively chargedion. FxamplP.: CICATION
- A positively
What do you think happenedto the ammonia?
Figure #32
CONDUCTIVITY
- The ability to allow electricity
a substance.
What gas do you think caused the change in the filter
paper?
Chemical compounds
whendissolved in a water solution often
break up into charged particles called IONS. The presence of
these chargedparticles or IONS,allow the solution to conduct
electricity.
The experiment above showedwhich compounds
contain ions. Ions react with each other in solution.
Cations react with anions to form new compounds.As in any
chemical reaction, when two chemicals react, the reaction
sometimesproducesproducts which have totally different properties from the beginning compounds.
t)
5)
Place 4 drops of ferrous sulfate solution in the secondrow
of small wells across the microplate.
6)
Continueto put 4 drops of each chemical solution in Group
1 chemicals in an individual ROWof wells across the
microplate. See Figure #32.
7)
Add 4 drops of potassium iodide solution (Group 2 chemicals) to each of the wells in the first COLUMN
of the
microplate. See Figure #33.
Divide the chemical compoundswhich have been made
into solutions into two groups of chemicals as shownin
Table #5.
DISSOLVE
- To becomepart of a solution.
SECTION 15 - REACTION OF AMMONIUM_CHLORIDE
ANDCALC_J.U_MHYDROXIDE
ELECTROLYTE
- A solution which conducts an electric
ELECTRODE
- A wire in an electrolyte which carries an electrical charge.
LIST OF MATERIALS
Ammonium
chloride solution (from your chemistry set)
HOMOGENEOUS
- The same throughout.
ION- A positively chargedor negatively chargedatomor group
of atoms.
Plastic pipette
000000000
000000000
C 000000000
O 000000000
Group 1
Copper Sulfate
Ferrous Sulfate
Calcium Nitrate
Group 2
PotassiumIodide
SodiumChloride
SodiumSulfate
RndiumBicarbonate
Sodium Carbonate
AmmoniumChloride
A
NONELECTROLYTE
- A solution
electric current.
Filter paper
0
0 0 0 .
0 0 0
0 0 0
PRECIPITATE
- A solid which does not dissolve in water.
BE SURETO WEARGOGGLES_W_H._I~.N..DOING
1)
Place 1/2 of a pipette of ammonium
chloride solution into a
well of your microplate.
2)
Moistena piece of filter
lution.
Solutions are mixtures. Solutions are most often a mixture of a
solid dissolvedin a liquid or a liquid dissolvedin anotherliquid.
The material which DOESthe dissolving is called the SOLVENT. The material which is DISSOLVEDis called the
SOLUTE.
In solutions, the mostplentiful material in the mixture
is called the solvent, while the material dissolved is the solute.
Figure #33
2)
3)
4)
8)
Remembering how you used the ELECTROLYTE
DETECTORfrom Section 2, write a small "e" for electrolyte after
each chemical you tested. Also write a small "n" for nonelectrolyte after the chemicalswhich you tested which were
non-electrolyte.
Remember
which of the chemicals in Table #5 are Electrolytes.
9)
Continueto put 4 drops of each chemical solution in Group
2 chemicals in an individual COLUMN
of wells.
Whichcombination of chemicals gave a chemical reaction?
Howdo you know that a chemical reaction has taken
place? DO NOT DISCARD THIS MICROPLATE OF
REACTIONS!
10) Preparea chart whichrecords all of these reactions similar
to Table #6 - REACTIONRECORDING
TABLE.
Place 4 drops of coppersulfate solution in eachwell in the
first ROW
of small wells across the microplate. SeeFigure
#32.
11) Recordeach reaction (or non-reaction) in the blank spaces
in your table.
Page 29
which does not conduct an
Goggles
O000OO
~t_u....
current.
Microplate
B
to flow through
CONDUCTOR
- A solid or solution which allows electric current
to flow throughit.
What would happen if you mixed the household vinegar
with a mixture of ammonium
chloride and calcium hydroxide?
Calcium hydroxide solution (from your chemistry set)
TABLE #5
charged ion. Example: Na+
paperwith Universal Indicator so-
3)
Add1/2 of a pipette of calcium hydroxide solution to the
well containing ammonium
chloride.
4)
Place 1/2 pipette of household vinegar in the samewell.
Whatis the nameof the acid in householdvinegar?
5)
Mix the two solutions together. Wait a few moments
for the
two liquids to react together.
6)
Allow the paper to stay abovethe well for a few minutes.
7)
What happens to the paper? What is the compound
formed when the acid reacts with the ammonia?Howdo
you knowthat a reaction occurred?
A solution is a special kind of mixture becausea solution contains the sameamountof solute throughout the solvent. Since
a solute is evenly distributed throughoutthe solvent, a solution
is often referred to as a HOMOGENEOUS
mixture. A mixture
(solution) of sugar dissolved in water is an exampleof a homogeneousmixture or a solution.
Canyou think of a solution of a solid dissolved in solid?
(These solutions are called ALLOYS.)
B)
Canyou think of a solution of a gas dissolved in a gas?
Whichgas is the solvent, which is the solute? (Air is such
a solution.)
Page 26
A)
SECTION 1 -&N ELECTROLYTE DETECTOR
1)
LED
/
An electrolyte detector is easily made.The detector will allow
you to determineif a solution conductsan electric current. You
will be able to find out if a solution is an electrolyte._ or a nonelectrolyte.
2)
I
I
LIST OF MATERIALS
LED(light emitting diode)
--I 9-volt battery
II I
II I
/~,,.~.
-
~
./"/"
,,
~,\
I}
,~
]1 // insulation
]/ kk fromends
/~)of
Place 7 drops of water in one of the small wells in the
microplate. Usewell B-12.
4)
Place the two electrodes in the well containing 7 drops of
water. Doespure water conduct? Remember,tap water is
NOTpure water. If your parents have DISTILLEDWATER,
try the experiment again using distilled water. Distilled
water is used in electric steamirons. Why?
5)
Place the two electrodes in each of the solutions and rate
themaccordingto the ability to conductelectricity. Be sure
not to let the two electrodes touch eachother while they are
in the solution. (The glow of the LEDis a goodindication
of the solution being an ELECTROLYTE.
The more the
LEDglows, the better the electrolyte.)
1-K ohmresistor
Figure #31
[] Spring clips (2)
The chemicalsmost used in your chemistry set are solutions in
which a solid or liquid chemicalis dissolved in water. Solutions
of chemicals dissolved in water are called AQUEOUS
SOLUTIONS.
Insulated wire (red length andblack length)
Goggles
1)
Fromyour chemistry set, obtain the LED(light emitting
diode), 1-K ohmresistor, battery clip, andspring clips, and
the pair of red and black wires. Fromthe store, obtain a 9volt battery.
2)
Attach the battery clip to the battery.
3)
The LEDhas two wires, one of which is longer than the
other. Attach the LONG
wire of the LEDto the positive
(red) wire of the battery clip. To connect them, carefully
twist the bare metal endof the wires together.
4)
5)
6)
7)
8)
Someaqueousor water solutions conduct electricity. Theseare
called ELECTROLYTES.
Other solutions
DO NOTconduct
electricity.
These solutions are called NON-ELECTROLYTES.
The ability of a water solution of dissolved chemicalto conduct
or not conduct electricity tells something about the way the
chemicalitself is held together in a molecule.
SECTION 2 - ELECTROLYTES AND NON-ELECTROLYTES
It is importantto knowwhethera solution is an electrolyte or not.
Usually, electrolyte solutions are madeof a chemicalsalt which
is dissolved in water. These WILL conduct small or large
amountsof electrical current. The "Electrolyte Detector" which
you madewill allow you to determineif a solution is conducting
evena small amountof electrical current...the detector will even
tell you if a solid will conductan electrical current.
Attach oneof the resistor wire endsto the negative (black)
wire of the battery clip. Connectthese two wires by carefully twisting the bare endsof the metal wires together.
Next, find the two lengths of wire supplied in your set. One
has black insulation, one has red insulation. Carefully strip
the insulation from the endsof these wires so that you have
both ends of the black wire stripped back about 1/2" (one
half inch) and both ends of the red wire stripped backabout
1/2" (onehalf inch).
Using a spring clip as a connector, carefully insert between
the coils of the spring clip, the free endwire of the LEDand
the stripped wire endof the red length of wire. The free end
of this red wire is one ELECTRODE.
[]
Place a pipette of water in one of the large wells in your
microplate. This well is used to rinse off the electrodes
betweeneach test.
3)
wire
SpringClips
[] 9-volt battery clip
Using a pipette, place 7 drops of _EACHCHEMICAL
SOLUTION IN YOURCHEMISTRYSET SEPARATELYin the
small wells in the microplate. Rinse the pipette with clean
water betweeneach chemical which your pipette touches.
Usesmall wells A-1 through A-12, and B-1 through B-4.
6)
As you do your experiment, group the ELECTROLYTES
together.
Group the NON-ELECTROLYTES
together.
Makea Data Table on a separate sheet of paper similar to
the Data Table shown, with Electrolytes separated from
Non-electrolytes.
DATATABLE #4
Water
Microplate
Electrolyte Detector (madein SECTION
1)
Pipette
[]
Test somecommon
household solutions to see if they are
electrolytes or non-electrolytes. For example,test household bleach, ammonia, detergent, milk, etc. Use small
wells D-1 through D-12for these tests.
9)
Try testing somesamplesof food for conductivity. DONOT
EAT THE FOODAFTER YOU HAVE TESTED IT!
SECTION 3 - ANOTHERUSE FOR THE
ELECTROLYTE DETECTOR
LIST OF MATERIALS
Electrolyte Detector
Householdsolids (see list below)
Goggles
Conductor/Non
Conductor
CobaltChlorideSolution
Goggles
Sodium
Silicate Solution
Your electrolyte detector will tell you if a solid is a CONDUCTOR. Place the two electrodes from the tester on a piece of
copper wire from your chemistry set. Whathappens?Try this
test on a copper penny.
CalciumHydroxideSolution
CalciumNitrate Solution
Citric AcidSolution
Test several solids in your hometo see if they are conductors.
FerrousSulfate Solution
Somesolids to test:
A tissue, a pencil (try the "lead" in the pencil; it isn’t really lead),
a teaspoon, toothbrush, window, pen, woodenor plastic ruler,
etc.
Potassium
Iodide Solution
Sodium
Sulfate Solution
AluminumAmmonium
Sulfate Solution
Ammonium
Chloride Solution
EXPERIM._E_._N_.T_S
IN THISCHE_.M.ISTR.Y
S__ET!
List all the conductors. Whatwas common
about all the conductors?
Magnesium
Sulfate Solution
SodiumCarbonateSolution
List all the non-conductors. What was commonabout all the
non-conductors?
Phenolphthalein
Solution
UniversalIndicator Solution
Page 27
8)
CopperSulfate Solution
LIST OF MATERIALS
--I Solutions of all the chemicalsin the chemistry set
Usingyour other spring clip as a connector,carefully insert
between
the coils of this spring clip, the free endwire of the
1-K ohmresistor and the stripped wire end of the black
length of wire. The free end of this black wire is the other
ELECTRODE.
See Figure #31 for a picture of the completedElectrolyte
Detector.
Whatis common
about the non-electrolytes? Whatis true
about electrolytes?
EXPERIMENTS
IN E_H../_S. CHEMISTRY
SET!
DataTablefor Conductivity
Substance
7)
Enter all tests you makeinto the Data Table you prepared in
Section 2.
Page 28

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