Experiments in general chemistry 6th edition murov solutions manual

INSTRUCTOR'S GUIDE for

EXPERIMENTS IN GENERAL CHEMISTRY Table of Contents

LAB EQUIPMENT and RECOMMENDED LOCKER EQUIPMENT

1

CHEMICALS REQUIRED

3

Experiment 1

EARLY EXPLORATIONS AND TERMINOLOGY

11

Experiment 2

SEPARATION OF MIXTURESC

17

Experiment 3

MEASUREMENTS AND IDENTIFICATION TECHNIQUESC

21

Experiment 4

DENSITY, ACCURACY, PRECISION AND GRAPHINGC

25

Experiment 5

EMPIRICAL FORMULASM

29

Experiment 6

CLASSIFICATION OF CHEMICAL REACTIONS

33

Experiment 7

QUANTITATIVE PRECIPITATIONM

37

Experiment 8

ELECTRICAL CONDUCTIVITY AND ELECTROLYTES

41

Experiment 9

IONIC REACTIONS

45

Experiment 10

ACTIVITIES OF METALS

51

Experiment 11

QUANTITATIVE SOLUTION CHEMISTRYM

53

Experiment 12

THERMOCHEMISTRYC

55

Activity 13

PROPERTIES OF ELEMENTS AND COMPOUNDS: AN INTERNET STUDY

59

Experiment 14

SPECTROSCOPY OF COBALT(II) IONC

63

Activity 15

LEWIS STRUCTURES AND MOLECULAR MODELS

65

Experiment 16

MOLECULAR POLARITY AND CHROMATOGRAPHY

71

iii

Experiment 17

GAS LAW STUDIESC

75

Experiment 18

COOLING CURVES AND CRYSTAL STRUCTURESC

77

Experiment 19

WATER PURIFICATION AND ANALYSISC

79

Activity 20

ORGANIC MODELS AND ISOMERISM

81

Experiment 21

ACIDS AND BASES: REACTIONS AND STANDARDIZATIONM

85

Experiment 22

ACIDS AND BASES: ANALYSISM

89

Experiment 23

ACIDS AND BASES: pH, pKa MEASUREMENTS

91

Experiment 24

EQUILIBRIUM - SOLUBILITY PRODUCTC

95

Experiment 25

EQUILIBRIUM - DETERMINATION OF Keq

99

Experiment 26

COMPLEXES

103

Experiment 27

RATES AND MECHANISMS OF REACTIONS

113

Experiment 28

SYNTHESIS OF COPPER(II) GLYCINATEC

117

Experiment 29

STANDARDIZATION OF THIOSULFATEM

119

Experiment 30

ANALYSIS OF BLEACH AND COPPER(II) GLYCINATEM

121

Experiment 31

REDOX REACTIONS

123

Experiment 32

ELECTROCHEMISTRYM

129

Experiment 33

SPECTROSCOPIC ANALYSIS OF ASPIRINC

131

Experiment 34

POLYMER PROPERTIES AND SELECTION

135

Activity 35

ADDITIONAL CHALLENGES AND EXPERIMENTS

139

Activity 36

GRAPHING OF QUANTITATIVE RELATIONSHIPS

143

Appendix

SOLUTIONS TO PRELABORATORY PROBLEMS

147

C M

iv

indicates that a centigram balance will suffice for this experiment. indicates that a milligram balance is recommended for this experiment.

Instructor's Guide Labs should be equipped with: Aspirators Balances Beaker Tongs Buret Clamps Burners Hoods Hot Plates/Stirrers Rings Ring Supports Test Tube Clamps Three-Pronged Clamps Spectronic 20's or alternative

Recommended Locker Equipment: 5 Beakers 100, 150, 250, 400, 600 ml.

1 Clay Triangle 1 Crucible 1 Crucible Cover 1 Crucible Tongs 1 Evaporating Dish 1 Flame Spreader 3 Flasks, Erlenmeyer 125, 250, 500 ml.

1 Flask, Florence 500 ml.

1 Funnel, long stem 2 Graduated Cylinders 10, 50 ml.

1 Medicine Dropper 1 Piece of Rubber Tubing 50 cm.

1 Pinch Clamp 1 Pipet, 10 ml.

6 Test Tubes 13 X 100 mm.

6 Test Tubes 18 X 150 mm.

1 Test Tube Brush 1 Test Tube Clamp 1 Test Tube Rack 1 Thermometer 110o C 1 Wash Bottle 2 Watch Glasses 1 Wire Gauze

1

2

Chemicals Required: * means that this solution requires special preperation instructions, given in this manual.

Chemical Description Or Or Supply Concentration Exp # Qty/Student Acetic Acid Acetic Acid Acetic Acid *Acetic Acid/Sodium Acetate 0.1M in each Acetone

0.1M 0.2M 0.2M

Acetophenone *Adipoyl Chloride in Cyclohexane Aluminum foil

100% 0.25M

100%

Aluminum Shot Aluminum Nitrate *Ammonia -Ammonium chloride buffer Ammonium Chloride Ammonium Chloride

0.1M

Ammonium Hydroxide

0.1M

Ammonium Hydroxide Ammonium Hydroxide Ammonium Hydroxide Ammonium Oxalate Ammonium Thiocyanate

3.0M 6.0M Conc.

1.0M 100%

Antacid Tablet Aspirin Tablet Barium Chloride Benzoic Acid Beral pipets Bleach Boiling Chips Borax Boric Acid *Bromophenol Blue Indicator *Bromothymol Blue Indicatior *1:1:1 Butanol: Ethanol:Ammonia Calcium Acetate Calcium Chloride Calcium Chloride Calgon Candle

0.1M 100%

0.1M 100%

4% 100%

Saturated 0.1M 1.0M

8 5 23 23 16 28 34 4 34 8 21 1 12 1 19 23 12 6 24 8 23 26 9 16 9 5 24 23 33 1 18 6, 28 30 19 34 5 35 21 16 5 1 2 19 1 6

50 ml 10 mL 25 ml 20 ml 25 ml 10 ml 100 ml 6 ml 4 ml 50 cm2 50 cm2 Zero Zero Zero 40 Drops 25 ml 3g 3g 3g 50 ml 25 ml 10 ml 10 ml ? ?

4g 4g 1 1 Zero 2, 3 20 ml 2 5 ml 1g 3 Drops 10 Drops 40 ml 2 ml 4 ml 10 ml 15 g 1 1

3

Chemical Or Supply Capillary Tube (Sealed End) Carbon Ceric Ammonium Nitrate Cerium(III) Nitrate Cerium(IV) Sulfate *Chromatography Paper Whatman #1 Chromium(III) Chloride Cobalt(II) Chloride Cobalt(II) Chloride *Cobalt Chloride Test Papter Cobalt Nitrate Hexahydrate Copper Foil Squares Copper Foil Strips Copper Shot Copper Shot Copper Wire

Copper(II) Acetate Monohydrate Copper(II) Chloride Copper(II) Hydroxide Copper(II) Nitrate Copper(II) Salts Copper(II) Sulfate

Copper(II) Sulfate

Description Or Concentration

0.1M 0.1M

0.1M 0.1M 1.0M 1 cm2 1 cm X 10 cm

0.1M 100% 0.1M 0.1M

1.0M

Copper(II) Sulfate Pentahydrate

Copper(II) Sulfate Anhydrous *1,6 Diaminohexane in 0.5M NaOH *Diphenylamine in Conc. H2SO4 *EDTA, Disodium Elmers Glue *Eriochrome Black T Ethanol Ethanol, Denatured Fabrics Felt Tip Pens

4

1% 0.00500M 0.1M 95%

Exp #

Qty/Student

3 1 31 1 1 16 1 1 16 7 14 10 31 30 1 12 7 8 32 34 28 1 6 1 7 1 6 10 26 31 16 27 32 6 7 5 6 34 11 19 34 19 8 6 16 16 16

3 Zero 2 ml Zero Zero 2 Zero Zero 1 ml 2 Pieces 2.18 g 5 2 3 Zero Zero 1 Inch 2 cm 50 cm 10 cm 1.6 g Zero 0.5 g Zero 1.2 g Zero 3 ml 10 ml 20 ml 4 ml 1 ml 1 Drop 140 ml 2g 1.2 g 1g 0.5 g 4 ml 4 Drops 25 ml 20 g 4 drops 25 ml 15 ml 27 ml

Chemical Or Supply

Description Or Concentration

Filter Paper Filter Paper

5.5 cm 12.5 cm

Food Coloring Glass Rod Glass Tubing Glass Wool Glucose Glucose Glycine Green Grass Guar Gum Hydrochloric Acid Hydrochloric Acid Hydrochloric Acid Hydrochloric Acid

6 mm 0.1M 80 g/liter 100%

0.001M 0.01M 0.1M

Hydrochloric Acid Hydrochloric Acid Hydrochloric Acid Hydrochloric Acid

0.1M Or 0.2M Unknown Standard 0.5M Standard 1.0M 2.0M 3.0M

Hydrochloric Acid

6.0M

Hydrochloric Acid

6.0M

Hydrogen Peroxide

3%

Ice

Iodine

100% 100% 1x10-4 M

Exp #

Qty/Student

28 2 6 19 32 1 8 1 5 8 1 28 16 34 23 23 23 30

1 1 2 2 1 1 Drop 1 1 meter 1g 25 ml 15 ml 1.3 g 10 g 1g 50 ml 25 ml 25 ml 150 ml

23 35 8 12 1 6 21 29 2 6 5 17 16 29 30 19 21 26 31 5 31

50 ml 15 ml 25 ml 50 mL 6 ml 2 ml 6 ml 4 ml 10 Drops 5 ml 10 ml 25 ml 7 ml 3 ml 20 ml 10 ml 5 ml 40 Drops 1 Drop 50 ml 4 ml 2 4 18 29 Zero 1.2 25 ml

1 5 25

5

Chemical Or Supply

Description Or Concentration

Iodine Water Saturated Ion Exchange Resin H+ Form Iron Filings Iron (Steel Wool) *Iron(III) Chloride *Iron(III) Chloride Iron(III) Chloride Iron(III) Chloride Iron(III) Nitrate Iron(II) Sulfide Kerosene Lauric Acid Lead Shot

0.05M HCL 0.1M 0.5M 100% 0.1M 100% 100% 100%

Lead Chromate Lead Iodide Lead Nitrate Lithium Chloride

100% 100% 100% 0.1M

Lithium Chloride Lithium Sulfate Magnesium

100% 0.5M Ribbon

Magnesium Chloride Magnesium Chloride Magnesium Nitrate Magnesium Sulfate

0.1M 0.1M 0.1M 0.1M

Magnesium Sulfate Heptahydrate Maleic Acid Manganese Manganese(II) Chloride Manganese(II) Chloride Manganese Dioxide *Mercury(I) Nitrate *Mercury(II) Nitrate Methylene Blue Methylene Blue *Methyl Orange

0.1M Or 0.2M 100% 0.1M 1.0M 100% 0.1M 0.1M 0.4 g/L 0.4 g/L Indicator

Nickel Nickel(II) Chloride

Shot 0.1M

6

Exp #

Qty/Student

16 31 19 1 10 33 1 16 1 10 26 17 21 1 12 1 1 1 1 9 12 9 1 5 10 31 1 26 9 5 10 5 9 23 6 1 16 6 1 1 1 16 21 35 12 1

5 ml 2 ml 15 g Zero 5g 600 ml 2 ml 1 ml Zero 10 ml Zero 30 ml 4g Zero Zero Zero Zero Zero Zero 5 ml 3g 10 ml Zero 2 cm 10 cm 2 cm Zero 20 ml 10 ml 5 ml 10 ml 4g 10 ml 20 ml 7g Zero 1 ml 0.1 g Zero Zero 10 Drops 10 Drops 10 Drops 3 Drops Zero Zero

Chemical Or Supply

Description Or Concentration

Nitric Acid Pencils

2.0M

*pH 4 Buffer *pH 7 Buffer *Phenolphthalein Indicator Phenylcarbonate Phosphorous, Red Plastic Strips *Polyvinyl Alcohol Potassium Acetate Potassium Biphthalate Potassium Bitartrate Potassium Bromide Potassium Chloride Potassium Chloride Potassium Chloride Potassium Chromate Potassium Ferricyanide

4% 100% 100% 100% 0.1M 0.1M 0.2M 100% 100% 0.1M

Potassium Ferricyanide Potassium Ferrocyanide

1% 0.1M

Potassium Ferrocyanide Trihydrate Potassium Hydroxide Potassium Hydroxide Potassium Iodate Potassium Iodide Potassium Iodide Potassium Iodide Potassium Iodide Potassium Iodide

64 g/L 3.0M 0.1M 2.00x10-3 M 0.1M 0.2M 0.5 M 100%

Potassium Nitrate Potassium Nitrate Potassium Permanganate *Potassium Persulfate Potassium Phosphate Potassium Sulfate Potassium Thiocyanate Potassium Thiocyanate 1 Propanol *Rubber Rings Sand Silicon

100% 100%

0.1M 1.0M 0.1M 0.10M 1.0M 0.1M 0.1M 1.0M 100%

100%

Exp #

Qty/Student

12 8 16 23 23 21 23 3 1 8 34 5 21 24 31 1 27 24 1 1 31 11 1 26 11 1 12 31 25 31 27 25 29 30 1 32 1 24 9 27 1 26 28 3 16 1

50 ml 1 1 25 ml 25 ml 19 Drops 18 Drops Zero 1 5 ml 1g 3.6 g 1g 2 ml Zero 30 ml 1g Zero Zero 2 ml 6 Drops Zero 8 ml 1.1 g 15 ml 6 ml 2 ml 15 ml 8 ml 230 ml 10 ml 4.5 g 6g 2 ml 20 ml Zero 230 ml 10 ml 30 ml 2 ml 15 ml 20 ml 3 1g Zero

7

Chemical Or Supply

Description Or Concentration

Silver Nitrate

0.1M

Sodium Acetate

0.1M

Sodium Bicarbonate Sodium Bromide Sodium Carbonate

0.1M 0.1M 0.1M

Sodium Carbonate

1.0M

Sodium Chlorate Sodium Chloride Sodium Chloride Sodium Chloride Sodium Chloride

0.1M 1 X 10-5M 1 X 10-3M 0.1M 0.1M

Sodium Chloride Sodium Chloride Sodium Chloride Sodium Chloride Sodium Chloride Sodium Chromate Sodium Dichromate Sodium Hydroxide

5% 10% 15% 20% Saturated 0.1M 0.1M 0.1M

Sodium Hydroxide

0.2M Standard

Sodium Hydroxide

1.0M

Sodium Hydroxide Sodium Hydroxide

2.0M 3.0M

8

Exp #

Qty/Student

1 19 1 23 23 1 1 19 23 1 2 7 9 21 1 8 8 1 8 9 19 23 4 4 4 4 2 1 1 1 21 23 22 23 35 12 21 33 12 1 7 9 21 26

Zero 10 Drops Zero 25 ml 25 ml Zero Zero 20 Drops 25 ml 2 ml 10 ml 4 ml 10 ml 9 ml Zero 25 ml 25 ml Zero 25 ml 5 ml 20 Drops 25 ml Unknown Unknown Unknown Unknown 6 ml Zero Zero Zero 9 ml 25 ml 100 ml from Exp21 100 ml from Exp21 100 ml from Exp21 50 mL 50 Drops 10 ml 100 mL 2 ml 7 ml 10 ml 6 ml 15 ml

Chemical Or Supply

Description Or Concentration

Sodium Hydroxide

6.0M

Sodium Hydroxide Sodium Iodate Sodium Iodide Sodium Nitrate

Pellets 0.1M 0.1M 0.1M

Sodium Oxalate Sodium Phosphate

0.1M 0.1M

Sodium Salicylate Sodium Sulfate Sodium Sulfate

100% 0.01M 0.1M

Sodium Sulfate

1.0M

Sodium Sulfate Sodium Sulfite Sodium Thiocyanate Sodium Thiosulfate Sodium Thiosulfate Sodium Thiosulfate *Sodium Thiosulfate/Starch *Solution 0.1M in Mg, Na, Li, Sr *Solution A *Solution B *Solution C *Solution A *Solution B *Solution C *Starch Indicator

Decahydrate 0.1M 0.1M 0.1M 1.0M Pentahydrate 0.005M/0.4%

0.4%

Steel Ball Bearings Steel Wool Strontium Chloride

0.1M

Strontium Chloride Strontium Hydroxide Strontium Hydroxide Sulfur

Hexahydrate Octahydrate Octahydrate 100%

Exp #

Qty/Student

7 12 21 1 1 1 7 1 1 7 26 33 32 1 10 9 16 5 1 1 1 31 29 27 9 21 21 21 34 34 34 29 30 12 10 32 1 5 9 5 6 24 1

10 ml 6 ml 8g Zero Zero Zero 2 ml Zero Zero 2 ml 12 ml 0.4 g 250 ml Zero 10 ml 10 ml?

0.5 ml 1g Zero Zero Zero 4 ml 8.2 g 130 ml 1 ml 20 ml 10 ml 10 ml 10 ml 10 ml 10 ml 6 ml 12 ml 10 g 5g 1g Zero 1 ml 10 ml 4g 7g 7g Zero

9

Chemical Or Supply

Description Or Concentration

Sulfuric Acid Sulfuric Acid Sulfuric Acid Sulfuric Acid

0.05M 0.1M 1.5M 3.0M

Sulfuric Acid *Tin(II) Chloride *Tin(IV) Chloride *Vanillin *Vinegar White Paper Wood Splints

3.0M 0.1M 0.1M Crude Unknown

Zinc

Shot

Zinc

Ribbon 1 cm2

Zinc Zinc Zinc Nitrate

Ribbon 1X10 cm 20 mesh granular 0.1M

Zinc Sulfate

0.1M

Zinc Sulfate

1.0M

Zinc Sulfate Heptahydrate Zinc tablets (50 mg)

Exp #

Qty/Student

30 8 9 7 11 16 1 1 2 22 11 1 8 21 1 7 12 6 10 17 31 32 5 1 26 7 5 10 31 29 32 5 11

70 ml 50 ml 15 ml 2 ml 20 ml 2 Drops Zero Zero 2g 15 ml 1 Piece 1 1 3 Zero 6g Zero 2 5 1g 2 1 1.2 Zero 20 ml 3 ml 5 ml 10 ml 4 ml 36 ml 80 ml 4g 1

* means that this solution requires special preperation instructions, given in this manual.

10

Experiment 1 - Early Explorations and Terminology Chemicals And Supplies: 0.1M aluminum nitrate (demo), 0.1M barium chloride (demo), 0.1M calcium chloride (4 ml and demo), candle (1), 0.1M cerium (III) nitrate (demo), cerium(IV) sulfate (demo), 0.1M chromium (III) chloride (demo), 0.1M cobalt (II) chloride (demo), cobalt(II) nitrate (demo), cobalt(II) sulfate (demo), 0.1M copper (II) chloride (demo), food coloring (1 drop), 6 mm glass tubing (1 meter), 80 g/L glucose (15 ml), 3.0M hydrochloric acid (6 ml), iodine (demo), 0.1M iron (III) chloride (2 ml and demo), 0.1M lead (II) nitrate (demo), 0.1M lithium chloride (demo), magnesium ribbon (demo), 0.1M magnesium chloride (demo), 0.1M manganese (II) chloride (demo), match (1), 0.1M mercury (I) nitrate * (demo), 0.1M mercury (II) nitrate *(demo), 0.4 g/L methylene blue(10 drops), paper (preferably newspaper (1 sheet/student), 0.1M nickel (II) chloride (demo), 0.1M potassium chloride (demo), 0.1M potassium ferricyanide (demo), 0.1M potassium ferrocyanide (demo), 64 g/L potassium hydroxide (15 ml), 0.1M potassium nitrate (2 ml), 0.1M potassium permanganate (demo), 0.1M potassium thiocyanate (2 ml), 0.1M silver nitrate (demo), 0.1M sodium acetate (demo) 0.1M sodium bromide (demo), 0.1M sodium carbonate (2 ml and demo), 1.0M sodium carbonate (2 ml), 0.1M sodium chlorate (demo), 0.1M sodium chloride (demo), 0.1M sodium chromate (demo), solid sodium chromate (demo), 0.1M sodium dichromate (demo), 0.1M sodium hydroxide (demo), 3.0M sodium hydroxide (2 ml), 0.1M sodium iodate (demo), 0.1M sodium iodide (demo), 0.1M sodium nitrate (demo), 0.1M sodium oxalate (demo), 0.1M sodium phosphate (demo), 0.1M sodium sulfate (demo), 0.1M sodium sulfite (demo), sodium tetraborate (2.1 g), 0.1M sodium thiocyanate (demo), 0.1M sodium thiosulfate (demo), 0.1M strontium chloride (demo), 0.1M tin (II) chloride (demo), 0.1M tin (IV) chloride (demo), wood splints (1), 0.1M zinc nitrate (demo).

Equipment: 100 ml beaker, 150 ml beaker, 250 ml Erlenmeyer flask, flame spreader, 1 gas bottle, 100x20 mm Petri dish, 50 ml graduated cylinder, molecular models, stir rod, 5-18 X 150 mm test tubes, wire gauze.

General Instructions: 1.

Time:

4 hours

2.

Safety precautions a.

Burning wooden splints should be placed in fireproof recepticles. b.

Students should be warned that hot glass looks like cold glass. A student can detect if a glass piece is still hot by holding his hand over it. Hot glass produces warm convection currents. Students should place hot glass pieces on a wire gauze to protect the lab bench.

c.

There are several very toxic compounds students will be observing in this experiment. These chemicals should be in sealed containers and labeled "poison".

3.

4.

d.

Thiocyanate ion reacts with oxidizing agents to produce a foul smelling volatile compound (possibly thiocyanogen). Be certain that waste thiocyanate is not disposed of in a sink or container where it might come into contact with oxidizing agents. Thiocyanate ion is also supposed to decompose with heat or in the presence of strong concentrated acids to produce poisonous hydrogen cyanide. Precautions should also be taken against these possibilities.

e.

3M hydrochloric acid and 3M sodium hydroxide are somewhat corrosive.

f.

Some demonstration chemicals used in this experiment (e.g. Ba, Hg) present disposal problems. They should be stored from semester to semester (or quarter to quarter) rather than disposed of.

Special chemicals and unknowns: (the mercury solutions are for demonstration purposes only and should be stored for repeated use in sealed vials) a.

0.1M mercury (I) nitrate is prepared by dissolving 56.2 grams of Hg2(NO3)2â–Ş2H2O in 200 ml of 6M nitric acid and diluting to a liter.

b.

0.1M mercury (II) nitrate is prepared by dissolving 32.4 grams of Hg(NO 3)2 in 50 ml of 6M nitric acid and diluting to a liter.

c.

There are no unknowns in this experiment.

Comments: a.

Chemicals for part I should be put in small sealed vials. They may be stored and used again the following semester or quarter.

b.

The blue color of the solution in the "mystery flask" (part J) slowly fades as the glucose reduces the methylene blue to a colorless compound. When the mixture is swirled, oxygen from the air reoxidizes the methylene blue and the blue color returns. It may take several minutes for the color to fade initially. The potassium hydroxide solution is necessary because the reaction takes place only in base.

Prelaboratory Problems Solutions are in the Appendix.

Experiment 1 - Results and Discussion A.

The meniscus.

1.

The meniscus between water and glass should be concave upward.

3.

Why is water level higher near the glass than in the middle?

B.

The candle flame.

3.

Further observations: a. beaker partially over burning candle -

condensation of water on inside

b. stirring rod next to extinguished wick -

slight deposit of wax

c. burning match approaching extinguished wick 4.

candle reignites before match reaches wick

Was your first explanation (question 2) correct or do you want to modify it or suggest a new one? Explain your answer.

The paraffin vapor is burning. When the beaker is held over a burning candle, water vapor collects on the inside. Paraffin collects on a stir rod held above the candle just after it has been extinguished and the match reignites before the match reaches it..

D.

Rate Of Mixing 1.

Initial observations: Initially in the cold water, the food color will fall to the bottom of the beaker leaving a color trail. In the hot water mixing occurs very rapidly.

2.

Observations about 1/2 hour later: After 1/2 hour even the cold water solution should be approaching homogeneity.

3.

When two aqueous solutions are introduced into the same container, is stirring needed to achieve a homogeneous system? Explain your answer.

Yes, at low temperatures the mixing process is slow and if one solution is denser than the other there is a tendency to form layesr.

4.

How would you stir a solution freshly prepared in a volumetric flask?

By stoppering, inverting and swirling the flask several times.

E.

Tearing Paper The paper should tear rather straight in one direction and curve rapidly toward the favored direction when the paper is torn at right angles. Apparently industrial preparation of the paper leads to preferential alignment of the fibers or cellulose polymers in one direction. Tearing it one direction then requires breaking of weaker intermolecular forces while tearing in the other direction involves an attempt to break intramolecular bonds.

F.

Chemistry reference. acetic acid

formula C2H3O2 or HC2H3O2 b.p. 117.9 oC m.p. 16.6 oC TDLo 1.47 mg/kg LD50 3310 mg/kg

Meaning of TDLo lowest published toxic dose Meaning of LD50 lethal dose to kill half the population Household product(s) that contain acetic acid vinegar (about 5% acetic acid), cleaning agents, pickle preservative H.

Solutions.

1 –6.

I.

Both of the 0.05 g portions of sodium tetraborate decahydrate should dissolve fairly readily. The additional 2 g will result in a saturated solution and most will not dissolve until the solution is heated. The solid will dissolve upon heating and slow cooling results in the formation of neat looking crystals.

Colors.

1.

List the colored cations and their colors.

Ce3+ Cr3+ Co2+ Cu2+ Fe3+ Ni2+

2.

yellow green red or pink blue yellow green

Can you make any generalizations about color versus position in the periodic chart?

Apparently color is only common among the transition metal ions.

3.

List the colored anions and their colors.

CrO42Yellow Cr2O72Orange Fe(CN)63- Yellow to orange Fe(CN)64- Light Yellow MnO4Magenta

J.

Chemical Reactions A. B. C. D. E.

white precipitate heat no apparent reaction bubbles or evolution of a gas formation of a deep red color

K.

Mystery flask (see Anderson, L.; Wittkopp,S. M.; Painter, C. J.; Liegel, J.J.; Schreiner, R.; Bell, J. A.; Shakhashiri, B. Z. J. Chem. Educ., 2012, 89 (11), pp 1425– 1431 for recent article on blue bottle reaction) 1.

Observations upon standing: The solution should turn colorless (note that clear is not an adequate answer). A very important observation that is a valuable clue concerning the cause of the color change is that the top surface of the solution has a tinge of blue.

2.

Observations upon swirling: The blue color returns.

3.

Suggest an explanation for the change that occurs upon swirling.

Oxygen oxidizes the reduced colorless form of methylene blue back to the original blue compound.

4.

How could you test your explanation (it might be possible with your instructor's approval to actually perform the test).

Exclude oxygen by bubbling N2 through the solution before swirling.

Also test with a pure oxygen atmosphere by bubbling O2 through the solution.

L.

Classic Burning Candle Experiment.

The results are not very reproducible indicating that the oxygen consumption explanation is unlikely and some of the oxygen is replaced by carbon dioxide anyway. Actually, about 11% oxygen is needed to sustain the flame so there is still about half of the original amount of oxygen present when the flame goes out. The heat from the wax vapor combustion heats the air in the bottle causing it to expand and some heated air leaves the bottle. After the flame goes out, the air cools and the water rises to replace the space previously occupied by the air that has exited. In addition to checking for reproducibility, students could try other experiments such as replacing all of the air in the bottle with oxygen.

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