Sixth Edition - Alternate Version

CHEMICAL PRINCIPLES IN THE LABORATORY WITH QUALITATIVE ANALYSIS

Emil J . Slowinski Professor of Chemistry Macalester College St. Paul, Minnesota

Wayne C. Wolsey Professor of Chemistry Macalester College St. Paul, Minnesota

William L. Masterton Professor of Chemistry University of Connecticut Storrs, Connecticut

m Saunders Golden Sunburst Series Saunders College Publishing HARCOURT BRACE COLLEGE PUBLISHERS Fort Worth Philadelphia San Diego New York Orlando Austin San Antonio Toronto Montreal London Sydney Tokyo

U r able of Contents

Experiment 1

The Densities of Liquids and Solids 1

Experiment 2

Resolution of Matter into Pure Substances, I. Paper Chromatography 7

Experiment 3

Resolution of Matter into Pure Substances, II . Fractional Crystallization 15

Experiment 4

Determination of a Chemical Formula 23

Experiment 5

Identification of a Compound Using Mass Relationships 31

Experiment 6

Analysis of an Unknown Chloride 37

Experiment 7

Molar Mass of a Volatile Liquid 45

Experiment 8

Analysis of an Aluminum-Zinc Alloy 51

Experiment 9 The Atomic Spectrum of Hydrogen 61

Experiment 10

The Alkaline Earths and the Halogens—Two Families in the Periodic Table 71

Experiment 11

The Geometrical Structure of Molecules 79

Experiment 12

Heat Effects and Calorimetry 89

Experiment 13

The Vapor Pressure and Heat of Vaporization of Liquids 97

Experiment 14

Classification of Chemical Substances 107

Experiment 15

Rates of Chemical Reactions, I. The Iodination of Acetone 115

Experiment 16

Rates of Chemical Reactions, II . A Clock Reaction 125

Experiment 17

Properties of Systems in Equil ibr ium—Le Chatelier's Principle 137

Experiment 18

Determination of the Equilibrium Constant for a Reaction 149

X Contents

Experiment 19

Standardization of a Basic Solution and the Determination of the Molar Mass of an Acid 159

Experiment 20

pH—Buffers and Their Properties 167

Experiment 21 Determination of the Solubility Product of Pb l 2 179

Experiment 22 Relative Stabilities of Complex Ions and Precipitates Prepared from Cu(II) 187

Experiment 23

Determination of the Hardness of Water 197

Experiment 24

Synthesis and Analysis of a Coordination Compound 205

Experiment 25 Determination of Iron by Reaction with Permanganate—A Redox Titration 217

Experiment 26

Determination of an Equivalent Mass by Electrolysis 223

Experiment 27 Voltaic Cell Measurements 231

Experiment 28 Preparation of Copper(I) Chloride 241

Experiment 29

Preparation of Aspirin 249

Experiment 30

Analysis for Vitamin C 257

Introduction to the Qualitative Analysis of Cations and Anions 263

Experiment 31

Qualitative Analysis of the Group I Cations: Ag+ , P b 2 + , Hg22+ 269

Experiment 32

Qualitative Analysis of the Group II Cations: Cu2 + , Bi 3 + , Hg2*, Cd 2 + , Sn2 + and Sn 4 + , Sb3 +

and S b 5 \ (Pb2+) , 279

Experiment 33

Qualitative Analysis of the Group III Cations: N i 2 \ Co 2 + , Fe 2 + and Fe 3 + , Mn 2 + , Cr 3 + , Al3 + , Zn 2 + , (Cd2 +) 293

Experiment 34

Qualitative Analysis of the Group IV Cations: Ba 2 + , Ca2 + , Mg2*, N a + , K + , NH 4+ 307

Experiment 35

Qualitative Analysis ofAnions in the Sulfate Group: S 0 42 _ , S0 3

2~, C0 32 , P 0 4

3 ~ , Cr0 42 ,

C2042~ 319

Experiment 36

Qualitative Analysis ofAnions in the Chloride Group: Cl~, B r - , I - , S C N - , S2~ 329

Experiment 37

Qualitative Analysis ofAnions in the Nitrate Group: N 0 3 ~ , N 0 2 ~ , C10 3 ~, C2H302~ 339

Contents XI

Experiment 38

Identification of a Pure Ionic Compound 347

Appendix I

Vapor Pressure of Water 359

Appendix II

Summary of Solubility Properties of Ions and Solids 360

Appendix IM

Some Anion-Anion Reactions 362

Appendix IV

Making Measurements — Laboratory Techniques 363

Appendix V

Mathematical Considerations—Making Graphs 374

Appendix VI

Suggested Locker Equipment 379

Appendix VII

Table of Atomic Masses 380

Appendix VII I

Suggestions for Extension of the Experiments to "Rea l World Prob lems" 382