This Tenth Edition of CHEMICAL PRINCIPLES IN THE LABORATORY maintains the high-quality, time-tested experiments and techniques that have made it a perennial bestseller. Author Wayne Wolsey, with the help of new co-author Rob Rossi, continues to offer complete coverage of basic chemistry principles and present topics in a direct, easy-to-understand manner. Now, to benefit the environment and reduce the overall cost of the experiments, the new edition features a deepened commitment to green chemistry by reducing the volume and toxicity of experiments as much as possible.
Table of Contents
Experiment 1: The Densities of Liquids and Solids.
Experiment 2: Resolution of Matter into Pure Substances, I. Paper Chromatography.
Experiment 3: Resolution of Matter into Pure Substances, II. Fractional Crystallization.
Experiment 4: Determination of a Chemical Formula.
Experiment 5: Identification of a Compound by Mass Relationships.
Experiment 6: Properties of Hydrates.
Experiment 7: Analysis of an Unknown Chloride.
Experiment 8: Verifying the Absolute Zero of Temperature—Determination of the Barometric Pressure.
Experiment 9: Molar Mass of a Volatile Liquid.
Experiment 10: Analysis of an Aluminum-Zinc Alloy.
Experiment 11: The Atomic Spectrum of Hydrogen.
Experiment 12: The Alkaline Earths and the Halogens—Two Families in the Periodic Table.
Experiment 13: The Geometrical Structure of Molecules—An Experiment Using Molecular Models.
Experiment 14: Heat Effects and Calorimetry.
Experiment 15: The Vapor Pressure and Heat of Vaporization of a Liquid.
Experiment 16: The Structure of Crystals—An Experiment Using Models.
Experiment 17: Classification of Chemical Substances.
Experiment 18: Some Nonmetals and Their Compounds—Preparations and Properties.
Experiment 19: Molar Mass Determination by Depression of the Freezing Point.
Experiment 20: Rates of Chemical Reactions, I. The Iodination of Acetone.
Experiment 21: Rates of Chemical Reactions, II. A Clock Reaction.
Experiment 22: Properties of Systems in Chemical Equilibrium—Le Châtelier's Principle.
Experiment 23: Determination of the Equilibrium Constant for a Chemical Reaction.
Experiment 24: The Standardization of a Basic Solution and the Determination of the Molar Mass of an Acid.
Experiment 25: pH Measurements—Buffers and Their Properties.
Experiment 26: Determination of the Solubility Product of Ba(IO3)2.
Experiment 27: Relative Stabilities of Complex Ions and Precipitates Prepared from Solutions of Copper(II).
Experiment 28: Determination of the Hardness of Water.
Experiment 29: Synthesis and Analysis of a Coordination Compound.
Experiment 30: Determination of Iron by Reaction with Permanganate—A Redox Titration.
Experiment 31: Determination of an Equivalent Mass by Electrolysis.
Experiment 32: Voltaic Cell Measurements.
Experiment 33: Preparation of Copper(I) Chloride.
Experiment 34: Development of a Scheme for Qualitative Analysis.
Experiment 35: Spot Tests for Some Common Anions.
Experiment 36: Qualitative Analysis of Group I Cations.
Experiment 37: Qualitative Analysis of Group II Cations.
Experiment 38: Qualitative Analysis of Group III Cations.
Experiment 39: Identification of a Pure Ionic Solid.
Experiment 40: The Ten Test Tube Mystery.
Experiment 41: Preparation of Aspirin.
Experiment 42: Rate Studies on the Decomposition of Aspirin.
Experiment 43: Analysis for Vitamin C.
Appendix I: Vapor Pressure and Density of Liquid Water.
Appendix II: Summary of Solubility Properties of Ions and Solids.
Appendix IIA: Some Properties of the Cations in Groups I, II, and III.
Appendix III: Table of Atomic Masses (Based on Carbon-12).
Appendix IV: Making Measurements—Laboratory Techniques.
Appendix V: Mathematical Considerations—Making Graphs.
Appendix VI: Suggested Locker Equipment.
Appendix VII: Introduction to Excel.
Appendix VIII: Statistical Treatment of Laboratory Data.