Chemical Principles in the Laboratory
Published on 15. July 2009
Book
Paperback/Softback
400 pages
978-0-538-73744-9 (ISBN)
Description
CHEMICAL PRINCIPLES IN THE LABORATORY, 8e, International Edition continues to build on its strengths by clearly presenting the basic principles of chemistry. The lab manual maintains the high-quality, time-tested experiments and techniques that have become hallmark features throughout the life of this title.
More details
Edition
International ed of 9th revised ed
Language
English
Place of publication
CA
United States
Publishing group
Cengage Learning, Inc
Target group
Professional and scholarly
Dimensions
Height: 274 mm
Width: 216 mm
Thickness: 24 mm
Weight
907 gr
ISBN-13
978-0-538-73744-9 (9780538737449)
Copyright in bibliographic data is held by Nielsen Book Services Limited or its licensors: all rights reserved.
Schweitzer Classification
Content
1. The Densities of Liquids and Solids. 2. Resolution of Matter into Pure Substances, I. Paper Chromatography. 3. Resolution of Matter into Pure Substances, II. Fractional Crystallization. 4. Determination of a Chemical Formula. 5. Identification of a Compound by Mass Relationships. 6. Properties of Hydrates. 7. Analysis of an Unknown Chloride. 8. Verifying the Absolute Zero of Temperature: Determination of the Barometric Pressure. 9. Molar Mass of a Volatile Liquid. 10. Analysis of an Aluminum-Zinc Alloy. 11. The Atomic Spectrum of Hydrogen. 12. The Alkaline Earths and the Halogens: Two Families in the Periodic Table. 13. The Geometrical Structure of Molecules: An Experiment Using Molecular Models. 14. Heat Effects and Calorimetry. 15. Vapor Pressure and Heat of Vaporization of Liquids. 16. The Structure of Crystals -- An Experiment Using Models. 17. Classification of Chemical Substances. 18. Some Nonmetals and Their Compounds -- Preparations and Properties. 19. Molar Mass Determination by Depression of the Freezing Point. 20. Rates of Chemical Reactions, I. The Iodination of Acetone. 21. Rates of Chemical Reactions, II. A Clock Reaction. 22. Properties of Systems in Chemical Equilibrium -- Le Chatelier's Principle. 23. Determination of the Equilibrium Constant for a Chemical Reaction. 24. The Standardization of a Basic Solution and the Determination of the Molar Mass of an Acid. 25. pH Measurements: Buffers and Their Properties. 26. Determination of the Solubility Product of PbI2. 27. Relative Stabilities of Complex Ions and Precipitates Prepared from Solutions of Copper(II). 28. Determination of the Hardness of Water. 29. Synthesis and an Analysis of a Coordination Compound. 30. Determination of Iron by Reaction with Permanganate -- A Redox Titration. 31. Determination of an Equivalent Mass by Electrolysis. 32. Voltaic Cell Measurements. 33. Preparation of Copper(I) Chloride. 34. Development of a Scheme for Qualitative Analysis. 35. Spot Tests for Some Common Anions. 36. Qualitative Analysis of Group I Cations. 37. Qualitative Analysis of Group II Cations. 38. Qualitative Analysis of Group III Cations. 39. Identification of a Pure Ionic Solid. 40. The Ten Test Tube Mystery. 41. Preparation of Aspirin. 42. Rate Studies on the Decomposition of Aspirin. 43. Analysis for Vitamin C. Appendix I: Vapor Pressure of Water. Appendix II: Summary of Solubility Properties of Ions and Solids. 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: Suggestions for Extension of the Experiments to "Real World Problems".