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Chemical Principles in the Laboratory

Chemical Principles in the Laboratory - 9th edition

ISBN13: 978-0495112884

Cover of Chemical Principles in the Laboratory 9TH 09 (ISBN 978-0495112884)
ISBN13: 978-0495112884
ISBN10: 0495112887
Cover type: Spiral
Edition/Copyright: 9TH 09
Publisher: Brooks/Cole Publishing Co.
Published: 2009
International: No

List price: $252.00

Chemical Principles in the Laboratory - 9TH 09 edition

ISBN13: 978-0495112884

Emil Slowinski

ISBN13: 978-0495112884
ISBN10: 0495112887
Cover type: Spiral
Edition/Copyright: 9TH 09
Publisher: Brooks/Cole Publishing Co.

Published: 2009
International: No

CHEMICAL PRINCIPLES IN THE LABORATORY, continues to build on its strengths by clearly presenting the basic principles of chemistry. The lab manual continues to maintain the high quality, time-tested experiments and techniques which have become hallmark features throughout the life of this title.

Author Bio

Emil Slowinski
Emil J. Slowinski is an Emeritus DeWitt Wallace Professor of Chemistry at Macalester College. He earned a B.S. degree from Massachusetts State College in 1946 and a Ph.D. in physical chemistry from the Massachusetts Institute of Technology in 1949. He taught at Swarthmore College, 1949-1952; the University of Connecticut, 1952-1964; and Macalester College, 1964-1988. His sabbatical leaves were at Oxford University in 1960 and the University of Warsaw in 1968. He is a co-author, with Bill Masterton and/or Wayne Wolsey, of more than 25 books on various areas of general chemistry. He is retired, but has continued his writing with new editions of the laboratory manual.
Wayne C. Wolsey
Wayne C. Wolsey, an inorganic chemist, received his B.S. from Michigan State University in 1958 and his Ph.D. from the University of Kansas in 1962. He joined the Macalester College faculty in 1965 and is now in "semi-retirement." His last three sabbaticals were spent at the Oak Ridge National Laboratory. In 2001-2002, he investigated various complexing agents for their effectiveness in dissolving calcium oxalate kidney stones, in collaboration with a former student, now a urologist. He has received various awards, including the Minnesota College Science Teacher of the Year in 1989; Macalester's Thomas Jefferson Award in 1993; designation as a MegaMole contributor to Minnesota Chemical Education in 1997; and an award from the Minnesota State AAUP Conference in 2001 for his support of academic freedom and shared governance. He remains professionally active in a number of scientific organizations.

Table of Contents

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".