Chemical Principles in the Laboratory
12th Edition
Published on 1. January 2020
Book
Spiral bound
400 pages
978-0-357-36453-6 (ISBN)
Description
Succeed in chemistry with CHEMICAL PRINCIPLES IN THE LABORATORY, 12th Edition! Clear, user-friendly and direct, this lab manual gives you the tools you need to successfully complete lab experiments and lab reports. Analyzing the data you observe in lab sessions is easy with the manual's numerous Advance Study Assignments that give you extra practice with processing data through sample questions. In addition, a special section shows you how to use both Excel and Google Sheets to simplify making calculations.
More details
Edition
12th edition
Language
English
Place of publication
CA
United States
Publishing group
Cengage Learning, Inc
Target group
College/higher education
Dimensions
Height: 20 mm
Width: 228 mm
Thickness: 274 mm
Weight
862 gr
ISBN-13
978-0-357-36453-6 (9780357364536)
Copyright in bibliographic data and cover images is held by Nielsen Book Services Limited or by the publishers or by their respective licensors: all rights reserved.
Schweitzer Classification
Other editions
New editions
Emil Slowinski | Wayne Wolsey | Robert Rossi
Chemical Principles in the Laboratory
Book
03/2023
13th Edition
Brooks/Cole
€79.50
Shipment within 15-20 days
Persons
Emil J. Slowinski, Ph.D., earned a bachelor of science from Massachusetts State College in 1946 and a doctorate in physical chemistry from the Massachusetts Institute of Technology in 1949. Over the course of his prolific teaching career, he taught at Swarthmore College, the University of Connecticut and Macalester College. His sabbatical leaves were taken at Oxford University and the University of Warsaw. He was a co-author, working with other authors like Bill Masterton and Wayne Wolsey, of more than 25 books in various areas of general chemistry. Even after retiring, Dr. Slowinski was actively involved in editions one through nine of Chemical Principles in the Laboratory, and after leaving active writing he offered insights, advice and support to his coauthors; he remains the main content source of this edition. Dr. Slowinski was an Emeritus DeWitt Wallace Professor of Chemistry at Macalester College until his death in 2015. Wayne C. Wolsey, Ph.D., is an inorganic chemist who received his bachelor of science from Michigan State University in 1958 and his doctorate from the University of Kansas in 1962. He joined the Macalester College faculty in 1965 and spent three sabbaticals at the Oak Ridge National Laboratory. Dr. Wolsey is noted for his work (in collaboration with a former student) in investigating various complexing agents for their effectiveness in dissolving calcium oxalate kidney stones. 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. Now retired, he remains professionally active in a number of scientific organizations and continues his contributions to Chemical Principles in the Laboratory. Robert C. Rossi, Ph.D., is an entrepreneur in technology, education and applied science. He earned his bachelor of science in chemical engineering from the University of Wisconsin, Madison. Upon graduation he joined the Peace Corps and served as a teacher in the Fiji Islands. He then joined the California Institute of Technology, teaching and researching in the fields of applied photoelectrochemistry and semiconductor physics and eventually earning a doctorate in 2001. After several years teaching as a visiting professor at Carleton College, he moved to Macalester College, where he served as the Laboratory Supervisor in the chemistry department from 2003 to 2014. In 2011 he became a co-author of Chemical Principles in the Laboratory, with his contributions first appearing in the 10th Edition.
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 Atmospheric 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 Geometric Structure of Molecules-An Experiment Using Molecular Models.
14. Heat Effects and Calorimetry.
15. The Vapor Pressure and Heat of Vaporization of a Liquid.
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 Ba(IO3).
27. Relative Stabilities of Complex Ions and Precipitates Prepared from Solutions of Copper(II).
28. Determination of the Hardness of Water.
29. Synthesis and 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.
44. Fundamentals of Quantum Mechanics.
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: Standard Atomic Weights of the Elements (Scaled relative to Carbon-12 = 12 g/mol).
Appendix IV: Making Measurements-Laboratory Techniques.
Appendix V: Mathematical Considerations-Significant Figures and Making Graphs.
Appendix VI: Suggested Locker Equipment.
Appendix VII: Introduction to Excel.
Appendix VIII: Introduction to Google Sheets.
Appendix IX: Statistical Treatment of Laboratory Data.
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 Atmospheric 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 Geometric Structure of Molecules-An Experiment Using Molecular Models.
14. Heat Effects and Calorimetry.
15. The Vapor Pressure and Heat of Vaporization of a Liquid.
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 Ba(IO3).
27. Relative Stabilities of Complex Ions and Precipitates Prepared from Solutions of Copper(II).
28. Determination of the Hardness of Water.
29. Synthesis and 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.
44. Fundamentals of Quantum Mechanics.
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: Standard Atomic Weights of the Elements (Scaled relative to Carbon-12 = 12 g/mol).
Appendix IV: Making Measurements-Laboratory Techniques.
Appendix V: Mathematical Considerations-Significant Figures and Making Graphs.
Appendix VI: Suggested Locker Equipment.
Appendix VII: Introduction to Excel.
Appendix VIII: Introduction to Google Sheets.
Appendix IX: Statistical Treatment of Laboratory Data.