Designed to meet the needs of the various levels of students who take freshman chemistry—including those preparing to become chemists as well as nonscience majors—this lab manual contains 41 self-contained, low-cost, qualitative and quantitative experiments that require students to collect experimental data, use their reasoning powers to draw logical conclusions about the meaning of the data, and report the results critically and knowledgeably. The manual is an ideal supplement to core General Chemistry texts, such as Chemistry: The Central Science, 8/e by Brown, LeMay, and Bursten.

• NEW - All experiments carefully edited for accuracy, safety, and cost.

  • Each experiment modified based on recent class-testing. This ensures each experiment will work when performed as indicated. Ex.___

• NEW - New and revised review questions.

  • Updated questions encourage students to work the questions themselves rather than relying on students who completed the course previously. Ex.___

• NEW - Added Experiment 11 on VSEPR.

  • Provides more complete coverage on this important topic. Ex.___

• NEW - Several experiments modified to be less toxic and to reduce waste products.

  • Eliminates the risk involved with using toxic chemicals, such as benzene and bromoform, and reduces the amount of waste produced. Ex.___

• 41 self-contained experiments—Each contains sufficient background material to conduct and understand the experiment, and each has a pedagogical objective to exemplify one or more specific principles.

  • Allows experiments to be used with any core text and to be undertaken in any order. Ex.___

• A broad representation of the essential principles and techniques—e.g., uses balances, pH meters, and spectrophotometers.

  • Keeps in mind that many students gain no other exposure to analytical techniques. Ex.___

• Substantive, challenging, hands-on experiments—Most experiments contain unknowns. Very few of the experiments may be “dry-labbed.”

  • Discourages memorization or rote repetition. Ex.___

• A mix of qualitative and quantitative experiments.

  • Enables students to gain hands-on experience in determining the nature of processes and the amount of a measurable change. Ex.___

• Minimal cost experiments.

  • Saves the institution money. Ex.___

• List of necessary materials—At the beginning of each experiment.

  • Helps students and lab coordinators prepare quickly. Ex.___

• Review questions to be answered before the experiments are begun—Answers to some of these questions are provided in an appendix.

  • Helps students understand the experiment and provides an incentive to read the experiment in advance. Ex.___

• A detachable report sheet for each experiment—Easily graded.

  • Provides an easy-to-use, uniform way to report results.

• Annotated Instructor's Edition—Includes answers to all questions and additional prep and disposal information.

  • Helps instructors prepare easily, especially for labs they are performing for the first time. Ex.___

• All experiments carefully edited for accuracy, safety, and cost.

  • Each experiment modified based on recent class-testing. This ensures each experiment will work when performed as indicated. Ex.___

• New and revised review questions.

  • Updated questions encourage students to work the questions themselves rather than relying on students who completed the course previously. Ex.___

• Added Experiment 11 on VSEPR.

  • Provides more complete coverage on this important topic. Ex.___

• Several experiments modified to be less toxic and to reduce waste products.

  • Eliminates the risk involved with using toxic chemicals, such as benzene and bromoform, and reduces the amount of waste produced. Ex.___

To the Student.


Laboratory Safety and Work Instructions.


 1. Basic Laboratory Techniques.


 2. Identification of Substances by Physical Properties.


 3. Separation of the Components of a Mixture.


 4. Chemical Reactions.


 5. Chemical Formulas.


 6. Chemical Reactions of Copper and Percent Yield.


 7. Chemicals in Everyday Life: What Are They and How Do We Know?


 8. Gravimetric Analysis of a Chloride Salt.


 9. Gravimetric Determination of Phosphorus in Plant Food.


10. Paper Chromatography: Separation of Cations and Dyes.


11. Molecular Geometries of Covalent Molecules: Lewis Structures and VSEPR Theory.


12. Atomic Spectra and Atomic Structure.


13. Behavior of Gases: Molar Mass of a Vapor.


14. Determination of R: The Gas-Law Constant.


15. Activity Series.


16. Electrolysis, the Faraday, and Avogadro's Number.


17. Electrochemical Cells and Thermodynamics.


18. The Chemistry of Oxygen: Basic and Acidic Oxides and the Periodic Table.


19. Colligative Properties: Freezing-Point Depression and Molar Mass.


20. Titration of Acids and Bases.


21. Reactions in Aqueous Solution: Metathesis Reactions and Net Ionic Equations.


22. Determination of the Dissociation Constant of a Weak Acid.


23. Titration Curves of Polyprotic Acids.


24. Acid-Base Properties of Salt Solutions: Hydrolysis.


25. Determination of the Solubility-Product Constant for a Sparingly Soluble Salt.


26. Heat of Neutralization.


27. Rates of Chemical Reactions I: A Clock Reaction.


28. Rates of Chemical Reactions II: Rate and Order of H₂O₂ Decomposition.


29. Introduction to Qualitative Analysis.


30. Abbreviated Qualitative-Analysis Scheme—Part I: Group 1 Cations: Pb²⁺, Ag⁺, Hg₂ ²⁺. Part II: Group 2 Cations: Pb²⁺, Cu²⁺, Bi³⁺, Sn⁴⁺. Part III: Group 3 Cations: Fe³⁺, Ni²⁺, Mn²⁺, Al³⁺. Part IV: Group 4 Cations: Ba²⁺, Ca²⁺, NH₄ ⁺, Na⁺. Part V: Anions: SO₄ ^2-, NO₃ ^-, CO₃ ^2-, Cl^-, Br^-, I^-, CrO₄ ^2-, PO₄ ^3-, S^2-, SO₃ ^2-. Part VI: Analysis of a Simple Salt.


31. Colorimetric Determination of Iron.


32. Determination of Orthophosphate in Water.


33. Analysis of Water for Dissolved Oxygen.


34. Preparation and Reactions of Coordination Compounds: Oxalate Complexes.


35. Oxidation-Reduction Titrations I: Determination of Oxalate.


36. Preparation of Sodium Bicarbonate and Sodium Carbonate.


37. Oxidation-Reduction Titrations II: Analysis of Bleach.


38. Molecular Geometry: Experience with Models.


39. Preparation of Aspirin and Oil of Wintergreen.


40. Analysis of Aspirin.


41. Ion-Exchange Resins: Analysis of a Calcium, Magnesium, or Zinc Salt.


Appendix A. Chemical Arithmetic


Appendix B. Graphical Interpretation of Data: Calibration Curves and Least-Squares Analysis.


Appendix C. Summary of Solubility Properties of Ions and Solids.


Appendix D. Solubility-Product Constants for Compounds at 25<198>C.


Appendix E. Dissociation Constants for Acids at 25<198>C.


Appendix F. Dissociation Constants for Bases at 25<198>C.


Appendix G. Selected Standard Reduction Potentials at 25<198>C.


Appendix H. Spreadsheets.


Appendix I. Qualitative-Analysis Techniques.


Appendix J. Answers to Selected Review Questions.


Appendix K. Vapor Pressure of Water at Various Temperatures.


Appendix L. Names, Formulas, and Charges of Common Ions.


Appendix M. Some Molar Masses.


Appendix N. Basic SI Units, Some Derived SI Units, and Conversion Factors.

General Chemistry Laboratory  [LAB MANUALS]   (Chemistry)

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