Laboratory Experiments for Chemistry: The Central Science

by Brown, Theodore E.; LeMay, H. Eugene; Bursten, Bruce E.; Murphy, Catherine; Woodward, Patrick; Stoltzfus, Matthew E.; Nelson, John H.; Kemp, Kenneth C.

• ISBN13: 9780134566207
• ISBN10: 0134566203
• Additional ISBN(s): 9780321949912
• Edition: 14th
• Format: Workbook
• Copyright: 2017-07-14
• Publisher: Pearson
• More Book Details

Summary

For two-semester general chemistry lab courses

Introducing basic lab techniques and illustrating core chemical principles

Prepared by John H. Nelson and Kenneth C. Kemp, both of the University of Nevada, this manual contains 43 finely tuned experiments chosen to introduce basic lab techniques and to illustrate core chemical principles. In the 14th Edition, all experiments were carefully edited for accuracy, safety, and cost. Pre-labs and questions were revised and new experiments added concerning solutions, polymers, and hydrates.

Each of the experiments is self-contained, with sufficient background material, to conduct and understand the experiment. Each has a pedagogical objective to exemplify one or more specific principles. Because the experiments are self-contained, they may be undertaken in any order, although the authors have found in their General Chemistry course that the sequence of Experiments 1 through 7 provides the firmest background and introduction. The authors have included pre-lab questions to answer before starting the lab. The questions are designed to help in understanding the experiment, learning how to do the necessary calculations to treat their data, and as an incentive for reading the experiment in advance. These labs can also be customized through Pearson Collections, our custom database program. For more information, visit https://www.pearsonhighered.com/collections/

Table of Contents

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.              Solubility and the Effect of Temperature on Solubility

10.           Paper Chromatography: Separation of Cations and Dyes

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

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.           Freezing Point Depression

20.           Titration of Acids and Bases

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

22.           Colorimetric Determination of an Equilibrium Constant in Aqueous Solution

23.           Chemical Equilibrium: Le Châtelier’s Principles

24.           Hydrolysis of Salts and pH of Buffer Solutions

25.           Determination of the Dissociation Constant of a Weak Acid

26.           Titration Curves of Polyprotic Acids

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

28.           Heat of Neutralization

29.           Rates of Chemical Reactions I: A Clock Reaction

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

31.           Introduction to Qualitative Analysis

32.           Abbreviated Qualitative Analysis Scheme

Part I: Chemistry of Group 1 Cations: Pb²⁺, Ag⁺, Hg₂ ²⁺

Part II: Chemistry of Group 2 Cations: Pb²⁺, Cu²⁺, Bi³⁺, Sn⁴⁺

Part III: Chemistry of Group 3 Cations: Fe³⁺, Ni²⁺, Mn²⁺, Al³⁺

Part IV: Chemistry of Group 4 Cations: Ba²⁺, Ca²⁺, NH₄ ⁺, Na⁺

Part V: Chemistry of Anions: SO₄ ^2—, NO₃ ^—, CO₃ ^2—, Cl^—, Br^—, I^—, CrO₄ ^2—, PO₄ ^3—, S^2—, SO₃ ^2—

Part VI: Analysis of a Simple Salt

33.           Molarity, Dilutions, and Preparing Solutions

34.           Solubility and Thermodynamics

35.           Analysis of Water for Dissolved Oxygen

36.           Preparation and Reactions of Coordination Compounds: Oxalate Complexes

37.           Oxidation-Reduction Titrations I: Determination of Oxalate

38.           Enthalpy of Vaporization and Clausius-Clapeyron Equation

39.           Oxidation-Reduction Titrations II: Analysis of Bleach

40.           Molecular Geometry: Experience with Models

41.           Polymers

42.           Hydrates of Magnesium Sulfate and its Reactions

43.           Crystalline Solids

 

APPENDICES

A.     The Laboratory Notebook

B.     Chemical Arithmetic

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

D.    Summary of Solubility Properties of Ions and Solids

E.     Solubility-Product Constants for Compounds at 25°C

F.     Dissociation Constants for Acids at 25°C

G.    Dissociation Constants for Bases at 25°C

H.    Selected Standard Reduction Potentials at 25°C

I.      Spreadsheets

J.      Qualitative Analysis Techniques

K.     Vapor Pressure of Water at Various Temperatures

L.     Names, Formulas, and Charges of Common Ions

M.   Some Molar Masses

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

O.    Composition of Commercial Reagent Acids and Bases