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Introductory Chemistry - 1st Canadian Edition: End-of-Chapter Material

Introductory Chemistry - 1st Canadian Edition
End-of-Chapter Material
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table of contents
  1. Cover
  2. Title Page
  3. Copyright
  4. Table Of Contents
  5. Acknowledgments
  6. Dedication
  7. About BCcampus Open Education
  8. Chapter 1. What is Chemistry
    1. Some Basic Definitions
    2. Chemistry as a Science
  9. Chapter 2. Measurements
    1. Expressing Numbers
    2. Significant Figures
    3. Converting Units
    4. Other Units: Temperature and Density
    5. Expressing Units
    6. End-of-Chapter Material
  10. Chapter 3. Atoms, Molecules, and Ions
    1. Acids
    2. Ions and Ionic Compounds
    3. Masses of Atoms and Molecules
    4. Molecules and Chemical Nomenclature
    5. Atomic Theory
    6. End-of-Chapter Material
  11. Chapter 4. Chemical Reactions and Equations
    1. The Chemical Equation
    2. Types of Chemical Reactions: Single- and Double-Displacement Reactions
    3. Ionic Equations: A Closer Look
    4. Composition, Decomposition, and Combustion Reactions
    5. Oxidation-Reduction Reactions
    6. Neutralization Reactions
    7. End-of-Chapter Material
  12. Chapter 5. Stoichiometry and the Mole
    1. Stoichiometry
    2. The Mole
    3. Mole-Mass and Mass-Mass Calculations
    4. Limiting Reagents
    5. The Mole in Chemical Reactions
    6. Yields
    7. End-of-Chapter Material
  13. Chapter 6. Gases
    1. Pressure
    2. Gas Laws
    3. Other Gas Laws
    4. The Ideal Gas Law and Some Applications
    5. Gas Mixtures
    6. Kinetic Molecular Theory of Gases
    7. Molecular Effusion and Diffusion
    8. Real Gases
    9. End-of-Chapter Material
  14. Chapter 7. Energy and Chemistry
    1. Formation Reactions
    2. Energy
    3. Stoichiometry Calculations Using Enthalpy
    4. Enthalpy and Chemical Reactions
    5. Work and Heat
    6. Hess’s Law
    7. End-of-Chapter Material
  15. Chapter 8. Electronic Structure
    1. Light
    2. Quantum Numbers for Electrons
    3. Organization of Electrons in Atoms
    4. Electronic Structure and the Periodic Table
    5. Periodic Trends
    6. End-of-Chapter Material
  16. Chapter 9. Chemical Bonds
    1. Lewis Electron Dot Diagrams
    2. Electron Transfer: Ionic Bonds
    3. Covalent Bonds
    4. Other Aspects of Covalent Bonds
    5. Violations of the Octet Rule
    6. Molecular Shapes and Polarity
    7. Valence Bond Theory and Hybrid Orbitals
    8. Molecular Orbitals
    9. End-of-Chapter Material
  17. Chapter 10. Solids and Liquids
    1. Properties of Liquids
    2. Solids
    3. Phase Transitions: Melting, Boiling, and Subliming
    4. Intermolecular Forces
    5. End-of-Chapter Material
  18. Chapter 11. Solutions
    1. Colligative Properties of Solutions
    2. Concentrations as Conversion Factors
    3. Quantitative Units of Concentration
    4. Colligative Properties of Ionic Solutes
    5. Some Definitions
    6. Dilutions and Concentrations
    7. End-of-Chapter Material
  19. Chapter 12. Acids and Bases
    1. Acid-Base Titrations
    2. Strong and Weak Acids and Bases and Their Salts
    3. Brønsted-Lowry Acids and Bases
    4. Arrhenius Acids and Bases
    5. Autoionization of Water
    6. Buffers
    7. The pH Scale
    8. End-of-Chapter Material
  20. Chapter 13. Chemical Equilibrium
    1. Chemical Equilibrium
    2. The Equilibrium Constant
    3. Shifting Equilibria: Le Chatelier’s Principle
    4. Calculating Equilibrium Constant Values
    5. Some Special Types of Equilibria
    6. End-of-Chapter Material
  21. Chapter 14. Oxidation and Reduction
    1. Oxidation-Reduction Reactions
    2. Balancing Redox Reactions
    3. Applications of Redox Reactions: Voltaic Cells
    4. Electrolysis
    5. End-of-Chapter Material
  22. Chapter 15. Nuclear Chemistry
    1. Units of Radioactivity
    2. Uses of Radioactive Isotopes
    3. Half-Life
    4. Radioactivity
    5. Nuclear Energy
    6. End-of-Chapter Material
  23. Chapter 16. Organic Chemistry
    1. Hydrocarbons
    2. Branched Hydrocarbons
    3. Alkyl Halides and Alcohols
    4. Other Oxygen-Containing Functional Groups
    5. Other Functional Groups
    6. Polymers
    7. End-of-Chapter Material
  24. Chapter 17. Kinetics
    1. Factors that Affect the Rate of Reactions
    2. Reaction Rates
    3. Rate Laws
    4. Concentration–Time Relationships: Integrated Rate Laws
    5. Activation Energy and the Arrhenius Equation
    6. Reaction Mechanisms
    7. Catalysis
    8. End-of-Chapter Material
  25. Chapter 18. Chemical Thermodynamics
    1. Spontaneous Change
    2. Entropy and the Second Law of Thermodynamics
    3. Measuring Entropy and Entropy Changes
    4. Gibbs Free Energy
    5. Spontaneity: Free Energy and Temperature
    6. Free Energy under Nonstandard Conditions
    7. End-of-Chapter Material
  26. Appendix A: Periodic Table of the Elements
  27. Appendix B: Selected Acid Dissociation Constants at 25°C
  28. Appendix C: Solubility Constants for Compounds at 25°C
  29. Appendix D: Standard Thermodynamic Quantities for Chemical Substances at 25°C
  30. Appendix E: Standard Reduction Potentials by Value
  31. Glossary
  32. About the Authors
  33. Versioning History

End-of-Chapter Material

Additional Exercises

  1. What is the relationship between the Ksp expressions for a chemical reaction and its reverse chemical reaction?
  2. What is the relationship between the Kw value for H2O and its reverse chemical reaction?
  3. For the equilibrium

    PCl3(g) + Cl2(g) ⇄ PCl5(g) + 60 kJ

    list four stresses that serve to increase the amount of PCl5.

  4. For the equilibrium

    N2O4 + 57 kJ ⇄ 2NO2

    list four stresses that serve to increase the amount of NO2.

  5. Does a very large Keq favour the reactants or the products? Explain your answer.
  6. Is the Keq for reactions that favour reactants large or small? Explain your answer.
  7. Show that Ka × Kb = Kw by determining the expressions for these two reactions and multiplying them together.

    HX(aq) ⇄ H+(aq) + X–(aq)
    X–(aq) + H2O(ℓ) ⇄ HX(aq) + OH–(aq)

  8. Is the conjugate base of a strong acid weak or strong? Explain your answer.
  9. What is the solubility in moles per litre of AgCl? Use data from Table 13.2 “Solubility Product Constants for Slightly Soluble Ionic Compounds”.
  10. What is the solubility in moles per litre of Ca(OH)2? Use data from Table 13.2.
  11. Under what conditions is Keq = KP?
  12. Under what conditions is Keq > KP when the temperature is 298 K?
  13. What is the pH of a saturated solution of Mg(OH)2? Use data from Table 13.2.
  14. What are the pH and the pOH of a saturated solution of Fe(OH)3? The Ksp of Fe(OH)3 is 2.8 × 10−39.
  15. For a salt that has the general formula MX, an ICE chart shows that the Ksp is equal to x2, where x is the concentration of the cation. What is the appropriate formula for the Ksp of a salt that has a general formula of MX2?
  16. Referring to Exercise 15, what is the appropriate formula for the Ksp of a salt that has a general formula of M2X3 if the concentration of the cation is defined as 2x, rather than x?
  17. Consider a saturated solution of PbBr2(s). If [Pb2+] is 1.33 × 10−5 M, find each of the following.
    1. [Br−]
    2. the Ksp of PbBr2(s)
  18. Consider a saturated solution of Pb3(PO4)2(s). If [Pb2+] is 7.34 × 10−14 M, find each of the following.
    1. [PO43−]
    2. the Ksp of Pb3(PO4)2(s)

Answers

  1. They are reciprocals of each other.
  1. increase the pressure; decrease the temperature; add PCl3; add Cl2; remove PCl5
  1. favour products because the numerator of the ratio for the Keq is larger than the denominator
  1. K_{\text{a}}\times K_{\text{b}}=\dfrac{[\ce{H+}]\cancel{[\ce{X-}]}}{\cancel{[\ce{HX}]}}\times \dfrac{\cancel{[\ce{HX}]}[\ce{OH-}]}{\cancel{[\ce{X-}]}}=[\ce{H+}][\ce{OH-}]=K_{\text{w}}
  1. 1.3 × 10−5 mol/L
  1. Keq = KP when the number of moles of gas on both sides of the reaction is the same.
  1. 10.35
  1. 4x3
    1. 2.66 × 10−5 M
    2. 9.41 × 10−15

Annotate

Next Chapter
Chapter 14. Oxidation and Reduction
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Chemistry

Copyright © 2014

                                by Jessie A. Key

            Introductory Chemistry - 1st Canadian Edition by Jessie A. Key is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted.
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