Table of Contents Last updated Save as PDF Page ID182235 Unit I: Fundamentals of Thermochemistry7.1: The Nature of Energy7.2: Heat7.3: Heats of Reaction and Calorimetry7.4: Work7.5: The First Law of Thermodynamics7.6: Heats of Reactions: ΔU and ΔH7.7: Indirect Determination of ΔH: Hess's Law7.8: Standard Enthalpies of Formation7.9: Fuels as Sources of Energy7.S: Temperature ConversionsUnit II: States of Matter12: Intermolecular Forces (Liquids and Solids)12.1: Intermolecular Forces12.2: Some Properties of Liquids12.3: Some Properties of Solids12.4: Phase Diagrams12.5: Changes of State12.5: Network Colvalent Solids and Ionic Solids12.6: Crystal Structures13: Solutions and their Physical Properties13.1: Types of Solutions: Some Terminology13.2: Solution Concentration13.3: Intermolecular Forces and the Solution Process13.4: Solution Formation and Equilibrium13.5: Solubilities of Gases13.6: Vapor Pressures of Solutions13.7: Osmotic Pressure13.8: Freezing-Point Depression and Boiling-Point Elevation of Nonelectrolyte Solutions13.9: Solutions of Electrolytes13.10: Colloidal MixturesUnit III: Chemical Equilibria14: Principles of Chemical Equilibria15.1: Dynamic Equilibrium15.2: The Equilibrium Constant Expression15.3: Relationships Involving Equilibrium Constants15.4: The Magnitude of an Equilibrium Constant15.5: Factors That Affect Equilibrium15.6: Altering Equilibrium Conditions: Le Châtelier’s Principle15.7: Equilibrium Calculations: Some Illustrative Examples15.S: The Quadratic Formula17: Solubility and Complex-Ion Equilibria17.1: Solubility Product Constant, Ksp17.2: Relationship Between Solubility and Ksp17.3: Common-Ion Effect in Solubility Equilibria17.4: Limitations of the Ksp Concept17.5: Criteria for Precipitation and its Completeness17.6: Fractional Precipitation17.7: Solubility and pH17.8: Equilibria Involving Complex Ions17.9: Qualitative Cation AnalysisUnit IV: Acids and Bases15: Acids and Bases15.1: Arrhenius Theory: A Brief Review15.2: Brønsted-Lowry Theory of Acids and Bases15.3: Self-Ionization of Water and the pH Scale15.4: Strong Acids and Strong Bases15.5: Weak Acids and Weak Bases15.6: Polyprotic Acids15.7: Ions as Acids and Bases15.8: Molecular Structure and Acid-Base Behavior15.9: Lewis Acids and Bases16: Additional Aspects of Acid-Base Equilibria16.1: Common-Ion Effect in Acid–Base Equilibria16.2: Buffer Solutions16.3: Acid–Base Indicators16.4: Neutralization Reactions and Titration Curves16.5: Solutions of Salts of Polyprotic Acids16.6: Acid–Base Equilibrium Calculations: ASummaryUnit V: Principles of Thermodynamics18.1: Spontaneity: The Meaning of Spontaneous Change18.2: The Concept of Entropy18.3: Evaluating Entropy and Entropy Changes18.4: Criteria for Spontaneous Change: The Second Law of Thermodynamics18.5: Standard Gibbs Energy Change, ΔG°18.6: Gibbs Energy Change and Equilibrium18.7: ΔG° and K as Functions of Temperature18.8: Coupled ReactionsBack MatterIndexGlossary
