This is completed downloadable of Solutions Manual to accompany Introduction to Chemical Principles 11th 0321814630 / 9780321814630
Product Details:
- ISBN-10 : 0321814630
- ISBN-13 : 978-0321814630
- Author:
Newly updated based on extensive reviewer feedback, this affordable introductory text remains focused on the essentials necessary for success in General Chemistry. Introduction to Chemistry Principles, Eleventh Edition focuses on the most important topics ― omitting organic and biochemistry chapters ― and teaches the problem-solving skills readers need. Each topic is introduced and developed step by step until reaching the level of sophistication required for further course work.
Table of Content:
- Chapter 1 The Science of Chemistry
- 1.1 Chemistry—A Scientific Discipline
- 1.2 Scientific Research and Technology
- 1.3 The Scope of Chemistry
- 1.4 How Chemists Discover Things—The Scientific Method
- Experiments, Observations, and Data
- Example 1.1 Distinguishing between Qualitative and Quantitative Data
- Solution
- Scientific Facts
- Scientific Laws
- Scientific Hypotheses
- Example 1.2 Relating Scientific Hypotheses to Experimental Information
- Solution
- Example 1.3 Differentiating among Terminologies Associated with the Scientific Method
- Solution
- Scientific Theories
- 1.5 The Limitations of the Scientific Method
- 1.6 Application Limitations for Methods of Science
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Scientific Disciplines (Sec. 1.1)
- Scientific Research and Technology (Sec. 1.2)
- The Scientific Method (Sec. 1.4)
- Multiple-Choice Practice Test
- Chapter 2 Numbers from Measurements
- 2.1 The Importance of Measurement
- 2.2 Exact and Inexact Numbers
- 2.3 Accuracy, Precision, and Error
- Example 2.1 Determining the Accuracy and Precision of a Series of Measurements
- Solution
- 2.4 Uncertainty in Measurements
- Example 2.2 Recording Measurements to the Proper Uncertainty Level
- Solution
- 2.5 Significant Figures
- Example 2.3 Determining the Number of Significant Figures in a Numerical Value
- Solution
- Example 2.4 Determining the Number of Significant Figures and Magnitude of Uncertainty in a Numerical Value
- Solution
- Example 2.5 Uncertainty and the Number of Significant Figures in a Measurement
- Solution
- 2.6 Significant Figures and Mathematical Operations
- Rounding Off Numbers
- Example 2.6 Rounding Numbers to a Specified Number of Significant Figures
- Solution
- Operational Rules for Mathematical Operations
- Example 2.7 Predicting the Number of Significant Figures That Should be Present in the Answer to a Multiplication Problem
- Solution
- Example 2.8 Expressing Multiplication/Division Answers to the Proper Number of Significant Figures
- Solution
- Example 2.9 Expressing Addition/Subtraction Answers to the Proper Number of Significant Figures
- Solution
- Significant Figures and Exact Numbers
- Multiplication by a Small Whole Number
- Example 2.10 Significant Figures in Calculations Involving Multiplication by a Small Whole Number
- Solution
- 2.7 Expressing Numbers in Scientific Notation
- Exponents
- Converting from Decimal to Scientific Notation
- Example 2.11 Expressing Decimal Numbers in Scientific Notation
- Solution
- Significant Figures and Scientific Notation
- Converting from Scientific to Decimal Notation
- Example 2.12 Expressing Scientific Notation Numbers in Decimal Notation
- Solution
- Uncertainty and Scientific Notation
- Example 2.13 Determining the Uncertainty Associated with Numbers Expressed in Scientific Notation
- Solution
- Example 2.14 Uncertainty Considerations for a Number Expressed in Scientific Notation
- Solution
- 2.8 Mathematical Operations in Scientific Notation
- Multiplication in Scientific Notation
- Example 2.15 Multiplication of Scientific Notation Numbers
- Solution
- Example 2.16 Multiplication of Numbers in Scientific Notation Form
- Solution
- Division in Scientific Notation
- Example 2.17 Division of Scientific Notation Numbers
- Solution
- Addition and Subtraction in Scientific Notation
- Example 2.18 Addition and Subtraction of Scientific Notation Numbers
- Solution
- Example 2.19 Adding Scientific Notation Numbers without Equalizing Exponents
- Solution
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Exact and Inexact Numbers (Sec. 2.2)
- Accuracy and Precision (Sec. 2.3)
- Uncertainty in Measurements (Sec. 2.4)
- Significant Figures (Sec. 2.5)
- Rounding Off (Sec. 2.6)
- Significant Figures in Multiplication and Division (Sec. 2.6)
- Significant Figures in Addition and Subtraction (Sec. 2.6)
- Calculations Involving Both Significant Figure Rules (Sec. 2.6)
- Significant Figures and Exact Numbers (Sec. 2.6)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 3 Unit Systems and Dimensional Analysis
- 3.1 The Metric System of Units
- SI Units
- Metric System Prefixes
- Example 3.1 Recognizing the Mathematical Meanings of Metric System Prefixes
- Solution
- 3.2 Metric Units of Length
- 3.3 Metric Units of Mass
- 3.4 Metric Units of Volume
- 3.5 Units in Mathematical Operations
- 3.6 Conversion Factors
- English-to-English Conversion Factors
- Metric-to-Metric Conversion Factors
- Metric-to-English and English-to-Metric Conversion Factors
- 3.7 Dimensional Analysis
- Metric-to-Metric Conversion Factor Use
- Example 3.2 One-Step Metric-to-Metric Conversion Factor Problem
- Solution
- Example 3.3 Two-Step Metric-to-Metric Conversion Factor Problem
- Solution
- Example 3.4 Metric-to-Metric Conversion Factor Problem Involving Cubic Dimensions
- Solution
- English-to-English Conversion Factor Use
- Example 3.5 Multistep English-to-English Conversion Factor Problem
- Solution
- English-to-Metric and Metric-to-English Conversion Factor Use
- Example 3.6 English-to-Metric Conversion Factor Problem
- Solution
- Example 3.7 Multistep Metric-to-English Conversion Factor Problem
- Solution
- Example 3.8 Metric-to-English Conversion Factor Problem Involving Cubic Units
- Solution
- Units Involving More Than One Type of Measurement
- Example 3.9 Conversion Factor Problem Involving Two Types of Units
- Solution
- 3.8 Density
- Example 3.10 Using Mass and Volume to Calculate Density
- Solution
- Using Density as a Conversion Factor
- Example 3.11 Using Density as a Conversion Factor to Relate Mass and Volume
- Solution
- 3.9 Equivalence Conversion Factors Other Than Density
- Concentration and Dosage Relationship Conversion Factors
- Example 3.12 Using Concentration Conversion Factors
- Solution
- Chemical Insight: VITAMIN A
- Rate Relationship Conversion Factors
- Example 3.13 Using Rate Conversion Factors
- Solution
- Cost Relationship Conversion Factors
- Example 3.14 Using Cost Conversion Factors
- Solution
- 3.10 Percentage And Percent Error
- Example 3.15 Percentage Calculation
- Solution
- Using Percentage as a Conversion Factor
- Example 3.16 Using Percentage as a Conversion Factor
- Solution
- Example 3.17 Multiple Use of Percentages in a Conversion Factor Problem
- Solution
- Percent Error
- Example 3.18 Calculation of Percent Error
- Solution
- Student 1
- Student 2
- Student 3
- 3.11 Temperature Scales
- Example 3.19 Fahrenheit-to-Celsius Temperature Conversion
- Solution
- Example 3.20 Celsius-to-Fahrenheit Temperature Conversion
- Solution
- Example 3.21 Temperature Scale Conversions
- Solution
- Temperature Readings and Significant Figures
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Metric System Units (SECS. 3.1–3.4)
- Area and Volume Measurements (SECS. 3.4 and 3.5)
- Conversion Factors (Sec. 3.6)
- Dimensional Analysis’Metric–Metric Unit Conversions (Sec. 3.7)
- Dimensional Analysis—Metric–English Unit Conversions (Sec. 3.7)
- Dimensional Analysis’Units Involving Two Types of Measurement (Sec. 3.7)
- Density (Sec. 3.8)
- Equivalence Conversion Factors (Sec. 3.9)
- Percentage and Percent Error (Sec. 3.10)
- Temperature Scales (Sec. 3.11)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 4 Basic Concepts About Matter
- 4.1 Chemistry—The Study of Matter
- 4.2 Physical States of Matter
- 4.3 Propertires of Matter
- Physical and Chemical Properties
- Example 4.1 Classifying Properties as Physical or Chemical
- Solution
- Intensive and Extensive Properties
- Example 4.2 Classifying Properties as Intensive or Extensive
- Solution
- 4.4 Changes in Matter
- Use of the Terms Physical and Chemical
- Example 4.3 Correct Use of the Terms Physical and Chemical
- Solution
- 4.5 Pure Substances and Mixtures
- 4.6 Heterogeneous and Homogeneous Mixtures
- Use of the Terms Homogeneous and Heterogeneous
- 4.7 Elements and Compounds
- Example 4.4 “Composition” Difference between a Mixture and a Compound
- Solution
- Example 4.5 Classifying Substances as Element, Compound, or Mixture
- Solution
- 4.8 Discovery and Abundance of the Elements
- 4.9 Names and Chemical Symbols of the Elements
- Example 4.6 Writing Correct Names for Elements
- Solution
- Example 4.7 Writing Correct Chemical Symbols for Elements
- Solution
- Concepts to Remember
- Key Terms Listing
- Practice Problems by Topic
- Physical States of Matter (Sec. 4.2)
- Properties of Matter (Sec. 4.3)
- Changes In Matter (Sec. 4.4)
- Pure Substances and Mixtures (SECS. 4.5 AND 4.6)
- Elements and Compounds (Sec. 4.7)
- Discovery and Abundance of the Elements (Sec. 4.8)
- Names and Chemical Symbols of the Elements (Sec. 4.9)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 5 Atoms, Molecules, and Subatomic Particles
- 5.1 The Atom
- 5.2 The Molecule
- Example 5.1 Classifying Molecules Based on Numbers of and Types of Atoms Present
- Solution
- Example 5.2 Classifying Matter Based on Molecular, Phase, and Substance Characteristics
- Solution
- 5.3 Natural and Synthetic Compounds
- 5.4 Chemical Formulas
- Example 5.3 Interpreting Chemical Formulas in Terms of Atoms and Elements Present
- Solution
- 5.5 Subatomic Particles: Protons, Neutrons, and Electrons
- Arrangement of Subatomic Particles Within an Atom
- Charge Neutrality of an Atom
- Size Relationships within an Atom
- Additional Subatomic Particles
- 5.6 Atomic Number and Mass Number
- Atomic Number
- Mass Number
- Subatomic Particle Makeup of an Atom
- Example 5.4 Determining the Subatomic Makeup of an Atom Given Its Atomic Number and Mass Number
- Solution
- Example 5.5 Determining the Subatomic Makeup of an Atom Given Its Complete Chemical Symbol
- Solution
- 5.7 Isotopes
- Example 5.6 Identifying Characteristics of Isotopes of an Element
- Solution
- Example 5.7 Distinguishing between Isotopes and Isobars
- Solution
- 5.8 Atomic Masses
- Relative Mass
- Example 5.8 Constructing a Relative Mass Scale
- Solution
- Average Atom
- Weighted Averages
- Example 5.9 Calculation of a Weighted Average
- Solution
- Example 5.10 Calculation of Atomic Mass from Isotopic Masses and Percent Abundances
- Solution
- Mass Spectrometry Experiments
- 5.9 Evidence Supporting the Existence and Arrangement of Subatomic Particles
- Discharge Tube Experiments
- Metal Foil Experiments
- Concepts to Remember
- Key Terms Listing
- Practice Problems by Topic
- Atoms and Molecules (SECS. 5.1 AND 5.2)
- Chemical Formulas (Sec. 5.4)
- Subatomic Particles (Sec. 5.5)
- Atomic Number and Mass Number (Sec. 5.6)
- Isotopes (Sec. 5.7)
- Atomic Masses (Sec. 5.8)
- Evidence Supporting the Existence and Arrangement of Subatomic Particles (Sec. 5.9)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 6 Electronic Structure and Chemical Periodicity
- 6.1 The Periodic Law
- Student Learning Focus:
- 6.2 The Periodic Table
- Student Learning Focus:
- Periods and Groups of Elements
- Example 6.1 Identifying Groups, Periods, and Specially Named Groups of Elements
- Solution
- The Shape of the Periodic Table
- 6.3 The Energy of an Electron
- Student Learning Focus:
- 6.4 Electron Shells
- Student Learning Focus:
- 6.5 Electron Subshells
- Student Learning Focus:
- 6.6 Electron Orbitals
- Student Learning Focus:
- Example 6.2 Interrelationships among Electron Shells, Electron Subshells, and Electron Orbitals
- Solution
- Electron Spin
- 6.7 Electron Configurations
- Student Learning Focus:
- Aufbau Principle
- Aufbau Diagram
- Writing Electron Configurations
- Example 6.3 Writing Electron Configurations for Elements
- Solution
- Answer Double Check:
- Chemical Insight: SELENIUM
- Condensed Electron Configurations
- Example 6.4 Writing Condensed Electron Configurations
- Solution
- Answer Double Check:
- Chemical Insight: IODINE
- 6.8 Electron Orbital Diagrams
- Student Learning Focus:
- Example 6.5 Writing Electron Orbital Diagrams for the Electrons in Atoms
- Solution
- Answer Double Check:
- Chemical Insight: TITANIUM
- 6.9 Electron Configurations and the Periodic Law
- Student Learning Focus:
- 6.10 Electron Configurations and the Periodic Table
- Student Learning Focus:
- Example 6.6 Using the Periodic Table as a Guide in Obtaining Information about Distinguishing Electrons
- Solution
- Chemical Insight: CALCIUM
- Example 6.7 Using the Periodic Table as a Guide in Writing an Electron Configuration
- Solution
- Answer Double Check:
- Chemical Insight: MERCURY
- 6.11 Classification Systems for the Elements
- Student Learning Focus:
- 6.12 Chemical Periodicity
- Student Learning Focus:
- Metallic and Nonmetallic Character
- Atomic Size
- Example 6.8 Predicting Atomic Size Relationships, Using General Periodic Table Trends
- Solution
- Chemical Insight: NITROGEN INFLATION
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Periodic Law and Periodic Table (SECS. 6.1 AND 6.2)
- Terminology Associated With Electron Arrangements (SECS. 6.3–6.6)
- Electron Configurations (Sec. 6.7)
- Electron Orbital Diagrams (Sec. 6.8)
- Electron Configurations and the Periodic Law (Sec. 6.9)
- Electron Configurations and the Periodic Table (Sec. 6.10)
- Classification Systems for the Elements (Sec. 6.11)
- Chemical Periodicity (Sec. 6.12)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 7 Chemical Bonds
- 7.1 Types of Chemical Bonds
- Student Learning Focus:
- 7.2 Valence Electrons and Lewis Symbols
- Student Learning Focus:
- Example 7.1 Determining the Number of Valence Electrons an Atom Possesses
- Solution
- Example 7.2 Writing Lewis Symbols for Elements
- Solution
- 7.3 The Octet Rule
- Student Learning Focus:
- 7.4 The Ionic Bond Model
- Student Learning Focus:
- Example 7.3 Writing Chemical Symbols for Ions
- Solution
- Answer Double Check:
- Example 7.4 Determining the Number of Protons and Electrons in Ions
- Solution
- Answer Double Check:
- 7.5 The Sign and Magnitude of Ionic Charge
- Student Learning Focus:
- Example 7.5 Predicting Sign and Magnitude of Ionic Charge
- Solution
- Isoelectronic Species
- 7.6 Lewis Structures for Ionic Compounds
- Student Learning Focus:
- Example 7.6 Using Lewis Structures to Depict Ionic Compound Formation
- Solution
- Chemical Insight: Aluminum Oxide
- 7.7 Chemical Formulas for Ionic Compounds
- Student Learning Focus:
- Example 7.7 Using Ionic Charges to Determine the Chemical Formula of an Ionic Compound
- Solution
- Answer Double Check:
- Chemical Insight: Magnesium Chloride
- 7.8 Structure of Ionic Compounds
- Student Learning Focus:
- 7.9 Polyatomic Ions
- Student Learning Focus:
- Example 7.8 Writing Chemical Formulas for Ionic Compounds Containing Polyatomic Ions
- Solution
- Answer Double Check:
- 7.10 The Covalent Bond Model
- Student Learning Focus:
- 7.11 Lewis Structures for Molecular Compounds
- Student Learning Focus:
- Example 7.9 Writing Lewis Structures for Simple Molecular Compounds
- Solution
- Chemical Insight: Phosphine
- 7.12 Single, Double, and Triple Covalent Bonds
- Student Learning Focus:
- 7.13 Valence Electron Count and Number of Covalent Bonds Formed
- Student Learning Focus:
- Example 7.10 Predicting Chemical Formulas for Simple Molecular Compounds
- Solution
- 7.14 Coordinate Covalent Bonds
- Student Learning Focus:
- 7.15 Resonance Structures
- Student Learning Focus:
- 7.16 Systematic Procedures for Drawing Lewis Structures
- Student Learning Focus:
- Example 7.11 Drawing a Lewis Structure for a Molecular Compound, Using Systematic Procedures
- Solution
- Answer Double Check:
- Chemical Insight: Acid Rain
- Example 7.12 Drawing a Lewis Structure for a Polyatomic Ion, Using Systematic Procedures
- Solution
- Answer Double Check:
- Chemical Insight: Sodium Sulfite
- Example 7.13 Drawing a Lewis Structure for a Molecule That Has Resonance Forms
- Solution
- Answer Double Check:
- Chemical Insight: Ozone
- 7.17 Molecular Geometry
- Student Learning Focus:
- Electron Pairs versus Electron Groups
- Molecules with Two VSEPR Electron Groups
- Molecules with Three VSEPR Electron Groups
- Molecules with Four VSEPR Electron Groups
- Example 7.14 Using VSEPR Theory to Predict Molecular Geometry
- Solution
- Answer Double Check:
- 7.18 Electronegativity
- Student Learning Focus:
- Example 7.15 Predicting Electronegativity Relationships, Using General Periodic Table Trends
- Solution
- 7.19 Bond Polarity
- Student Learning Focus:
- Example 7.16 Predicting the Polarity Characteristics of Chemical Bonds
- Solution
- 7.20 Molecular Polarity
- Student Learning Focus:
- Example 7.17 Predicting the Polarity of Molecules Given Their Lewis Structure and Molecular Geometry
- Solution
- Chemical Insight: Hydrogen Sulfide
- Concepts to Remember
- Key Terms Listing
- Practice Problems by Topic
- Valence Electrons (Sec. 7.2)
- Lewis Symbols for Atoms (Sec. 7.2)
- Notation for Ions (Sec. 7.4)
- The Sign and Magnitude of Ionic Charge (Sec. 7.5)
- Lewis Structures for Ionic Compounds (Sec. 7.6)
- Chemical Formulas for Ionic Compounds (Sec. 7.7)
- Polyatomic-Ion-Containing Ionic Compounds (Sec. 7.9)
- Lewis Structures for Covalent Compounds (SECS. 7.10–7.15)
- Systematic Procedures for Drawing Lewis Structures (Sec. 7.16)
- Molecular Geometry (Vsepr Theory) (Sec. 7.17)
- Electronegativity (Sec. 7.18)
- Bond Polarity (Sec. 7.19)
- Molecular Polarity (Sec. 7.20)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 8 Chemical Nomenclature
- 8.1 Classification of Compounds for Nomenclature Purposes
- Student Learning Focus:
- Example 8.1 Classifying Compounds for Nomenclature Purposes
- Solution
- 8.2 Types of Binary Ionic Compounds
- Student Learning Focus:
- 8.3 Nomenclature for Binary Ionic Compounds
- Student Learning Focus:
- Fixed-Charge Binary Ionic Compounds
- Example 8.2 Naming Fixed-Charge Binary Ionic Compounds, Given Their Chemical Formulas
- Solution
- Answer Double Check:
- Example 8.3 Writing Chemical Formulas for Fixed-Charge Binary Ionic Compounds, Given Their Names
- Solution
- Answer Double Check:
- Variable-Charge Binary Ionic Compounds
- Example 8.4 Naming Variable-Charge Binary Ionic Compounds, Given Their Chemical Formulas
- Solution
- Answer Double Check:
- Example 8.5 Writing Chemical Formulas for Variable-Charge Binary Ionic Compounds, Given Their Names
- Solution
- Example 8.6 Naming Variable-Charge Binary Ionic Compounds Using the -ic, -ous System for denoting metal Ion charge
- Solution
- 8.4 Chemical Formulas for Polyatomic Ions
- Student Learning Focus:
- 8.5 Nomenclature for Ionic Compounds Containing Polyatomic Ions
- Student Learning Focus:
- Example 8.7 Naming Polyatomic-Ion-Containing Compounds, Given Their Chemical Formulas
- Solution
- Answer Double Check:
- Example 8.8 Writing Chemical Formulas for Polyatomic-Ion-Containing Compounds, Given Their Names
- Solution
- Answer Double Check:
- 8.6 Nomenclature for Binary Molecular Compounds
- Student Learning Focus:
- Example 8.9 Determining the Correct Order of Elemental Symbols in the Chemical Formula of a Binary Molecular Compound
- Solution
- Example 8.10 Naming Binary Molecular Compounds, Given Their Chemical Formulas
- Solution
- Common Names for Binary Molecular Compounds
- 8.7 Nomenclature for Acids
- Student Learning Focus:
- Example 8.11 Naming Hydrogen-Containing Compounds as Acids, Given Their Chemical Formulas
- Solution
- Answer Double Check:
- Example 8.12 Writing Chemical Formulas for Acids, Given Their Names
- Solution
- 8.8 Systematic Procedures for Using Nomenclature Rules
- Student Learning Focus:
- Example 8.13 Naming Compounds Given Their Chemical Formulas Using Systematic Procedures to Decide Which Nomenclature Rules Apply
- Solution
- Example 8.14 Writing Chemical Formulas for Compounds Given Their Names Using Systematic Procedures to Decide Which Nomenclature Rules Govern Each Situation
- Solution
- Concepts to Remember
- Key Terms Listing
- Practice Problems by Topic
- Nomenclature Classifications for Compounds (Sec. 8.1)
- Types of Binary Ionic Compounds (Sec. 8.2)
- Nomenclature for Binary Ionic Compounds (Sec. 8.3)
- Chemical Formulas for Polyatomic Ions (Sec. 8.4)
- Nomenclature for Polyatomic-Ion-Containing Compounds (Sec. 8.5)
- Nomenclature for Binary Molecular Compounds (Sec. 8.6)
- Nomenclature for Acids (Sec. 8.7)
- Systemic Procedures for Using Nomenclature Rules (Sec. 8.8)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 9 Chemical Calculations: The Mole Concept and Chemical Formulas
- 9.1 The Law of Definite Proportions
- Student Learning Focus:
- Example 9.1 Using Decomposition Data to Illustrate the Law of Definite Proportions
- Solution
- Chemical Insight: AMMONIA
- 9.2 Calculation of Formula Masses
- Student Learning Focus:
- Example 9.2 Using Chemical Formulas and Atomic Masses to Calculate Formula Masses
- Solution
- Chemical Insight: Ferric Oxide
- 9.3 Significant Figures and Formula Mass
- Student Learning Focus:
- Example 9.3 Treating Formula Mass Calculations as Addition Problems
- Solution
- Answer Double Check:
- 9.4 Mass Percent Composition of a Compound
- Student Learning Focus:
- Example 9.4 Using a Compound’s Chemical Formula to Calculate Its Percent by Mass Composition
- Solution
- Answer Double Check:
- Chemical Insight: Acetaminophen
- Example 9.5 Using Synthesis Data to Calculate Percent by Mass Composition
- Solution
- Answer Double Check:
- Chemical Insight: Adrenaline
- 9.5 The Mole: The Chemist’s Counting Unit
- Student Learning Focus:
- Example 9.6 Calculating the Number of Objects in a Molar Quantity
- Solution
- Answer Double Check:
- 9.6 The Mass of a Mole
- Student Learning Focus:
- Example 9.7 Calculating the Mass, in Grams, of a Molar Quantity
- Solution
- Answer Double Check:
- Summary of Mass Terminology
- Example 9.8 Calculating Molar Mass from Mass and Mole Data
- Solution
- Chemical Insight: Nitric Oxide
- 9.7 Significant Figures and Avogadro’s Number
- Student Learning Focus:
- 9.8 Relationship Between Atomic Mass Units and Gram Units
- Student Learning Focus:
- Example 9.9 Using the Relationship between Grams and Atomic Mass Units as a Conversion Factor
- Solution
- 9.9 The Mole and Chemical Formulas
- Student Learning Focus:
- Example 9.10 Calculating Molar Quantities of Compound Components
- Solution
- Answer Double Check:
- Chemical Insight: Menthol
- 9.10 The Mole and Chemical Calculations
- Student Learning Focus:
- Example 9.11 Calculating the Number of Particles in a Given Mass of Substance
- Solution
- Answer Double Check:
- Chemical Insight: Nicotine
- Example 9.12 Calculating the Mass of a Given Number of Particles of a Substance
- Solution
- Answer Double Check:
- Chemical Insight: Nitrogen Dioxide
- Example 9.13 Calculating the Mass of a Single Atom or a Single Molecule
- Solution
- Answer Double Check:
- Example 9.14 Calculating the Mass of an Element Present in a Given Mass of Compound
- Solution
- Answer Double Check:
- Chemical Insight: Caffeine
- Example 9.15 Calculating the Number of Atoms of an Element Present in a Given Mass of a Compound
- Solution
- Chemical Insight: Cholesterol
- 9.11 Purity of Samples
- Student Learning Focus:
- Example 9.16 Calculating Masses of Substances in an Impure Sample
- Solution
- Answer Double Check:
- Chemical Insight: Nitric Acid
- Example 9.17 Calculating Atoms of a Substance in an Impure Sample
- Solution
- Answer Double Check:
- Chemical Insight: Steel
- 9.12 Empirical and Molecular Formulas
- Student Learning Focus:
- Example 9.18 Obtaining Empirical Formulas from Molecular Formulas
- Solution
- Answer Double Check:
- 9.13 Determination of Empirical Formulas
- Student Learning Focus:
- Empirical Formulas from Direct Analysis Data
- Example 9.19 Determining an Empirical Formula from Percent by Mass Composition Data
- Solution
- Chemical Insight: Chlorofluorocarbons
- Example 9.20 Determining an Empirical Formula Using Mass Data
- Solution
- Answer Double Check:
- Chemical Insight: Ibuprofen and Naproxen
- Empirical Formulas from Indirect Analysis Data
- Example 9.21 Determining an Empirical Formula Using Combustion Analysis Data
- Solution
- Chemical Insight: Ethylene
- Example 9.22 Determining an Empirical Formula Using Combustion Analysis Data
- Solution
- Answer Double Check:
- Chemical Insight: Acetone
- 9.14 Determination of Molecular Formulas
- Student Learning Focus:
- Example 9.23 Calculating a Molecular Formula from an Empirical Formula and Molecular Formula Mass Data
- Solution
- Answer Double Check:
- Example 9.24 Calculating a Molecular Formula from Mass Percent Composition and Molecular Formula Mass Data
- Solution
- Chemical Insight: Natural Gas
- Concepts to Remember
- Key Terms Listing
- Practice Problems by Topic
- Law of Definite Proportions (Sec. 9.1)
- Formula Masses (Secs. 9.2 and 9.3)
- Mass Percent Composition (Sec. 9.4)
- The Mole: The Chemist’s Counting Unit (Sec. 9.5)
- Molar Mass (Sec. 9.6)
- Relationship Between Atomic Mass Units and Gram Units (Sec. 9.8)
- The Mole and Chemical Formulas (Sec. 9.9)
- The Mole and Chemical Calculations (Sec. 9.10)
- Purity of Samples (Sec. 9.11)
- Determination of Empirical Formulas (Secs. 9.13 and 9.14)
- Empirical Formula Determination Using Combustion Analysis (Sec. 9.13)
- Determination of Molecular Formulas (Sec. 9.14)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 10 Chemical Calculations Involving Chemical Equations
- 10.1 The Law of Conservation of Mass
- 10.2 Writing Chemical Equations
- 10.3 Chemical Equation Coefficients
- Example 10.1 Using Both Equation Coefficients and Chemical Formulas to Determine Number of Atoms Present
- Solution
- 10.4 Balancing Procedures for Chemical Equations
- Example 10.2 Balancing a Chemical Equation
- Solution
- Example 10.3 Balancing a Chemical Equation
- Solution
- Example 10.4 Deriving a Balanced Chemical Equation from Molecular Models of Reactants and Products
- Solution
- 10.5 Special Symbols Used in Chemical Equations
- 10.6 Classes of Chemical Reactions
- Synthesis Reactions
- Decomposition Reactions
- Single-Replacement Reactions
- Double-Replacement Reactions
- Example 10.5 Classification of Chemical Reactions into the Categories Synthesis, Decomposition, Single-Replacement, and Double-Replacement
- Solution
- Combustion Reactions
- Example 10.6 Writing and Balancing an Equation for a Combustion Reaction
- Solution
- 10.7 Chemical Equations and the Mole Concept
- Example 10.7 Calculating Molar Quantities Using a Balanced Chemical Equation
- Solution
- 10.8 Balanced Chemical Equations and the Law of Conservation of Mass
- Example 10.8 Verifying the Law of Conservation of Mass Using a Balanced Chemical Equation
- Solution
- 10.9 Calculations Based on Chemical Equations’Stoichiometry
- Example 10.9 Calculating the Needed Mass of a Reactant in a Chemical Reaction
- Solution
- Example 10.10 Calculating the Mass of a Product in a Chemical Reaction
- Solution
- Example 10.11 Calculating Moles of Product Produced in a Chemical Reaction
- Solution
- Example 10.12 Calculating the Amount of a Substance Produced in a Chemical Reaction
- Solution
- 10.10 The Limiting Reactant Concept
- Example 10.13 Determining a Limiting Reactant in a Nonchemical Context
- Solution
- Example 10.14 Determining the Limiting Reactant from Given Reactant Amounts
- Solution
- Example 10.15 Calculating the Mass of Product from Masses of Reactants
- Solution
- 10.11 Yields: Theoretical, Actual, and Percent
- Example 10.16 Calculating the Theoretical Yield and Percent Yield for a Chemical Reaction
- Solution
- 10.12 Simultaneous and Sequential Chemical Reactions
- Example 10.17 A Calculation Based on Simultaneous Chemical Reactions
- Solution
- Example 10.18 A Calculation Based on Sequential Chemical Reactions
- Solution
- Combining Sequential Chemical Reaction Equations into a Single Overall Chemical Reaction Equation
- Example 10.19 Combining Sequential Chemical Equations to Produce a Single Overall Chemical Equation
- Solution
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- The Law of Conservation of Mass (Sec. 10.1)
- Chemical Equation Notation (Secs. 10.2 and 10.5)
- Balancing Chemical Equations (Sec. 10.4)
- Classes of Chemical Reactions (Sec. 10.6)
- Chemical Equations and The Mole Concept (Sec. 10.7)
- Balanced Chemical Equations and The Law of Conservation of Mass (Sec. 10.8)
- Calculations Based on Chemical Equations (Sec. 10.9)
- Limiting Reactant Calculations (Sec. 10.10)
- Theoretical Yield and Percent Yield (Sec. 10.11)
- Simultaneous Chemical Reactions (Sec. 10.12)
- Sequential Chemical Reactions (Sec. 10.12)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 11 States of Matter
- 11.1 Factors that Determine Physical State
- Student Learning Focus:
- 11.2 Property Differences among Physical States
- Student Learning Focus:
- 11.3 The Kinetic Molecular Theory of Matter
- Student Learning Focus:
- 11.4 The Solid State
- Student Learning Focus:
- 11.5 The Liquid State
- Student Learning Focus:
- 11.6 The Gaseous State
- Student Learning Focus:
- 11.7 A Comparison of Solids, Liquids, and Gases
- Student Learning Focus:
- 11.8 Endothermic and Exothermic Changes of State
- Student Learning Focus:
- 11.9 Heat Energy and Specific Heat
- Student Learning Focus:
- Heat Energy Units
- Example 11.1 Interrelationships among Heat Energy Units
- Solution
- Answer Double Check:
- Chemical Insight: Ethyl Alcohol
- Specific Heat
- Example 11.2 Calculating the Amount of Heat Energy Absorbed by a Substance Undergoing a Specific Temperature Increase
- Solution
- Answer Double Check:
- Chemical Insights: Beryllium
- Example 11.3 Calculating the Temperature Change Caused by Addition of a Specific Amount of Heat Energy
- Solution
- Answer Double Check:
- Example 11.4 Using Heat Capacity Data to Calculate Specific Heat
- Solution
- Answer Double Check:
- Chemical Insight: Gold
- Example 11.5 Calculation Involving “Heat Lost Is Equal to Heat Gained.”
- Solution
- Answer Double Check:
- 11.10 Temperature Changes as a Substance is Heated
- Student Learning Focus:
- 11.11 Energy and Changes of State
- Student Learning Focus:
- Example 11.6 Calculating the Heat Energy Absorbed as a Substance Melts
- Solution
- Chemical Insight: Copper
- Example 11.7 Calculating the Heat of Vaporization from Given Thermochemical Data
- Solution
- Answer Double Check:
- 11.12 Heat Energy Calculations
- Student Learning Focus:
- Example 11.8 Thermochemical Calculation Involving Both Change of State and Change of Temperature
- Solution
- Answer Double Check:
- Example 11.9 Thermochemical Calculation Involving All Three States of Matter
- Solution
- Answer Double Check:
- 11.13 Evaporation of Liquids
- Student Learning Focus:
- Rate of Evaporation and Temperature
- Evaporation and Equilibrium
- 11.14 Vapor Pressure of Liquids
- Student Learning Focus:
- 11.15 Boiling and Boiling Points
- Student Learning Focus:
- Factors that Affect Boiling Point
- 11.16 Intermolecular Forces in Liquids
- Student Learning Focus:
- Dipole–Dipole Interactions
- Hydrogen Bonds
- Example 11.10 Predicting Whether Molecules Can Participate in Hydrogen Bonding
- Solution
- London Forces
- Ion–Dipole Interactions
- Ion–Ion Interactions
- 11.17 Hydrogen Bonding and The Properties of Water
- Student Learning Focus:
- Vapor Pressure
- Thermal Properties
- Density
- Surface Tension
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Physical States of Matter (Secs. 11.1 and 11.2)
- Kinetic Molecular Theory of Matter (Secs. 11.3–11.6)
- Physical Changes of State (Sec. 11.8)
- Heat Energy and Specific Heat (Sec. 11.9)
- Energy and Changes of State (Sec. 11.11)
- Heat Energy Calculations (Sec. 11.12)
- Properties of Liquids (Secs. 11.13–11.15)
- Intermolecular Forces in Liquids (Sec. 11.16)
- Hydrogen Bonding and The Properties of Water (Sec 11.17)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 12 Gas Laws
- 12.1 Properties of Some Common Gases
- Student Learning Focus:
- 12.2 Gas Law Variables
- Student Learning Focus:
- Example 12.1 Interconverting between Various Pressure Units
- Solution
- Answer Double Check:
- Pressure Readings and Significant Figures
- 12.3 Boyle’s Law: A Pressure–Volume Relationship
- Student Learning Focus:
- Example 12.2 Calculating Final Volume of a Gas Using Boyle’s Law with Pressure Values Given in the Same Units
- Solution
- Answer Double Check:
- Example 12.3 Calculating Final Volume of a Gas Using Boyle’s Law with Pressure Values Given in Different Units
- Solution
- Answer Double Check:
- 12.4 Charles’s Law: A Temperature–Volume Relationship
- Student Learning Focus:
- Example 12.4 Calculating Final Volume of a Gas Using Charles’s Law
- Solution
- Answer Double Check:
- 12.5 Gay-Lussac’s Law: A Temperature–Pressure Relationship
- Student Learning Focus:
- Example 12.5 Calculating Final Temperature of a Gas Using Gay-Lussac’s Law
- Solution
- Answer Double Check:
- 12.6 The Combined Gas Law
- Student Learning Focus:
- Example 12.6 Mathematical Manipulation of the Combined Gas Law
- Solution
- Example 12.7 Calculating Final Volume of a Gas Using the Combined Gas Law
- Solution
- Answer Double Check:
- Chemical Insight: Hydrogen
- Example 12.8 Calculating Final Temperature of a Gas Using the Combined Gas Law
- Solution
- Answer Double Check:
- Chemical Insight: Helium
- 12.7 Avogadro’s Law
- Student Learning Focus:
- Example 12.9 Calculating Final Volume of a Gas Using Avogadro’s Law
- Solution
- Answer Double Check:
- Chemical Insight: Helium
- Example 12.10 Calculating Final Volume of a Gas When None of the Other Gas Law Variables Are Constant
- Solution
- Answer Double Check:
- Chemical Insight: Nitrogen
- 12.8 An Ideal Gas
- Student Learning Focus:
- 12.9 The Ideal Gas Law
- Student Learning Focus:
- Example 12.11 Calculating the Volume of a Gas Using the Ideal Gas Law
- Solution
- Answer Double Check:
- Chemical Insight: Carbon Monoxide
- Example 12.12 Calculating the Temperature of a Gas Using the Ideal Gas Law
- Solution
- Answer Double Check:
- Chemical Insight: Nitrous Oxide
- 12.10 Modified Forms of the Ideal Gas Law Equation
- Student Learning Focus:
- The Molar Mass of a Gas
- Example 12.13 Calculating the Molar Mass of a Gas Using the Ideal Gas Law in Modified Form
- Solution
- Answer Double Check:
- Chemical Insight: Chlorine
- The Density of a Gas
- Example 12.14 Calculating the Density of a Gas Using the Ideal Gas Law in Modified Form
- Solution
- Using Density to Calculate Molar Mass
- Example 12.15 Calculating the Molar Mass of a Gas Given Its Density
- Solution
- Answer Double Check:
- 12.11 Volumes of Gases in Chemical Reactions
- Student Learning Focus:
- Example 12.16 Using Gay-Lussac’s Law of Combining Volumes to Determine Reactant–Product Volume Relationships
- Solution
- Answer Double Check:
- Chemical Insight: Ammonia
- 12.12 Volumes of Gases and The Limiting Reactant Concept
- Student Learning Focus:
- Example 12.17 Calculating a Limiting Reactant Using Volumes of Gases
- Solution
- Answer Double Check:
- Chemical Insight: AcetylenE
- 12.13 Molar Volume of a Gas
- Student Learning Focus:
- Example 12.18 Calculating the Molar Volume of a Gas
- Solution
- Answer Double Check:
- Example 12.19 Calculating the Molar Volume of a Gas
- Solution
- Answer Double Check:
- Standard Temperature and Standard Pressure Conditions
- Using Molar Volume to Calculate Density
- Example 12.20 Calculating Density Using Molar Volume and Molar Mass
- Solution
- Chemical Insight: Hyrdogen Cyanide
- 12.14 Chemical Calculations Using Molar Volume
- Student Learning Focus:
- Example 12.21 Calculating the Volume of a Gas at STP Given Its Mass
- Solution
- Answer Double Check:
- Chemical Insight: FlUOrine
- Example 12.22 Calculating the Mass of a Gas Given Its Volume
- Solution
- Answer Double Check:
- Example 12.23 Calculating the STP Volume of a Gaseous Reactant in a Chemical Reaction
- Solution
- Answer Double Check:
- Chemical Insight: Lithium
- Example 12.24 Calculating the Mass of a Reactant from the Volume of a Gaseous Product
- Solution
- Chemical Insight: Oxygen
- Example 12.25 Calculating Gaseous Product Volume from Gaseous Reactant Volumes
- Solution
- Chemical Insight: Nitrogen
- 12.15 Mixtures of Gases
- Student Learning Focus:
- Example 12.26 Applying the Ideal Gas Law to a Mixture of Gases
- Solution
- Answer Double Check:
- 12.16 Dalton’s Law of Partial Pressures
- Student Learning Focus:
- Example 12.27 Using Dalton’s Law to Calculate a Partial Pressure
- Solution
- Example 12.28 Calculating the Mole Fraction for a Gas in a Gaseous Mixture
- Solution
- Answer Double Check:
- Example 12.29 Calculating Partial Pressures Using Mole Fractions
- Solution
- Answer Double Check:
- Example 12.30 Calculating the Partial Pressure of a Gas Using the Ideal Gas Law
- Solution
- Answer Double Check:
- Example 12.31 Calculating the Partial Pressure of a Gas Collected over Water
- Solution
- Example 12.32 Expressing Gaseous Mixture Composition in Mole Percent, Pressure Percent, and Volume Percent
- Solution
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Measurement of Pressure (Sec. 12.2)
- Boyle’s Law (Sec. 12.3)
- Charles’s Law (Sec. 12.4)
- Gay-Lussac’s Law (Sec. 12.5)
- The Combined Gas Law (Sec. 12.6)
- Avogadro’s Law (Sec. 12.7)
- The Ideal Gas Law (Sec. 12.9)
- Modified Forms of the Ideal Gas Law Equation (Sec. 12.10)
- Volumes of Gases in Chemical Reactions (Sec. 12.11)
- Volumes of Gases and The Limiting Reactant Concept (Sec. 12.12)
- Molar Volume of a Gas (Sec. 12.13)
- Chemical Calculations Using Molar Volume (Sec. 12.14)
- Mixtures of Gases (Sec. 12.15)
- Dalton’s Law of Partial Pressures (Sec. 12.16)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 13 Solutions
- 13.1 Characteristics of Solutions
- Student Learning Focus:
- 13.2 Solubility
- Student Learning Focus:
- Effect of Temperature on Solubility
- Effect of Pressure on Solubility
- Terminology for Relative Amount of Solute in a Solution
- Aqueous and Nonaqueous Solutions
- 13.3 Solution Formation
- Student Learning Focus:
- Factors Affecting the Rate of Solution Formation
- 13.4 Solubility Rules
- Student Learning Focus:
- Example 13.1 Using Solubility Guidelines to Predict Compound Solubilities
- Solution
- 13.5 Solution Concentrations
- Student Learning Focus:
- 13.6 Percentage Concentration Unit
- Student Learning Focus:
- Example 13.2 Calculating Mass Percent Concentration from Mass of Solute and Mass of Solvent
- Solution
- Answer Double Check:
- Chemical Insight: Sucrose
- Example 13.3 Calculating the Percent by Volume Concentration of a Solution
- Solution
- Answer Double Check:
- Chemical Insight: Methyl Alcohol
- Using Percent Concentrations as Conversion Factors
- Example 13.4 Calculating the Mass of Solute Necessary to Produce a Solution of a Given Mass Percent Concentration
- Solution
- Answer Double Check:
- Chemical Insight: Iodine
- Example 13.5 Calculating the Mass of Solute Present in a Solution of a Given Mass–Volume Percent Concentration
- Solution
- Answer Double Check:
- Chemical Insight: Vinegar
- Example 13.6 Calculating the Volume of Solution Necessary to Supply a Given Mass of Solute Using Density and Mass Percent Concentration
- Solution
- Answer Double Check:
- 13.7 Parts Per Million and Parts Per Billion Concentration Units
- Student Learning Focus:
- Example 13.7 Expressing Concentrations in Parts per Million and Parts per Billion
- Solution
- Answer Double Check:
- Chemical Insight: Fluoridation
- Example 13.8 Calculating the Volume of Solute Present Given a Parts per Million Concentration
- Solution
- Chemical Insight: Carbon Monoxide
- 13.8 Molarity Concentration Unit
- Student Learning Focus:
- Example 13.9 Calculating the Molarity of a Solution from Mass/Amount and Volume Data
- Solution
- Answer Double Check:
- Using Molarity as a Conversion Factor
- Example 13.10 Calculating the Amount of Solute Present in a Given Amount of Solution Using Molarity as a Conversion Factor
- Solution
- Answer Double Check:
- Chemical Insight: Citric Acid
- Example 13.11 Calculating the Amount of Solution Necessary to Supply a Given Amount of Solute
- Solution
- Chemical Insight: Iron
- Example 13.12 Calculating Molarity from Density and Percent by Mass
- Solution
- Example 13.13 Using Molarity and Density to Calculate the Amount of Solvent Present in a Solution
- Solution
- Answer Double Check:
- Chemical Insight: Sulfuric Acid
- 13.9 Molarity and Chemical Reactions in Aqueous Solution
- Student Learning Focus:
- Example 13.14 Calculating the Volume of a Reactant Given the Volume and Concentration of Another Reactant
- Solution
- Answer Double Check:
- Example 13.15 Calculating the Volume of a Solution of Known Concentration Needed to React With a Known Mass of Another Reactant
- Solution
- Answer Double Check:
- Example 13.16 Calculating a Product Amount Given Two Reactant Solution Volumes
- Solution
- Answer Double Check:
- Example 13.17 Calculating the Gaseous Volume of a Product from the Solution Volume of a Reactant
- Solution
- 13.10 Dilution Calculations
- Student Learning Focus:
- Example 13.18 Calculating the Molarity of a Solution After It Has Been Diluted
- Solution
- Answer Double Check:
- Chemical Insight: Nitric Acid
- Example 13.19 Calculating the Amount of Solvent That Must Be Added to a Solution to Dilute It to a Specified Concentration
- Solution
- Answer Double Check:
- Example 13.20 Calculating Molarity when Two Like Solutions of Differing Concentration Are Mixed
- Solution
- Answer Double Check:
- Chemical Insight: Hydrochloric Acid
- 13.11 Molality Concentration Unit
- Student Learning Focus:
- Example 13.21 Calculating the Molality of a Solution
- Solution
- Answer Double Check:
- Chemical Insight: Common Salt
- Example 13.22 Calculating the Amount of Solute Needed to Prepare a Solution of Specified Molality
- Solution
- Answer Double Check:
- Chemical Insight: Isopropyl Alcohol
- Example 13.23 Calculating Molarity from Molality and Density
- Solution
- Answer Double Check:
- Example 13.24 Calculating Molality from Molarity and Density
- Solution
- Answer Double Check:
- Chemical Insight: Lactose
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Characteristics of Solutions (Sec. 13.1)
- Solubility (Sec. 13.2)
- Solution Formation (Sec. 13.3)
- Solubility Rules (Sec. 13.4)
- Mass Percent (Sec. 13.6)
- Volume Percent (Sec. 13.6)
- Mass–Volume Percent (Sec. 13.6)
- Parts Per Million and Parts Per Billion (Sec. 13.7)
- Molarity (Sec. 13.8)
- Molarity and Chemical Equations (Sec. 13.9)
- Dilution (Sec. 13.10)
- Molality (sec 13.11)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 14 Acids, Bases, and Salts
- 14.1 Arrhenius Acid–Base Theory
- Student Learning Focus:
- 14.2 Brønsted–Lowry Acid–Base Theory
- Student Learning Focus:
- 14.3 Conjugate Acids and Bases
- Student Learning Focus:
- Example 14.1 Determining the Members of a Conjugate Acid–Base Pair
- Solution
- Answer Double Check:
- Example 14.2 Determining the Formula of One Member of a Conjugate Acid–Base Pair when Given the Other Member
- Solution
- Answer Double Check:
- Amphiprotic Substances
- 14.4 Mono-, Di-, and Triprotic Acids
- Student Learning Focus:
- 14.5 Strengths of Acids and Bases
- Student Learning Focus:
- 14.6 SALTS
- Student Learning Focus:
- 14.7 Reactions of Acids
- Student Learning Focus:
- Reaction with Metals
- Reaction with Bases
- Reaction with Carbonates and Bicarbonates
- 14.8 Reactions of Bases
- Student Learning Focus:
- 14.9 Reactions of Salts
- Student Learning Focus:
- Reaction with Metals
- Reaction with Acids
- Reaction with Bases
- Reaction of Salts with Each Other
- Example 14.3 Predicting Whether a Reaction Will Occur and Writing an Equation for the Reaction If It Does Occur
- Solution
- Answer Double Check:
- 14.10 Self-Ionization of Water
- Student Learning Focus:
- Ion Product Constant for Water
- Effect of Solutes on Water Self-Ionization
- Example 14.4 Calculating the Hydroxide Ion Concentration of a Solution with a Known Hydronium Ion Concentration
- Solution
- Answer Double Check:
- Effect of Temperature Change on Water Self-Ionization
- Acidic, Basic, and Neutral Solutions
- 14.11 The pH Scale
- Integral pH Values
- Example 14.5 Calculating the pH of a Solution when Given Its Hydronium Ion or Hydroxide Ion Concentration
- Solution
- Nonintegral pH Values
- Example 14.6 Calculating the pH of a Solution Given Its Hydronium Ion Concentration
- Solution
- Answer Double Check:
- Example 14.7 Calculating the Molar Hydronium Ion Concentration of a Solution from the Solution’s pH
- Solution
- Answer Double Check:
- 14.12 Hydrolysis of Salts
- Student Learning Focus:
- Types of Salt Hydrolysis
- Example 14.8 Predicting Whether a Salt’s Aqueous Solution Will Be Acidic, Basic, or Neutral
- Solution
- Chemical Equations for Salt Hydrolysis Reactions
- Example 14.9 Writing Chemical Equations for Hydrolysis Reactions
- Solution
- 14.13 Buffers
- Student Learning Focus:
- Example 14.10 Recognizing Pairs of Chemical Substances that Can Function as a Buffer in an Aqueous Solution
- Solution
- Answer Double Check:
- Chemical Equations for Buffer Action
- Example 14.11 Writing Equations for Reactions that Occur in a Buffered Solution
- Solution
- Answer Double Check:
- 14.14 Acid–Base Titrations
- Student Learning Focus:
- Example 14.12 Calculating an Unknown Molarity, Using Acid–Base Titration Data
- Solution
- Answer Double Check:
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Acid–Base Definitions (Secs. 14.1 and 14.2)
- Conjugate Acids and Bases (Sec. 14.3)
- Mono-, Di-, and Triprotic Acids (Sec. 14.4)
- Strength of Acids and Bases (Sec. 14.5)
- Salts (Sec. 14.6)
- Reactions of Acids and Bases (Secs. 14.7 and 14.8)
- Reactions of Salts (Sec. 14.9)
- Hydronium Ion and Hydroxide Ion Concentrations (Sec. 14.10)
- The pH Scale (Sec. 14.11)
- Hydrolysis of Salts (Sec. 14.12)
- Buffers (Sec. 14.13)
- Acid–Base Titrations (Sec. 14.14)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Chapter 15 Chemical Equations: Net Ionic and Oxidation–Reduction
- 15.1 Types of Chemical Equations
- Student Learning Focus:
- 15.2 Electrolytes
- Student Learning Focus:
- 15.3 Ionic and Net Ionic Equations
- Student Learning Focus:
- Example 15.1 Converting a Molecular Equation into a Net Ionic Equation
- Solution
- Answer Double Check:
- Example 15.2 Converting a Molecular Equation into a Net Ionic Equation
- Solution
- Answer Double Check:
- Example 15.3 Converting a Molecular Equation into a Net Ionic Equation
- Solution
- Answer Double Check:
- 15.4 Oxidation–Reduction Terminology
- Student Learning Focus:
- 15.5 Oxidation Numbers
- Student Learning Focus:
- Example 15.4 Assigning Oxidation Numbers to Elements in a Compound or Polyatomic Ion
- Solution
- Answer Double Check:
- Example 15.5 Determining Oxidation Numbers and Identifying Oxidizing Agents and Reducing Agents
- Solution
- Answer Double Check:
- 15.6 Redox and Nonredox Chemical Reactions
- Student Learning Focus:
- Example 15.6 Classifying Chemical Reactions as Redox or Nonredox
- Solution
- 15.7 Balancing Oxidation–Reduction Equations
- Student Learning Focus:
- 15.8 Oxidation Number Method for Balancing Redox Equations
- Student Learning Focus:
- Example 15.7 Balancing a Molecular Redox Equation Using the Oxidation Number Method
- Solution
- Answer Double Check:
- Example 15.8 Balancing a Net Ionic Redox Equation Using the Oxidation Number Method
- Solution
- Answer Double Check:
- Example 15.9 Balancing a Net Ionic Redox Equation Using the Oxidation Number Method
- Solution
- Answer Double Check:
- 15.9 Half-Reaction Method for Balancing Redox Equations
- Student Learning Focus:
- Example 15.10 Balancing a Net Ionic Redox Equation Using the Half-Reaction Method
- Solution
- Answer Double Check:
- Example 15.11 Balancing a Net Ionic Redox Equation Using the Half-Reaction Method
- Solution
- Answer Double Check:
- Example 15.12 Balancing a Net Ionic Redox Equation Using the Half-Reaction Method
- Solution
- Answer Double Check:
- 15.10 Disproportionation Reactions
- Student Learning Focus:
- Example 15.13 Balancing a Disproportionation Redox Equation
- Solution
- Answer Double Check:
- 15.11 Stoichiometric Calculations Involving Ions
- Student Learning Focus:
- Example 15.14 Calculating the Mass of an Ion Present in a Solution
- Solution
- Example 15.15 Calculating the Volume of Solution Needed to Supply a Given Amount of an Ion
- Solution
- Answer Double Check:
- Example 15.16 Calculating the Volume of Solution Needed for a Reaction Involving Ions
- Solution
- Answer Double Check:
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Electrolytes (Sec. 15.2)
- Ionic and Net Ionic Equations (Sec. 15.3)
- Oxidation–Reduction Terminology (Secs. 15.4 and 15.5)
- Oxidation Numbers (Sec. 15.5)
- Characteristics of Oxidation–Reduction Reactions (Sec. 15.5)
- Redox and Nonredox Chemical Reactions (Sec. 15.6)
- Balancing Redox Equations: Oxidation Number Method (Sec. 15.8)
- Balancing Redox Equations: Half-Reaction Method (Sec. 15.9)
- Balancing Redox Equations: Disproportionation Reactions (Sec. 15.10)
- Stoichiometric Calculations Involving Ions (Sec 15.11)
- Multi-Concept Problems
- Multiple-Choice Practice Test
- Chapter 16 Reaction Rates and Chemical Equilibrium
- 16.1 Collision Theory
- Student Learning Focus:
- Molecular Collisions
- Activation Energy
- Collision Orientation
- 16.2 Endothermic and Exothermic Chemical Reactions
- Student Learning Focus:
- 16.3 Factors that Influence Chemical Reaction Rates
- Student Learning Focus:
- Physical Nature of Reactants
- Reactant Concentration
- Reaction Temperature
- Presence of Catalysts
- 16.4 Chemical Equilibrium
- Student Learning Focus:
- 16.5 Equilibrium Mixture Stoichiometry
- Student Learning Focus:
- Example 16.1 Determining the Composition of an Equilibrium Mixture in Terms of Moles of Each Substance Present
- Solution
- Answer Double Check:
- 16.6 Equilibrium Constants
- Student Learning Focus:
- Example 16.2 Using Balanced Chemical Equations to Determine Equilibrium Constant Expressions
- Solution
- Answer Double Check:
- Example 16.3 Using Equilibrium Concentrations to Calculate the Value of an Equilibrium Constant
- Solution
- Answer Double Check:
- 16.7 Equilibrium Position
- Student Learning Focus:
- 16.8 Temperature Dependency of Equilibrium Constants
- Student Learning Focus:
- 16.9 Le Châtelier’s Principle
- Student Learning Focus:
- Concentration Changes
- Henri-Louis Le Châtelier (1850–1936)
- Temperature Changes
- Pressure Changes
- Addition of a Catalyst
- Example 16.4 Using Le Châtelier’s Principle to Predict the Effects of Changes on the Equilibrium Position in an Equilibrium System
- Solution
- 16.10 Forcing Chemical Reactions to Completion
- Student Learning Focus:
- Concepts to Remember
- Key Terms Listing
- Practice Problems By Topic
- Collision Theory (Sec. 16.1)
- Endothermic and Exothermic Chemical Reactions (Sec. 16.2)
- Factors that Influence Chemical Reaction Rates (Sec. 16.3)
- Chemical Equilibrium (Sec. 16.4)
- Equilibrium Mixture Stoichiometry (Sec. 16.5)
- Equilibrium Constants (Sec. 16.6)
- Le Châtelier’s Principle (Sec. 16.9)
- Multi-Concept Problems
- Multiple Choice Practice Test
- Glossary
- Answers to Odd-Numbered Practice Problems
- Credits
- Index
- A
- B
- C
- D
- E
- F
- G
- H
- I
- J
- K
- L
- M
- N
- O
- P
- Q
- R
- S
- T
- U
- V
- W
- Y
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