Chemistry Bernice Segal

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Bernice G. Segal

BARNARD COLLEGE

COLUMBIA UNIVERSITY

Chemistry

Experiment

and Theory

Second Edition

John Wiley Sons

NEW YORK • CHICHESTER • BRISBANE • TOR ON TO • SINGAPO RE



Detailed Contents

Introduction

1

Some Fundamental Definitions

2

Units of Measurement

4

Mass and Weight 5

Length 6

Volume 6

Density 7

Temperature 8

Physical and Chemical Properties

10

Intensive and Extensive Propertie s 10

Dimensional

A nalysis

10

Significant Figures

12

Rounding Numbers

13

Determining the Number of Significant

Figures in a Calculated Value

14

Exact versus Experimental Numbers

16

Computational

Techniques

16

Problems

18

Chapter 1 Atom ic S tructure and

Stiochiometry 22

1.1

Subatomic Particles and the Structure of

Atoms 23

1.2 Isotopes ofan Element 25

1.3 The

Atomic Weight Scale

25

4

Avogadro's Numb er and the Concept ofa

Mole

28

1.5

Molecular Formulas and Molecular

Weightsfor Discrete Molecules

30

1.6

The Significance o f Molecular Formulas

and Molecular Weigh ts for Ionic Crystalline

Solids

34

1.7

Distinction between the Terms Molecular

Weight, Formula Weight, and Gram Atomic

Weight

36

1.8 Empirical Formulas 37

1.9 The Significance ofBalanced Chem ical

Equations

39

Significance of the CoefBcients in a Balanced

Equation 42

1.10

Stoichiometric Calculations

46

1.11

The Limiting Reagent and the Yield of

Product 51

Summary 54

Exercises 55

Multiple Choice Q uestions 58

Problems

59

Chapter 2 Introduction to the Periodic Table,

Some Families of Elements, and Inorganic

Nomendature 63

2.1

The Sections ofthe Periodic Table

64

2.2

The Metals

67

The Active Me tals 69

2.3

The Noble Gases

71

2.4

The Nonm etals

72

The Halogens 73

The Chalcogens 74

2.5 The Unique Position ofHydrogen 76

2.6 The Transition Metals 11

2.7

Ionic Crystalline Solids

78

2.8

M olecular Compounds

78

2.9

Some Simple

Inorganic

Nomendature

80

2.10

Nonstoichiometric Compounds

83

Summary

84

Multiple Choice Q uestions

85

Problems

86

Chapter 3 T he Gas Laws and Stoichiometry

Involving Gases 89

3.1

Avogadro's Law a nd Its Use in

Determining

Molecular

Formulas

90

Avogadro s Law 90

3.2

The Pressure of Gases: D efinition,

Measurement, and U nits

93

3.3

Boyle's Law

96

3.4

The Law of Charles and Gay-Lussac

100

3.5

The Ideal Gas L aw

103

3.6

Dalton 's Law ofPartial Pressures

110

Summary

116

XV



xv i Detailed Contents

Exercises 116

Multiple Cho ice Q uestions

119

Problems

120

Chapter

4

The Properties

of

Gases

and

the

Kinetic -

Molecular Theory

125

4 1 The Postulates ofthe Kinetic Theory of

Gases 126

4.2

Correlations between the Observed

Properties of Gases and the Postulates ofthe

Kinetic-Molecular Theory 127

4.3

A Critical Look a t Two ofthe Postulates of

the Kinetic Theory of Gases

129

4 4

An Outline ofthe Derivation ofBoyle's

Lawfrom the Postulates of Kinetic Th eory

131

4 5 The Kinetic Theory of Temperature 135

4.6

Energy U nits for PV and RT

136

4.7

The Mean-Square Speed, the Root-Mean-

Square

Speed,

and the Mean Speed

139

4.8

Graham 's Law ofEffusion 141

4.9

The Distribution of Molecular

Velocities

144

4 10

van der W aals' Equation

145

Summary 149

Exercises

150

Multiple Choice Questions 151

Problems 153

Chapter

5

Intermolecular

Forces,

Condensed

Phases, and

Changes

of Phase 156

5 1

van der Waals Forces

157

Dipole-Dipole Interactions 157

London or Dispersion Forces 160

5.2

The Hydrogen Bond 162

5.3

The Intermolecular Potential Energy

Function

165

5 4 Molecular Arrangements

in the

Solid,

Liquid,

and Gaseous States

166

5 5 Vaporization, Fusion, and

Sublimation

167

Vaporization 167

Fusion 168

Sublimation 168

5.6

The Equilibrium between a Liquid and Its

Vapor 169

The Equilibrium Vapor Pressu re 170

5.7

The Nature ofthe Equilibrium S tate: The

Tendency to Decrease the Potential Energy

and to Increase Molecular Disorder

173

5 8 A Summary of Properties ofthe

Equilibrium State

174

5.9

The Temperature Dependence ofthe

Equilibrium Vapor Pressure and the Normal

Boiling Point 175

The Normal Boiling Point 176

5 10 Phase Diagramsfor Pure Substances 177

The Vapor Pressure of Solids 177

One-Component Phas e Diagrams 178

Critical Temp erature and Pressure 180

Summary 181

Exercises

182

Multiple Cho ice Qu estions

186

Chapter 6 Properties ofDilute Solutions 189

6 1

Dynam ic Equilibrium in Saturated

Solutions

190

Saturated and Unsaturated Solutions 190

Equilibrium in Saturated Solutions 190

6.2

C oncen tration Un its for Solutions

192

The Mole Fraction 192

The Molality 193

The Molarity 194

Formality versus Mo larity 198

Weight Percentage 199

6.3

The Vapor Pressure ofa Solution of a

Nonvolatile

Solute in a

Volatile

Solvent:

Raoult 's Law

200

Raoult s Law 200

6.4

The Elevation ofthe Boiling Point of

Dilute Solutions ofa Non volatile Solute 203

6.5

The Depression o fthe Freezing Point of

Dilute Solutions ofa Nonvolatile Solute

205

6.6

Freezing Point Depressions and Boiling

Point Elevations for Solutions of

Electrolytes

208

6.7

Osmotic Pressure

210

6.8

Solutions of Two Volatile Liquids

212

Fractional Distillation 215

Nonideal Solutions 216



Detailed Contents xvii

6.9 Henry's Law

218

Summary 219

Exercises 220


223

Problems TLA

Chapter 7 Aqueous Solutions

and Ionic

Reactions 228

7 1 The Role of Water as a Solven t for Ionic

Crystalline Solids 229

The Dipole Moment of Water and the Hydration of

Ions 229

The Dielectric Constant of Wa ter 231

7.2 Nonelectrolytes 233

7.3 Strong and W eak Electrolytes 234

Acids 235

Bases 235

Salts 236

7.4 Proton-Transfer

Reactions:

The

Br0nsted-

Lowry Theory ofAcids and Bases

237

Acidic Hydrogen Atoms 240

7 5

A Summ ary of Information about the

Solubilities of Electrolytes in Water

241

7.6 Writing Correctly Balanced Net Ionic

Equations 242

7.7 Stoichiometry of Ionic R eactions in

Aqueous Solutions

247

Summary 252

Exercises

253

Multiple Choice Questions

255

Problems 257

Chapter

8

Introduction

to the Law of

Chemical Equilibrium

260

8 1 The Ideal Law of Chemical Equilibrium

or the Law ofMass Action 261

The Equilibrium Constant for a Gas-P hase Reaction:

K,aaAK

c

262

Reactions in Aqueous Solution in Wh ich W ater is a

Reactant or Product 264

Equilibrium Constants for Heterogeneous

Reactions 265

8.2 The Magnitude ofthe Equilibrium

Constant and the Direction o f Reac tion 266

The Reaction Quotient, ß 267

The Significance of the Magnitude of

K„,

268

8.3 Factors Ajfecting the Eq uilibrium

Constant

271

8.4

Le Chatelier's Principle

272

1. The Effect on a System at E quilibrium of Changing

the Concentration of One of the Reacting Species 272

Dissolving Solids That are Insoluble in Pure

Water 273

Removing an Ion from Solution by Precipitation of an

Insoluble Salt Containing Tha t Ion 274

2. Pressure Effects for Gas-P hase Reactions 275

3.

The Effect of a Change in Tem perature 276

8.5 Numerical Values of Equilibrium

Con stants for Rea ctions W ritten in the Reverse

Direction and for Simultaneous

Equilibria 279

The Effect of Reversing the Equilibrium Equation 279

The Effect of Mu ltiplying an Equation by a

Constant 280

Simultaneous Equilibria 281

8.6 Some Typical Problems in Gas-Phase

Equilibria 283

Summary 286

Exercises

287

Multiple Choice Qu estions 292

Problems 294

Chapter

9 Acids, Bases, and Salts 298

9 1 The Ion Product of Water and the pH

Scale 299

Self-Ionization Reactions 299

The Ion Product of W ater, K

w

300

The pH Scale 301

9.2 Weak Acids and Bases 305

The Acidity Co nstant,

K„

305

The Basicity Constant, K

b

305

The Degree of Dissociation, a 306

9 3 Conjugate Acids and B ases and Their

Relative Strengths 313

9.4 Weak Polyprotic Acids

316

9.5 A cidic, Basic, and Ne utral Salts 318

Acidic Salts 318

Basic Salts 320

Neutral Salts 321

Salts of Both a Weak Acid and a Weak B ase 323

Ampholytes 323

Acidic and Basic Oxides 324

9.6 The Leveling Effect of Water on the

Strengths of Strong Acids and Bases 326



Detailed Contents xix

13 2 The Spin Quantum Number and the

Pauli Exclusion Principle

453

13 3 The Aufbau Process and the Periodic

Table

456

The Building-Up (Aufbau) of the Periodic Table 457

13 4

Group 18

(VIIIA),

The Noble Gases: The

Relationship between Their Chem istry and

Their Electronic Configurations 460

13 5

The Periods ofthe Periodic Table and the

Electronic Configurations ofthe First Series of

Transition Metals

462

Transition M etal Ions 463

The Long Periods of the Periodic Table 463

13.6

A

Periodic Property:

The Ionization

Energy 466

13.7 A Periodic Property: The Electron

Affinity

469

13 8 A Periodic Property: The

Electronegativity 470

13.9

A Periodic

Property:

Atomic Size

471

13 10 Periodicity in

Bonding:

Ionic versus

Covalent Bonding Across the Short

Periods 473

Lewis Dot Formulas 473

Validity of the Octet Rule 474

Electronegativity and Bond Type 474

13 11

The Relationship between the Chemistry

and the Electronic Configurations ofthe Alkali

and the Alkaline Earth Metals

476

The Alkali Metals 476

The Alkaline Earth Me tals 477

13 12

T he Halogens: The Relationship

between Their Chemistry and Their Electronic

Configurations 480

13 13 The Chalcogens (O xygen Family): The

Relationship between Their Chem istry and

Their Electronic Configurations

481

Isoelectronic Ions 482

Summary

482

Exercises 485

Multiple Choice Qu estions

487

Problems 490

Chapter

14

The Nature

ofthe

Chemical

Bond 492

14 1 Ionic versus Covalent Bonding 493

14 2 Lewis Structures 496

Multiple Bonds 496

Formal Charges 499

The Concept of Resonance 500

Exceptions to the Octet Rule 502

Species with an Odd Number of Valence

Electrons 502

Electron Deflcient Compounds 502

Expanded Valence Shells 503

14 3

Valence-Shell Electron-Pair Repulsion

(VSEPR) Theory

504

14 4

Mo lecular Orbitals

ofH

2

511

Sigma (<r)-Molecular Orbita ls 512

The Bonding Molecular Orb ital 512

The Potential Energy Curve for H

2

513

Molecular Orbitals as Linear Combinations of Atomic

Orbitals 514

Species with Valence Electrons in the a ls and

a*ls

Molecular Orbitals 515

The Species H

2

and He

2

515

14 5 Hom onuclear Diatomic Molecules ofthe

Second Period

516

The a ls and a*2s Molecular Orbitals 516

7t-Molecular Orb itals 517

Bonding in B

2

, C

2

, and N

2

519

Bonding in 0

2

522

14 6

Heteronuclear Diatomic Molecules ofthe

Second Period

523

14 7

Hybrid Atomic Orbitals and the

Molecular Geom etry of Polyatomic

Molecules 525

14 8

M ultiple Bonds

533

Delocalized Orb itals 534

4 9

Hydrogen Bridge Bonds; the Boranes

537

Summary 537

Exercises 541

Multiple Cho ice Q uestions

542

Problems 544

Chapter

15 O xidation States and

Oxidation

-

Reduction Reactions 547

15 1 D efinitions of Oxidation and

Reduction

548

15 2 The Oxidation State ofan Element 549

Formal Charge versus Oxidation State 551

Intermediate Oxidation State s 552

Fractional Oxidation State s 552

The Oxidation State as a Periodic Property 553



xx Detailed Contents

15 3

Balancing Oxidation-Reduction

Equations

554

The Ion - Electron Method 560

Balancing Oxidation-Reduction Equations in Basic

Solution 562

Disproportionation 563

15 4 The Redox Chemistry of Group 15 (VA)

Elements 565

The Oxidation States of Phosphorus 570

The Oxidation States of

A s,

Sb, and Bi 571

15 5

The Oxidation States of Chlorine and

Other Group 17 (VIIA) Elements

572

Other Halogens 575

15 6 Oxidation States ofthe Transition Me tals

Chromium and Manganese 575

Redox Chemistry of Chromium 575

Redox Chemistry of Man ganese 577

Summary 578

Exercises 579


581

Problems

583

Chapter 16 Energy, E nthalpy, and

Thermochemistry 586

16 1 State Functions 587

16 2 Heat and Work 588

Work 588

Sign Convention for Wo rk 588

The Work of Expansion 589

Heat 591

The Mechanical Equivalent of Hea t 592

16 3

The First Law of Thermodynamics

593

Statements of the First Law of Thermodynam ics 595

16 4 E nergy and Enthalpy 595

Reactions Carried Out at Constant Volume 596

Reactions Carried Out at Constant Pressure 596

The R elationship betwen

A H

and A £ 597

16 5 Thermochemistry 599

Standard Heats of Formation,

A H}

600

Calculations Using He ss Law 601

Heats of Combustion 603

16 6

Bond Enthalpies

604

The C— H Bond Enthalpy 605

The C—C Bond Enthalpy 606

Tabulation of Bond Enth alpies 607

16 7 Heat Capacity 609

The Relation between

C

p

and C„ 611

Molecular Origins of Heat Capacity 612

16 8

C alorimetry

614

Summary

617

Exercises 619


Problems 624

Chapter 17 Entropy, Free Energy, and

Equilibrium 627

17.1

Energy and

Spontaneity:

The Needfor a

Second Law

628

Spontaneity and Molecular Disorder 629

17.2 Reversible Processes 630

17 3 Derivation ofthe Reversible W ork of

Expansion ofan Ideal Gas 632

17 4 The Maximum Work That Can Be Done

by an Isothermal Expansion ofan Ideal

Gas

632

17 5

The Entropy Changefor an Isothermal

Process

633

AS

for Isothermal Phase Changes 634

The Entropy of Vaporization, A 5

va p

634

The Entropy Change on Fusion 636

17 6 The Second Law of

Thermodynamics 636

17 7 The Gibbs F ree Energy Function 637

17 8 Calculation of AG" 639

Absolute Entropies 639

Calculation ofA 5° 641

Calculation of G° Values 642

Free Energies of Formation,

A G}

644

17 9 AG " and the Equilibrium Constant 645

17 10 The Temperature Dependence ofAH,

AS,AG,andK

eq

648

The Temperature Dependence of

AH

and

A S

648

The Temperature Dependence of AG 648

The Temperature Dependence of

K ^

649

Summary

652

Exercises 654


Problems 658

Chapter 18 Electrochemistry 661

18 1

The Use o f Oxidation - Reduction



Detailed Contents xxi

Reactions to Produce Electricity: The Galvanic

Cell

662

The Design of Galvanic Cells 662

The Need for a Salt Bridge 663

Anode and Cathode Reactions 664

Definition of the Farad ay 664

Cells with M etal Electrodes That Take P art in the

Reaction 664

Electrical Current 665

18 2 The EMF ofa Galvanic Cell 667

Deflning the Zero of Poten tial Energy 667

Definition of Electromotive Force (EM F) 667

The Standard Hydrogen Electrode 668

18 3

Cell Conventions and Half-Cell

Potentials 668

18 4 Significance ofthe Sign ofthe Cell

Potential 672

18 5

The Table of Standard Reduction

Potentials 673

18 6 Concentration Dependence ofthe Cell

EM F 676

The Relation between AG and A ^ , , 676

The Nernst Equation 678

18.7 ProofThat the Cell Poten tial Is

Independent

ofthe Form ofthe Net Cell

Reaction

680

18 8 Concentration Cells 681

18 9 Use ofthe Nernst Equation to Determine

the Equilibrium Constant 684

The Use of the Nernst Equation to Determine

Solubility Produ cts 688

18 10

The Relation between All the Criteria

for Predicting the Direction ofa Spontaneous

Reaction 689

18 11

C omm ercial Batteries

690

The Lead Storage Battery 690

The Dry Cell 692

The Mercury Cell 693

Nickel-Cadmium Batteries 693

18 12 Electrolysis 694

Electrolysis of Mo lten Salts 695

The Commercial Production of Aluminum 696

Electrolysis of Aqueous Solutions 698

Overvoltage 700

Electroplating 700

Summary 702

Exercises 704


Problems 709

Chapter

19

Chemical

Kinetics 712

19 1 Factors Affecting the Rates of Chemical

Reactions 714

19 2

The Rate Exp ression

714

The Order of Reaction 717

Units of Rates and Rate Constants 720

19 3 Determination ofthe Order of Reaction

by the Method of Initial R ates 720

19 4

First-Order Reactions

723

TheHalf-Life 725

Radioactive Decay 727

Pseudo-Order Reactions 728

19 5

Second-Order

Reactions 729

19 6 The Temperature Dependence of Rate

Constants 731

Effective Collisions 732

The Activation Energy 734

The Arrhenius Equation 734

19 7 Transition State Theory and the Activated

Complex 731

Potential Energy versus Reaction Coordinate

Diagrams 737

19 8 The Relation between the Mechanism of

a Reaction and Kinetics Data

739

The Hydrogen Iodide Reaction 741

Molecularity versus Order 741

Catalysis 743

19 9

Chain Reactions

746

19 10 Reaction Rates and Equilibrium 746

Summary 747

Exercises 750


Problems 756

Chapter 2 0 Coordination Compounds 761

20 1 Ligands and the Coordinate Bond 762

20 2 The

Coordination

Number 763

20 3 Lewis Acids and Bases 765

Cation Acids 766

20 4 Inert versus Labile C omplexes 768



xxii Detailed Contents

20 5 Evidence for the Existence ofCom plex

Ions

769

20.6

N omenclature 773

Rules for Naming S alts th at contain a Com plex Ion or

Ions 773

The Rule for Naming Nonionic or Molecular

Complexes 774

The Rule for Nam ing Compounds with a Bridging

Ligand or Ligands 774

20 7

The G eometry of Coordination

Comp ounds; Isomers 116

Geometries for Coordination Number 4 776

Cis-Trans Isomerism for Four-Coordinate

Complexes 776

Geometries for Coordination Num ber 5 777

Octahedral Geometry for Coordination Number 6 778

Linkage Isomerism 780

20.8

Optica

Isomerism 780

20 9

The Effective Atomic N umber (EAN)

Rule 782

20 10 Magnetic Mom ents of Transition Metal

Complexes

784

Diamagnetism and Paramagnetism 784

Spin-Only Magnetic Mom ents 786

High-Spin and Low-Spin Complexes 786

The Colors of Transition Metal Complexes 786

20 11

Theories of Bonding in Coordination

Complexes

787

Crystal Field Theory for Octahedral Complexes 787

High-Spin versus Low-Spin Octahedral

Complexes 789

The Spectrochemical Series 790

Crystal Field Splittings for Geometries Other Than

Octahedral 791

Absorption Spectra 793

Ligand Field Theory 795

Summary 796

Exercises

797


800

Problems 802

Chapter 2 Properties and Structures of

Metallic and

Ionic

Crystalline Solids 805

21 1

Crystalline and Amorphous Solids

806

21 2

Crystal Defects

807

21 3

The Structures o f Metals

808

Hexagonal and Cubic Close Packing 808

Body-Centered Cubic Structures 810

21.4

Metallic Bond ing 811

Band Theory of M etals 812

21 5

The Seven Crystal Systems

813

The Fourteen Bravais Lattices 815

21 .6

X-Ray Diffraction

816

Constructive and Destructive Interference 817

21.7

Atomic Dimensions and Unit Cell

Geometry

820

Structural Relations for the Three Cubic Lattices 820

Calculation of Ionic Radii 822

21.8

The La ttice Energy oflonic Crystals

825

The Effect of Cations without Rare Gas Electronic

Configuration 827

21.9

The Born

-

Hab er Cycle

828

Summary

829

Multiple Choice Questions

831

Problems

833

Chapter

22 R adioactivity and

Nuclear

Chemistry 836

22 1 Subatomic Particles and Nuclides 837

22 2

Nuclear Binding Energies

838

Nucleon Pairing 842

Fusion 843

Fission 844

Breeder Reactors 847

22.3

Ra dioactivity

847

Nuclear Stability 847

Shell Model of the Nucleus 849

Beta Decay for Neutron-Rich Nuclei 849

Decay Processes for Neutron-Poor Nuclei 851

Electron Capture 851

Positron Emission 851

a Decay 853

Gamma-Ray Emission 855

22.4

Naturally Occurring Radioactive

Substances 856

The Uranium Series 856

The Thorium Series 856

The Actinium Series 857

22.5

The Rate of Radioactive Decay

857

22 6 The Uses of Radioactivity 859

Isotope Dilution 859

Radiocarbon Dating 861

Isotopic Tracer Techniques 865

Summary

865



Detailed Contents xxiii

Exercises 867

Multiple

Choice Questions 869

Problems

871

Chapter

2 3

Introduction

to

Organic

Chemistry 874

23 1 Bonding in Organic Compounds 875

Methane and Ethane 875

Ethylene 877

Aeetylene 878

Comparing sp

3

, sp

2

, and sp Hybridization 878

23 2

Geometrie Isomerism

879

23 3 Op tica Isomerism 880

23 4

A romaticity 882

Heterocyclic Aromatic Compounds 884

23 5 The Alkanes 885

Straight-Chain or Normal Alkanes 885

Branched-Chain Alkanes 886

Nomenclature of Alkanes 887

23 6 Functional Croups 889

Alkenes 889

Alcohols 891

Ethers 891

Amines 893

Aldehydes and Ketones 894

Carboxylic Acids and Their Derivative s 895

Esters 897

Amides 897

23 7 Oxidation States of Carbon 898

23 8 Brief Survey of

Biologically

Important

Compounds

898

Fats 899

Phospholipids 900

Proteins 900

Carbohydrates 903

23 9 Synthetic Polymers

904

Nylon: A Condensation Polymer 905

Polyvinyl Chloride: An Addition Polymer 905

Summary

906


Problems

910

Appendix A Units

and

Conversion

Factors 915

Appendix

B Mathem atical

Operations

and

Techniques 917

B l Exponents 917

Expo nential (Scientific) Notation 917

Addition and Subtraction of Expon ential Num bers 917

Multiplication of Expon ential Num bers 917

Division of Exponential Num bers 918

Powers of Exponential Num bers 918

Roots of Exponential Num bers 918

Exercises Involving Expo nential

Numbers

919

B2.

Logarithms

919

Base 10 Logarithms 919

Base 10 Antilogarithms 920

Exercises Involving Logarithms

921

Fundamental Properties of Logarithms 921

Natural Logarithms 922

m.Graphs 923

B4. Quadratic Equations

924

Exercises in the Use ofthe Quadratic

Formula

924

Appendix C Experimental

Uncertainties

925

Problems 926

Appendix D Derivat ion ofthe Conversion

Factor between

Two

Units

o f

Pressure,

the

Atmosphere

and

the

Pascal 927

Appendix E

Equilibrium Constants

at

25 °C 929

Table El

Acidity C onstants of Weak

Acids 929

Table E2

Solubility Product Con stants

930

Appendix F Standard

Chemical

Thermo-

dynamic Data at 25 °Cand 101.325 kPa

latm)

932



xxiv Detailed Contents

Appendix G Standard Electrode Potentials

at25°C 938

Appendix I Derivat ion ofthe Relations

AG = AG° +RTlnQ and

AG = RT ln(Q/K

eq

) 943

Appendix J Derivation ofthe Integrated

Forms ofthe First- and Second-Order Rate

Laws 946

Appendix K Methods ofSolving Problems in

Acid-Base Equilibria when the Self-

Ionization of Wa ter Cannot Be Neglected 947

K l . Solutions of Strong Acids 947

K 2.

Solutions ofWeakA cids 948

Glossary 949

Credits 990

Index 993

Appendix H Bohr Theory ofthe H A tom 940

Chemistry Bernice Segal

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