北京大学的分析化学课程2003年被评为国家级精品课，是全国分析化学课程中首门国家级精品课程。编者从2003年以来开始对定量化学分析课进行英文讲授。本书是其中双语课的教材。本书可与《分析化学教程》(“十五”规划教材)配合使用。

CHAPTER 1 INTRODUCTION OF ANALYTICAL CHEMISTRY

 1.1 What is Analytical Chemistry  2

 1.2 Steps in the Development of an Analytical Method   5

 1.3 Classification of Quantitative Analytical Methods  7

1.3.1 Chemical Analysis   7

1.3.2 Instrumental Analysis   8

 1.4 Principles of Volumetric Titration  8

1.4.1 Basic Terms   9

1.4.2 Requirements of Titration Reactions   9

1.4.3 Classification of Titration Processes   10

1.4.4 Primary Standards and Standard Solutions   10

1.4.5 Basic Apparatus in Chemical Analyses   11

 1.5 Calculations in Volumetric Titration   15

1.5.1 Preparation of Standard Solutions   15

1.5.2 Titration Results   18

CHAPTER 2 DATA ANALYSIS  22

 2.1 Error and Classification  23

2.1.1 Accuracy and Precision   23

2.1.2 Errors and Deviation   24

2.1.3 Systematic and Random Errors   25

 2.2 Distribution of Random Errors  26

2.2.1 Frequency Distribution   27

2.2.2 Normal Distribution   28

2.2.3 Predicting the Probability of Random Errors--Area under Gaussian Curve   30

 2.3 Statistical Data Treatment   31

2.3.1 Estimation of Population Mean (μ) and Population Standard Deviation (α)   31

2.3.2 Confidence Interval for Population Mean   34

2.3.3 Statistical Aids to Hypothesis Testing   37

2.3.4 Detection of Gross Errors   42

 2.4 Propagation of Error  43

2.4.1 Systematic Errors   43

2.4.2 Random Errors (Standard Deviation)   43

2.4.3 Maximum Errors (ER)   44

2.4.4 Distribution of Errors   44

 2.5 Significant Figure Convention  45

2.5.1 Significant Figures   45

2.5.2 Numerical Rounding in Calculations   47

CHAPTER 3 ACID-BASE EQUILIBRIUM  50

 3.1 Equilibrium Constants and Effect of Electrolytes  51

 3.2 Acid-base Reactions and Equilibria   53

3.2.1 Acid and Base--Bronsted Concept   53

3.2.2 Dissociation of Acid or Base and Acid-base Equilibria   55

3.2.3 Magnitude of Dissociating Species at a Given pH： x-values   57

 3.3 Solving Equilibrium Calculations Using pH Calculations as an Example   61

3.3.1 General Approaches (Systematic Approaches)   61

3.3.2 pH Calculations   64

 3.4 Buffer Solutions  71

3.4.1 pH Calculations of Buffer Solutions   71

3.4.2 Buffer Capacity   72

3.4.3 Preparation of Buffers   74

CHAPTER 4 ACID-BASE TITRATION  78

 4.1 Acid/Base Indicators  79

4.1.1 Principle   79

4.1.2 Examples   80

4.1.3 Titration Errors   82

4. 1.4 Factors Influencing Performance   82

 4.2 Titration Curves and Selection of Indicators   83

4.2.1 Strong Acids (Bases)   83

4.2.2 Monoprotic Acids (Bases)   86

4.2.3 Strong and Weak Acids (Bases)   91

4.2.4 Polyfunctional Weak Acids (Bases)   92

4.2.5 Mixture of Weak Acids (Bases)   95

 4.3 Titration Error Calculations   95

4.3.1 Strong Acids (Bases)   95

4.3.2 Monoprotic Weak Acids (Bases)   96

4.3.3 Polyfunctional Acids (Bases)   97

 4.4 Preparation of Standard Solutions  98

4.4.1 Standard Acid Solutions   98

4.4.2 Standard Base Solutions   99

4.4.3 The Carbonate Error   100

 4.5 Examples of Acid-base Titrations   101

4.5.1 Determination of Total Alkalinity   101

4.5.2 Determination of Nitrogen   102

4.5.3 Determination of Boric Acid   103

 4.6 Acid-base Titrations in Non-aqueous Solvents   104

4.6.1 Non-aqueous Solvents   104

4.6.2 Examples of Non-aqueous Titrations   105

CHAPTER 5 COMPLEXATION REACTION AND COMPLEXOMETRIC TITRATION  108

 5.1 Complexes and Formation Constants  109

5.1.1 Formation Constants   109

5.1.2 Concentration of MLn in Complexation Equilibria   111

5.1.3 Ethylenediaminetetraacetic Acid (EDTA) and Metal-EDTA Complexes   113

5.1.4 Side Reaction Coefficients and Conditional Formation Constants in Complexation Reactions   115

 5.2 Metallochromic Indicators   122

5.2.1 How a Metallochromic Indicator Works   122

5.2.2 Color Transition Point pM ((pM)t) for Metallochromic Indicators   123

5.2.3 Frequently Used Metallochromic Indicators   125

 5.3 Titration Curves and Titration Errors   126

5.3.1 Titration Curves   126

5.3.2 Titration Errors   128

5.3.3 pH Control in Complexometric Titrations   129

 5.4 Selective Titrations of Metal Ions in the Presence of Multiple Metal Ions  130

  5.4.1 Selective Titration by Regulating pH   131

  5.4.2 Selective Titration Using Masking Reagents   133

 5.5 Applications of Complexometric Titrations  137

5.5.1 Buffer Selection in Complexometric Titrations   !37

5.5.2 Titration Methods and Applications   138

5.5.3 Preparation of Standard Solutions   142

CHAPTER 6 REDOX EQUILIBRIUM AND TITRATION   146

 6.1 Standard Electrode Potentials, Formal Potentials and Redox Equilibria  147

6.1.1 Standard Electrode Potentials   147

6.1.2 The Nernst Equation and Formal Potentials   149

6.1.3 Factors Affecting the Formal Potential   150

6.1.4 The Equilibrium Constant of Redox Reaction   154

 6.2 Factors Affecting the Reaction Rate   155

6.2.1 Concentrations   156

6.2.2 Temperature   157

6.2.3 Catalysts and Reaction Rate   157

6.2.4 Induced Reaction   157

 6.3 Redox Titrations  158

6.3.1 Constructing Redox Titration Curves   158

6.3.2 Indicators   162

6.3.3 Auxiliary Oxidizing and Reducing Agents   164

 6.4 Examples of Redox Titrations  165

6.4.1 Potassium Permanganate (KMnO4)   165

6.4. 2 Potassium Dichromate (K2Cr2O7)   168

6.4. 3 Iodine: Iodimetry and Iodometry   169

6.4. 4 Potassium Bromate (KBrO3)   173

6.4.5 Ceric Sulfate (Ce(SO4)2)   174

CHAPTER 7 PRECIPITATION EQUILIBRIUM, TITRATION, AND GRAVIMETRY  177

 7.1 Precipitation Equilibria and Solubility  178

7.1.1 Solubility of Precipitates in Pure Water   178

7.1.2 Ionic Strength and the Solubility of Precipitates   178

7.1.3 Common Ion and the Solubility of Precipitates   179

7.1.4 pH and the Solubility of Precipitates   179

7.1.5 Complexing Agents and the Solubility of Precipitates   182

 7.2 Precipitation Titrations  184

7.2.1 Titration Curves   184

7.2.2 Examples of Methods Classified by Endpoint Indication   186

7.2.3 Preparation of Standard Solutions   189

 7.3 Precipitation Gravimetry  190

7.3.1 Classification of Gravimetric Methods of Analysis   190

7.3.2 General Procedure and Requirements for Precipitation   190

7.3.3 Precipitate Formation   192

7.3.4 Obtaining High Purity Precipitates   193

7.3.5 Experimental Considerations   197

7.3.6 Examples of Organic Precipitating Reagents   200

CHAPTER 8 SPECTROPHOTOMETRY  206

 8.1 Principle of Spectrochemical Analysis   207

8.1.1 Properties of Electromagnetic Radiation   207

8.1.2 Interaction of Electromagnetic Radiation with Matter   208

8.1.3 Beer's Law, the Quantitative Principle of Light Absorption   213

8.1.4 Limitations to Beer's Law   216

 8.2 Principles of Instrumentation   217

8.2.1 Instrumentation   217

8.2.2 Instrumental Errors in Absorption Measurement   226

 8.3 Applications of Spectrophotometry  226

8.3.1 Single Component Analyses   226

8.3.2 Multicomponent Analyses   228

8.3.3 Spectrophotometric Titrations   230

8.3.4 Studies of Complex Formation in Solutions   231

8.3.5 Measurements of Dissociation Constants of Organic Acids/Bases   233

CHAPTER 9 INTRODUCTION TO ANALYTICAL SEPARATION   238

 9.1 General Considerations of Separation Efficiency   239

 9.2 Separation by Precipitation  241

9.2.1 Inorganic Precipitants   241

9.2.2 Organic Precipitants   242

9.2.3 Coprecipitation of Species in Trace Amounts for Separation   243

9.2.4 Improving the Selectivity of Precipitation Separation   244

 9.3 Separation by Extraction   245

9.3.1 Principles for Liquid-liquid Extraction   245

9.3.2 Percent Extraction   247

9.3.3 Extraction of Inorganic Species   249

9.3.4 Other Extraction Methods   254

 9.4 Separation by Ion Exchange   257

9.4.1 Ion Exchange Resins   257

9.4.2 Cross-linkage and Exchange Capacity   259

9.4.3 Ion Exchange Equilibria   260

9.4. 4 Applications of Ion Exchange Separation   261

 9.5 Separation by Chromatography  263

9.5.1 Classification   263

9.5.2 Chromatogram   264

9.5.3 Column Chromatography   265

9.5.4 Planar Chromatography   266

CHAPTER 10 SOLVING A REAL ANALYTICAL PROBLEM  271

 10.1 Definition of the Analytical Problem  272

 10.2 Literature Review   273

 10.3 Choosing a Method  275

 10.4 Developing and Evaluating the Method  276

10.4.1 Selectivity   276

10.4.2 Accuracy   277

10.4.3 Sensitivity and Linear Dynamic Range   279

 10.5 Conclusion   280

APPENDICES    281

 Appendix A References   281

 Appendix B Indicators  283

 Appendix C Activity Coefficients(г) for Ions at 25℃   285

 Appendix D Constants for Acid-base, Complexometric, Redox, and Precipitation Titrimetry  286

 Appendix E Molecular Masses   299

ANSWERS  302

INDEX  305

PERIODIC TABLE OF THE ELEMENTS  309