定量化学分析

CHAPTER 1 INTRODUCTION OF ANALYTICAL CHEMISTRY
1.1 What is Analytical Chemistry
1.2 Steps in the Development of an Analytical Method
1.3 Classification of Quantitative Analytical Methods
1.3.1 Chemical Analysis
1.3.2 Instrumental Analysis
1.4 Principles of Volumetric Titration
1.4.1 Basic Terms
1.4.2 Requirements of Titration Reactions
1.4.3 Classification of Titration Processes
1.4.4 Primary Standards and Standard Solutions
1.4.5 Basic Apparatus in Chemical Analyses
1.5 Calculations in Volumetric Titration
1.5.1 Preparation of Standard Solutions
1.5.2 Titration Results
CHAPTER 2 DATA ANALYSIS
2.1 Error and Classification
2.1.1 Accuracy and Precision
2.1.2 Errors and Deviation
2.1.3 Systematic and Random Errors
2.2 Distribution of Random Errors
2.2.1 Frequency Distribution
2.2.2 Normal Distribution
2.2.3 Predicting the Probability of Random Errors——Area under Gaussian Curve
2.3 Statistical Data Treatment
2.3.1 Estimation of Population Mean and Population Standard Deviation
2.3.2 Confidence Interval for Population Mean
2.3.3 Statistical Aids to Hypothesis Testing
2.3.4 Detection of Gross Errors
2.4 Propagation of Error
2.4.1 Systematic Errors
2.4.2 Random Errors (Standard Deviation)
2.4.3 Maximum Errors
2.4.4 Distribution of Errors
2.5 Significant Figure Convention
2.5.1 Significant Figures
2.5.2 Numerical Rounding in Calculations
CHAPTER 3 ACID-BASE EQUILIBRIUM
3.1 Equilibrium Constants and Effect of Electrolytes
3.2 Acid-base Reactions and Equilibria
3.2.1 Acid and Base——Bronsted Concept
3.2.2 Dissociation of Acid or Base and Acid-base Equilibria
3.2.3 Magnitude of Dissociating Species at a Given pH： x-values
3.3 Solving Equilibrium Calculations Using pH Calculations as an Example
3.3.1 General Approaches (Systematic Approaches)
3.3.2 pH Calculations
3.4 Buffer Solutions
3.4.1 pH Calculations of Buffer Solutions
3.4.2 Buffer Capacity
3.4.3 Preparation of Buffers
CHAPTER 4 ACID-BASE TITRATION
4.1 Acid/Base Indicators
4.1.1 Principle
4.1.2 Examples
4.1.3 Titration Errors
4.1.4 Factors Influencing Performance
4.2 Titration Curves and Selection of Indicators
4.2.1 Strong Acids (Bases)
4.2.2 Monoprotic Acids (Bases)
4.2.3 Strong and Weak Acids (Bases)
4.2.4 Polyfunctional Weak Acids (Bases)
4.2.5 Mixture of Weak Acids (Bases)
4.3 Titration Error Calculations
4.3.1 Strong Acids (Bases)
4.3.2 Monoprotic Weak Acids (Bases)
4.3.3 Polyfunctional Acids (Bases)
4.4 Preparation of Standard Solutions
4.4.1 Standard Acid Solutions
4.4.2 Standard Base Solutions
4.4.3 The Carbonate Error
4.5 Examples of Acid-base Titrations
4.5.1 Determination of Total Alkalinity
4.5.2 Determination of Nitrogen
4.5.3 Determination of Boric Acid
4.6 Acid-base Titrations in Non-aqueous Solvents
4.6.1 Non-aqueous Solvents
4.6.2 Examples of Non-aqueous Titrations
CHAPTER 5 COMPLEXATION REACTION AND COMPLEXOMETRIC TITRATION
5.1 Complexes and Formation Constants
5.1.1 Formation Constants
5.1.2 Concentration of ML. in Complexation Equilibria
5.1.3 Ethylenediaminetetraacetic Acid (EDTA) and Metal-EDTA Complexes
5.1.4 Side Reaction Coefficients and Conditional Formation Constants in Complexation Reactions
5.2 Metallochromic Indicators
5.2.1 How a Metallochromic Indicator Works
5.2.2 Color Transition Point pM　for Metallochromic Indicators
5.2.3 Frequently Used Metallochromic Indicators
5.3 Titration Curves and Titration Errors
5.3.1 Titration Curves
5.3.2 Titration Errors
5.3.3 pH Control in Complexometric Titrations
5.4 Selective Titrations of Metal Ions in the Presence of Multiple Metal Ions
5.4.1 Selective Titration by Regulating pH
5.4.2 Selective Titration Using Masking Reagents
5.5 Applications of Complexometric Titrations
5.5.1 Buffer Selection in Complexometric Titrations
5.5.2 Titration Methods and Applications
5.5.3 Preparation of Standard Solutions
CHAPTER 6 REDOX EQUILIBRIUM AND TITRATION
6.1 Standard Electrode Potentials， Formal Potentials and Redox Equilibria
6.1.1 Standard Electrode Potentials
6.1.2 The Nernst Equation and Formal Potentials
6.1.3 Factors Affecting the Formal Potential
6.1.4 The Equilibrium Constant of Redox Reaction
6.2 Factors Affecting the Reaction Rate
6.2.1 Concentrations
6.2.2 Temperature
6.2.3 Catalysts and Reaction Rate
6.2.4 Induced Reaction
6.3 Redox Titrations
6.3.1 Constructing Redox Titration Curves
6.3.2 Indicators
6.3.3 Auxiliary Oxidizing and Reducing Agents
6.4 Examples of Redox Titrations
6.4.1 Potassium Permanganate
6.4.2 Potassium Dichromate
6.4.3 Iodine： Iodimetry and Iodometry
6.4.4 Potassium Bromate
6.4.5 Ceric Sulfate
CHAPTER 7 PRECIPITATION EQUILIBRIUM， TITRATION， AND GRAVIMETRY
7.1 Precipitation Equilibria and Solubility
7.1.1 Solubility of Precipitates in Pure Water
7.1.2 Ionic Strength and the Solubility of Precipitates
7.1.3 Common Ion and the Solubility of Precipitates
7.1.4 pH and the Solubility of Precipitates
7.1.5 Complexing Agents and the Solubility of Precipitates
7.2 Precipitation Titrations
7.2.1 Titration Curves
7.2.2 Examples of Methods Classified by Endpoint Indication
7.2.3 Preparation of Standard Solutions
7.3 Precipitation Gravimetry
7.3.1 Classification of Gravimetric Methods of Analysis
7.3.2 General Procedure and Requirements for Precipitation
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CHAPTER 8 SPECTROPHOTOMETRY
CHAPTER 9 INTRODUCTION TO ANALYTICAL SEPATION
CHAPTER 10 SOLVING A REAL ANALYTICAL PROBLEM
APPENDICES
ANSWERS
INDEX
PETIODIC TABLE OF THE ELEMENTS