內容大鋼
Quantitative analytical chemistry is a cornerstone course in the undergraduate curriculum at higher agricultural institutions. The comprehensive coverage of this textbook encompasses fundamental knowledge, classical methods, and modern techniques in quantitative analytical chemistry. Each analytical method is meticulously explained, with detailed discussions on principles, operational steps, data processing, and result interpretation. The textbook includes numerous practical examples and exercises to reinforce and apply the acquired knowledge, emphasizing theoretical exposition, and practical application. This textbook is an ideal bilingual teaching resource for undergraduates studying biotechnology, agronomy, plant protection, food science, environmental science, animal science, horticulture, tobacco science, applied chemistry, and bioengineering at higher agricultural and forestry institutions. Additionally, it is an invaluable reference for graduate students and scientific researchers specializing in chemical analysis.
目錄
Chapter 1 Introduction
1.1 Tasks and Functions of Analytical Chemistry
1.2 Classification of Analytical Chemistry Methods
1.3 General Procedure for Quantitative Analysis
Chapter 2 Experimental Error and Statistics
2.1 Significant Figures
2.1.1 Significant Figures in Mass
2.1.2 Significant Figures in Arithmetic
2.2 Types of Error
2.2.1 Systematic Error
2.2.2 Random Error
2.2.3 Precision and Accuracy
2.2.4 Absolute and Relative Uncertainty
2.3 Statistics
2.3.1 Gaussian Distribution
2.3.2 Mean Value and Standard Deviation
2.3.3 Significant Figures in Mean and Standard Deviation
2.4 Confidence Intervals
2.4.1 Calculating Confidence Intervals
2.4.2 Meaning of a Confidence Interval
2.4.3 Standard Deviation and Confidence Interval as Estimates of Experimental Uncertainty
2.5 Comparison of Means with Student's Test
2.6 Comparison of Standard Deviations with the F Test
2.7 Test for an Outlier
2.7.1 Q Test for an Outlier
2.7.2 Grubbs Test for an Outlier
Chapter 3 Introduction to Titrimetric Analysis
3.1 Overview
3.1.1 Characteristics of Titration Analysis Methods
3.1.2 Requirements for Titration Reactions in Titration Analysis
3.1.3 Methods of Titration Analysis
3.1.4 Approach to Conducting Titration Analysis
3.2 Standard Solution
3.2.1 Methods of Representing Standard Solution Concentration
3.2.2 Methods of Preparing a Standard Solution
3.3 Calculation of Titration Analysis
3.3.1 Calculation Related to Solution Preparation
3.3.2 Calculation Relationship Between the Quantities of Reactants
3.3.3 Calculation of Analysis Results
3.4 Errors in Titration Analysis
3.4.1 Method Error
3.4.2 Weighing Error
3.4.3 Error in Measuring Volume
3.4.4 Operational Negligence or Error
Chapter 4 Acid Base Titrations
4.1 Visual Indicators for Acid Base Titrations
4.2 Mixed Indicators
4.3 Neutralization Curves
4.4 Neutralization of a Strong Acid with a Strong Base
4.5 Neutralization of a Weak Acid with a Strong Base
4.6 Neutralization of a Weak Base with a Strong Acid
4.7 Neutralization of a Polyprotic Acid with a Strong Base
4.8 Determination of a Mixture of Carbonate and Hydroxide
4.9 Determination of a Mixture of Carbonate and Hydrogen Carbonate
Chapter 5 Precipitation Titration and Gravimetric Analysis
5.1 Precipitation Titration
5.1.1 Introduction
5.1.2 Principle of Argentometry
5.1.3 Determining the Endpoint
5.2 Gravimetric Analysis
5.2.1 Introduction
5.2.2 General Process of Gravimetric Analysis
5.2.3 Solubility of Precipitate and Effect Factor of Solubility
5.2.4 Precipitation Formation and Selection of Precipitation Condition
5.2.5 Purity of Precipitation
5.2.6 Filtration, Washing, Drying, and Ignition of Precipitation
5.2.7 Calculation of Gravimetric Analysis
Chapter 6 Complexometric Titration
6.1 Overview
6.1.1 Inorganic Ligands and Simple Complexes
6.1.2 Organic Ligands and Chelate Complexes
6.1.3 Ethylenediaminetetra acetic Acid(EDTA)
6.1.4 EDTA Metal Ion Complexes
6.1.5 Formation Constants of Complexes
6.1.6 Side Reaction Coefficient and Conditional Formation Constant
6.2 Metal Ion Indicators
6.2.1 Principle of Metal Ion Indicator
6.2.2 Theoretical Discoloration Point of Metal Ion Indicator
6.2.3 Common Metal Ion Indicator
6.2.4 Announcements of Using Metal Ion Indicator
6.3 Complexometric Titration Curve
6.3.1 Curve Drawing
6.3.2 Factors Affecting the Range of Titration Jump
6.4 Conditions of Complexometric Titration
6.4.1 Single Metal Ion Titration
6.4.2 Selective Titration of Mixed Ions
6.5 EDTA Titration Methods
6.5.1 Direct Titration
6.5.2 Back Titration
6.5.3 Displacement Titration
6.5.4 Indirect Titration
Chapter 7 Redox Titration
7.1 Characteristics of Redox Titration
7.2 Electrode Potential
7.2.1 Standard Electrode Potential
7.2.2 Condition Electrode Potential
7.2.3 Factors Affecting the Conditions Electrode Potential
7.3 Degree of Redox Reaction
7.4 Factors Influencing Redox Reaction Rate
7.5 Titration Curves and Indicator of Redox Titration
7.5.1 Titration Curves of Redox Titration
7.5.2 Indicator of Redox Titration
7.6 Common Redox Titration
7.6.1 Potassium Permanganate Titration
7.6.2 Potassium Dichromate Titration
7.6.3 Iodimetry Titration
7.7 Calculation Practice of Redox Titration
Chapter 8 Absorption Spectrophotometry
8.1 Outline
8.1.1 Characteristic and Application of Absorption Spectrophotometry
8.1.2 Basic Properties of Light
8.1.3 Selective Absorption of Light and the Color of Solution
8.1.4 Absorption Curve
8.2 Beer Lambert Law
8.3 Application of Beer Lambert Law
8.4 Color Reaction
8.4.1 Color Reaction and Color Reagent
8.4.2 Influencing Factors of Color Reaction
8.5 Absorbance Spectrophotometry and the Instrument
8.5.1 Visual Colorimetry
8.5.2 Spectrophotometry
8.6 Condition Choice of Spectrophotometer
8.7 Error of Spectrophotometry
8.7.1 Error Deviated from Beer Lambert Law
8.7.2 Absorbance Error in Measurements
8.8 Other Absorption Spectrophotometry
8.8.1 Differential Spectrophotometry
8.8.2 Dual Wavelength Spectrophotometry
8.8.3 Derivative Spectrophotometry
8.9 Application of Absorbance
Chapter 9 Potentiometric Analysis
9.1 Basic Principle of Potentiometry
9.1.1 Nernst Equation and Cell Potential
9.1.2 Indicator Electrode
9.1.3 Reference Electrode
9.2 Potentiometric Analysis of pH
9.2.1 Glass Membrane Electrode
9.2.2 Measured by Potentiometry
9.3 Ion Selective Electrode
9.3.1 Principle of Ion Selective Electrode
9.3.2 Type of Ion Selective Electrode
9.3.3 Measurement of Ion Selective Electrode
9.3.4 Factors Affecting Measurement
9.3.5 Application of Ion selective Electrodes
9.4 Potentiometric Titration
9.4.1 Device
9.4.2 Determination of Titration Endpoint
9.4.3 Applications of Potentiometric Titration
Chapter 10 Separation Techniques in Quantitative Analytical Chemistry
10.1 Overview
10.2 Precipitation Separation Method
10.2.1 Precipitation Method
10.2.2 Co precipitation
10.3 Extraction Separation Method
10.3.1 Fundamentals
10.3.2 Applications
10.3.3 Precautions
10.4 Ion Exchange Separation Method
10.4.1 Structure and Properties of Ion Exchangers
10.4.2 Application of Ion Exchange Separation
10.5 Chromatographic Separation Method
10.5.1 Fundamental Concepts
10.5.2 Extraction Chromatography
10.5.3 Thin Layer Chromatography and Paper Chromatography
10.5.4 High Performance Liquid Chromatography
10.5.5 Gas Chromatography
10.6 Membrane Separation Technology
10.6.1 Composition and Properties of Liquid Membranes
10.6.2 Separation Principles and Processes
10.6.3 Factors Influencing Liquid Membrane Extraction
10.6.4 Applications
Appendixes
Appendix 1 Relative Atomic Masses
Appendix 2 Formula Weights
Appendix 3 Relative Densities and Concentrations of the Common Acids and Bases
Appendix 4 Dissociation Constants of the Common Acids and Bases (25 ℃)
Appendix 5 Solubility Product Constants of Insoluble Compounds(18 25 ℃)
Appendix 6 Formation Constants of Some Complexes(18 25 ℃)
Appendix 7 Formation Constants of Metal Ions with Various Chelating Agents (18 25 ℃)
Appendix 8 Standard Electrode Potentials(25 ℃)
Appendix 9 Formal Potentials of Some Oxidation Reduction Electron Pairs
References
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