: Erzsébet Néher-Neumann
: Advanced Potentiometry Potentiometric Titrations and Their Systematic Errors
: Springer-Verlag
: 9781402095252
: 1
: CHF 136.20
:
: Physikalische Chemie
: English
: 350
: Wasserzeichen/DRM
: PC/MAC/eReader/Tablet
: PDF

'Advanced Potentiometry' details the accurate calculation of potentiometric titrations. Additional terms such as the ideal diffusion potential together with the contribution of activity factors furnish calculated stability constants which do not include systematic errors and thus present a complete and correct description of equilibrium processes. Moreover, serious systematic errors resulting from the recent use of curve-fitting computer programs are highlighted later in the text.

'Advanced Potentiometry' can advantageously be used by lecturers, researchers, PhD graduates and undergraduate students working in the fields of Solution Chemistry, Physical Chemistry, Inorganic Chemistry and Analytical Chemistry and Environmental Research.
Contents6
List of Definitions and Symbols10
Preface14
References16
Acknowledgement18
to 1 Introduction 19
1.1 The Titration of Weak Acids (HL, H 3 L) with a Strong Base19
1.2 The Measurement of the Concentration of the H + or the Metal Ion B z(B)+ by Means of an Emf Cell20
1.2.1 The Total Emf of Cell B21
1.2.2 The Total Emf of Cell H25
1.2.3 The Constant Ionic Medium Method28
1.3 On the Curve-Fitting Computer Treatment [2d]29
1.4 On the Deduction of Theoretical Equations31
to 2 Emf Cells with Mixtures of Strong Electrolytes and Liquid Junctions of the Type AY | AY + HY + BYz(B)35
2.1 Studies on Emf Cells Where [A + ] = C M, Constant [1]35
2.1.1 Cell B Using an Amalgam/Ion-Selective Indicator Electrode36
2.1.1.1 The Determination of E 0B and Some Slope Functions36
2.1.1.2 The Estimation of the Systematic Errors in the Equilibrium Constants, 0 log 10 0 pqr , Caused by the Use of the Conditional Experimental Constant E 0B1 40
2.1.2 Cell H Using a Glass Indicator Electrode41
2.1.2.1 The Determination of E 0H and Some Slope Functions41
2.1.2.2 The Estimation of the Systematic Errors in the Equilibrium Constant, 0 log 10 0 pqr , Caused by the Use of the Conditional Experimental Constant E 0H1 45
2.2 Studies on Emf Cells Where [Y ] = C M, Constant [1]46
2.2.1 Cell B Using an Amalgam/Ion-Selective Indicator Electrode47
2.2.1.1 The Determination of E 0B and Some Slope Functions47
2.2.1.2 The Estimation of the Systematic Errors in the Equilibrium Constant, 0 log 10 0 pqr , Caused by the Use of the Conditional Experimental Constant E 0B1 49
2.2.2 Emf Studies in Cell H Using a Glass Indicator Electrode50
2.2.2.1 The Determination of the Constant E 0H and Some Slope Functions50
2.2.2.2 The Estimation of the Systematic Errors in the Equilibrium Constants, 0 log 10 0 pqr , Caused by the Use of the Conditional Constant E 0H1 52
2.3 Studies on Emf Cells Where the Ionic Strength (I) = C M, Constant [1]52
2.3.1 Emf Studies in Cell B Using an Amalgam Indicator Electrode54
2.3.1.1 The Determination of E 0B and Some Slope Functions54
2.3.1.2 The Estimation of the Systematic Errors in the Equilibrium Constants, 0 log 10 0 pqr , Caused by the Use of the Conditional Constant E 0B1 55
2.3.2 Emf Studies in Cell H Using a Glass Indicator Electrode55
2.3.2.1 The Determination of E 0H and Some Slope Functions56
2.3.2.2 The Estimation of the Systematic Errors in the Equilibrium Constants, 0 log 10 0 pqr , Caused by the Use of the Conditional Constant E 0H1 57
2.4 Conclusion on Emf Studies of Mixtures of Strong Electrolytes57
to 3 Determination of the Ionic Molar Conductivities in Mixtures of the Strong Electrolytes HClO4 + NaClO4 + Cd(ClO4)265
3.1 Introduction65
3.2 Conductivity Measurements66
3.2.1 Conductivity Measurements in Mixtures Where [Na + ] = 30M, Constant [ 1 ]66
3.2.1.1 Conductivity Measurements in Mixture 1 Where c B is Varied While c H is Kept Constant66
3.2.1.2 Conductivity Measurements in Mixture 2 Where c H is Varied While c B is Kept Constant70
3.2.1.3 Conductivity Measurements in Mixture 3 Where Both c B and c H Are Varied73
3.2.1.4 Conclusion Which Can Be Obtained from Tables 2.2 and 3.1 73
3.2.1.5 Measurement of the Molar Conductivity of Concentrated Aqueous Cd(ClO 4 ) 2 Solutions74
3.2.2 Conductivity Measurements in Mixtures Where [ClO 4 0 ] = 30M, Constant [ 7 ]75
3.2.2.1 Conductivity Measurements in Mixture 2 Where c H Is Varied While c B Is Kept Constant76
3.2.2.2 Conductivity Measurements in Mixture 1 Where c B Is Varied While c H Is Kept Constant79
3.2.2.3 Conductivity Measurements in Mixture 3 Where Both c B and c H Are Varied83
3.2.3 Conductivity Measurements in Mixtures Where I = C M, Constant [ 8 ]84
3.2.3.1 Conductivity Measurements in Mixture 1 Where c B Is Varied While c H Is Kept Constant84
3.2.3.2 Conductivity Measurements in Mixture 2 Where c H Is Varied While c B Is Kept Constant88
3.2.3.3 Conductivity Measurements in Mixture 3 Where Both c B and c H Are Varied91
3.3 Conclusion on Conductivity Measurements91
3.4 Experimental Details93
to 4 Studies on Emf Cells Where Complex Formation Takes Place Using Liquid Junctions of the Type AY AY + HY + BYz(B) + AyL and -- log10 [H+] 795
4.1 Deduction of the General Equations [ 1 ]95
4.1.1 Introduction95
4.1.2 Definitions and Symbols Used in Equilibrium Systems96
4.1.3 Deduction of the Potential Functions E D , E Df , E B and E H 99
4.1.4 Calculation of the Ideal Diffusion Potential, E D, in Cells with Complex Formation100
4.1.5 The Suggested Function for E D for the Preliminary Treatment of Emf Data102
4.1.6 Calculation of the Contribution of the Activity Coefficients to the Ideal Diffusion Potential, E Df , in Cells with Complex Formation103
4.1.7 The Suggested Function for E Df for the Preliminary Treatment of Emf Data103
4.1.8 The Total Cell Emf in Cells with Complex Formation104
4.1.8.1 The Total Emf of Cell B with an Amalgam Indicator Electrode104
4.1.8.2 The Total Emf of Cell H with a H + -Sensitive Indicator Electrode105
4.1.9 The Validity of the Equations105
4.2 Emf Cells Where [A + ] = C M, Is Kept Constant [ 23 ]107
4.2.1 Potential Functions for the Formation of Strong Complexes108
4.2.1.1 The Study of the Formation of Metal Ion Complexes