{"product_id":"ionic-and-electrochemical-equilibria-hardback-9781848218697","title":"Ionic and Electrochemical Equilibria (Hardback) 9781848218697","description":"\u003cfont face=\"Georgia\"\u003e\r\n\u003cp\u003e\u003cfont size=\"6\"\u003eIonic and Electrochemical Equilibria\u003c\/font\u003e\u003cbr\u003e\r\n\r\n\r\n\r\n\r\n\r\n\u003c\/p\u003e\n\u003cp\u003e\u003cfont size=\"4\"\u003eMichel Soustelle (Author)\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003e9781848218697, Wiley\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003eHardback, published 10 June 2016\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003e308 pages\u003cbr\u003e24.1 x 16.3 x 2.3 cm, 0.612 kg\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\r\n\r\n\r\n\r\n\u003cp align=\"justify\"\u003e\u003cstrong\u003e\u003cfont size=\"3\"\u003e\u003cp\u003eThis book is part of a set of books which offers advanced students successive characterization tool phases, the study of all types of phase (liquid, gas and solid, pure or multi-component), process engineering, chemical and electrochemical equilibria, and the properties of surfaces and phases of small sizes. Macroscopic and microscopic models are in turn covered with a constant correlation between the two scales. Particular attention has been paid to the rigor of mathematical developments.\u003c\/p\u003e \u003cp\u003eThis sixth volume is made up of two parts. The first part focuses on the study of ionic equilibria in water or non-aqueous solvents. The following are then discussed in succession: the dissociation of electrolytes, solvents and solvation, acid-base equilibria, formation of complexes, redox equilibria and the problems of precipitation.\u003c\/p\u003e \u003cp\u003ePart 2 discusses electrochemical thermodynamics, with the study of two groups: electrodes and electrochemical cells. The book concludes with the study of potential-pH diagrams and their generalization in an aqueous or non-aqueous medium.\u003c\/p\u003e\u003c\/font\u003e\u003c\/strong\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003e\u003cp\u003ePreface xi\u003c\/p\u003e \u003cp\u003eNotations and Symbols  xv\u003c\/p\u003e \u003cp\u003e\u003cb\u003ePart 1. Ionic Equilibria 1\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 1. Dissociation of Electrolytes in Solution 3\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e1.1. Strong electrolytes – weak electrolytes 3\u003c\/p\u003e \u003cp\u003e1.1.1. Dissolution 3\u003c\/p\u003e \u003cp\u003e1.1.2. Solvolysis 4\u003c\/p\u003e \u003cp\u003e1.1.3. Melting 4\u003c\/p\u003e \u003cp\u003e1.2. Mean concentration and mean activity coefficient of ions 5\u003c\/p\u003e \u003cp\u003e1.3. Dissociation coefficient of a weak electrolyte 6\u003c\/p\u003e \u003cp\u003e1.4. Conduction of electrical current by electrolytes 9\u003c\/p\u003e \u003cp\u003e1.4.1. Transport numbers and electrical conductivity of an electrolyte 9\u003c\/p\u003e \u003cp\u003e1.4.2. Equivalent conductivity and limiting equivalent conductivity of an electrolyte 10\u003c\/p\u003e \u003cp\u003e1.4.3. Ionic mobility 11\u003c\/p\u003e \u003cp\u003e1.4.4. Relation between equivalent conductivity and mobility – Kohlrausch’s law 14\u003c\/p\u003e \u003cp\u003e1.4.5. Apparent dissociation coefficient and equivalent conductivity 16\u003c\/p\u003e \u003cp\u003e1.4.6. Variations of equivalent conductivities with the concentrations 16\u003c\/p\u003e \u003cp\u003e1.5. Determination of the dissociation coefficient 20\u003c\/p\u003e \u003cp\u003e1.5.1. Determination of the dissociation coefficient by the cryometric method 21\u003c\/p\u003e \u003cp\u003e1.5.2. Determination of the dissociation coefficient on the basis of the conductivity values 22\u003c\/p\u003e \u003cp\u003e1.6. Determination of the number of ions produced by dissociation 23\u003c\/p\u003e \u003cp\u003e1.6.1. Use of limiting molar conductivity 23\u003c\/p\u003e \u003cp\u003e1.6.2. Use of cryometry 24\u003c\/p\u003e \u003cp\u003e1.7. Thermodynamic values relative to the ions 27\u003c\/p\u003e \u003cp\u003e1.7.1. The standard molar Gibbs energy of formation of an ion 27\u003c\/p\u003e \u003cp\u003e1.7.2. Standard enthalpy of formation of ions 29\u003c\/p\u003e \u003cp\u003e1.7.3. Absolute standard molar entropy of an ion 29\u003c\/p\u003e \u003cp\u003e1.7.4. Determination of the mean activity of a weak electrolyte on the basis of the dissociation equilibrium 30\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 2. Solvents and Solvation 31\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e2.1. Solvents 31\u003c\/p\u003e \u003cp\u003e2.2. Solvation and structure of the solvated ion 33\u003c\/p\u003e \u003cp\u003e2.3. Thermodynamics of solvation 35\u003c\/p\u003e \u003cp\u003e2.3.1. Thermodynamic values of solvation 36\u003c\/p\u003e \u003cp\u003e2.3.2. Gibbs energy of salvation – Born’s model 37\u003c\/p\u003e \u003cp\u003e2.4. Transfer of a solute from one solvent to another 44\u003c\/p\u003e \u003cp\u003e2.5. Mean transfer activity coefficient of solvation of an electrolyte 48\u003c\/p\u003e \u003cp\u003e2.6. Experimentally determining the transfer activity coefficient of solvation 49\u003c\/p\u003e \u003cp\u003e2.6.1. Determining the activity coefficient of a molecular solute 50\u003c\/p\u003e \u003cp\u003e2.6.2. Determination of the mean transfer activity coefficient of a strong electrolyte 51\u003c\/p\u003e \u003cp\u003e2.6.3. Evaluation of the individual transfer activity coefficient of an ion 51\u003c\/p\u003e \u003cp\u003e2.7. Relation between the constants of the same equilibrium achieved in two different solvents 55\u003c\/p\u003e \u003cp\u003e2.7.1. General relation of solvent change on an equilibrium constant 55\u003c\/p\u003e \u003cp\u003e2.7.2. Influence of the dielectric constant of the solvent on the equilibrium constant of an ionic reaction 56\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 3. Acid\/Base Equilibria 61\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e3.1. Definition of acids and bases and acid–base reactions 62\u003c\/p\u003e \u003cp\u003e3.2. Ion product of an amphiprotic solvent 63\u003c\/p\u003e \u003cp\u003e3.3. Relative strengths of acids and bases 64\u003c\/p\u003e \u003cp\u003e3.3.1. Definition of the acidity constant of an acid 64\u003c\/p\u003e \u003cp\u003e3.3.2. Protic activity in a solvent 67\u003c\/p\u003e \u003cp\u003e3.4. Direction of acid–base reactions, and domain of predominance 69\u003c\/p\u003e \u003cp\u003e3.5. Leveling effect of a solvent 71\u003c\/p\u003e \u003cp\u003e3.6. Modeling of the strength of an acid 75\u003c\/p\u003e \u003cp\u003e3.6.1. Model of the strength of an acid 75\u003c\/p\u003e \u003cp\u003e3.6.2. Comparison of an acid’s behavior in two solvents 78\u003c\/p\u003e \u003cp\u003e3.6.3. Construction of activity zones for solvents 81\u003c\/p\u003e \u003cp\u003e3.7. Acidity functions and acidity scales 84\u003c\/p\u003e \u003cp\u003e3.8. Applications of the acidity function 88\u003c\/p\u003e \u003cp\u003e3.8.1. Measuring the pKa of an indicator 89\u003c\/p\u003e \u003cp\u003e3.8.2. Measuring the ion products of solvents 89\u003c\/p\u003e \u003cp\u003e3.9. Acidity in non-protic molecular solvents 91\u003c\/p\u003e \u003cp\u003e3.10. Protolysis in ionic solvents (molten salts) 92\u003c\/p\u003e \u003cp\u003e3.11. Other ionic exchanges in solution 93\u003c\/p\u003e \u003cp\u003e3.11.1. Ionoscopy 93\u003c\/p\u003e \u003cp\u003e3.11.2. Acidity in molten salts: definition given by Lux and Flood 94\u003c\/p\u003e \u003cp\u003e3.12. Franklin and Gutmann’s solvo-acidity and solvo-basicity 96\u003c\/p\u003e \u003cp\u003e3.12.1. Definition of solvo-acidity 96\u003c\/p\u003e \u003cp\u003e3.12.2. Solvo-acidity in molecular solvents 96\u003c\/p\u003e \u003cp\u003e3.12.3. Solvo-acidity in molten salts 98\u003c\/p\u003e \u003cp\u003e3.13. Acidity as understood by Lewis 100\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 4. Complexations and Redox Equilibria 101\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e4.1. Complexation reactions 101\u003c\/p\u003e \u003cp\u003e4.1.1. Stability of complexes 101\u003c\/p\u003e \u003cp\u003e4.1.2. Competition between two ligands on the same acceptor 106\u003c\/p\u003e \u003cp\u003e4.1.3. Method for studying perfect complexes 108\u003c\/p\u003e \u003cp\u003e4.1.4. Methods for studying imperfect complexes 110\u003c\/p\u003e \u003cp\u003e4.1.5. Study of successive complexes 115\u003c\/p\u003e \u003cp\u003e4.2. Redox reactions 117\u003c\/p\u003e \u003cp\u003e4.2.1. Electronegativity – electronegativity scale 117\u003c\/p\u003e \u003cp\u003e4.2.2. Degrees of oxidation 124\u003c\/p\u003e \u003cp\u003e4.2.3. Definition of redox reactions 128\u003c\/p\u003e \u003cp\u003e4.2.4. The two families of redox reactions 128\u003c\/p\u003e \u003cp\u003e4.2.5. Dismutation and antidismutation 130\u003c\/p\u003e \u003cp\u003e4.2.6. Redox reactions, and calculation of the stoichiometric numbers 131\u003c\/p\u003e \u003cp\u003e4.2.7. Concept of a redox couple 132\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 5. Precipitation Reactions and Equilibria 135\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e5.1. Solubility of electrolytes in water – solubility product 135\u003c\/p\u003e \u003cp\u003e5.2. Influence of complex formation on the solubility of a salt 136\u003c\/p\u003e \u003cp\u003e5.3. Application of the solubility product in determining the stability constant of complex ions . 137\u003c\/p\u003e \u003cp\u003e5.4. Solution with multiple electrolytes at equilibrium with pure solid phases 138\u003c\/p\u003e \u003cp\u003e5.4.1. Influence of a salt with non-common ions on the solubility of a salt 139\u003c\/p\u003e \u003cp\u003e5.4.2. Influence of a salt with a common ion on the solubility of a salt 141\u003c\/p\u003e \u003cp\u003e5.4.3. Crystallization phase diagram for a mixture of two salts in solution 141\u003c\/p\u003e \u003cp\u003e5.4.4. Formation of double salts or chemical combinations in the solid state 142\u003c\/p\u003e \u003cp\u003e5.4.5. Reciprocal quaternary systems – square diagrams 144\u003c\/p\u003e \u003cp\u003e5.5. Electrolytic aqueous solution and solid solution 147\u003c\/p\u003e \u003cp\u003e5.5.1. Thermodynamic equilibrium between a liquid ionic solution and a solid solution 147\u003c\/p\u003e \u003cp\u003e5.5.2. Solubility product of a solid solution 150\u003c\/p\u003e \u003cp\u003e5.6. Solubility and pH 155\u003c\/p\u003e \u003cp\u003e5.6.1. Solubility and pH 155\u003c\/p\u003e \u003cp\u003e5.6.2. Solubility of oxides in molten alkali hydroxides 156\u003c\/p\u003e \u003cp\u003e5.6.3. Solubility in oxo-acids and oxo-bases (see section 3.12.2) 157\u003c\/p\u003e \u003cp\u003e5.7. Calculation of equilibria in ionic solutions 158\u003c\/p\u003e \u003cp\u003e\u003cb\u003ePart 2. Electrochemical Thermodynamics 163\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 6. Thermodynamics of the Electrode 165\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e6.1. Electrochemical systems 165\u003c\/p\u003e \u003cp\u003e6.1.1. The electrochemical system 166\u003c\/p\u003e \u003cp\u003e6.1.2. Electrochemical functions of state 167\u003c\/p\u003e \u003cp\u003e6.1.3. Electrochemical potential 167\u003c\/p\u003e \u003cp\u003e6.1.4. Gibbs–Duhem relation for electrochemical systems 169\u003c\/p\u003e \u003cp\u003e6.1.5. Chemical system associated with an electrochemical system 170\u003c\/p\u003e \u003cp\u003e6.1.6. General conditions of an equilibrium of an electrochemical system 171\u003c\/p\u003e \u003cp\u003e6.2. The electrode 173\u003c\/p\u003e \u003cp\u003e6.2.1. Definition and reaction of the electrode 173\u003c\/p\u003e \u003cp\u003e6.2.2. Equilibrium of an insulated metal electrode – electrode absolute voltage 174\u003c\/p\u003e \u003cp\u003e6.2.3. Voltage relative to a metal electrode – Nernst’s relation 175\u003c\/p\u003e \u003cp\u003e6.2.4. Chemical and electrochemical Gibbs energy of the electrode reaction 178\u003c\/p\u003e \u003cp\u003e6.2.5. Influence of pH on the electrode voltage 179\u003c\/p\u003e \u003cp\u003e6.2.6. Influence of the solvent and of the dissolved species on the electrode voltage 181\u003c\/p\u003e \u003cp\u003e6.2.7. Influence of temperature on the normal potentials 183\u003c\/p\u003e \u003cp\u003e6.3. The different types of electrodes 184\u003c\/p\u003e \u003cp\u003e6.3.1. Redox electrodes 184\u003c\/p\u003e \u003cp\u003e6.3.2. Metal electrodes 189\u003c\/p\u003e \u003cp\u003e6.3.3. Gas electrodes 192\u003c\/p\u003e \u003cp\u003e6.4. Equilibrium of two ionic conductors in contact  193\u003c\/p\u003e \u003cp\u003e6.4.1. Junction potential with a semi-permeable membrane 193\u003c\/p\u003e \u003cp\u003e6.4.2. Junction potential of two electrolytes with a permeable membrane 194\u003c\/p\u003e \u003cp\u003e6.5. Applications of Nernst’s relation to the study of various reactions 196\u003c\/p\u003e \u003cp\u003e6.5.1. Prediction of redox reactions 196\u003c\/p\u003e \u003cp\u003e6.5.2. Relations between the redox voltages of different systems of the same element 197\u003c\/p\u003e \u003cp\u003e6.5.3. Predicting the dismutation and anti-dismutation reactions 201\u003c\/p\u003e \u003cp\u003e6.5.4. Redox catalysis 202\u003c\/p\u003e \u003cp\u003e6.6. Redox potential in a non-aqueous solvent 203\u003c\/p\u003e \u003cp\u003e6.6.1. Scale of redox potential in a non-aqueous medium 203\u003c\/p\u003e \u003cp\u003e6.6.2. Oxidation and reduction of the solvent 206\u003c\/p\u003e \u003cp\u003e6.6.3. Influence of solvent on redox systems in a non-aqueous solvent 207\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 7. Thermodynamics of Electrochemical Cells 209\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e7.1. Electrochemical chains – batteries and electrolyzer cells 209\u003c\/p\u003e \u003cp\u003e7.2. Electrical voltage of an electrochemical cell 210\u003c\/p\u003e \u003cp\u003e7.3. Cell reaction 212\u003c\/p\u003e \u003cp\u003e7.4. Influence of temperature on the cell voltage; Gibbs–Helmholtz formula 213\u003c\/p\u003e \u003cp\u003e7.5. Influence of activity on the cell voltage 214\u003c\/p\u003e \u003cp\u003e7.6. Dissymmetry of cells, chemical cells and concentration cells 215\u003c\/p\u003e \u003cp\u003e7.7. Applications to the thermodynamics of electrochemical cells 216\u003c\/p\u003e \u003cp\u003e7.7.1. Determining the standard potentials of cells 216\u003c\/p\u003e \u003cp\u003e7.7.2. Determination of the dissociation constant of a weak electrolyte on the basis of the potential of a cell 218\u003c\/p\u003e \u003cp\u003e7.7.3. Measuring the activity of a component in a strong electrolyte 221\u003c\/p\u003e \u003cp\u003e7.7.4. Influence of complex formation on the redox potential 224\u003c\/p\u003e \u003cp\u003e7.7.5. Electrochemical methods for studying complexes 226\u003c\/p\u003e \u003cp\u003e7.7.6. Determining the ion product of a solvent 234\u003c\/p\u003e \u003cp\u003e7.7.7. Determining a solubility product 235\u003c\/p\u003e \u003cp\u003e7.7.8. Determining the enthalpies, entropies and Gibbs energies of reactions 236\u003c\/p\u003e \u003cp\u003e7.7.9. Determining the standard Gibbs energies of the ions 237\u003c\/p\u003e \u003cp\u003e7.7.10. Determining the standard entropies of the ions 238\u003c\/p\u003e \u003cp\u003e7.7.11. Measuring the activity of a component of a non-ionic conductive solution (metal solution) 238\u003c\/p\u003e \u003cp\u003e7.7.12. Measuring the activity coefficient of transfer of a strong electrolyte 241\u003c\/p\u003e \u003cp\u003e7.7.13. Evaluating the individual activity coefficient of transport for an ion 242\u003c\/p\u003e \u003cp\u003e\u003cb\u003eChapter 8. Potential\/Acidity Diagrams 245\u003c\/b\u003e\u003c\/p\u003e \u003cp\u003e8.1. Conventions 245\u003c\/p\u003e \u003cp\u003e8.1.1. Plotting conventions 245\u003c\/p\u003e \u003cp\u003e8.1.2. Boundary equations 246\u003c\/p\u003e \u003cp\u003e8.2. Intersections of lines in the diagram 249\u003c\/p\u003e \u003cp\u003e8.2.1. Relative disposition of the lines in the vicinity of a triple point 249\u003c\/p\u003e \u003cp\u003e8.2.2. Shape of equi-concentration lines in the vicinity of a triple point 250\u003c\/p\u003e \u003cp\u003e8.3. Plotting a diagram: example of copper 256\u003c\/p\u003e \u003cp\u003e8.3.1. Step 1: list of species and thermodynamic data 256\u003c\/p\u003e \u003cp\u003e8.3.2. Step 2: choice of hydrated forms 256\u003c\/p\u003e \u003cp\u003e8.3.3. Step 3: study by degrees of oxidation of acid–base reactions; construction of the situation diagram 257\u003c\/p\u003e \u003cp\u003e8.3.4. Step 4: elimination of unstable species by dismutation 259\u003c\/p\u003e \u003cp\u003e8.3.5. Step 5: plotting the e\/pH diagram 261\u003c\/p\u003e \u003cp\u003e8.4. Diagram for water superposed on the diagram for an element 262\u003c\/p\u003e \u003cp\u003e8.5. Immunity, corrosion and passivation 263\u003c\/p\u003e \u003cp\u003e8.6. Potential\/pX (e\/pX) diagrams 264\u003c\/p\u003e \u003cp\u003e8.7. Potential\/acidity diagrams in a molten salt 265\u003c\/p\u003e \u003cp\u003eAppendix 267\u003c\/p\u003e \u003cp\u003eBibliography 275\u003c\/p\u003e \u003cp\u003eIndex 279\u003c\/p\u003e\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\u003cp\u003e\u003cfont size=\"3\"\u003eSubject Areas: Chemistry [\u003ca title=\"See our other books on Chemistry\" href=\"https:\/\/freshlyprintedbooks.co.uk\/search?q=%22Chemistry%20%5BPN%5D%22\"\u003ePN\u003c\/a\u003e]\u003c\/font\u003e\u003c\/p\u003e\r\n\r\n\r\n\u003c\/font\u003e","brand":"Wiley-ISTE","offers":[{"title":"Brand New","offer_id":52449399111960,"sku":"9781848218697","price":100.57,"currency_code":"GBP","in_stock":true}],"thumbnail_url":"\/\/cdn.shopify.com\/s\/files\/1\/0730\/2037\/5320\/files\/9781848218697.jpg?v=1785198103","url":"https:\/\/freshlyprintedbooks.co.uk\/products\/ionic-and-electrochemical-equilibria-hardback-9781848218697","provider":"Freshly Printed Books","version":"1.0","type":"link"}