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This work aims to serve as a useful manual for those beginning to work with metal complexes in solution and to establish uniform guidelines for those already engaged in the measurement and use of metal complex stability constants. It describes new developments like the use of graphic illustrations to test the self-consistency of calculated results. Descriptions are provided for the development and use of a comprehensive database applicable to the determination of individual molecular species in multicomponent systems of the type found in the environment, biological fluids and other complex natural systems.
(source: Nielsen Book Data)

• Monoprotic Acid-Bases
• Polyprotic Acid-Base Equilibrium
• Buffers, Acid-Base Titrations, Laboratory Strategies
• Metal-Ligand Equilibria.
• (source: Nielsen Book Data)

An approach to the academic treatment of solution equilibria is presented here as the author unifies homonuclear equilibrium calculations in one concept. The alpha (species fraction) and bound proton (and bound ligand) ration n, as a function of a single master variable (the unbound H or L), yield complete balances. A single logic is maintained for all cases by equating the chemical binding expressed as an equilibrium condition and as a material balance condition.
(source: Nielsen Book Data)

• Part 1 Introduction: stability constants - early work
• recent developments
• historical evolution of computational methods
• purpose of this book. Part 2 Equilibrium constants, protonation constants, formation constants: concentration constants and activity constants
• conventions employment for expressing equilibrium constants
• equilibrium constants and stability constants for EDTA
• species distribution curves. Part 3 Experimental methods for measuring equilibrium constants: methods available
• potentiometric pH measurements
• displacement methods
• pH and p[H]measurement of metal complex equilibria: materials, the reaction mixture
• calibration of the potentiometric apparatus
• the experimental runs
• computation of stability constants.Part 4 Common errors and their elimination or minimization: measurements errors
• calibration and electrode care
• reagents
• equilibrium measurements
• calculations
• selection of the model. Part 5 Examples of stability constant determination: iminodiacetic acid (IDA)
• procedure for IDA
• C-BISTREN
• procedure for C-BISTREN. Part 6 Macroscopic and microscopic constants: some definitions and concepts
• ionization of tyrosine
• microscopic protonation equilibria of DOPA
• general comments and conclusions. Determination of stability constants and species concentrations of complex systems: a mixed-ligand binuclear dioxygen system
• non-aqueous solvents
• complex multicomponent systems
• equilibrium with solid phases
• equilibrium involving hydrolytic species
• species distributions of hydroxo and fluoro complexes of AI(III). Part 7 Critical stability constants and their selection: general criteria
• examples of critical data selection
• need for additional critical constants. Part 8 Development of a complete metal complex data base: introduction
• linear stability. constant correlations
• estimation of estability constants not measured experimentally
• metal speciation in sea water with and without added ligands.
• (source: Nielsen Book Data)

This book describes potentiometric methods for determining stability constants and explains how these constants can be used to describe metal ion speciation in complex environmental and biological systems. It also provides three original computer programs on disk for calculating stability constants and for using them to determine concentrations of molecular species in solution. Numerous sample calculations show how to avoid common errors. The authors give examples of calculations for simple metal chelates, for metal complexes of large organic molecules, and for mixtures containing several metal ions and complexing agents in aqueous solution. They also describe common errors in calculating stability constants and how to avoid them.
(source: Nielsen Book Data)

• Preface to the first edition
• Preface to the fourth edition
• List of symbols
• Values of physical constants
• Part I. The Principles of Thermodynamics: 1. First and second laws
• 2. Auxiliary functions and conditions of equilibrium
• Part II. Reaction and Phase Equilibria: 3. Thermodynamics of gases
• 4. Equilibria of reactions involving gases
• 5. Phase rule
• 6. Phase equilibria in single component systems
• 7. General properties of solutions and the Gibbs-Duhem equation
• 8. Ideal solutions
• 9. Non-ideal solutions
• 10. Reaction equilibrium in solution
• Part III. Thermodynamics in Relation to the Existence of Molecules: 11. Statistical analogues of entropy and free energy
• 12. Partition function of a perfect gas
• 13. Perfect crystals and the third law
• 14. Configurational energy and entropy
• 15. Chemical equilibrium in relation to chemical kinetics
• Appendix
• Index.
• (source: Nielsen Book Data)

This is the fourth edition of an established textbook of chemical thermodynamics used by university and technical college students of chemistry and chemical engineering. The text covers the same ground as previous editions, presenting the general theory of chemical equilibrium, including its statistical development, and illustrating its many applications in the laboratory and industry. This edition has been extensively revised in the light of recent contributions to the literature. Many new references have been added; the re-writing of certain passages, especially of those concerning the statistical interpretation of entropy and the present understanding of order-disorder transitions, also reflects changes of emphasis.
(source: Nielsen Book Data)