Studies On The Hydrolysis Of Metal Ions

Filling the need for a comprehensive treatment that covers the theory, methods and the different types of metal ion complexes with water (hydrolysis), this handbook and ready reference is authored by a nuclear chemist from academia and an industrial geochemist. The book includes both cation and anion complexes, and approaches the topic of metal ion hydrolysis by first covering the background, before proceeding with an overview of the dissociation of water and then all different metal-water hydrolysis complexes and compounds. A must-have for scientists in academia and industry working on this interdisciplinary topic.

Filling the need for a comprehensive treatment that covers the theory, methods and the different types of metal ion complexes with water (hydrolysis), this handbook and ready reference is authored by a nuclear chemist from academia and an industrial geochemist. The book includes both cation and anion complexes, and approaches the topic of metal ion hydrolysis by first covering the background, before proceeding with an overview of the dissociation of water and then all different metal-water hydrolysis complexes and compounds. A must-have for scientists in academia and industry working on this interdisciplinary topic.

The hydrolysis equilibria of In(III) were studied at 25C in the ionic medium 3 M(Na(+)Cl( - ) by measuring the hydrogen ion concentration with a glass electrode. The (In(III)) ranged from 0.001 to 0.04 M, and the hydrogen ion concentration was varied from values high enough for the hydrolysis to be negligible to those low enough for a precipitate to be formed. Comparison with the equilibrium constants for the formation of the species InOH(2+) and In(OH)2(4+) in 3 M(Na(+))Cl4( - ) indicates that in 3 M (Na(+)Cl( - ) medium the species denoted by the collective formulas 'InOH(2+)' and In(OH)2(4+) are in reality mainly mixed Cl( - )-OH( - ) complexes (just as 'In(3+)' denotes mainly Cl( - ) complexes). (Author).

An emf study was made in a system of various concentrations of lithium and hydroxide ions in sodium perchlorate medium using a hydrogen electrode at 25C. The general composition of the cell is Pt/H2, B M Li(+), (3-B) M Na(+), A M OH( - ), (3-A) M ClO4( - )/Ref where Ref =/3 M NaClO4/ 2.99 M Na(+), 0.01 M Ag(+), 3 M ClO4( - )/AgCl, Ag. From the difference in emfs between sodium hydroxide solutions with and without lithium ions, the following formation constant of lithium hydroxide was estimated: Li(+) + OH( - ) reversibly yields LiOH, K = 0.66 = 0.02 (log K = -0.18 = 0.01). (Author).

A scaled-down version of a conventional solubility column which uses only about 2 g of solid material is described. It is well-adapted for handling radioactive materials, and was used for radiochemical measurements of the solubility of red mercury (II) oxide in 3 M NaC1O4 solutions in the pH range 1-5. The presence of Hg(2+), HgOH(+), and Hg(OH)2 as the only mercury containing species was confirmed, and the values for the equilibrium constants were calculated.

The hydrolysis equilibria of the La(III) ion have been studied at 25C by hydrogen ion concentration measurements, using a glass electrode. The total (La(III)) was varied between 0.1 and 1.0 M, whilst the concentration of the ClO4- ion was held constant at 3 M by the addition of LiClO4. The experimental conditions necessary for accurate results to be obtained, when the hydrolysis equilibria must be studied in poorly buffered solutions, are discussed in some detail.