Solubility of inorganic compounds

Table 5.2 Solubilities of Inorganic Compounds and Metal Salts of Organic...

TABLE 2-120 Solubilities of Inorganic Compounds in Water at Various Temperatures ... 

Extensive tables of solubility of inorganic compounds and densities of aqueous solutions... 

In this chapter the Rruustcd I own llicon of acids and liasc -in aqueous solutions is described. Inn hydrolysis, the reaction between an ion and solvent water molecules that governs the forms of ions in solution, is described and explained. The factors that govern the solubility of inorganic compounds in water are discussed. 

The various ways in which solubility data are presented are discussed in Section 1.1. This section consists of a description of the factors governing the solubility of inorganic compounds in water. The discussion is restricted mainly to the Group 1 halides with some concluding generalizations. 

The nature of ions in solution is described in some detail and enthalpies and entropies of hydration of many ions are defined and recalculated from the best data available. These values are used to provide an understanding of the periodicities of standard reduction potentials. Standard reduction potential data for all of the elements, group-bygroup, covering the s-and p-, d- and/- blocks of the Periodic Table is also included. Major sections are devoted to the acid/base behaviour and the solubilities of inorganic compounds in water. 

Appendix 1 presents numerous reference tables containing most important data on the solubility of inorganic compounds in water, the density, dissociation constants, solubility products, ionization potentials of various atoms, etc., as well as thermochemical constants because many laws of inorganic chemistry cannot be explained without these quantities. 

As a result, special techniques are often required in nonaqueous solvent chemistry. The physical properties of some of the commonly used nonaqueous solvents are shown in Table 5.4, and solubilities of inorganic compounds in some solvents have been described in Chapter 4. 

The solubility of inorganic compounds, such as e.g. salts, decreases in the same way as the solubility of organic compounds in the supercritical state increases. This decrease is combined with the decrease of the dielectric constant of water. The supercritical water oxidation process is described in the following figure. 

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