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Description: Please note that the content of this book primarily consists of articles available from Wikipedia or other free sources online. Pages: 43. Chapters: Solubility, Solution, Raoult's law, Osmotic pressure, Solvation, Solubility equilibrium, Solvent, Aqueous solution, Percentage solution, Solubility table, Metal ions in aqueous solution, Evaporator, Macromolecular crowding, Flory-Huggins solution theory, Ideal solution, Solubility chart, Inorganic nonaqueous solvent, Osmolarity, Dispersion, Solvated electron, Colligative properties, AdBlue, Common-ion effect, Diluent, Free-energy relationship, Hofmeister series, Enthalpy change of solution, Molar solubility, Solubilization, Solvation shell, Crenation, Hot water extraction, Holtfreter's solution, Duhring's rule, Cold water extraction, Osmolyte, Concentrate, Bunsen solubility coefficient, Solvophobic, Rate of solution, Dissolving, Krebs-Henseleit solution, Folch solution, Scheutjens-Fleer theory, Condosity, Free energy of solvation. Excerpt: The table below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, under 1 atm pressure, units of solubility in g/100g H2O. The substances are listed in alphabetical order. A metal ion in aqueous solution is a cation, dissolved in water, of chemical formula . The solvation number, n, determined by a variety of experimental methods is 4 for Li and Be and 6 for elements in rows 3 and 4 of the periodic table. Lanthanide and actinide aqua ions have solvation number of 8 and 9. The strength of the bonds between the metal ion and water molecules in the primary solvation shell increases with the electrical charge, z, on the metal ion and decreases as its radius, r, increases. Aqua ions are subject to hydrolysis. The logarithm of the first hydrolysis constant is proportional to z/r for most aqua ions. The aqua ion is associated, through hydrogen bonding with other water molecules in a secondary solvation...