Abstract
In dilute aqueous solutions, at pH values below 3.5, aluminium salts dissolve to yield a triply-charged positive ion which interacts with solvent water to form the species [Al(H2O)6]3+, frequently written as Al3+. At physiological pH (7.4) in aqueous solution and in the absence of potential ligands other than water, the coordinated water molecules lose protons leading to the hydrolysed species [Al(OH)4]-, an aluminium ion tetrahedrally surrounded with four OH- groups. At intermediate pH values the species [Al(H2O)5(OH)]2+, [Al(H2O)4(OH)2]+ and [Al(OH)3] coexist. The exact proportions of each, which depend on the pH value of the solution, can in principle be calculated from their known stability constants [1]. However, at concentrations of Al3+ > 1 µM the low solubility of [Al(OH)3] in its amorphous form or as Gibbsite may be important.
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Cochran, M., Coates, J.H., Elliott, D.C. (1990). Aluminium interaction with macromolecules and membranes. In: de Broe, M.E., Coburn, J.W. (eds) Aluminum and renal failure. Developments in Nephrology, vol 26. Springer, Dordrecht. https://doi.org/10.1007/978-94-009-1868-9_10
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DOI: https://doi.org/10.1007/978-94-009-1868-9_10
Publisher Name: Springer, Dordrecht
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