Abstract
The equilibrium constant of the reaction Al 3+ + H 4SiO 4 0, (aq) = AlH 3SiO 4 2+ + H + (K 1) has been determined at temperatures from 25 to 150°C from the pH of aqueous solutions containing H 4SiO 4(aq), HCI, and KCl with and without added AlCl 3. Log K 1 values obtained in this study at 25, 90, and 150°C are −2.38 ± 0.10, −0.35 ± 0.20, and 1.07 ± 0.30, respectively. These values are linearly related to the reciprocal temperature and yield an association enthalpy of 66.6 kJ/mol. The K 1 value derived at 25°C is in close agreement with that determined by Farmer and Lumsdon (1994) and implies that aluminum silicate complexes do not play a significant role in most surficial natural waters. However, thermodynamic calculations indicate that these complexes form in significant amounts in acid (pH < 3) hydrothermal solutions where they can affect the solubility of Al/Si-bearing minerals.
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