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A common way of removing Cr3+ from solution is by precipitation of Cr(OH)3(s). An environmental engineer tells you that adjusting the pH to 8.5 will decrease total soluble Cr(III) to below 1 mg/L (1.92 x 10-5 M). Is this true? In other words, is the solubility of Cr(III) in the presence of Cr(OH)3(s) at a pH of 8.5 ? 1 mg/L. The pKsp of Cr(OH)3(s) is 30.22. Cr3+ forms 4 complexes with hydroxide: log K1 = 10.00, log K2 = 8.38, log K3 = 6.87, log K4 = 2.98. Assume no other solids or ligands are present.

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