As pH decreases, [H+] increases and solubility increases. The effect of pH on solubility is dramatic. A saturated solution of Mg(OH)2 has a calculated pH of 10.52 and contains [Mg2+] = 1.710-4 M. Now suppose that solid Mg(OH)2 is equilibrated with a more acidic solution with pH of 9.00. What is the molar solubility of Mg(OH)2 in this solution? KSP = 1.8 10-11 for Mg(OH)2. A saturated solution of Mg(OH)2 has a calculated pH of 10.52 and contains [Mg2+] = 1.710-4 M. Now suppose that solid Mg(OH)2 is equilibrated with a more acidic solution with pH of 9.00. What is the molar solubility of Mg(OH)2 in this solution?