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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?
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2.00 L of H2 at a pressure of 368 torr and 1.00 L of N2 at an unknown pressure. If the total pressure in the flasks is 336 torr after the stopcock is opened.
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