At 25°C, the solubility product of Mg(OH)2 is 1.0 $\times$ 10–11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001 M Mg2+ ions?

Question

At 25°C, the solubility product of Mg(OH)₂ is 1.0 $\times$ 10^–11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001 M Mg²⁺ ions?

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