In a saturated solution that is in contact with solid Mg(OH)2, the concentration of Mg2 is 1.31 X 10-4M. What is the solubility product for Mg(OH)2

Ksp = 8.99x10⁻¹²

Explanation:

The solubility of Mg(OH)₂ is described with the reaction:

Mg(OH)₂(s) → Mg²⁺(aq) + 2OH⁻(aq)

The solubility product, Ksp, is:

Ksp = [Mg²⁺] [OH⁻]²

As you can see from the reaction, when 1 mole of Mg²⁺ is produced, 2 moles of OH⁻ are produced too, if [Mg²⁺] is 1.31x10⁻⁴M, [OH⁻] = 2.62x10⁻⁴M

Replacing:

Ksp = [Mg²⁺] [OH⁻]²

Ksp = [1.31x10⁻⁴M] [2.62x10⁻⁴M]²

explanation:

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2b2t

explanation:

2b2t