What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_spfor Mg(OH)₂ is 5.6 × 10^-12. A)5.6 × 10^-10 M B)5.6 × 10^-8 M C)2.4 × 10^-6 M D)1.1 × 10^-4 M

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The solubility product (Ksp) for Mg(OH)2 is given as 5.6 × 10^-12. In a basic solution with a pH of 12, the concentration of OH- ions ([OH-]) can be calculated using the pH scale and the relationship pOH = 14 - pH, which gives pOH = 2, and thus [OH-] = 10^-2 M. The dissolution of Mg(OH)2 can be represented as: Mg(OH)2(s) ⇌ Mg2+(aq) + 2OH-(aq). The Ksp expression is Ksp = [Mg2+][OH-]^2. Since the solution is already basic, the concentration of OH- ions due to the dissociation of water can be considered significant compared to the additional OH- produced by the dissolution of Mg(OH)2. Therefore, the increase in [OH-] due to Mg(OH)2 dissolution is negligible, and [OH-] can be approximated as 10^-2 M. Substituting the given Ksp and the calculated [OH-] into the Ksp expression gives 5.6 × 10^-12 = [Mg2+](10^-2)^2. Solving for [Mg2+] gives a molar solubility of 5.6 × 10^-8 M for Mg(OH)2 in a solution with pH 12.

What Is the Molar Solubility of Mg(OH)2 in a Basic

What Is the Molar Solubility of Mg(OH)₂ in a Basic