---
title: "A student adds excess solid magnesium hydroxide, \\(\\text{Mg(OH)}_2(s)\\), to distilled water at \\(25\\ ^\\circ\\text{C}\\) and stirs until equilibrium is reached according to the equation below.  \\[\\text{Mg(OH)}_2(s) \\rightleftharpoons \\text{Mg}^{2+}(aq) + 2\\,\\text{OH}^-(aq)\\]  The student filters the mixture to remove undissolved solid and measures the \\(\\text{pH}\\) of the saturated solution to be \\(10.00\\). Based on this measurement, what is the value of the solubility product constant, \\(K_{sp}\\), for \\(\\text{Mg(OH)}_2\\) at \\(25\\ ^\\circ\\text{C}\\)?"
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url: "https://nerd-notes.com/ubq/120003/"
date_modified: "2026-08-21T08:31:48+00:00"
---

# A student adds excess solid magnesium hydroxide, \(\text{Mg(OH)}_2(s)\), to distilled water at \(25\ ^\circ\text{C}\) and stirs until equilibrium is reached according to the equation below.

\[\text{Mg(OH)}_2(s) \rightleftharpoons \text{Mg}^{2+}(aq) + 2\,\text{OH}^-(aq)\]

The student filters the mixture to remove undissolved solid and measures the \(\text{pH}\) of the saturated solution to be \(10.00\). Based on this measurement, what is the value of the solubility product constant, \(K_{sp}\), for \(\text{Mg(OH)}_2\) at \(25\ ^\circ\text{C}\)?

A student adds excess solid magnesium hydroxide, \(\text{Mg(OH)}_2(s)\), to distilled water at \(25\ ^\circ\text{C}\) and stirs until equilibrium is reached according to the equation below.

\[\text{Mg(OH)}_2(s) \rightleftharpoons \text{Mg}^{2+}(aq) + 2\,\text{OH}^-(aq)\]

The student filters the mixture to remove undissolved solid and measures the \(\text{pH}\) of the saturated solution to be \(10.00\). Based on this measurement, what is the value of the solubility product constant, \(K_{sp}\), for \(\text{Mg(OH)}_2\) at \(25\ ^\circ\text{C}\)?

- **A.** \(5.0 \times 10^{-14}\)
- **B.** \(1.3 \times 10^{-13}\)
- **C.** \(2.5 \times 10^{-13}\)
- **D.** \(5.0 \times 10^{-13}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120003/*