---
title: "A student measures the solubility of a sparingly soluble salt, \\(\\text{MX}_2\\), in pure water at \\(25^\\circ\\text{C}\\) according to the dissolution equilibrium below.  \\[ \\text{MX}_2(s) \\rightleftharpoons \\text{M}^{2+}(aq) + 2\\text{X}^-(aq) \\]  The student finds that the solubility of \\(\\text{MX}_2\\) is \\(0.40\\text{ g/L}\\) at \\(25^\\circ\\text{C}\\). Given that the molar mass of \\(\\text{MX}_2\\) is \\(200\\text{ g/mol}\\), what is the value of the solubility product constant, \\(K_{sp}\\), for \\(\\text{MX}_2\\) at this temperature?"
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url: "https://nerd-notes.com/ubq/120278/"
date_modified: "2026-08-23T04:04:13+00:00"
---

# A student measures the solubility of a sparingly soluble salt, \(\text{MX}_2\), in pure water at \(25^\circ\text{C}\) according to the dissolution equilibrium below.

\[
\text{MX}_2(s) \rightleftharpoons \text{M}^{2+}(aq) + 2\text{X}^-(aq)
\]

The student finds that the solubility of \(\text{MX}_2\) is \(0.40\text{ g/L}\) at \(25^\circ\text{C}\). Given that the molar mass of \(\text{MX}_2\) is \(200\text{ g/mol}\), what is the value of the solubility product constant, \(K_{sp}\), for \(\text{MX}_2\) at this temperature?

A student measures the solubility of a sparingly soluble salt, \(\text{MX}_2\), in pure water at \(25^\circ\text{C}\) according to the dissolution equilibrium below.

\[
\text{MX}_2(s) \rightleftharpoons \text{M}^{2+}(aq) + 2\text{X}^-(aq)
\]

The student finds that the solubility of \(\text{MX}_2\) is \(0.40\text{ g/L}\) at \(25^\circ\text{C}\). Given that the molar mass of \(\text{MX}_2\) is \(200\text{ g/mol}\), what is the value of the solubility product constant, \(K_{sp}\), for \(\text{MX}_2\) at this temperature?

- **A.** \(8.0 \times 10^{-9}\)
- **B.** \(3.2 \times 10^{-8}\)
- **C.** \(4.0 \times 10^{-6}\)
- **D.** \(8.0 \times 10^{-6}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120278/*