🤓 Based on our data, we think this question is relevant for Professor Watson's class at UNM.

The ** osmotic pressure (Π)** of a solution is related to the molarity of the solution:

$\overline{){\mathbf{\Pi}}{\mathbf{=}}{\mathbf{iMRT}}}$

where:

**i** = van’t Hoff factor**M** = molarity of the solution (in M or mol/L)**R** = gas constant (0.08206 atm • L/mol • K)

T = temperature

M_{3}X_{2} is an *electrolyte* that dissociates in the following manner:

M_{3}X_{2} → 3 M^{2}^{+} + 2 X^{3}^{–}

The dissociation formed a total of 5 ions which means **i = 5**.

**Calculate Molarity M _{3}X_{2}:**

$\frac{\mathbf{\Pi}}{\mathbf{iRT}}\mathbf{=}\frac{\overline{)\mathbf{i}}\mathbf{M}\overline{)\mathbf{RT}}}{\overline{)\mathbf{iRT}}}\phantom{\rule{0ex}{0ex}}\mathbf{M}\mathbf{=}\frac{\mathbf{\Pi}}{\mathbf{iRT}}\phantom{\rule{0ex}{0ex}}\mathbf{M}\mathbf{=}\frac{(2.64\times {10}^{-2}\overline{)\mathrm{atm}})}{\left(5\right)(0.08206{\displaystyle \frac{L\xb7\overline{)\mathrm{atm}}}{\mathrm{mol}\xb7\overline{)K}}})(298.15\overline{)K})}\phantom{\rule{0ex}{0ex}}\mathbf{M}\mathbf{=}\mathbf{2}\mathbf{.}\mathbf{1581}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{4}}\mathbf{}\frac{\mathbf{mol}}{\mathbf{L}}$

**M = 2.1581x10 ^{-4} M = x (solubility)**

**Calculate K _{sp}:**

A solution saturated with a salt of the type M_{3}X_{2} has an osmotic pressure of 2.64 X 10^{-2} atm at 25°C. Calculate the K_{sp} value for the salt, assuming ideal behavior.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.