# Problem: A solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 X 10-2 atm at 25°C. Calculate the Ksp value for the salt, assuming ideal behavior.

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###### FREE Expert Solution

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

M3X2 is an electrolyte that dissociates in the following manner:

M3X2  3 M2+ + 2 X3

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

Calculate Molarity M3X2:

M = 2.1581x10-4 M = x (solubility)

Calculate Ksp:

###### Problem Details

A solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 X 10-2 atm at 25°C. Calculate the Ksp value for the salt, assuming ideal behavior.