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.

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

FREE Expert Solution

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

Π=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:

ΠiRT=iMRTiRTM=ΠiRTM=(2.64×10-2 atm)(5)(0.08206L·atmmol·K)(298.15 K)M=2.1581×10-4 molL

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


Calculate Ksp:

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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.

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

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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.