A 0.1 M solution has an osmotic pressure of 3.69 atm at 300 K. If R = 0.082 L atm K−1 mol−1, what is the van’t Hoff factor i for the solute?
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Answer and explanation
Correct answer: 1.5
For osmotic pressure, the relation is π = iCRT, where C is the molarity of the solution. Rearranging gives i = π/(CRT). Substitution gives i = 3.69/(0.1 × 0.082 × 300) = 3.69/2.46 = 1.5. Thus the solute produces an effective particle concentration 1.5 times that expected for a non-electrolyte at the stated concentration.
Frequently asked questions
What is the correct answer to this question?
1.5
Why is this the correct answer?
For osmotic pressure, the relation is π = iCRT, where C is the molarity of the solution. Rearranging gives i = π/(CRT). Substitution gives i = 3.69/(0.1 × 0.082 × 300) = 3.69/2.46 = 1.5. Thus the solute produces an effective particle concentration 1.5 times that expected for a non-electrolyte at the stated concentration.
Which subject and chapter does this question cover?
This is a Class 11 Chemistry question. Chapter: Chapter 01: Solutions.
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