Question:
The van't Hoff factor for 0.5 m aqueous CH₃COOH solution is 1.075. What is the experimentally observed \(\Delta T_f\) (in K) for this solution?
\( K_f = 1.86 \, \text{K kg mol}^{-1} \)
The van't Hoff factor for 0.5 m aqueous CH₃COOH solution is 1.075. What is the experimentally observed \(\Delta T_f\) (in K) for this solution?
\( K_f = 1.86 \, \text{K kg mol}^{-1} \)
Show Hint
The van't Hoff factor accounts for the number of particles into which a solute dissociates in solution. Multiply by the freezing point depression constant to calculate \(\Delta T_f\).
Updated On: Jan 6, 2026
- 1.156
- 1.075
- 1.0
- 0.95
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The Correct Option is A
Solution and Explanation
The freezing point depression (\(\Delta T_f\)) is given by the formula:
\[
\Delta T_f = i . K_f . m
\]
Where:
- \(i\) is the van't Hoff factor (1.075),
- \(K_f\) is the freezing point depression constant (1.86 K kg mol\(^{-1}\)),
- \(m\) is the molality (0.5 m).
Substituting these values, the calculated value of \(\Delta T_f\) is 1.156 K.
Substituting these values, the calculated value of \(\Delta T_f\) is 1.156 K.
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