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JEE MAIN 2019
09-04-2019 S2
Question
Molal depression constant for a solvent is $4.0 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. The depression in the freezing point of the solvent for $0.03 \mathrm{~mol} \mathrm{~kg}^{-1}$ solution of $\mathrm{K}_2 \mathrm{SO}_4$ is (Assume complete dissociation of the electrolyte)
Select the correct option:
A
0.36 K
B
0.18 K
C
0.12 K
D
0.24 K
✓ Correct! Well done.
✗ Incorrect. Try again or view the solution.
Solution
$\begin{aligned} & \mathrm{K}_2 \mathrm{SO}_4 \longrightarrow 2 \mathrm{~K}^{+}+\mathrm{SO}_4^{2-} \\ & \mathrm{i}(\text { Van't Hoff Factor })=3 \\ & \begin{aligned} \therefore \Delta \mathrm{Tf} & =\mathrm{i} \mathrm{K}_{\mathrm{f}} \mathrm{m} \\ & =3 \times 4 \times 0.03 \\ & =0.36 \mathrm{~K}\end{aligned}\end{aligned}$
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