Molal depression constant...|LIQUID SOLUTION|JEE-Main-2019

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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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