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Q.

Molal depression constant for a solvent is 4.0 K kg ${mol}^{- 1}$ . Calculate the depression in the freezing point (in K) of the solvent for 0.03 mol ${kg}^{- 1}$ solution $K_{2} {SO}_{4}$ .
(Assume complete dissociation of the electrolyte)

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answer is 0.36.

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Detailed Solution

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Dissociation of Potassium Sulphate $(K_{2} {SO}_{4})$

$K_{2} {SO}_{4} ⟶ 2 K^{+} + {SO}_{4}^{2 -}$

i (van't Hoff factor) = 3

We known that $Δ T_{f} = i K_{f} m$ where, $k_{f}$ is molal depression constant and m is molarity.

$∴$ $Δ T_{f} = 3 \times 4 \times 0.03 = 0.36 K$

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Molal depression constant for a solvent is 4.0 K kg mol-1. Calculate the depression in the freezing point (in K) of the solvent for 0.03 mol kg-1solution K2SO4.(Assume complete dissociation of the electrolyte)