Molar depression constant for a solvent is $8.0 K kg {mol}^{- 1}$ . The depression in freezing point of the solvent for $0.03 mol {kg}^{- 1}$ solution of $K_{2} S O_{4}$ is ______

(Assume complete dissociation of the electrolyte)

Question

Molar depression constant for a solvent is $8.0 K kg {mol}^{- 1}$ . The depression in freezing point of the solvent for $0.03 mol {kg}^{- 1}$ solution of $K_{2} S O_{4}$ is ______ ?

(Assume complete dissociation of the electrolyte)

Smart Achievers · Accepted Answer

(1)

$K_{2} S O_{4} \to 2 K^{+} + S O_{4}^{2 -} i = 3$

Solution

Q.
Molar depression constant for a solvent is $8.0 K kg {mol}^{- 1}$ . The depression in freezing point of the solvent for $0.03 mol {kg}^{- 1}$ solution of $K_{2} S O_{4}$ is ______

(Assume complete dissociation of the electrolyte)

1 0.72 K

2 0.24 K

3 0.36 K

4 0.12 K

Ans.
(1)

$K_{2} S O_{4} \to 2 K^{+} + S O_{4}^{2 -} i = 3$

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