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Molal depression constant for a solvent ...

Molal depression constant for a solvent is `4.0 K kg "mol"^(-1)` The depression in the freezing point of the solvent for `0.03 "mol kg^(-1)` solution of `K_(2)SO_(4)` is: (Assume complete dissociation of the electrolyte)

A

0.18 K

B

0.24 K

C

0.36 K

D

0.12 K

Text Solution

AI Generated Solution

To solve the problem, we need to calculate the depression in the freezing point of the solvent using the formula for freezing point depression. Here are the steps to arrive at the solution: ### Step 1: Identify the given values - Molal depression constant (Kf) = 4.0 K kg mol^(-1) - Molality (m) of the solution = 0.03 mol kg^(-1) - The solute is K2SO4, which dissociates into ions. ### Step 2: Determine the van 't Hoff factor (i) ...
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