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 $\mathrm{K_2SO_4}$ is:

(Assume complete dissociation of the electrolyte)

Question

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 $\mathrm{K_2SO_4}$ is:

(Assume complete dissociation of the electrolyte)

Paaras Thakur · Accepted Answer

0.36 K. Strategy: Freezing point depression is calculated using Tf = i Kf m. Identify the van't Hoff factor for the completely dissociated salt.Step 1: Identify } i \{ for } {K2SO4} \{{K2SO4 - 2K+ + SO4^2-} ions (n) = 3. Since dissociation is complete, i = 3.Step 2: Calculate } T_f \{_f = 4.0, m = 0.03. T_f = 3 \ 4.0 \ 0.03 = 12 \ 0.03 = 0.36\{ K}{\{Answer: (1)}}

Answer

0.36 K

Answer

0.24 K

Answer

0.18 K

Answer

0.12 K

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…

Practice this question with progress tracking

More JEE Main Solutions PYQs