NEET 2020 · ChemistryPrevious Year Question

The freezing point depression constant ( $K_{f}$ ) of benzene is 5.12 K kg mol⁻¹. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off upto two decimal places):

Answer: (A) 0.40 K. \textbf{Answer:} (A) 0.40 K \textbf{Solution:} For a non-electrolyte solute the van't Hoff factor $i = 1$ , so the freezing-point depression is: $Δ T_{f} = K_{f} m = 5.12 \times 0.078 = 0.399 \approx 0.40$ K.

A.0.40 K✓
B.0.60 K
C.0.20 K
D.0.80 K

Correct Answer

(A) 0.40 K

Solution & Explanation

\textbf{Answer:} (A) 0.40 K \textbf{Solution:} For a non-electrolyte solute the van't Hoff factor $i = 1$ , so the freezing-point depression is: $Δ T_{f} = K_{f} m = 5.12 \times 0.078 = 0.399 \approx 0.40$ K.

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The freezing point depression constant (Kf​) of benzene is 5.12 K kg mol⁻¹. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off upto two decimal places):

Solution & Explanation

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The freezing point depression constant ( $K_{f}$ ) of benzene is 5.12 K kg mol⁻¹. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off upto two decimal places):