25 mL of an aqueous solution of KCl was found to require 20 mL of 1 M solution when titrated using as an indicator. What is the depression in freezing point of KCl solution of the given concentration? (Nearest integer). (Given: = 2.0 K kg ) Assume (1

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Solution

Q.
25 mL of an aqueous solution of KCl was found to required 20 mL of 1 M ${AgNO}_{3}$ solution when titrated using $K_{2} {CrO}_{4}$ as an indicator. What is the depression in freezing point of KCl solution of the given concentration (Nearest integer). (Given: $K_{f}$ = 2.0 K kg ${mol}^{- 1}$ )

Assume

(1) 100% ionization and

(2) density of the aqueous solution as 1 g ${mL}^{- 1}$ [2023]

Ans.
(3)

${25 mL KCl v/s 20 mL of 1M AgNO}_{3}$

$Molarity of KCl = \frac{20 \times 1}{25} = \frac{4}{5} M = \frac{0.8 mol}{L}$

$1 L solution has 0.8 mol KCl$

$Δ T_{f} = i k_{f} m$

$= 2 \times 2 \times 0.8 = 3.2 \approx 3$

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