Lead storage battery contains $38\%$ by weight solution of ${\mathrm{H}}_2{\mathrm{SO}}_4$. The van't Hoff factor is $2.67$ at this concentration. The temperature in Kelvin at which the solution in the battery will freeze is _____ (Nearest integer).

Given ${\mathrm{K}}_{\mathrm{f}}=1.8 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$

Evaluate the following statements for their correctness.

A. The elevation in boiling point temperature of water will be same for $0.1 \mathrm{M}$ $\mathrm{NaCl}$ and $0.1 \mathrm{M}$ urea.
B. Azeotropic mixture boil without change in their composition.
C. Osmosis always takes place from hypertonic to hypotonic solution.
D. The density of $32\%$ ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution having molarity $4.09 \mathrm{M}$ is approximately $1.26 \mathrm{g} {\mathrm{mL}}^{–1}$.
E. A negatively charged sol is obtained when $\mathrm{KI}$ solution is added to silver nitrate solution.

Choose the correct answer from the options given below:

$25 \mathrm{mL}$ of an aqueous solution of $\mathrm{KCl}$ was found to require $20 \mathrm{mL}$ of $1\mathrm{M} {\mathrm{AgNO}}_3$ solution when titrated using ${\mathrm{K}}_2{\mathrm{CrO}}_4$ as an indicator. What is the depression in freezing point of $\mathrm{KCl}$ solution of the given concentration?
(Nearest integer).

(Given : ${\mathrm{K}}_{\mathrm{f}}=2.0 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$ )

Assume
1) $100\%$ ionization and
2) density of the aqueous solution as $1 \mathrm{g} {\mathrm{mL}}^{-1}$

$20\%$ of acetic acid is dissociated when its $5 \mathrm{g}$ is added to $500 \mathrm{mL}$ of water. The depression in freezing point of such water is $\_\_\_\_\_\times {10}^{-3}{}^{\circ }\mathrm{C}$. Atomic mass of $\mathrm{C},\mathrm{H}$ and $\mathrm{O}$ are $12, 1$ and $16$ a.m.u. respectively.

[Given : Molal depression constant and density of water are $1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$ and $1 \mathrm{g} {\mathrm{cm}}^{-3}$ respectively.