Embibe Experts Solutions for Chapter: Solutions, Exercise 1: JEE Main - 12th January 2019 Shift 1

Match List-I and List-II

Choose the correct answer from the options given below:

A $300\mathrm{mL}$ bottle of soft drink has $0.2{\mathrm{MCO}}_2$ dissolved in it. Assuming ${\mathrm{CO}}_2$ behaves as an ideal gas, the volume of the dissolved ${\mathrm{CO}}_2$ at STP is _____ $\mathrm{mL}$. (Nearest integer)

Given: At STP, molar volume of an ideal gas is $22.7\mathrm{L} {\mathrm{mol}}^{-1}$

A solution containing $2 \mathrm{g}$ of a non-volatile solute in $20 \mathrm{g}$ of water boils at $373.52 \mathrm{K}$. The molecular mass of the solute is _____ ${\mathrm{gmol}}^{-1}$. (Nearest integer)

Given, water boils at $373 \mathrm{K},{\mathrm{K}}_{\mathrm{b}}$ for water $=0.52\mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$

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

At $27°\mathrm{C}$, a solution containing $2.5 \mathrm{g}$ of solute in $250.0 \mathrm{mL}$ of solution exerts an osmotic pressure of $400 \mathrm{Pa}$. The molar mass of the solute is g ${\mathrm{mol}}^{-1}$ (Nearest integer)
(Given : $\mathrm{R}=0.083 \mathrm{L}$ bar ${}^{-1} {\mathrm{mol}}^{-1}$ )

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.