Solutions practice · Hard

At $35^\circ \mathrm{C}$, the vapour pressure of $C{S_2}$ is 512 mm Hg and that of acetone is 344 mm Hg. A solution of $C{S_2}$ in acetone has a total vapour pressure of 600 mm Hg. The false statement amongst the following is

Which of the aqueous equimolal solution will have its vapour pressure near to solvent?

The size of a raw mango shrinks to a much smaller size when kept in a concentrated salt solution. Which one of the following processes can explain this?

The solution that forms maximum boiling azeotrope is

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 $32\%$ $H_2S{O_4}$ solution having molarity 4.09 M is approximately $1.26 \,g \,mL^{–1}.$
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.

$20\;g$ of binary electrolyte (mol. wt. =100) are dissolved in $500\;g$ of water. The depression in freezing point of the solution is $0.74^\circ C\;({k_f} = 1.86\;K{m^{ - 1}})$ the degree of ionisation of the electrolyte is

Liquid $M$ and liquid $N$ form an ideal solution. The vapour pressures of pure liquids $M$ and $N$ are 450 and 700 mmHg, respectively, at the same temperature. Then correct statement is
${x_M} =$ mole fraction of $M$ in solution; $\,\,\,\,\,\,\,\,\,\,\,{x_N} =$ mole fraction of $N$ in solution;
${y_M} =$ mole fraction of $M$ in vapour phase; $\,\,\,\,\,\,\,\,\,\,\,\,\,\,{y_N} =$ mole fraction of $N$ in vapour phase;

Solution of azeotropic nitric acid mixture contain

Statement I: When urea is added to water, boiling point of water increases.

Statement II: When a volatile solute is added to a volatile solvent, elevation in boiling point is observed.

A current of dry air was passed through a series of bulbs containing $1.25 \mathrm{~g}$ of a solute $\mathrm{A}_2 \mathrm{B}$ (molar mass $=90 \mathrm{~g} / \mathrm{mol}$) in $49 \mathrm{~g}$ of water and then through pure water. The loss in weight of the former series of bulbs was $0.98 \mathrm{~g}$ and in the later series $0.01 \mathrm{~g}.$ The percentage dissociation of solute is

The freezing point $(in\;^\circ C)$ of a solution containing $0.1\;g\;of\;{\mathrm{K}_3}\left[ {\mathrm{Fe}{{\left( {\mathrm{CN}} \right)}_6}} \right]$ (mol.wt.329) in 100 g of water is : $({K_f} = 1.86\;K\;\mathrm{kg}\;\mathrm{mo}{\mathrm{l}^{ - 1}})$

A set of solutions is prepared using 180 g of water as a solvent and 10 g of different non-volatile solutes A, B and C. The relative lowering of vapour pressure in the presence of these solutes are in the order [Given, molar mass of A = 100 $g\,\,mo{l^{ - 1}};$ $B = 200\,\,g\,mo{l^{ - 1}}\,;\,\,C = 10,000\,\,g\,\,mo{l^{ - 1}}]$

${K_2}Hg{I_4}$ is 40% ionized in aqueous solution. The value of its van’t Hoff factor $(i)$ is

The K for ${\mathrm{I}_2}$ between $\mathrm{C}{\mathrm{S}_2}$ and ${\mathrm{H}_2}\mathrm{O}$ is 588 in favour of $\mathrm{C}{\mathrm{S}_2}$. One litre of aqueous solution containing 1 g of ${\mathrm{I}_2}$ is shaken with 50 mL of $\mathrm{C}{\mathrm{S}_2}$. What will be the amount of ${\mathrm{I}_2}$ in aqueous layer?

${{K_f}}$ for water is ${1.86\;K\;kg\;\mathrm{mo}{\mathrm{l}^{ - 1}}}$. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol $\left( {{\mathrm{C}_2}{\mathrm{H}_6}{\mathrm{O}_2}} \right)$ must you add to get the freezing point of the solution lowered to $\mathrm{ - 2}\mathrm{.8}^\circ \mathrm{C}$?

Which of the following statements is true about bends?

Assume a living cell with $0.9 \%(\omega / \omega)$ of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water.

(Consider the data upto first decimal place only)

The cell will:

The relationship which describes the variation of vapour pressure of a liquid with temperature is called :

Assertion (A): Experimentally determined molar mass is always lower than the true value.

Reason (R): Lower molar mass is due to dissociation of solute into ions.

The freezing point of an aqueous solution of ${KCN}$ containing 0.2 mole/kg water was $-0.8^{\circ} \mathrm{C}$. On addition of 0.1 mole of ${Hg}({CN})_2$ in the solution containing 1 kg of water, the freezing point of the solution was $-0.6^{\circ} \mathrm{C}$. Assuming that the complex is formed according to the following equation:
${Hg}({CN})_2+{mCN}^{-} \longrightarrow {Hg}({CN})_{{m}+2}^{-{m}}$ and ${Hg}({CN})_2$ is the limiting reagent, the value of $4 \mathrm{~m}$ is:

At certain temperature a 5.12% solution of cane sugar is isotonic with a 0.9% solution of an unknown solute. The molar mass of solute is

1 mole of heptane (V.P = 92 mm of Hg) was mixed with 4 moles of octane (V.P = 31 mm of Hg). The V.P of resulting ideal solution is

The degree of dissociation $(\alpha)$ of a week electrolyte, $\mathrm{A}_2 \mathrm{SO}_4$ is related to Vant Hoff factor (i) by the expression