Solutions practice · Hard

Two elements $A$ and $B$ form compounds having formulae $A B_2$ and $A B_4$. When dissolved in $20 \mathrm{~g}$ benzene, $1 \mathrm{~g}$ of $A B_2$ lowers the freezing point by $2.3^{\circ}$ whereas $1.0 \mathrm{~g}$ of $A B_4$ lowers it by $1.3^{\circ} \mathrm{C}$. $K_f$ for benzene is $5.1 \mathrm{~K} \mathrm{~mol}^{-1} \mathrm{~kg}$. The atomic masses of $A$ and $B$ are respectively

Two solvents '$A$' and '$B$' have $K_{\mathrm{f}}$ values $1.86$ and $2.79 \mathrm{~K} \mathrm{~mol}^{-1} \mathrm{~kg},$ respectively. A given amount of a substance when dissolved in $500 \mathrm{~g}$ of '$A$' completely dimerizes and when the same amount of the substance is dissolved in $500 \mathrm{~g}$ of '${B}$', the solute undergoes trimerization. The ratio of observed lowering of freezing point in two cases is

A $10 \%$ (mass/mass) solution of cane-sugar undergoes partial conversion into glucose and fructose to show inversion of cane-sugar as:
$\text { Sucrose + Water } \longrightarrow \text { Glucose + Fructose. }$

If the solution boils at $100.27^{\circ} {C}$ at this state, calculate the average mass of the dissolved material. What fraction of the sugar has inverted? Given ${K}_b$ for ${H}_2 {O}$ is $0.512 {~K} {~mol}^{-1} {~kg}$.

The vapour pressure of chloroform $\left(\mathrm{CHCl}_3\right)$ and dichloromethane $\left(\mathrm{CH}_2 \mathrm{Cl}_2\right)$ at $298 \mathrm{~K}$ is $200 \mathrm{~mm} \mathrm{Hg}$ and $415 \mathrm{~mm} \mathrm{Hg}$, respectively. If a solution is prepared by mixing $25.5 \mathrm{~g}$ of $\mathrm{CHCl}_3$ and $40 \mathrm{~g}$ of $\mathrm{CH}_2 \mathrm{Cl}_2$ at $298 \mathrm{~K}$, calculate the mole fractions of chloroform in vapour phase.

The distribution coefficient of ${\mathrm{I}_2}$ in between $\mathrm{CC}{\mathrm{l}_4}$ and ${\mathrm{H}_2}\mathrm{O}$ is 85 in favour of $\mathrm{CC}{\mathrm{l}_4}$ at $25^\circ \mathrm{C}$. If solubility of ${\mathrm{I}_2}$ in ${\mathrm{H}_2}\mathrm{O}$ at $25^\circ \mathrm{C}$ is 0.33 g $\mathrm{litr}{\mathrm{e}^{ - 1}},\mathrm{the \;solubility\; of}\,{\mathrm{I}_2}$ in $\mathrm{CC}{\mathrm{l}_4}$ is ……..g $\mathrm{litr}{\mathrm{e}^{ - 1}}$.

$\Delta T_f / K_f$ has the same value of $1 \mathrm{~mol} \mathrm{~kg}^{-1}$ for $8 \%$ $A B_2$ and $10 \% A_2 B$ by mass of solvent, both $A B_2$ and $A_2 B$ being non- electrolytes. Atomic masses of $A$ and $B$ will be respectively

The distribution coefficient of ${\mathrm{I}_2}$ in between $\mathrm{CC}{\mathrm{l}_4}$ and ${\mathrm{H}_2}\mathrm{O}$ is 85 in favour of $\mathrm{CC}{\mathrm{l}_4}$ at $25^\circ \mathrm{C}$. If solubility of ${\mathrm{I}_2}$ in ${\mathrm{H}_2}\mathrm{O}$ at $25^\circ \mathrm{C}$ is 0.33 g $\mathrm{litr}{\mathrm{e}^{ - 1}},\mathrm{the \;solubility\; of}\,{\mathrm{I}_2}$ in $\mathrm{CC}{\mathrm{l}_4}$ is ……..g $\mathrm{litr}{\mathrm{e}^{ - 1}}$.

The elevation in boiling point of a solution of 13.44 g of $\mathrm{CuC}{\mathrm{l}_2}$ in 1 kg of water using the following information will be (molecular weight of $\mathrm{CuC}{\mathrm{l}_2} = 134.4\;and\;{k_b} = 0.52\;K{m^{ - 1}})$

Two components A and B form an ideal solution. The mole fractions of $A$ and $B$ in ideal solution are $X_A$ and $X_B$, while that of in vapour phase, these components have their mole fractions as $\mathrm{Y}_{\mathrm{A}}$ and $\mathrm{Y}_{\mathrm{B}}$. Then, the slope and intercept of plot of $\frac{1}{\mathrm{Y}_{\mathrm{A}}}$ vs. $\frac{1}{\mathrm{X}_{\mathrm{A}}}$ will be:

Osmotic pressure of $3 \%$ aqueous solution of a non-volatile, non-electrolyte solute $A$ at $298 \mathrm{~K}$ is $3.632 \mathrm{~atm}$. Thus, its vapour pressure is ( $p_{\mathrm{H}_2 \mathrm{O}}^{\circ}=23.7 \mathrm{~mm}$ at $298 \mathrm{~K}$ )

Partition coefficient of benzoic acid-ether-water in favour of ether is 2. A solution containing 8 g/litre benzoic acid in ether layer is shaken with 2 litre water. The concentration of acid in water layer is :

What is the mass ratio of ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right.$, molar mass $=62 \, \mathrm{g} / \mathrm{mol}$ ) required for making $500 \, \mathrm{g}$ of 0.25 molal aqueous solution and $250 \, \mathrm{mL}$ of 0.25 molal aqueous solution?

Two liquids $\mathrm{A}$ and $\mathrm{B}$, form an ideal solution. At a specific temperature, the vapour pressure of pure ' $\mathrm{A}$ ' is $200 \mathrm{~mm}$ of ${Hg}$. While that of pure $\mathrm{B}$ is $100 \mathrm{~mm}$ of ${Hg}$. The vapour over mixture consists of $50 \%$ moles of $\mathrm{A}$, what is the $\%$ of $\mathrm{A}$ in the liquid ?

At $300 \mathrm{~K} \,36 \mathrm{~g}$ of glucose present in a litre of its solution has an osmotic pressure of $4.98 \,\mathrm{bar}$. If the osmotic pressure of the solution is 1.52 bar at the same temperature, what would be its concentration?

When $100\, {ml}$ of $\frac{{M}}{10} {H}_2 {SO}_4$ is mixed with $500 \,{ml}$ of $\frac{{M}}{10} {NaOH}$ then nature of resulting solution and normality of excess of reactant left is

Calculate the entropy change for vaporisation of water if latent heat of vaporisation for water is $540 {cal} / {g}$. Given $K_b$ for ${H}_2 {O}=0.51 {~K} /$ molality.

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