Solutions practice · Mixed difficulty

Molarity and molality of a solution of ${NaOH}$ is calculated. If now temperature of the solution is increased then which of the following statement(s) is/are correct ?

(i) Molarity of solution decreases

(ii) Molality of the solution increases

Relative lowering of vapour pressure of an aqueous solution of $2 \,mole$ of binary solute $(X Y)$ in $3 \,{~mol}$ of solvent is 0.5 then select the correct statement among the following

Density of 2.05 M solution of acetic acid in water is 1.02 g/ml. The molality of the solution is:

Assertion (A): Observed molecular mass of ${CaCl}_2$ determined by any colligative property is less than ideal molecular mass.

Reason (R): ${CaCl}_2$ gets ionised in water as it is a strong electrolyte.

The vapour pressure of benzene at $90^\circ C$ is 1020 torr. A solution of 5 g of a solute in 58.5 g benzene has vapour pressure 990 torr. The molecular weight of the solute is :

Assertion (A): Isotonic solutions must have same elevation in boiling point.

Reason (R): Osmotic pressure, $\pi=i C R T$

Enthalpy of solution is:

For a solution in which $CHC{l_3}$ is dissolved in ${C_6}{H_6},$ molality is 0.1 m. Then mole fraction of ${C_6}{H_6},$ in the solution 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 water at room temperature is lowered by $5 \%$ on dissolving a non-volatile solute in it. The molality of the solution is

Vant Hoff’s factor (i) for acetic acid in benzene is (assuming 30%) dimerization of acetic acid in benzene)

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.

Osmotic pressure of $0.1 \,{M}$ solution of ${NaCl}$ and ${Na}_2 {SO}_4$ will be

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 $\mathrm{CuC}{\mathrm{l}_2} = 134.4\;and\;{k_b} = 0.52\;K{m^{ - 1}})$

Maximum freezing point will be for 1 molal solution, assuming equal ionization in each case:

Assertion: Elevation in boiling point of $0.1 \mathrm{M} \mathrm{KCl}$ and $0.1 \mathrm{M} \mathrm{CaCl}_2$ is same.

Reason: Because colligative properties depends on molarity only.

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:

The vapor pressure in $\mathrm{mm}$ of $\mathrm{Hg}$ of an ideal solution of $\mathrm{A}$ and $\mathrm{B}$ at $25^{\circ} \mathrm{C}$ is given by $p_{\mathrm{AB}}=33 x+94,$ whereas that of an ideal solution of $\mathrm{A}$ and $\mathrm{C}$ at $25^{\circ} \mathrm{C}$ is given by $p_\text{AC}=81 x+46;$ $x$ being mole fraction of $\mathrm{A}$ in the solution. The vapor pressure of solution containing $2 \mathrm{~mol} \mathrm{~A}, 3 \mathrm{~mol} \mathrm{~B}$ and $\text{4 mol of C}$ will be

Assertion: When two volatile liquids are mixed then vapour pressure of one increases and other decreases.

Reason: Vapour pressure of solution decreases.

Which of the following salts has the same value as of van't Hoff factor (i) as that of ${K}_3\left[{Fe}({CN})_6\right]$ ?

Which of the following is correct for a solution showing positive deviations from Raoult's law?

Van’t Hoff factor more than unity indicates that the solute in solution has

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 $298 \mathrm{~K}$ )

What is the total number of moles of ${H_2}S{O_4}$ needed to prepare $5.0\;L$ of a $2.0\;M$ solution of ${H_2}S{O_4}$ ?

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 :

Van't Hoff factors are $x, y$ and $z$ in case of association, ionisation and no change, respectively. Their increasing order 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?