Solutions practice · Medium

Two solutions of different osmotic pressure. The solution of lower osmotic pressure is called

pH of $0.1 \mathrm{~M}$ monobasic acid solution is found to be 2. Thus its osmotic pressure at $\mathrm{T}.\mathrm{K}$ elvin is:

The mass of ${KCl}$ required to depress the freezing point of $500 \mathrm{~g}$ water by $2 \mathrm{~K}$ is $\left(K_{\mathrm{f}}=1.86, \mathrm{~K}=39\right)$

Assertion (A): The water pouch of instant cold pack for treating athletic injuries breaks when squeezed and $\mathrm{NH}_4 \mathrm{NO}_3$ dissolves in water to lower the temperature.

Reason (R): Addition of non-volatile solute into solvent results into depression of freezing point of the solvent.

A super saturated solution is a metastable state of solution in which solute concentration.

$0.1 {~M} \mathrm{~NaCl}$ and $0.05 {~M} \mathrm{~BaCl}_2$ solutions are separated by a semi-permeable membrane in a container. For this system, choose the correct answer.

Osmosis of A into solution B will not take place if

The vapour pressure of benzene at $80^\circ C$ is lowered by 10 mm by dissolving 2g of a non-volatile substance in 78 g of benzene. The vapour pressure of pure benzene at $80^\circ C$ is 750 mm. The molecular weight of the substance will be :

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 :

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

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

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

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.

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 ${K}_3\left[{Fe}({CN})_6\right]$ ?

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

The freezing point depression of 0.1 molal solution of acetic acid in benzene is $0.256 \mathrm{~K} . k_f$ for benzene is $5.12 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. What conclusion can you draw about the molecular state of acetic acid in benzene?

The vapour pressure of two liquids $P$ and $Q$ are 80 and 60 torr resp. The total vapour pressure of solution obtained by mixing 3 mole of $P$ and 2 mol of $Q$ would be

Essential quantity of ammonium sulphate taken for preparation of 1 molar solution in 2 litres is