In a mixture of liquids $A$ and $B$, if the mole fractions of component $A$ in vapour phase and liquid mixture are $x_1$ and $x_2$ respectively, then the total vapour pressure of liquid mixture is

(Where $p_{\mathrm{A}}^0$ and $p_{\mathrm{B}}^0$ are the vapour pressure of pure $A$ and $B$ )

Two liquids ' $A$ ' and ' $B$ ' form an ideal solution. At 300 K , the vapour pressure of a solution containing 1 mole of ' $A$ ' and 3 moles of ' $B$ ' is 550 mm Hg . At the same temperature, if one more mole of ' $B$ ' is added to the solution, the vapour pressure of solution increases to 560 mm Hg . Then the ratio of vapour pressures of $A$ and $B$ in their pure state is

Which one of the following mixtures can be separated by steam distillation technique?

Observe the following data given in the table ( $K_H=$ Henry's law constant)

$ \begin{aligned} &\begin{array}{ccccc} \hline \text { Gas } & \mathrm{CO}_2 & \mathrm{Ar} & \mathrm{HCHO} & \mathrm{CH}_4 \\ \hline\left(\boldsymbol{K}_{\mathrm{H}} \text { bar at } \mathbf{2 9 8 ~ K}\right) & 1.67 & 40.3 & 1.83 \times 10^{-5} & 0.413 \\ \hline \end{array}\\ &\text { The correct order of their solubility in water is } \end{aligned} $

The osmotic pressure (in atm) of an aqueous solution containing 0.01 mol of NaCl (degree of dissociation 0.94 ) and 0.03 mol of glucose in 500 mL at $27^{\circ} \mathrm{C}$ is $\left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

Which of the following solution has highest amount of solute?

Observe the following statements

Statement I : The boiling point of 0.1 M urea solution is less than that of 0.1 M KCl solution.

Statement II : Elevation of boiling point is inversely proportional to molar mass of solute.

The correct answer is

At 300 K , the vapour pressure of toluene and benzene are 3.63 kPa and 9.7 kPa respectively. What is the composition of vapour in equilibrium with the solution containing 0.4 mole fraction of toluene?

(Assume the solution is ideal)

An aqueous solution of a non-volatile solute boils at $100.17^{\circ} \mathrm{C}$. The temperature at which this solution will freeze (in ${ }^{\circ} \mathrm{C}$ ) is

$ \begin{aligned} & \left(K_b\left(\mathrm{H}_2 \mathrm{O}\right)=0.512^{\circ} \mathrm{C} \mathrm{~kg} \mathrm{~mol}^{-1},\right. \\ & \left.K_f\left(\mathrm{H}_2 \mathrm{O}\right)=1.86^{\circ} \mathrm{C} \mathrm{~kg} \mathrm{~mol}^{-1}\right) \end{aligned} $

At $50^{\circ} \mathrm{C}$, the vapour pressure of pure benzene is 268 torr. The number of moles of non-volatile solute per mole of benzene required to prepare a solution having a vapour pressure of 167 torr at the same temperature is (molar mass of benzene $=78 \mathrm{~g} \mathrm{~mol}^{-1}$ )

Liquids $A$ and $B$ form an ideal solution. The vapour pressures of $A$ and $B$ are 50 and 32 mm Hg respectively at 300 K . One mole of liquid $A$ is mixed with 1 mole of liquid $B$. What is the approximate mole fraction of $A$ in vapour phase?

' $x^{\prime} \mathrm{g}$ of urea (molar mass $60 \mathrm{gmol}^{-1}$ ) is completely dissolved in ' $y^{\prime} \mathrm{g}$ of pure water and the solution boiled at 373.202 K . If the boiling point of pure water at $1.01^3$ bar is 373.15 K , then $x: y$ is $\left(K_b\left(\mathrm{H}_2 \mathrm{O}\right)=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

At 300 K , the osmotic pressure of a decinormal solution of sodium chloride is 4.82 atm . The degree of dissociation of sodium chloride is $x \times 10^{-2}$. The value of $x$ is $\left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

If 2 g of NaOH is dissolved to make 200 mL solution at $25^{\circ} \mathrm{C}$, the molarity ( $M$ ) at $90^{\circ} \mathrm{C}$ is

A solvent freezes at $17^{\circ} \mathrm{C}$ and its latent heat of fusion is $180 \mathrm{Jg}^{-1}$. The molal depression constant of the solvent is [units of $K_f=\mathrm{K} \mathrm{kg} \mathrm{mol}^{-1}$ ]

A liquid mixture is an ideal solution, if

(A) it obeys ideal gas equation

(B) it obeys Raoult's law at all concentrations

(C) solute - solute, solute - solvent and solvent solvent interactions are similar

The freezing point of equimolal aqueous solution will be highest for

Calculate the quantity of $\mathrm{CO}_2$ required to prepare 1 L of soda water when the soda water was packed under 2 atm of $\mathrm{CO}_2$.

[Henry's law constant for $\mathrm{CO}_2$ is $1.67 \times 10^8 \mathrm{~Pa}$ ]

Which of the following substances show the highest colligative properties?

The Henry's law constant for the solubility of $\mathrm{N}_2$ gas in Water at 298 K is $1 \times 10^5 \mathrm{~atm}$. The mole fraction of air is 0.8 . The number of moles of $\mathrm{N}_2$ from air dissolved in 10 moles of water at 298 K and 5 atm pressure is

What is the effect of external pressure on the osmotic pressure (OP) of a solution?

Which of the following is/are "not correct" for $\mathrm{CH}_3 \mathrm{OH}+\mathrm{CH}_3 \mathrm{COOH}$ mixture solution?

1. 1. $\Delta H_{\text {mix }}<0$

2. 2. Does not obey Raoult's law.

3. 3. $\Delta H_{\text {mix }}>0$

4. 4. An example of ideal solution.

Henry's law is valid for

(A) ammonia gas dissolution in water

(B) $\mathrm{O}_2$ gas dissolution in unsaturated blood

(C) $\mathrm{O}_2$ dissolution in water

(D) $\mathrm{CO}_2$ dissolution in water

Which of the following are correct for an ideal solution?

(A) $\Delta V_{\text {mix }}=0$

(B) $V_{\text {solvent }}+V_{\text {solute }}=V_{\text {solution }}$

(C) $\Delta H_{\text {mix }}=0$

(D) $\mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2 \longrightarrow \mathrm{H}_2 \mathrm{CO}_3$ is an example of ideal solution

At $0^{\circ} \mathrm{C}$ urea solution has an osmotic pressure of 400 mm . On dilution by $x$ times, its osmotic pressure decreased to 100 mm at $20^{\circ} \mathrm{C}$. The dilution factor $x$ is approximately

A 1.17\% solution of solute $A$ is isotonic with 7.2\% solution of glucose. If the molecular weight of solute $A$ is 58.5, the value of van't Hoff factor, ' $i$ ' is

A mixture of 3.0 moles of $\mathrm{Na}_2 \mathrm{O}$ and 1.5 mol of $\mathrm{KO}_2$ is dissolved in 1000 mL of water. The vapour pressure of the solution in Torr, at $100^{\circ} \mathrm{C}$ is

Relative lowering of vapour pressure of a dilute solution is 0.5 . What is the mole fraction of the non-volatile solute?

The solubility product of a sparingly soluble $A B_2$ salt is $2.56 \times 10^{-4} \mathrm{M}^3$ at $25^{\circ} \mathrm{C}$. The $K_f$ of water is 1.8 K kg mol ${ }^{-1}$. The depression in freezing point of a standard solution of $A B_2$ is

An aqueous solution of $98 \%(w / w) \mathrm{H}_2 \mathrm{SO}_4$ has density of $1.02 \mathrm{~g} / \mathrm{cc}$. The molality of the solution is

The freezing point of equimolal aqueous solution will be highest for