Liquid Solution - Physical Chemistry - Chemistry Previous Year Questions

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 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.

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

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 $\left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

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 $\left(K_b\left(\mathrm{H}_2 \mathrm{O}\right)=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

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 $=78 \mathrm{~g} \mathrm{~mol}^{-1}$ )

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

Which of the following substances show the highest colligative properties?

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 $1.67 \times 10^8 \mathrm{~Pa}$ ]

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?

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 $K_f=\mathrm{K} \mathrm{kg} \mathrm{mol}^{-1}$ ]

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 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