Solutions · Chemistry · NEET

Consider the following statements about the solutions formed by mixing two liquids.

A. An ideal solution thus formed obeys Raoult's law throughout the composition range.

B. Mixture of chloroform and acetone shows negative deviation from Raoult's law.

C. Mixture of aniline and phenol shows positive deviation from Raoult's law

Assertion A: For an ideal solution formed by mixing liquids $\mathbf{P}$ and $\mathbf{Q}, \Delta_{\text {mix }} H=0$ and $\Delta_{\text {mix }} V=0$

Reason R: No interactions occur between P and Q

In the light of the above statements, choose the most appropriate answer from the options given below.

Identify the correct statements :

(A) The molality of 2.5 g of ethanoic acid (Molar mass : $60 \mathrm{~g} \mathrm{~mol}^{-1}$ ) in 75 g of benzene solution is 0.556 m .

(B) The molarity of a solution containing 5 g of NaOH (molar mass : $40 \mathrm{~g} \mathrm{~mol}^{-1}$ ) in 450 mL of solution is 0.278 M at 298 K .

(C) Aquatic species are more comfortable in cold water.

(D) The solubility of gas increases with decrease in pressure.

(E) For a binary mixture of $A$ and $B$, the number of moles of $A$ and $B$ are $n_A$ and $n_B$ respectively. The mole fraction of $B$ will be $x_B=\frac{n_A}{n_A+n_B}$.

Choose the correct answer from the options given below :

Mixture of chloroform and acetone forms a solution with negative deviation from Raoult's law due to :

Match List-I with List-II

Choose the correct answer from the options given below:

5 moles of liquid X and 10 moles of liquid Y make a solution having a vapour pressure of 70 torr. The vapour pressures of pure $X$ and $Y$ are 63 torr and 78 torr respectively. Which of the following is true regarding the described solution?

Mass of glucose $$(\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6)$$ required to be dissolved to prepare one litre of its solution which is isotonic with $$15 \mathrm{~g} \mathrm{~L}^{-1}$$ solution of urea $$(\mathrm{NH}_3 \mathrm{CONH}_2)$$ is (Given: Molar mass in $$\mathrm{g} \mathrm{mol}^{-1} \mathrm{C}: 12, \mathrm{H}: 1, \mathrm{O}: 16, \mathrm{~N}: 14$$)

The Henry's law constant $$(\mathrm{K}_{\mathrm{H}})$$ values of three gases $$(\mathrm{A}, \mathrm{B}, \mathrm{C})$$ in water are $$145, 2 \times 10^{-5}$$ and $$35 \mathrm{~kbar}$$ respectively. The solubility of these gases in water follow the order:

The plot of osmotic pressure (П) vs concentration $$(\mathrm{mol} \mathrm{~L}^{-1})$$ for a solution gives a straight line with slope $$25.73 \mathrm{~L} \mathrm{~bar} \mathrm{~mol}^{-1}$$. The temperature at which the osmotic pressure measurement is done is

(Use $$\mathrm{R}=0.083 \mathrm{~L} \mathrm{~bar} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$$)

Which amongst the following aqueous solution of electrolytes will have minimum elevation in boiling point? Choose the correct option :-

K_H value for some gases at the same temperature 'T' are given :

where K_H is Henry's Law constant in water. The order of their solubility in water is :

Which of the following aqueous solution will exhibit highest boiling point?