Total vapour pressure of a mixture of 1 mol A (p_A°  = 150 torr) and 2 mol B (${\mathrm{p}}_{\mathrm{B}}^{°}$ = 240 torr) is 200 torr. In this case:-

1. There is a positive deviation from Raoult's law
2. There is a negative deviation from Raoult's law
3. There is no deviation from Raoult's law
4. None of these 

Which of the following aqueous solution should have the highest osmotic pressure?
(1) 0.011 M AICI₃ at 50°C
(2) 0.03 M NaCI at 25°C
(3) 0.012 M (NH₄)₂SO₄ at 25°C
(4) 0.03 M NaCI at 50°C

Calculate the mass of ice that separates when 50 g of ethylene glycol is added to 200 g of water
 and the solution is cooled to −9.3°C.
Given:
Kf of water = 1.86 K kg mol⁻¹
Molar mass of ethylene glycol, C₂H₆O₂ = 62 g mol⁻¹

1. 42 mg
2. 42 g
3. 38.71 g
4. 38.71 mg

Calculate the freezing point of a pure solvent if 40 g of NaOH (i = 2) is dissolved in 1 L of the solvent and the vapour pressure of the resulting solution becomes equal to that of the solid solvent at 300 K.
Given:
Density of solvent = 1 g mL⁻¹
Kf = 1.8 K kg mol⁻¹
Molar mass of NaOH = 40 g mol⁻¹

1. 296.4 K

2. 303.6 K 

3. 297.5 K

4. 302.4 K

P₁ and P₂ are vapour pressure of solvent and solution at temperature T. The solution is prepared by dissolving non-volatile solute in the same solvent. P₁ =760 torr, P₂ =684 mm Hg, Mole fraction of solvent in the solution will be:-

1. 0.1

2. 0.2

3. 0.9

4. Can't be predicted

100 g solute is dissolved in 1400 g of solvent. Density of resultant solution is 1.5 g/mL. The ratio of its molarity and molality will be :-
(1) 1.5

(2) 1.3

(3) 1.4

(4) 1.2
 

As scuba divers ascend towards the surface of the water from underwater, the solubility of gases in their blood:
1. Increases
2. Decreases
3. First increases and then decreases
4. First decreases and then Increases

Solution A & B are formed by dissolving a certain amount of glucose and sucrose in water. The Vapour pressure of these solutions is 660 and 560 mm Hg respectively at 100^oC. The ratio of molality of solutions A & B will be:-

$1.<mspace\; width="1em"></mspace>\frac{14}{33}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$
$2.<mspace\; width="1em"></mspace>\frac{33}{14}$
$3.<mspace\; width="1em"></mspace>\frac{15}{35}$
$4.<mspace\; width="1em"></mspace>\frac{35}{15}$

Saturated solution of Ag₂SO₄ shows 0.003K rise in boiling point, K_sp will be :(K_b = 5 K kg mol^-1)(1m=1M)

1. 3.2 x 10^-11

2.  3.2 x 10^-10

3.  3.2 x 10^-9

4.  3.2 x 10^-12

When 36 g of a solute having the empirical formula CH₂O is dissolved in 1.2 kg of water, the solution freezes at -0.93°C. What is the molecular formula of solute (K_f = 1.86 kg K mol^-1)

(1) C₂H₄O
(2) C₂H₂O₂
(3) C₂H₄O₃
(4) C₂H₄O₂