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

6g urea is dissolved in 1kg solvent. Value of (T₁-T₂) will be : (K_f=2 kg K mol^-1)

1. 0.2°C
2. -0.2°C
3. 0.1°C
4. -0.1 K

A solution containing 0.03659 g/ml of HCl and a solution containing 0.04509 g/ml of acetic acid Then:

(1) N_HCl is more

(2)N_{CH3COOH is more}

_{(3) Both have same normality}

_{(4) None of these}