Lowering in vapour pressure is the highest for:

1. 0.2 m urea

2. 0.1 m glucose

3. 0.1 m MgSO₄

4. 0.1 m BaCl₂

The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in vapour phase in contact with an equimolar solution of benzene and toluene is -

The osmotic pressure of 5 % (mass-volume) solution of cane sugar at 150 °C (mol. mass of sugar = 342 g/mole) is:

An aqueous solution containing 1 g of urea boils at 100.25 °C. The aqueous solution containing 3 g of glucose in the same volume will boil at:
1. 100.75 °C
2. 100.5 °C
3. 100 °C
4. 100.25 °C

Freezing point of an aqueous solution is -0.166$°$C. Elevation of boiling point of same solution would be-

(K_b = 0.512 K m^-1 and K_f = 1.66 K m^-1)

If partial pressure of oxygen is 0.5 atm and K_H = 1.4 × 10^-3 M/atm, then the amount of oxygen dissolved in 100 ml water at 298K is-

The relative lowering of vapour caused by dissolving 71.3 g of a substance in 1000 g of water is 7.13 x 10^-3. The molecular mass of the substance is-

1. 180 g mol^-1

2. 18 g mol^-1

3. 1.8 g mol^-1

4. 360 g mol^-1

Aluminium phosphate is 100 % ionized in 0.01 m aqueous solution. Hence, $∆{\mathrm{T}}_{\mathrm{b}}/{\mathrm{k}}_{\mathrm{b}}$ is-

The relationship between osmotic pressure at 273 K, when 10 gm glucose (P₁), 10 gm urea (P₂), and 10 gm sucrose (P₃) are dissolved in 250 ml of water, is-

1. P₁ > P₂ > P₃

2. P₃ > P₁ > P₂

3. P₂ > P₁ > P₃

4. P₂ > P₃ > P₁

The equal weight of a solute is dissolved in an equal weight of two solvents A and B to form a very dilute solution. The relative lowering of vapour pressure for solution B has twice the relative lowering of vapour pressure for solution A.

If ${\mathrm{M}}_{\mathrm{A}}$ and ${\mathrm{M}}_{\mathrm{B}}$ are the molecular weights of solvents A and B respectively, then:

1. ${\mathrm{M}}_{\mathrm{A}}$ = ${\mathrm{M}}_{\mathrm{B}}$

2. ${\mathrm{M}}_{\mathrm{B}}$ = 2${\mathrm{M}}_{\mathrm{A}}$

3. ${\mathrm{M}}_{\mathrm{A}}$ = 4${\mathrm{M}}_{\mathrm{B}}$

4. ${\mathrm{M}}_{\mathrm{A}}$ = 2${\mathrm{M}}_{\mathrm{B}}$