Osmotic pressure of 40% (w/V) urea solution is 1.64 atm. and that of 3.42% (w/V) cane sugar solution is 2.46 atm. When equal volumes of the above two solutions are mixed, the osmotic pressure of the resulting solution will be?  
 

(1) 1.64 atm

(2) 2.46 atm

(3) 4.10 atm

(4) 2.05 atm 
 

20g of naphthoic acid (C₁₁H₈O₂) dissolved in 50g of benzene (K_f=1.72 K Kg mol^-1) shows a depression in freezing point of 2K. The Vant Hoff factor is?

1. 0.5

2. 0.1

3. 2

4. 3

A 0.002 molar solution of NaCl having degree of dissociation of 90% at 27⁰C, has osmotic pressure equal to:-

1. 0.94 bar

2. 9.4 bar

3. 0.094 bar

4. 9.4 x 10^-4 bar

Determining the normality of a solution with a density of 0.6 g/ml and composed of 35% NH₄OH by mass.

1. 4.8 N

2. 10 N

3. 0.5 N

4. 6 N

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

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