The correct statement regarding a solution of two components A and B exhibiting positive deviation from ideal behaviour is :

1.	Intermolecular attractive force between A-A and B-B are stronger than those between A-B
2.	∆mixH = 0 at constant T and P
3.	∆mixV = 0 at constant T and P
4.	Intermolecular attractive forces between A-A and B-B are equal to those between A-B

40% (w/V) of NaCl solution (density = 1.14 g/ml) is equivalent to: 
1. $0.35\times {10}^5 ppm$
2. $4\times {10}^6 ppm$
3. $3.5\times {10}^6 ppm$
4. $0.35\times {10}^6 ppm$

The value of Henry's law constant:

Which of the following mixtures forms the maximum boiling azeotrope?

For an ideal solution, the correct option is:

1. ${∆}_{\mathrm{mix}}$ $\mathrm{G}=0$ at constant T and P

2. ${∆}_{\mathrm{mix}}$ $\mathrm{S}=0$ at constant T and P

3. ${∆}_{\mathrm{mix}}$ $\mathrm{V}\ne 0$ at constant T and P

4. ${∆}_{\mathrm{mix}}$ $\mathrm{H}=0$ at constant T and P

A solution containing 10 g/dm³ of urea (molecular mass = 60 g mol^-1) is isotonic with a 5 % solution of a non-volatile solute. The molecular mass of this non-volatile solute is:

A solution of sucrose (molar mass = 342 g mol^–1) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be: 
(k_f for water = 1.86 K kg mol^–1)
1. –0.372 ^oC
2. –0.520 ^oC
3. +0.372 ^oC
4. –0.570 ^oC

p_A and p_B are the vapour pressure of pure liquid components, A and B, respectively of an ideal binary solution.
If X_A represents the mole fraction of component A, the total pressure of the solution will be:

1. p_A + X_A (p_B-p_A)
2. p_A + X_A (p_A-p_B)
3. p_B + X_A (p_B-p_A)
4. p_B + X_A (p_A-p_B)

The largest freezing point depression among the following 0.10 m solutions is shown by:

The electrolyte having the same value of Van't Hoff factor (i) as that of Al₂(SO₄)₃  (if all are 100% ionized) is:

1. K₂SO₄
2. K₃[Fe(CN)₆]
3. Al(NO₃)₃
4. K₄[Fe(CN)₆]