The Van't Haff factor of a 0.005 M aqueous solution of KCl is 1.95. The degree of ionisation of KCl is:

(1) 0.95

(2) 0.97

(3) 0.94

(4) 0.96

K₄[Fe(CN)₆] is 60% ionised. Then the value of Van't Hoff factor is

1. 1.6

2. 2.4

3. 3

4. 3.4

Which of the following is dependent on temperature?

(1) Molality
(2) Molarity
(3) Mole fraction
(4) Weight percentage

Ionic mobility of which of the following alkali metal ions is lowest when an aqueous solution of their salts are put under an electric field?

(1) Na                       

(2) K

(3) Rb                       

(4) Li

Which one is not equal to zero for an ideal solution?
(1)ΔH_mix 
(2)ΔS_mix
(3)ΔV_mix
(4)ΔP=P_Observed-P_Raoult

Which one of the following electrolytes has the same value of van't Hoff's factor(i) as that of Al₂(SO₄)₃ (if all are 100% ionised)? 
1. K₂SO₄

2. K₃[Fe(CN)₆]

3. Al(NO₃)₃

4. K₄[Fe(CN)₆]

Of the following 0.10 m  aqueous solutions, which one will exhibit the largest freezing point depression?

(a) KCl

(b) C₆H₁₂O₆

(c) Al₂(SO₄)₃

(d) K₂SO₄

The van't Hoff factor, i for a compound which undergoes dissociation in one solvent and association in other solvent is respectively.

(1) less than one and less than one

(2) greater than one and less than one

(3) greater than one and greater than one

(4) less than one and greater than one

 A solution containing 10 g per 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:

(1) 250 g mol^-1               

(2) 300 g mol^-1

(3) 350 g mol^-1               

(4) 200 g mol^-1

1.00 g of a non-electrolyte solute (molar mass 250g mol) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K_f of benzene is 5.12 K kg mol^-1, the freezing point of benzene will be lowered by:
1. 0.4 K
2. 0.3 K
3. 0.5 K
4. 0.2 K