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

The van't Hoff 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

The temperature dependent term among the following is -

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 elctrolytes 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?

1. KCl

2. C₆H₁₂O₆

3. Al₂(SO₄)₃

4. K₂SO₄

6.02 x 10²⁰ molecules of urea are present in 100 mL of its solution. The concentration of the solution is: 

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