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

Subtopic:  Van’t Hoff Factor |
 83%
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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

Subtopic:  Van’t Hoff Factor |
 74%
From NCERT
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Which of the following is dependent on temperature?

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

Subtopic:  Concentration Terms & Henry's Law |
 91%
From NCERT
NEET - 2017
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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

Subtopic:  Physical Properties |
 82%
From NCERT
NEET - 2017
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Which one is not equal to zero for an ideal solution?
(1)ΔHmix 
(2)ΔSmix
(3)ΔVmix
(4)ΔP=PObserved-PRaoult

Subtopic:  Introduction & Colligative properties |
 85%
From NCERT
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Which one of the following electrolytes has the same value of van't Hoff's factor(i) as that of Al2(SO4)(if all are 100% ionised)? 

1. K2SO4

2. K3[Fe(CN)6]

3. Al(NO3)3

4. K4[Fe(CN)6]

Subtopic:  Introduction & Colligative properties | Van’t Hoff Factor |
 90%
From NCERT
NEET - 2015
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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

Subtopic:  Depression of Freezing Point |
 84%
From NCERT
NEET - 2014
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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

Subtopic:  Van’t Hoff Factor |
 88%
From NCERT
NEET - 2011
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 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

Subtopic:  Concentration Terms & Henry's Law |
 85%
From NCERT
NEET - 2006
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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, Kf 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

Subtopic:  Depression of Freezing Point |
 88%
From NCERT
NEET - 2006
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