The Van't Hoff factor of solutes A,B and C in aqueous solutions are 0.8,1.6 and 1.2 respectively. The freezing point of equimolar solutions follow the order :

Question

The Van't Hoff factor of solutes A,B and C in aqueous solutions are 0.8,1.6 and 1.2 respectively. The freezing point of equimolar solutions follow the order : (A) A>B>C (B) A>C>B (C) B>A>C (D) B>C>A

Tardigrade Admin · Accepted Answer

Formula of depression in freezing point is as follow-

Δ T_{f} = i \times K_{f} \times

molality
When solvent and molality of different salt is same then

Δ T_{f} \propto i

More the Van't Hoff factor of solutes and more will be the depression in freezing point and lesser will be the freezing point.
Given for solute

A, B

and

C

the Van't Hoff factor's are

0.8, 1.6

and

1.2

respectively.
As for solute

B

the Van't Hoff factor is maximum so its freezing point will be minimum.
Similarly for solute

A

the Van't Hoff factor is minimum so its freezing point will be maximum.
Hence the freezing point of equimolar solutions follow the order as

A > C > B

.

Q. The Van't Hoff factor of solutes $A, B$ and $C$ in aqueous solutions are $0.8, 1.6$ and $1.2$ respectively. The freezing point of equimolar solutions follow the order :

$A > B > C$

$A > C > B$

$B > A > C$

$B > C > A$

Q. The Van't Hoff factor of solutes A,B and C in aqueous solutions are 0.8,1.6 and 1.2 respectively. The freezing point of equimolar solutions follow the order :

A>B>C

A>C>B

B>A>C

B>C>A

Q. The Van't Hoff factor of solutes $A, B$ and $C$ in aqueous solutions are $0.8, 1.6$ and $1.2$ respectively. The freezing point of equimolar solutions follow the order :

$A > B > C$

$A > C > B$

$B > A > C$

$B > C > A$