In an aqueous solution of potassium ferrocyanide,the degree of dissociation of the salt is $80\%$. The value of the van't Hoff factor is:

In equimolar solutions of glucose,$NaCl$,and $BaCl_2$,the order of osmotic pressure is as follows:

The Van't Hoff factor will be highest for

What is the freezing point (in $^\circ C$) of a solution containing $0.1 \ g$ of $K_3[Fe(CN)_6]$ (molar mass = $329 \ g \ mol^{-1}$) in $100 \ g$ of water? (Given $K_f = 1.86 \ K \ kg \ mol^{-1}$)

The experimental molecular weight of an electrolyte will always be less than its calculated value because the value of Van't Hoff factor $i$ is

We have three aqueous solutions of $NaCl$ labelled as '$A$','$B$' and '$C$' with concentrations $0.1 \ M$,$0.01 \ M$,and $0.001 \ M$ respectively. The value of the Van't Hoff factor for these solutions will be in the order . . . . . . .