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

The correct order of boiling point of the given aqueous solutions is:

The relationship between the van’t Hoff factor $(i)$ and the degree of dissociation $(\alpha)$ is:

If a compound $AB$ dissociates to the extent of $75\,\%$ in an aqueous solution,the molality of the solution which shows a $2.5\, K$ rise in the boiling point of the solution is $......$ molal.
(Rounded-off to the nearest integer) $[K_{b} = 0.52\, K\, kg\, mol^{-1}]$

$0.004 \ M$ $Na_2SO_4$ solution is isotonic with $0.01 \ M$ glucose solution,then the degree of dissociation of $Na_2SO_4$ is ........... $\%$.

The addition of a polar solvent to a solid electrolyte results in