For a $0.25 \ m$ solution of $SrCl_2$,the van't Hoff factor is found to be $2.5$. What will be the effective molality of the solution in $m$?

An aqueous solution of a salt $MX_2$ at a certain temperature has a van't Hoff factor of $2$. The degree of dissociation for this solution of the salt is

For a $0.01 \ m$ aqueous solution of $K_4[Fe(CN)_6]$,if $K_b = 0.52 \ K \ kg \ mol^{-1}$ for the solvent,then its boiling point will be ..... $^\circ C$.

$A$ compound contains $1.08 \ mol$ of $Na, 0.539 \ mol$ of $Cu$ and $2.16 \ mol$ of $F$. Its aqueous solution shows osmotic pressure which is three times that of urea having the same molar concentration. The formula of the compound is:

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

The Van't Hoff factor for a $0.005 \ M$ aqueous solution of $KCl$ is $1.95$. The degree of ionisation of $KCl$ is