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 ..... $^\circ C$.

Van't Hoff factor of $BaCl_2$ in its aqueous solution will be: ($BaCl_2$ is $60 \%$ ionized in the solution)

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

If the freezing point of a $0.01 \ m$ aqueous solution of a cobalt $(III)$ chloride-ammonia complex (which behaves as a strong electrolyte) is $-0.0558^{\circ} C$,the number of chloride $(Cl^-)$ ions in the coordination sphere of the complex is.
$\left[ K_{f} \text{ of water } = 1.86 \ K \ kg \ mol^{-1} \right]$

In which case is Raoult's law not applicable?

When mercuric iodide $(HgI_2)$ is added to an aqueous solution of potassium iodide $(KI)$,the