The elevation in boiling point of a solution is 13.44 g of CuCl₂ in 1 kg of water using the following information will be (molecular weight of CuCl₂ =134.4 and K_b= 0.52 Km^-1).

CuCl₂ is an electrolyte, which ionises in solution as follows 
             $$\begin{gathered} {\mathrm{CuCl}}_2\leftrightharpoons {\mathrm{Cu}}^{2+}+2{\mathrm{Cl}}^{-} \\ \mathrm{At} \mathrm{t}=0 1 \mathrm{mol} 0 0 \\ \mathrm{After} \mathrm{ionisation} (1-\mathrm{\alpha })\mathrm{mol} \mathrm{\alpha } \mathrm{mol} 2\mathrm{\alpha } \mathrm{mol} \end{gathered}$$
Thus, number of particles after ionisation 
                $=1-\mathrm{\alpha }+\mathrm{\alpha }+2\mathrm{\alpha }=1+2\mathrm{\alpha }$
$\therefore$van't Hoff factor
      $\left(\mathrm{i}\right)=\frac{\mathrm{number} \mathrm{of} \mathrm{particles} \mathrm{after} \mathrm{ionisation}}{\mathrm{number} \mathrm{of} \mathrm{particles} \mathrm{before} \mathrm{ionisation}}$
or $$\begin{gathered} \left(\mathrm{i}\right)=\frac{1+2\mathrm{\alpha }}{1} \left(\mathrm{on} 100\% \mathrm{ionisation} \mathrm{\alpha }=1\right) \\ =\frac{1+2\times 1}{1}=3 \end{gathered}$$
The elevation in boiling point (when colligative property is abnormal)
          $$\begin{gathered} ∆{\mathrm{T}}_{\mathrm{b}}=\mathrm{i}\times {\mathrm{K}}_{\mathrm{b}}\times \mathrm{m} \\ \mathrm{m}-\mathrm{molality} \mathrm{of} \mathrm{solution} \\ \mathrm{Molality} \mathrm{of} {\mathrm{CuCl}}_2 \mathrm{solution} \end{gathered}$$
                               $$\begin{gathered} =\frac{{\displaystyle \frac{\mathrm{Weight} \mathrm{of} {\mathrm{CuCl}}_2 (\mathrm{in} \mathrm{gram})}{\mathrm{molecular} \mathrm{weight} \mathrm{of} {\mathrm{CuCl}}_2}}}{\mathrm{Weight} \mathrm{of} \mathrm{water} \left(\mathrm{solvent}\right) \mathrm{in} \mathrm{kg}} \\ =\frac{{\displaystyle \frac{13.44}{13.44}}}{1}=0.1 \mathrm{m} \\ \mathrm{Thus}, ∆{\mathrm{T}}_{\mathrm{b}}=3\times 0.52\times 0.1-0.156-0.{16}^{\mathrm{o}}\mathrm{C} \end{gathered}$$