Chemistry - Liquid Solution Question with Solution | TestHub

Given, $$\begin{array}{rl}\text{ molality, }\mathrm{m}& =0.0020\mathrm{m}\\ \Delta {\mathrm{T}}_{\mathrm{f}}& =0^{\circ }\mathrm{C}-0.00732^{\circ }\mathrm{C}=0.00732^{\circ }\mathrm{C}\\ {\mathrm{k}}_{\mathrm{f}}& =1.86^{\circ }\mathrm{C}/\mathrm{m}\\ \Delta {\mathrm{T}}_{\mathrm{f}}& =\mathrm{i}\cdot {\mathrm{k}}_{\mathrm{f}}\times \mathrm{m}\\ \mathrm{i}& =\frac{\Delta {\mathrm{T}}_{\mathrm{f}}}{{\mathrm{k}}_{\mathrm{f}}\times \mathrm{m}}\\ & =\frac{0.00732}{1.86\times 0.0020}\\ & =1.96\approx 2\end{array}$$ Since, the compound is ionic, so number of moles produced is equal to vant' Hoff factor, $i$. Hence, 2 moles of ions are produced.