(a) Calculate the freezing point of solution when $1.9\mathrm{g}$ of ${\mathrm{MgCl}}_2\left(\mathrm{M}=95\mathrm{g}{\mathrm{mol}}^{-1}\right)$ was dissolved in $50\mathrm{g}$ of water, assuming ${\mathrm{MgCl}}_2$ undergoes complete ionization. $({\mathrm{K}}_{\mathit{f}}.$ for water $=1.86\mathrm{K}\mathrm{kg}$ ${\mathrm{mol}}^{-1}$ )
(b) (i) Out of $1\mathrm{M}$ glucose and $2\mathrm{M}$ glucose, which one has a higher boiling point and why?
(ii) What happens when the external pressure applied becomes more than the osmotic pressure of solution?
OR
(a) When $2.56\mathrm{g}$ of sulphur was dissolved in $100\mathrm{g}$ of ${\mathrm{CS}}_2$, the freezing point lowered by $0.383\mathrm{K}$. Calculate the formula of sulphur $\left({\mathrm{S}}_{\mathrm{X}}\right)$. $({\mathrm{K}}_{\mathit{f}}.$ for ${\mathrm{CS}}_2=3.83\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1}$, Atomic mass of Sulphur $=32\mathrm{g}{\mathrm{mol}}^{-1})$
(b) Blood cells are isotonic with $0.9\%$ sodium chloride solution. What happens if we place blood cells in a solution containing;
(i) $1.2\%$ sodium chloride solution ?
(ii) $0.4\%$ sodium chloride solution ?.