(a) (i) Calculate the freezing point of a solution when 10 · 5 g of MgBr_2 was dissolved in 250 g of water, assuming MgBr_2 undergoes complete…

Calculate the freezing point of a solution when $\displaystyle 10 \cdot 5 \mathrm{~g}$ of $\displaystyle \mathrm{MgBr}_{2}$ was dissolved in $\displaystyle 250$ g of water, assuming $\displaystyle \mathrm{MgBr}_{2}$ undergoes complete dissociation. (Given : Molar mass of $\displaystyle \mathrm{MgBr}_{2}=184 \mathrm{~g} \mathrm{~mol}^{-1}$, $\displaystyle \mathrm{K}_{\mathrm{f}}$ for water $\displaystyle =1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ )

Write two differences between ideal and non-ideal solutions.

A solution is prepared by dissolving $\displaystyle 0.025$ g of potassium sulphate in $\displaystyle 2$ L of water at $\displaystyle 27$°C. Assuming potassium sulphate is completely dissociated, determine its osmotic pressure. (Given : $\displaystyle \mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$, Molar mass of $\displaystyle \mathrm{K}_{2} \mathrm{SO}_{4}=174 \mathrm{~g} \mathrm{~mol}^{-1}$ )

What type of azeotrope will be formed by a solution of acetone and chloroform ? Give reason. []