Calculate the boiling point of solution when 4g of Mg `SO_(4) (M=120g "mol"^(-1))` was dissolved in 100g of water, assuming `MgSO_(4)` undergoes complete ionization
`(K_(b) " for water " = 0.52 K " kg mol"^(-1))`

Calculate the boiling point of solution when 2 g of Na_(2)SO_(4) (M = 142 g mol^(-1) ) was dissolved in 50g of water , assuming Na_(2)SO_(4) undergoes complete ionization . ( k_(b) for water = 0.52 K kg mol^(-1) ).

Calculate the boiling point of solution when 2 g of Na_2SO_4 (M=142gmol^-1) was dissolved in 50 g of water, assuming Na_2SO_4 undergoes complete ionization. (K_b for water=0.52 K kg mol^-1) .

Calculate the freezing point of solution when 1.9 g of MgCl_(2) (M = 95 g Mol^(-1) ) was dissolved in 50g of water, assuming MgCl_(2) undergoes complete ionization. ( K_(f) for water = 1.86 K kg mol^(-1) ).

(a) Calculate the freezing point of solution when 1.9 g of MgCl_(2) (M = 95 g Mol^(-1) ) was dissolved in 50g of water, assuming MgCl_(2) undergoes complete ionization. ( K_(f) for water = 1.86 K kg mol^(-1) ). (b) (i) Out of 1 M glucose and 2 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?

Calculate the freezing point of a solution when 3 g of CaCI_(2) (M=111 g mol^(-1)) was dissolved in 100g of water assuming that CaCI_(2) undergoes complete ionisation (K_(f) "for water"=1.86 K kg mol^(-1)) .