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))`.

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 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 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) ).