Calculate the freezing point of solution when 1.9 g of `MgCl_2(M=95 g mol^-1)` was dissolved in 50 g of water, assuming `MgCl_2` undergoes complete ionization. `(K_f for water= 1.86 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) .

18 g of glucose is dissolved in 1 kg of water. At what temperature will the solution boil ? ( K_b for water is 0.52 K kg "mol"^(-1) )

Ethylene glycol (molar mass = 62gmol^-1) is a common automobile antifreeze. Calculate the freezing point of a solution containing 12.4 g of this substance in 100 g of water. Would it be advisable to keep this substance in car radiator during summer? (K_f for water=1.86Km^-1 and K_b for water=0.512Km^-1) .

45g of ethylene glycol (C_2H_6O_2) is mixed with 600 g of water. Calculate: the freezing point of the solution. (K_f for water=1.86K kg mol^-1) .

2.82g of glucose (Molar mass: 180g mol^-1 ) are dissolved in 30g of water . Calculate mole fraction of glucose and water.

Calculate the amount of CaCl_(2) (molar mass = 111g "mol"^(-1) ) which must be added to 500 g of water of lower its freezing point by 2K, assuming CaCl_(2) is completely dissociated. (Kf for water = 1.86 k kg "mol"^(-1) ).

The freezing point of a solution containing 0.1g of K_3[Fe(CN)_6] in 100 g of water. (K_f=1.86 K kg mol^-1) is

Calculate the molarity of a solution containing 11.7 g of NaCl in 2.0 L solution. (M_(NaCl)=58.5 g mol^-1)