Calculate the molality of NaCl solution whose elevtaion in boiling point is equal to the depresson in freezing point of 0.25 m sodium carbonate the solution in water assuming complete dissociation of salts. `(K_f=1.86 Km^-1, K_b=0.52Km^-1)`

0.01 M solution each of ura, common salt and sodium sulphate are taken, the ratio of depression in freezing point of thes solutions is

0.01 m aqueous solution of sodium sulphate depresses the freezing point of water by 0.0284^@C . Calculate the degree of dissociation of the salt. (k_f of water = 1.86 Km^-1)

0.5 molal aqueous solution of a weak acid is 20% iionized. If K_f for water is 1.86K kg mol^-1 . The lowering in freezing point of the solution is

Calculate the freezing point of an aqueous solution of a non electrolyte having an osmotic pressure at 2 atm at 300K (K_f=1.86Cm^-1, R=0.082 L atm K^-1 mol^-1)

True or false Elevation in boiling point of 0.1 m NaCl solution will be nearly twice that of 0.1 m glucose solution.

Calculate the depression in the freezing point of water when 10 g of CH_3CH_2CHClCOOH is added to 250 g of water. K_a = 1.4 x 10^(-3) , K_f = 1.86 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) .

0.2 m aqueous solution of a weak acid is 20% dissociated. The boiling point of this solution is (K_(b) of water= 0.52Km^-1)