Calculate the normal freezing point of a sample of sea water containing 3.8% NaCl and 0.12% `MgCl_2` by mass. `(K_f for water=1.86Km^-1)`

Calculate the boiling point of a solution prepared by adding 15.00 g of NaCl to 250.0 g of water. (K_b for water= 0.512 K kg mol^-1) and molar mass of NaCl= 58.44 g mol^-1

Calculate the freezing point of a one molar aqueous solutoin (density 1.04gL^-1) of KCl. ( K_f of water=1.86Kg mol^-1 , atomic masses of K=39, Cl=35.5)

Calculate mole fraction of ethanol and water in a sample of rectified spirit which contains 92% ethanol by mass.

in a cold climate water gets frozen causing damage to the radiator of a car . Ethylene glycol is used as an antifreezing agent . Calculate the amount of ethylene glycol to be added to 4kg of water to prevent it from freezing at -6^@ C . ( K_f for water 1.85 Km^-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 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)

Calculate the boiling point of a one molar aqueous solution of KBr (density 1.06g mL^-1) . ( K_b for water= 0.52kgmol^-1 , atomic masses: K=39, Br=80)

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)

If sodium sulphate is considered to be compeltely dissociated into cations and anions in aqueous soluton, the change in freezing point of water, when 0.01 mole of sodium sulphate is dissolved in 1 k gof water is (K_f=1.86K kg mol^-1)