Calculate elevation in boiling point for 2 molal aqueous solution of glucose.
`(Given : k_b(H_2O) = 0.5 K kg. mol^(-1))`

Calculate the elevation of boiling point of water when 0.6 gm urea is dissolved in 250 ml water given [ K_b 0.52 k.kg mol^(-1) ]

A solution contains 5.6 gm of glucose in 1000 gm of water. Calculate the boiling point of the solution. ( k_b for water = 0.52 K kg mol^-1 )

An aqueous solution of 0.1 molal concentration of sucrose should have freezing point (k_f = 1.86 k mol^(-1) kg)

For a dilute solution containing 2.5 g of a non- volatile non-electrolyte solute in 100 g of water, the elevation in boiling point at 1 atm pressure is 2^@C Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is (take k_b = 0.76 K kg mol^(-1)) .

Calculate the freezing point of an aqueous solution of a non-electrolyte having an osmotic pressure 2.0 atm at "300 K. Kf = 1.86 k.kg.mol"^(-1.)" R = 0.0821 lit.atm.k"^(-1)" mol"^(-1)

Calculate the mass of urea [CO(NH_2)_2] required in making 2.5 kg of 0.25 molal aqueous solution.

Calculate the mass of urea (NH_2CONH_2) required in making 2.5 kg of 0.25 molal aqueous solution.

KBr is 80% dissociated in aqueous solution. The freezing point of a 0.5 molal solution is K_f =1.86 K kg mol^-1

The elevation in boiling point of a solution of 13.44 g of CuCl_2 in 1 Kg of water using the following information will be: (Molecular weight of CuCl_2=134.4 and K_b=0.52 K molal^-1)