Calculate the boiling point of 1(M) KCI soln density 1.04 gm/cc `(Kb =0.52K. 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 )

Calculate the number of moles in 1.5 gm of amonia.

0.900g of a solute was dissolved in 100 ml of benzene at 25^(@)C when its density is 0.879 g/ml. This solution boiled 0.250^(@)C higher than the boiling point of benzene. Molal elevation constant for benzene is "2.52 K.Kg.mol"^(-1) . Calculate the molecular weight of the solute.

Calculate the molar conductance of 0.01 (M) KCI solution. Sp. conductance of KCI is 0.07 cm^(-1) ohm^(-1) . Define molar conductance?

A solution containing 6 gm of a solute dissolved in 250 ml of water gave an osmotic pressure of 4.5 atmosphere at 27^(@)C . Calculate the boiling point of the solution. The molal elevation constant for water is 0.52

A solution of 2.44xx10^-3 kg of a nonelectrolyte solute dissolved in 0.075 kg of water boiled at 100.413^@C . Calculate the molecular mass of the solute. K_b for water = 0.52 K kg mol^-1

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

Calculate the depression of freezing point of 0.1 (M) aqueous soln. of an weak acid for 20% dissociation given Kf = 1.86 k//hg mol^-1 .

The normality off 10% H_(2)SO_(4) solution having density 1.1g/cc is-

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) ]