2.00 g of non=electrolyte solute dissolved in 100 g of benzene lowered the freezing point of benzene by 0.50K. The freezing point depression constant of benzene is 5.12 K kg `mol^(-1)`. Find out the relative molar mass of the solute.

1.00 g of a non-electrolyte dissolved in 50.5g of benzene lowered its freezing point by 0.40K. The freezing point depression constant of benzene is "5.12K.kg mol"^(-1) . Find the molecular mass of the solute.

2g of benzoic acid (C_6H_5COOH) dissolved in 25 g of benzene shows a depression in freezing point equal to 1.62 K. Molal depression constant for benzene is 4.9 k kg mol^-1 . What is the percentage association of acid if it forms dimer in solution ?

34.2 gm Sucrose (Molecular wt 342) is dissolved in 1000 gm of water. Find the freezing-point of the solution kf = 1.86 K Kg mol^-1

The fraction of phenol dimerised in benzene if 20 g of phenol in 1 kg benzene exhibits a freezing point depression of 0.69 K. ( K_f benzene) =5.12 kkg/mol),(MW of phenol=94)

What is the weight of 1 mole of a solute,0.132g of which in 29.7 g benzene gave a freezing point depression of 0.108^@C ? ( K_f for benzene = 5.12)

When 20 g of naphthoic acid (C_11H_8O_2) is dissolved in 50 g of benzene , a freezing point depression of 2K is observed. The vant Hoff factor (i) is [ K_f="1.72 K kg mol"^(-1) ]

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.

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

A solution containing 2.5 g of a non-volatile solute in 100 gm of benzene boiled at a temperature 0.42K higher than at the pure solvent boiled. What is the molecular weight of the solute? The molal elevation constant of benzene is "2.67 K kg mol"^(-1) .

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)) .