1g of a non-electrolyte when dissolved in 50g benzene, the freezing point of solvent is lowered by 0.40K. Find molecular mass of solute. (`K_f` for benzene is 5.12 K kg `mol^-1`)

0.48g of a non volatile solute was dissolved in 10.6g benzene. The freezing point of the solution was lowered by 1.8^@ C. calculate molecular mass of the salute ( K_f for benzene is 5kgmol^(-1) )

The boiling point of benzene is 353.2 K .When 1.8 g of a non - volatile solute was dissolved in 90 g benzene the boiling point was raised to 354.1 K . Calculate the molecular mass of the solute. ( K_b of benzene = 2.53 K kg mol^-1 )

Addition of 1.5g of a non-volatile solute in 90g benzene increases its boiling point by 0.88^@C . calculate molecular mass of solute. ( k_b for benzene=2.53 k kg mol^-1 .

3g urea is dissolved in 100ml water. Find the freezing point of solution ( K_f = 1.86k kg mol_(-1) )

The freezing point of a solution containing 0.3 g of acetic acid in 30 g of benzene is lowered by 0.45^@c . Calculate the Vant's hoff factor (K_f for benzene = 5.12 K kg mol^-1) .

A solution containing 12.5 g of a non-electrolyte in 175 g of water gave elevation in boiling point of O.70 K . Calculate the molar mass of the substance. (K_(b)for water = 0.52 K kg mol^-1 )

Two elements A and B form compounds having molecular formula AB_(2) and AB_(4) When dissolved in 20 g of benzene, 1 g of AB_(2) lowers the freezing point by 2.3 K, whereas 1.0 g of AB_(4) lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol^-1 . Calculate the atomic mass of A and B.

2g of benzoic acid (C_(6)H_(5)COOH) dissolved in 25 g of benzene shows a depression in freezing point equal to 1.62 K. Molar depression constant for benzene is 4.9 K kg mol^-1 . What is the percentage association of acid if it forms double molecules (dimer) in solution ?