2 g of benzoic add `(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 `4.98 K kg mol^(-1)`. What is the percentage assodation of the acid if it forms dimer in solution.

1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene of 0.40K. The freezing point depression constant of benzene is 5.12K kgmol^(-1) . Find the molar mass of the solute .

0.440 g of a substance dissolved in 22.2 g of benzene lowered the freezing point of benzene by 0.567 ^(@)C . The molecular mass of the substance is _____ (K_(f) = 5.12 ^(@)C kg mol ^(-1))

A solution of citric acid C_6H_6O_7 in 50 g of acetic and has boiling point elevation of 1.76 K. if K_b for acetic acid is 3.07 K kg mol^(-1) , What is the molality of solution?

The observed depression in the freezing print of water for a particular solution is 0.087 K. Calculate the molality of the solution if molal depression constant for water is 1.86 K kg. mol^(-1) .

A 0.1m solution of K_2SO_4 in water has freezing point of -4.3^@C . What is the value of van't Hoff factor if Kf for water is 1.86 K kgmol^(-1) .

1.250 g of naphthalene was dissolved in 60 cm3 of benzene and freezing point of the solution was found to be 277.515 K while that of benzene 278.495 K. Density of benzene is 0.880 g cm^(-3) Kf = 5.1 K mol^(-1) kg. Calculate the molecular weight of naphthalene.

The freezing point of a solution containing 4.8 g of a compound in 60 g of benzene is 4.48 ^(@) C . What is the molar mass of the compound ? (K_(f)=5.1 Km^(-1) , freezing point of benzene =5.5^(@)C )

1.02 g of urea when dissolved in 98.5 g of certain solvent decreases its freezing point by 0.211K. 1.609 g of unknown compound when dissolved in 86 g of the same solvent depresses the freezing point by 0.34 K. Calculate the molar mass of the unknown compound.(molar mass of urea = 60 g/mol )