Addition of 0.643 `g` of a compound to 50. `mL` of benzene .(density 0.879 `g/mL` lowers the freezing point from 5.51^0C to 5.03^0C. If `K_(f)` for benzene is 5.12 `K kg mol^1`, calculate the molar mass of the compound.

When 1.3 g of a solute is dissolvedf in 169 g of water the boiling point of the solution is 100.025^@C at one atmospheric pressure. If K_b of water is 0.52 K kg mol^(-1) . Calculate the molecular mass of the solute.

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.

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) .

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 )

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 .

15 gm of a substance dissolved in 450 gms of water produces a depression of -0.34^@ C in the freezing point . Calulation the Mol. Wt. of the solid ( K_f for water is 1.86 K kg mol ^(-1) )

A current of 0.5 A flowing for 30 min deposits 0.2964g of a metal at the cathode. Calculate the equivalent mass of the metal.

The freezing point depression of 0.1 molal solution of acetic acid in benzene is 0.256 K kg mol^(-1) .Kf for benzene is 5.12 K kg Mol^(-1) . What conclusion can you draw about the molecular state of acetic acid in benzene.