19.5 g of `CH_2FCOOH` is dissolved in 500 gm water. The depression in freezing point in `1^@C`. Calculat the vant factor and dissociation constant of fluroacetic acid.

0.6 mL of acetic acid (CH_3COOH) , having density 1.06g mL^-1 , is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was 0.0205^@C . Calculate the van't Hoff factor and the dissociation constant of acid

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 ?

Calculate the depression of freezing point of water when 1.8 gm glucose dissolves in 250 ml water.

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 .

15 g of a solute in 100 g water makes a solution freeze at -1^@C . 30 g of a solute in 100 g of water will give a depression in freezing point equal to :

The depression in the freezing point of a benzene solution containing 0.784g of Acetic acid dissolved in 100ml of benzene is 0.35k. Calculate the van't Hoff factor and the degree of association of the solute at this concentration (k_(f)" for benzene = 5.10 k.kg.mol"^(-1)," molar mass of acetic acid is 60.01").

A 0.5 percent aqueous solution of KCl was found to freeze at 272.76K. Calculate the Van't Hoff factor and degree of dissociation of the solute at this concentration (K_(f)" for water = 1.86 k.kg.mol"^(-1)) . Normal molar mass of KCl = 74.5.

When some NaCl was dissolved in water, the freezing point depression was numerically equal to twice the molal depression constant. The relative lowéring of vapour pressure of the solution is

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.

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.