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

0 . 6 ml of acetic acid (CH_(3) CO OH) having density 1 . 0 6 g mL^(-1) dissolved in 1 litre of water . The depression in freezing point observed for this strength of acid was 0.0205 K. Calculate the Van't Hoff factor and dissociation constant of the acid .( K_(f) for water = 1. 86 K kg mol^(-1) )

19.5 g of CH_2FCOOH is dissolved in 500 g of water. The depression in the freezing point of water observed is 1.0° C. Calculate the van’t Hoff factor and dissociation constant of fluoroacetic acid.

Will the depression in freezing point be same or different if 0.1 mole of sugar or 0.1 mole of glucose is dissolved in one litre of water?

The density of a 2.05 M acetic acid in water is 1.02gcm^-3 . Calculate the molality of the solution.

0.01 m aqueous solution of sodium sulphate depresses the freezing point of water by 0.0284^@C . Calculate the degree of dissociation of the salt. (k_f of water = 1.86 Km^-1)

The density of 2.05 M acetic acid in water is 1.02 g/ml . Calculate the molality of solution.

3.9 g of benzoic acid dissolved in 49 g of benzene shows a depression in freezing point of 1.62K. Calculate the Van't Hoff factor and predict the nature of solute (associated or dissociated). (Given: Molar mass of benzoic acid= 122 gmol^-1 , K_f for benzene= 49 K kg mol^-1 )

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

1 . 5 of Ba (NO_(3))_(2) dissolved in 100 g of water shows a depression in freezing point equal to 0 . 28^(@)C . What is the percentage dissociation of the salt ? ( K_(f) for water = 1 . 86 K/m and molar mass of Ba (NO_(3))_(2) = 261.)