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.)

5 . 0 g of phenol dissolved in 250 g of benzene shows a depression in freezing point equal to 0 . 70^(@) C. What is the percentage association of phenol ? ( K_(f) for benzene = 5.12 K kg. MOL^(-1) )

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)

15 g of an unknown molecular substance was dissolved in 450 g of water. The resulting solution freezes at - 0 . 34^(@) C . What is them molar ass of the substance ? ( 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.

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) )

A 1.0 g sample of co (NH_(2)CH_(2)CH_(2)NH_(2))_(3)Cl_(3) is dissolved in 25.0 g if water and the freezing point of the solution is -0.87^(@)C . How many ions are produced per mole of compound? The K_(f) of water is 1.86^(@)C//"molal"

When 36.0 g of a solute having the empirical formula CH_(2)O is dissovled in 1.20 kg of water, the solution freezes at -0.93^(@)C . What is the moleculer formula of the solute ? ( K_(f) = 1.86^(@)C 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?