19.5g of `CH_(2)FCOOH` is dissolved in 500g of water. The depression in 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)COOH) , 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 . Calculate the van't Hoff factor and the dissociation constant of acid.

9.5g of MgCl_(2) is dissolved in 100 g of water . The freezing point of the solution is -4.836^(@)C Then .

0.1 mole of NaCl is dissolved in 100g of water. The mole fraction of NaCl is

1.2 mL acetic acid having density 1.06 g cm^(-3) is dissolved in 1 litre of water. The depression in freezing point observed for this concentration of acid was 0.041 ""^(@)C . The van't Hoff factor of the acid is ( K_(f) of water = 1.86 K kg mol^(-1) )

0.1 gram mole of urea is dissolved in 100g. of water. The molality of the solution is

0.1 gram mole of urea is dissolved in 100g. of water. The molality of the solution is

2 g of benzoic acid (C_(6)H_(5)COOH) dissolved in 25g 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 precentage association of acid if it forms dimer in solution ?