A solute 'A' undergoes association in a medium as `nAiffA_n`
If the degree of association is `'alpha'`, then Van't Hoff factor may be given as :

One mole of a solute A is dissolved in a given volume of a solvent. The association of the solute take place as follows, nA iff A_n If alpha is the degree of association of A, the van't Hoff factor i is expressed as

In which case van't Hoff factor are equal ?

When solute associates in a solution, the value of Vant Hoff factor is,

What is the maximum value of van't Hoff factor for AlCl_3 ?

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

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.

One molal solution of a carboxylic acid in benzene shows the elevation of boiling point of 1.518 K. The degree of association for dimerization of the acid in benzene is (K_b for benzene = 2.53 K kg mol^-1) :

The Van't Hoff factor of 0.005M aqueous solution of KCl is 1.95. The degree of ionisation of KCl is