Define van't Hoff factor . How is it rel...

Define van't Hoff factor . How is it related to the degree of dissociation ?

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**Step-by-Step Solution:** 1. **Definition of van't Hoff Factor (i):** The van't Hoff factor (i) is defined as the ratio of the actual number of particles in solution after dissociation to the number of formula units of the solute that were initially dissolved. It indicates how many particles a solute breaks into when it dissolves in a solvent. Mathematically, it can be expressed as: \[ i = \frac{\text{actual number of particles in solution}}{\text{number of formula units of solute dissolved}} ...

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van't Hoff factor (i)

Is less than one in case of dissociation

is more than one in case of association

i=normal molecular mass /oberved molecular mass

i=observed molecular mass/normal molecular mass

Benzoic acid undergoes dimerisation in benzene solution. The van't Hoff factor (i) is related to the degree of association (alpha) of the acid as

`i = 2 -alpha`

`i= 1 + (alpha//3)`

`i = 1 - (alpha//2)`

`i = 1 + (alpha//2)`

Benzoic acid undergoes dimerisation in benzene solution, the van't Hoff factor 'i' is related to the degree of association 'x' of the acid as

i= (1 - x)

i = (1 + x)

i = (1 - x/2)

i = (1 + x/2)