Why has van't Hoff factor `i` higher value for electrolyte in aqueous solution?

Explanation

In case of dissociation of an electrolyte, the number of particles in the solution is increased after dissociation.
If `x` is the number of particles before dissociation and y after dissociation, then `y gt x`.
van't Hoff factor `i` is ,
`"i"=("Observed colligative property")/("Theoretical colligative property")`
`=("Final number of particles (y)")/("Initial numner of particles (x)")`
`because y gt x`
`therefore i gt 1`