Van't Hoff factor of centimolal solution of `K_(3) [Fe(CN)_(6)]` is 3.333 . Calculate the percent dissociation of `K_(3) [Fe (CN)_(6)]`

Answer

78

Explanation

`K_3[Fe(CN)_6] hArr 3K^(+) +[Fe(CN)_6]^(3-)`
If `alpha` is the degree of dissociation, then
`{:(1-alpha,3alpha,alpha):}`
Total moles after dissociation `=1-alpha+3alpha + alpha`
`=1+3alpha`
`i=(1+3alpha)/1 = 3.333 `
`3alpha =3.333-1=2.333 `
`alpha = (2.333)/3` =0.78 or 78 %.