A decimolar solution of potassium ferrocyanide is `50%` dissociated at `300K`. Calculate osmotic pressure of the solution. (Given `R = 8.341 JK^(-1) mol^(-1)`)

Explanation

Given, Molarity `= (n)/(V) = 0.1` mol `litre^(-1)`
`(0.1)/(10^(-3))` mol `m^(-3) = 10^(2)` mol `m^(-3)`
because `pi_(N) xx V = nRT`
`pi_(N) = (n)/(V)RT`
`pi_(N) = 10^(2) xx 8.314 xx 300 Nm^(-2)`
For `{:(K_(4)Fe(CN)_(6),hArr,4K^(+)+,Fe(CN)_(6)^(4-),),(1,,0,0,),(1-alpha,,4alpha,alpha,):}`
where `'alpha'` is degree of dissociation.
Given, `alpha = 0.5`
`(pi_(exp.))/(pi_(N)) = 1+4alpha`
`therefore pi_("exp.") = pi_(N)(1+4alpha)`
`= 10^(2) xx 8.314 xx 300 xx (1+4xx0.5)`
`= 10^(2) xx 8.314 xx 300 xx (1+2)`
`= 7.483 xx 10^(5) Nm^(-2)`