KBr undergoes 80% dissociation in its 0.5(M) aqueous solution. Calculate osmotic pressure of the solution at `27^(@)C` temperature.

Explanation

Degree of dissociation , `alpha= (i-1)/(n-1)`
on dissociation in water, a molecule of KBr produces 2 ions. [`KBr(aq) to K^(+)(aq) +Br^(-)(aq) ].` Thus , n=2 Given: `alpha=0.8`,
`therefore -0.8 = (i-1)/(2-1)` or, i=1.8.
Hence, the osmotic pressure of the solution at `27^(@)C` or 300K temperature is -
`pi = i xx CRT = 1.8xx0.5xx0.0821xx300`