To `500 mL` of `0.150 M AgNO_(3)` solution were added `500 mL` of `1.09 M Fe^(2+)` solution and the reaction is allowed to reach an equilibrium at `25^(@)C`
`Ag^(o+)(aq)+Fe^(2+)(aq) hArr Fe^(3+)(aq)+Ag(s)`
For `25` mL of the solution, `30 mL` of `0.0832 M KMnO_(4)` was required for oxidation. Calculate the equilibrium constant for the the reaction `25^(@)C`.

Explanation

Initial conc. Of `AgNO_(3) = ( 0.150)/( 2) = 0.075`
Initial conc. of `Fe^(2+)` solution `= ( 1.09)/( 2)= 0.545`
Final conc. Of `Fe^(2+)` solution ` = ( 30 xx 0.0832 xx 5)/( 25) = 0. 499`
`underset( 0.029) ( Ag^(+)) + underset( 0.499) ( Fe^(2+)) rarr underset( 0.046) ( Fe^(3+)) + Ag`
`K_( C ) = ( [ Fe^(3+) ] )/( [ Ag^(+) ] [ Fe^(2+)] ) = ( 0.046)/( 0.029 xx 0.499)`
= 3.178