If the concentration of `OH^(-)` ions in the reaction
`Fe(OH)_(3)(s)hArrFe^(3+)(aq.)+3OH^(-)(aq.)`
is decreased by `1//4` times, then the equilibrium concentration of `Fe^(3+)` will increase by

Options

A. 64 times
B. 4 times
C. 8 times
D. 16 times

Explanation

`K_(c)=([Fe^(3+)] [OH^(-)]^(3))/([Fe(OH)_(3)])= [Fe^(3+)] [OH^(-)]^(3)`
When `[OH^(-)]` is decreased by 1//4 times then `[Fe^(3+)]` should increase by 64 times to make `K_(c)`, a constant.