The concentration of `[H^(+)]` and concentration of `[OH^(-)]` of a `0.1` aqueous solution of `2%` ionised weak acid is [Ionic product of water `=1xx10^(-14)`]

Options

A. `0.02 xx 10^(-3)` and `5 xx 10^(-11) M`
B. `1 xx 10^(-3) M` and `3 xx 10^(-11) M`
C. `2 xx 10^(-3) M ` and `5 xx 10^(-12) M`
D. ` 3 xx 10^(-2) M` and `4 xx 10^(-13) M`

Answer

C

Explanation

Concentration of `[H^(+)]` ions
`=1 xx 0.1 xx (2)/(100)M =2 xx 10^(-3)M`
But `[H^(+)][OH^(-)]=10^(-14)`
`[2 xx10^(-3)][OH^(-)]=10^(-14)`
or `[OH^(-)]=(10^(-14))/(2 xx 10^(-3))=5 xx 10^(-12)`