The `pH` of a `0.1` molar solution of the acid `HQ` is `3`. The value of the ionisation constant, `K_(a)` of the acid is

Options

A. `1 xx 10^(-3)`
B. `1xx 10^(-5)`
C. `1xx 10^(-7)`
D. `3xx 10^(-1)`

Answer

B

Explanation

`pH =3 , log [(1)/(H^(+))] =3`
`[(1)/(H^(+)]] = " Antilog " 3=10^(3)`
`[H^(+)] =10^(-3) , " Molarity "=0.1M`
`H^(+) sqrt(K_(a) C) " or " (10^(-3)) = sqrt(K_(a)C)`
`10^(-6) =K_(a) xx c " or " K_(a) = (10^(-6))/(c)`
`K_(a) =(10^(-6))/(0.1) =10^(-5)`