The concentration of $[H^{+}]$ and concentration of $[OH^{-}]$ of a $0.1 \ M$ aqueous solution of $2\%$ ionised weak acid is [Ionic product of water $= 1 \times 10^{-14}$]
- A$2 \times 10^{-3} \ M$ and $5 \times 10^{-12} \ M$
- B$1 \times 10^3 \ M$ and $3 \times 10^{-11} \ M$
- C$0.02 \times 10^{-3} \ M$ and $5 \times 10^{-11} \ M$
- D$3 \times 10^{-2} \ M$ and $4 \times 10^{-13} \ M$
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