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Byju's Answer

Standard XII

Chemistry

Auto Protolysis of Water

The concentra...

Question

The concentration of $[H^{+}]$ and concentration of $[O H^{+}]$ of a $0.1 M$ aqueous solution of $2 %$ ionised weak acid is [ionic product of water $= 1 \times 10^{- 14}$ ]

2 \times 10^{- 3} M

and

5 \times 10^{- 12} M

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1 \times 10^{- 3} M

and

3 \times 10^{- 11} M

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0.02 \times 10^{- 3} M

and

5 \times 10^{- 11} M

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3 \times 10^{- 2} M

and

4 \times 10^{- 13} M

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Solution

The correct option is B $1 \times 10^{- 3} M$ and $3 \times 10^{- 11} M$
$H A$ $⇌$ $H^{+} + A^{-}$
t=0: $c$
t=t: $c (1 - α)$ $c α$ $c α$
$∴$ $[H^{+}] = c α = 0.1 \times 0.02 = 2 \times 10^{- 3}$
Hence $[O H^{-}] = \frac{10^{- 14}}{2 \times 10^{- 3}} = 5 \times 10^{- 12}$

Hence, Option "B" is the correct answer.

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The concentration of [H+] and concentration of [OH+] of a 0.1M aqueous solution of 2% ionised weak acid is [ionic product of water =1×10−14]

The correct option is B 1×10−3M and 3×10−11M HA ⇌ H++A−t=0: c t=t: c(1−α) cα cα ∴ [H+]=cα=0.1×0.02=2×10−3Hence [OH−]=10−142×10−3=5×10−12Hence, Option "B" is the correct answer.

The concentration of $[H^{+}]$ and concentration of $[O H^{+}]$ of a $0.1 M$ aqueous solution of $2 %$ ionised weak acid is [ionic product of water $= 1 \times 10^{- 14}$ ]