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Common Ion Effect

Which of the ...

Question

Which of the following expressions is/are true?

[H^{+}] = [O H^{-}] = \sqrt{K_{w}}

for a neutral solution

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[O H^{-}] < \sqrt{K_{w}}

for an acidic solution

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p H + p O H = 14

at all temperature

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[O H^{-}] = 10^{- 7} M

25^{\circ} C

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Solution

The correct options are
A $[H^{+}] = [O H^{-}] = \sqrt{K_{w}}$ for a neutral solution
B $[O H^{-}] < \sqrt{K_{w}}$ for an acidic solution
D $[O H^{-}] = 10^{- 7} M$ at $25^{\circ} C$
For neutral water,

$K_{w} = [H^{+}] [O H^{-}]$ so $[H^{+}] = [O H^{-}] = \sqrt{K_{w}}$ .

And for acidic solution as hydrogen ion conc. increases so hydroxide ion decreases and $[O H^{-}] < \sqrt{K_{w}}$ .

$[O H^{-}] = 10^{- 7} M$ at $25^{o} C$ and $p H + p O H = 14$ at $25^{o} C$ only.

Suggest Corrections

Similar questions

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K_{w}

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[H^{+}] [O H^{-}] = 10^{- 14}

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