The H+ ion concentration of a solution is 4×10−5M . Then the OH− ion concentration of the same solution is

[OH−]=Kw[H+] =1×10−144×10−5 =2.5×10−10

The H+ ion concentration of a solution is 4×10−5M . Then the OH− ion concentration of the same solution is

[OH−]=Kw[H+] =1×10−144×10−5 =2.5×10−10

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The $H^{+}$ ion concentration of a solution is $4 \times 10^{- 5} M$ . Then the $O H^{-}$ ion concentration of the same solution is

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$4 \times 10^{- 5} M$

$2.5 \times 10^{- 10} M$

$1.0 \times 10^{- 7} M$

$2.5 \times 10^{- 9} M$

answer is D.

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Detailed Solution

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

$= \frac{1 \times 10^{- 14}}{4 \times 10^{- 5}}$

$= 2.5 \times 10^{- 10}$

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The H+ ion concentration of a solution is 4×10−5M . Then the OH− ion concentration of the same solution is

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The $H^{+}$ ion concentration of a solution is $4 \times 10^{- 5} M$ . Then the $O H^{-}$ ion concentration of the same solution is