What is the [OH-] in a solution that has a [H3O+] = 2.0 x 10-2 M?

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What is the [OH-] in a solution that has a [H3O+] = 2.0 x 10-2 M?

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Answer 1 · 2018-06-22T02:01:31

$5.0$ $5.0$ x $10^{- 13}$ $10^-13$

Explanation:

We'll use the ionic product of water formula,

$K_{w}$ $K_w$ = $[H_{3} O^{+}] \cdot [O H^{-}] = 1.0$ $[H_3O^+]*[OH^-] = 1.0$ x $10^{- 14}$ $10^-14$

rearrange the equation,
$[O H^{-}]$ $[OH^-]$
$= 1.0$ $= 1.0$ x $10^{- 14}$ $10^-14$ / $[H_{3} O^{+}]$ $[H_3O^+]$
$= 1.0$ $= 1.0$ x $10^{- 14}$ $10^-14$ / $2.0$ $2.0$ x $10^{- 2}$ $10^-2$
$= 5.0$ $=5.0$ x $10^{- 13}$ $10^-13$

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What is the [OH-] in a solution that has a [H3O+] = 2.0 x 10-2 M?

1 Answer

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