# What are the hydronium and hydroxide ion concentrations in a solution that has a pH of 12.330?

May 19, 2017

$\left[{H}^{+}\right] = 4.68 \times {10}^{-} 13 M$
$\left[O {H}^{-}\right] = 0.0214 M$

#### Explanation:

The $\left[{H}^{+}\right]$ can be found by raising $10$ to the power of the negative of the $p H$:

$\left[{H}^{+}\right] = {10}^{- 12.330} = 4.68 \times {10}^{-} 13 M$

The $\left[O {H}^{-}\right]$ can be found by dividing the value of the ion-product constant for water, ${K}_{w}$, by the $\left[{H}^{+}\right]$:

$\left[O {H}^{-}\right] = \frac{1.00 \times {10}^{-} 14 M}{4.68 \times {10}^{-} 13 M} = 0.0214 M$