# What is the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C?

May 27, 2016

$p O H$ $=$ $9.67$, i.e. $\left[H {O}^{-}\right]$ $=$ ${10}^{- 9.67}$

#### Explanation:

For water at $298 \cdot K$. $p {K}_{w}$ $=$ $14$

And $p {K}_{w}$ $=$ $p O H$ $+$ $p H$ $=$ $14$, thus $p O H$ $=$ $9.67$

$\left[H {O}^{-}\right]$ $=$ ${10}^{- 9.67} \cdot m o l \cdot {L}^{-} 1$.