# What is the [H^+] in a solution that has a pH of 3.35?

May 3, 2016

$\left[{H}^{+}\right] = 4.47 \times {10}^{- 4} M$

#### Explanation:

The pH of a solution is usually found by the following expression:

$p H = - \log \left[{H}^{+}\right]$

Therefore, to find the concentration of ${H}^{+}$ we can rearrange this expression and thus,

$\left[{H}^{+}\right] = {10}^{- p H}$

$\implies \left[{H}^{+}\right] = {10}^{- 3.35} = 4.47 \times {10}^{- 4} M$