# What is the H+ concentration (in molarity) of a solution with a pOH of 6.7?

Jun 7, 2016

$\left[{H}^{+}\right] = 5.01 \times {10}^{- 8} M$

#### Explanation:

You want to use the following relationship:

$p O H + p H = 14$

Since we are given the pOH, we can determine the pH by subtracting the pOH from 14 like so:

14 - pOH = 7.3.

7.3 represents the pH of the solution and we can obtain the concentration of hydrogen ions in solution by taking the antilog of the pH. The antilog is ${10}^{-}$ raised to some value, which is ${10}^{- 7.3}$ in our case.

${10}^{- 7.3}$ = $5.01 \times {10}^{- 8} M$

Tips:
$\left[{H}^{+}\right]$ = antilog(-pH)
pH = -log$\left[{H}^{+}\right]$

I hope this explanation is understandable!