pH is a unitless number used to convey the acidity of a substance without having to deal with numbers in scientific notation. You must use an *extra significant digit* when calculating it (and drop a digit when you are going from pH to concentration). You can go between pH and concentration with these equivalent formulae:

`"pH" = - log["H"^+] qquad <=> qquad ["H"^+] = 10^(-"pH")`.

The pH value tells us about the acidity of a solution:

- `"pH" = 7 =>` neutral
- `"pH" < 7 =>` acidic
- `"pH" > 7 =>` basic

pOH is just like pH, except it uses the hydroxide ion concentration:

`"pOH" = - log["OH"^-] qquad <=> qquad ["OH"^-] = 10^(-"pOH")`.

If you have one of pH and pOH, you can easily find the other (at SATP):

`"pH" + "pOH" = 14`.

Calculate the concentrations of H^{+}_{(aq)} and OH^{−}_{(aq)} and the values of pH and pOH for a 0.042 mol/L H_{2}SO_{4(aq)} solution.

H_{2}SO_{4(aq)} is a strong acid, so finding the H^{+}_{(aq)} concentration is trivial:

`["H"^+] = 2["H"_2"SO"_4] = 2(0.042\ "mol/L") = 0.084\ "mol/L"`.

Now we can use this to calculate pH. Remembering to keep an extra significant digit, we have

`"pH" = - log["H"^+] = - log(0.084\ "mol/L") = 1.08`,

and then we can calculate pOH with

`"pOH" = 14 - "pH" = 14 - 1.08 = 12.9`.

From that we can get the hydroxide ion concentration, remembering to drop the extra significant digit:

`["OH"^-] = 10^(-"pOH") = 10^(-12.9) = 1.2xx10^-13\ "mol/L"`.

We could have also used the ion product constant for water to get from H

^{+}concentration to OH^{−}concentration, but this way is faster.