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

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Answer 1 · 2016-05-03T13:44:21

$[H^{+}] = 4.47 \times 10^{- 4} M$ $[H^+]=4.47xx10^(-4)M$

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

$p H = - log [H^{+}]$ $pH=-log[H^+]$

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

$[H^{+}] = 10^{- p H}$ $[H^+]=10^(-pH)$

$\Rightarrow [H^{+}] = 10^{- 3.35} = 4.47 \times 10^{- 4} M$ $=>[H^+]=10^(-3.35)=4.47xx10^(-4)M$

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