What is the pH of a 0.10 M solution of barium hydroxide, Ba(OH)_2?

Jul 24, 2016

$\text{pH} = 13.30$.

Explanation:

Barium hydroxide is a strong base for both stages of dissociation:

${\text{Ba"("OH")_2(s) -> "Ba"^{2+}+2"OH}}^{-}$

So the solution will have 0.20 M hydroxide ions. Now use the autodissociation product for water:

["H"^+]["OH"^-]=1.0xx10^{-14}"M"^
["OH"^-]=2.0xx10^{-1}"M"
["H"^+]=5.0xx10^{-14}"M"

And then

"pH"=-log_{10}(["H"^+]=5.0xx10^{-14})=13.30.