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

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Express your answer using two decimal places.

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Answer 1 · 2016-07-24T11:08:15

#"pH"=13.30#.

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

#"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#.