What is the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2?

Express your answer using two decimal places.

1 Answer
Jul 24, 2016

pH=13.30.

Explanation:

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

Ba(OH)2(s)Ba2++2OH

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

[H+][OH]=1.0×1014M
[OH]=2.0×101M
[H+]=5.0×1014M

And then

pH=log10([H+]=5.0×1014)=13.30.