Are there any good approximation available

Reference no: EM13171804

Although it doesn't particularly want to give up a proton itself, boric acid, B(OH)3, acts as an acid in water because of the reaction:

B(OH)3 + H20 <-> B(OH)4^-1 + H+

Given that the Ka of boric acid is 5.8x10^-10M, what is the pH of a 0.50M boric acid solution? Are there any good approximation available?

Reference no: EM13171804

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