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Consider an experiment where 35.0 ml of 0.175 M acetic acetic acid, HC2H3O3, is titrated with...

Consider an experiment where 35.0 ml of 0.175 M acetic acetic acid, HC2H3O3, is titrated with

0.25 M NaOH. What is the pH at the equivalence point of this titration? The Ka for acetic acid is 1.8 x 10-5.  

Thanks!

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Answer #1

[OH-] = 7.56 x 10-6 M

pOH = -log(7.56 x 10-6) = 5.12

pH = 14.00 - 5.12 = 8.88

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