Thursday
July 24, 2014

Homework Help: Chemistry

Posted by Saira on Wednesday, July 15, 2009 at 12:40am.

A 0.040M solution of a monoprotic acid is 14% ionized. Calculate the Ka for the weak acid.

----------------
so:
HX <---> H+ + X-

Ka= [H+][X-]/ [HX]

Since its a monoprotic acis i know the concentration of H and X will be equal

And the HX will be 86% (100%-14%)

BUt i m not sure how to solve for it

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