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lha08
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Homework Statement
I'm a little confused, let's say i do a titration curve for a weak acid, at some point there's a buffering range near the pKa. Like i know that if we add a strong base like NaOH to acetic acid in a water solvent, then the OH- will combine with the H+ (hydronium ion) which will shift the equilibrium towards the acetate ion and hydronium ion. But will a different process occur when we add the OH- in the buffering region? Like in my book, it says that it will react with the acetic acid which will form the acetate ion...but i just don't see why this occurs differently then when the OH- reacted with the hydronium ion...
any help/clearing up would be much appreciated
Homework Equations
The Attempt at a Solution
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