(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

100mL of 0.10M HNO_{3}was added to a 100mL mixture containing 0.30M acetic acid and 0.10M sodium acetate.

Ka = 1.8 x 10-^{5 }

2. Relevant equations

CH_{3}COOH [tex]\rightarrow[/tex] H^{+}+ CH_{3}COO^{-}

CH_{3}COONa [tex]\rightarrow[/tex] Na^{+}+ CH_{3}COO^{-}

CH_{3}COO^{-}+ H^{+}[tex]\rightarrow[/tex] CH_{3}COOH

3. The attempt at a solution

CH_{3}COO^{-}+ H^{+}[tex]\rightarrow[/tex] CH_{3}COOH

I used the ICE table for this

and it turns out that the molarity of CH_{3}COO^{-}and H^{+}are both = 0 at equilibrium...

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# Homework Help: [Chem] Buffer solution with acetic acid

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