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

Calculate the pH after 0.030 mol NaOH is added to 1.00 L 0.100 M HC3H5O2 and 0.100 M NaC3H5O2

2. Relevant equations

Ka=[H+][A-]/[HA]

pH=-log([H+]) or 14-pOH=ph

3. The attempt at a solution

HC3H5O2 <-> H^{+}+ C3H5O2^{-}

NaC3H5O2 <-> Na^{+}+ C3H5O2^{-}

I know that Na+ has no acid/base properties, so I think that this equation is unimportant and I will be focusing on the first equation. I also know Ka_{eq1}=1.3x10^{-5}

I tried to set up an equilibrium equation, but I'm not sure if I should be completely ignoring the sodium equation.

1.3x10^{-5}=(x^{2})/(.100-.030)

the numerator= [H+][C3H5O2-]

Any input would be appreciated...

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# Homework Help: Buffers, pH, and strong base

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