chemistry

Q: Calculate the pH of a solution that is 0.56 M HC3H5O3 and 1.28 M NaC3H5O3.

I used the H-H equation for this and got this so far:
HC3H5O3 acid
NaC3H5O3 base
pH = pKa + log([NaC3H5O3]/[HC3H5O3])
= -log(Ka of HC3H5O3) + log(1.28/0.56)
= -log(1.4*10^-4) + log(1.28/0.56)
A: pH = 4.2129
However, I'm not sure about the Ka of HC3H5O3 or if it's correct, since I just found it online. Can someone check my numbers?

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  1. Most of your numbers are correct, i suggest you check brainly.com and submit your question.

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  2. I think 4.74 is a better number for pKa of acetic acid. Also, I submit that Jiskha.com is as good as any other site for checking issues.

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