Question

A buffer solution contains HC2H3O2 at a concentration of 0.225 M NaC2H3O at a concentration of 0.164 M. The value of Ka for acetic acid is 1.75 × 10-5. Calculate the pH of this solution using the Henderson-Hasselbalch equation. Could you please show steps...thanks a bunch...:)
If you can read and substitute there is nothing to this.
pH = pKa + log[(base)/(acid)]
Calculate pKa from pKa = -log Ka. I think that is something like 4.76. Then
(base) = the acetate = 0.164M
(acid) = the acetic acid = 0.225M
Plug and chug.

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