Posted by Alexis on Wednesday, August 6, 2008 at 12:18am.
The Henderson-Hasselbalch equation is
pH = pKa + log [(base)/(acid)]
pKa = 4.74 from Ka.
Generally it is easy to prepare a buffer within 1 pH of the pKa. You can work through the calculation if you wish; for example, if equal amounts of acid and base are chosen, then (B) = (A), the ratio is 1 and log of that term is 0 and pH = 4.74 which is very close to the desired pH.
After I went to bed I realized that part of my answer might be confusing. By (B)= (A), I am referring to base = acetate ion an acid = acetic acid. To GET equal amount of acetate ion and acetic acid, one reacts X amount of NaOH and twice that amount of acetic acid. That produces X amount of acetate ion, leaves an equal amount of acetic acid, and none of the NaOH you started with. I hope this helps clear things up.
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