[jdmbo1]

This is from a practice problem that I can't seem to figure out.

Acetic Acid M = .096
pH of Acetic Acid = 2.86
NaOH M = .101
Volume of NaOH = 8.11 ml
Volume of Acetic Acid and NaOH = 19.96 ml
pH for this buffer = 4.36

So far I figured out the [H+] for the volume of the acetic acid and NaOH as 4.47x10-5. My next step is to figure out the [A-] and [HA] of this solution. More information. I figured out the [H+] for acetic acid as .0014 and the [HA] for acetic acid as .0941. In the answer section, they give the values for [A-] of acetic acid after addition of NaOH as 0.0292 M and [HA] of acetic acid after addition of NaOH as .0387. I can't seem to replicate those answers. Can someone show me the basic concept on how to find solve this.

[Borek]

Treat neutralization as limiting reagent question and don't forget about dilution.

[jdmbo1]

ok, so I figured out the [A-], .101 M NaOH x .00811 L = .000819
19.96+8.11 = 28.07 ml --> .002807 L
(.000819)/(.002807) = .0292. Are those calculations correct?

How would I find the [HA] now?

[Borek]

Rest of the acid.