[_Alexis_]

Hello, this is for Biochemistry, but the math is basically high school Chemistry. Unfortunately, I've forgotten a lot of the logic when it comes to ICE problems. I'm trying to find the PH of a buffer after some strong base has been added to acetic acid. What do I do if more mols of the strong base are more than acetic acid? I wrote the formula (PH= pka + log(B/A)) afterward, but a negative value cannot be logged.

Here is what the ICE chart looks like:
      CH3COOH + KOH <-> CH3COO- + H2O
I         0.005      0.00525       0              -
C     -0.00525    -0.00525    +0.00525    -
E       -0.00025     0              0.00525

As you can see, I have a negative value for CH3COOH. That negative value cannot be put into log, so what do I do?

[mjc123]

Have you heard of the concept of the limiting reagent? What happens when all the acetic acid has reacted?

[_Alexis_]

Yes. Does this mean I solve and add together the PH together of (0.005 mols) CH3COO- and KOH (0.00025mols)

[mjc123]

No. [OH^-] will give you [H⁺] directly.
PS You do not have a buffer here!