What is the final pH of the second dilution after adding 1 drop of 0.1 M NaOH?

Question

There were 2 ml of buffer per well Calculate the final pH of the undiluted buffer after 0.25 ml of 0.1M NaOH is added. The Ka of CH3 COOH = 1.8 x 10 power -5. Use the CH3COOH bufffer concentration equation, an ICE table and a balanced dissociation equilibrium equation to help determine the pH.

Write the equation for the dissociation equilibrium of acetic acid.

Determine the volumes of 0.10M CH3COOH and 0.10M CH3COONa required to prepare 10 ml of the following pH buffers. (Note pka of CH3COOH = 4.7).

Please reply me thanks!

Answer 1

Your post is not clear enough for me to understand the question. The only part I could understand was the dissociation of acetic acid.
The dissociation of acetic acid is as follows:
CH3COOH ==> H^+ + CH3COO^-

Answer 2

In Activity2, there were 2 ml of bufffer per well. CALCULATE the final pH of the undiluted buffer after 0.25 ml of 0.1M NaOH is added. The Ka of CH3COOH = 1.8 x 10 power -5. Use the CH3COOH buffer concentration calculated in Data Tabe 2, a balanced CH3COOH + NaOH reaction equation, an ICe table and a balanced dissociation equilibrium equation to help determine the pH.

What is the final pH of the second dilution after adding 1 drop 0.1 M NaOH.