What is the pH of the solution resulting from 25 mL .25 M NaOH being added to 50 mL .25 M HCN
Ka HCN = 4.9 x[10][/-10]
I have tried this question countless times, using the henderson-hasselbalch equation. Since it is the midpoint of the titration, the HCN and CN will be equal, thus cancelling, so the pH of the solution should equal the pKa , which is 9.3. However, my instructor says that the answer is 5.2. Can someone explain why I am wrong?