You have two problems here. The first is the combination of NaOH and HCl. Work with that one first. The second one is NaOH and HC2H3O2. Work with that one second.
For the first one,
1. Write the balanced equation.
2. Calculate moles NaOH and moles HCl. moles = M x L.
3. Determine which is in excess, if either, and prepare an ICE chart if that will help.
4. pH = -log(H^+).
The second one involves the Henderson-Hasselbalch equation.
I don't get how to do this: What is the pH of the solution created by combining 11.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? What are the pH values if you take into
What is the pH of the solution created by combining 2.50 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? I believe if my calculations are correct the answer is 1.28 however i do not know how to answer this question