1. The problem statement, all variables and given/known data Titrating .1006M CH3COOH with .2012M NaOH. pKa=4.74, Ka=1.8*10^-5 What is the pH at the equivalence point of the titration? 2. Relevant equations pKa = -log(Ka) pH = -log[H+] 3. The attempt at a solution Alright, after setting up an ICE table (in order to find [H+] at the equivalence point) I realized that when you work it out Ka = [H+], however when I plugged that in I got a pH in th 4-5 range when it should be above 7. Here is my Ka reasoning Ka = [A-][H+]/[HA] Ka = [Co+x][x]/[Co-x] Co = Initial Concentration x is very small (Weak acid, no/little disassociation) Ka = x Ka = [H+] Am I missing something or is my logic just wrong? Anything that could point me in the correct direction would be greatly appreciated.