1. The problem statement, all variables and given/known data . A 50 mL acetate solution is titrated with a 0.2342 M HCl solution. The equivalence point occurs at 28.52 mL. Acetate is the conjugate base of acetic acid, for which Ka = 1.8 × 10-5 . b) Write down the titration reaction. c) Find the pH of the acetate solution at the start of the titration. d) What is the pH after 14.26 mL of HCl have been added? 2. Relevant equations Ka = [prod]/[react] using the ICE table method moles = CV KaKb=Kw = 1.0*10^-14 ph= -logH+ 3. The attempt at a solution for part b, my assumption is: CH3COO-(aq) +HCl(aq) ---> CH3COOH(aq) + Cl(aq) For part C i was thinking of converting Ka to Kb then using the Ice table...but i don't think that's going to work anymore. I've just been stuck on this for almost two days now. Any help would be greatly appreciated .