1. The problem statement, all variables and given/known data You need to produce a buffer solution that has a pH of 5.70. You already have a solution that contains 0.0200 moles of acetic acid. Using the Henderson-Hasselbalch equation calculate the moles of sodium acetate needed to create a buffer with the desired pH? The Ka of acetic acid is 1.8 × 10^-5. 2. Relevant equations pKa = -log (Ka) pH= pKa + log (base / acid) 3. The attempt at a solution pKa= -log (1.8 × 10^-5) = 4.74 5.70 = 4.74 + log (base/acid) Unfortunately, I have been staring at this problem for about an hour and am unsure how to find the concentration of the acid to discover the consent ration of the base. I am not sure how to proceed since the problem does not give a volume to find the molarity. Any help with this would be greatly appreciated!!