1. The problem statement, all variables and given/known data What will be the final pH of the solution if a drop (approximately equal to 1/20 mL) of 1.0M HCl is added to a 10mL 0.1 M CH3COOH sol'n? 2. Relevant equations pH = -log [H+] 3. The attempt at a solution I first determined the number of moles of H+ from the partial ionization of CH3COOH (CH3COOH <--> CH3COO- + H+) using the ICE table. The number of moles H+ from my computation is 4.024922359 x 10^-5. Then I also determined the number of moles of H+ from HCl--> H+ + Cl-. What I got is 5 x 10^-5 moles. I added the two values to get the total number of moles H+. The pH I got is 2.52. Is my answer correct? I'm not quite sure about how I solved it. Need help. Thanks.