[SOLVED] Anticipated pH of Buffer Solution (urgent!) 1. The problem statement, all variables and given/known data Can someone verify my process here? i did a lab where i had 100 mL CH3COOH/CH3CO2- buffer solution. I have to find the pH if 100 mL of 0.0983 M HCl is added to it. In the lab i got pH of 1.72 2. Relevant equations [H3O+][CH3CO2-] Ka= --------------------- [CH3COOH] Ka : 1.8x10-5 initial moles CH3COOH: 0.00996 Initial moles CH3CO2-: 0.0100 moles H+ in 100 mL 0.0983 M HCl: 0.00983 3. The attempt at a solution It's my understanding that the mole ratio of H+/CH3CO2- is one to one. Next i think i do this: moles CH3COOH = 0.00996 + 0.00983 = 0.0198 moles moles CH3CO2-= 0.0100- 0.00983= 0.00017 moles concentration CH3COOH= 0.0198 moles/(0.200 L) = 0.099 M concentration CH3CO2-= 0.00017/(0.200 L) = 0.00085 M Then by rearranging the equilibrium expression i can solve for [H3O+]. [H3O+]=(1.8x10-5)(0.099M) / (0.00085) = 0.00212 M pH= -log(0.00212M) = 2.67 is that how am supposed to go about doing this? because my other lab values are very strange. for instance, i keep getting a pH of 4.7 after adding 5, 10, and 20 mL of HCl to it.