Change in pH from adding HCl to a buffer?

What is the change in pH that results from adding 0.0060 mol HCl to a 300 mL buffer solution that is 0.250 M CH3COOH and 0.560 M NaCH3COO?

a) +0.052

b) -0.052

c) +0.049

d)-0.049 (correct answer)

e) -0.015



Just wondering how to do this. In my class, we learned to use Henderson-Hasselbalch equation or like ICE tables (Initial, Change, Equilibrian) set up, don't know how other people would go about it. But I solved it the other day and forgot how I did it lol, I found the initial pH with the Henderson-Hasselbalch, then did something with the HCl concentration to find the new pH but I'm lost now. Assistance please!!! Please list the step by stepChange in pH from adding HCl to a buffer?
You can use and ICE table very easily. WHen you add HCl ( a strong acid) to the buffer solution, the moles of CH3COOH will increase and the moles of CH3COO- will decrease by an amount equal to the moles of HCl added.



Then, calculate the new pH with the Henderson-Hasselbalch equation using the new concentrations of the CH3COOH and NaCH3COO.



To find the change in the pH, subtract the new pH from the original one.