I've been trying to solve the second part of this question for ages now and I'm not getting any closer to the answer, would anyone be able to help me please? my teacher said it's an A* question but I'd still like to be able to understand it. I've attached the question and my current workings below. Thanks in advance
The question is: Show that the pH of this buffer becomes 5.28 if 10cm^3 of 0.1M HCl are Added
-Calculate the moles of the buffer solution acid. -Calculate the moles of the HCl. -Add them up. -Calculate the moles of the salt. -Subtract moles of HCl from moles of salt. - Substitute new values into the Henderson-Hasselbalch equation.
-Calculate the moles of the buffer solution acid. -Calculate the moles of the HCl. -Add them up. -Calculate the moles of the salt. -Subtract moles of HCl from moles of salt. - Substitute new values into the Henderson-Hasselbalch equation.