1)I found the answer for the first half of the problem, but need help with part two. A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution.

The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places.
Answer: 4.44
Correct

A buffered solution resists a change in pH.

Calculate the pH when 21.5 mL of 0.044 M HCl is added to 100.0 mL of the above buffer.

Question

1)I found the answer for the first half of the problem, but need help with part two. A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution.

The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places.
Answer: 4.44
Correct

A buffered solution resists a change in pH.

Calculate the pH when 21.5 mL of 0.044 M HCl is added to 100.0 mL of the above buffer.

abb0t · Answer

Well, use M$_1$V$_1$ = M$_2$V$_2$ to fnd the second molar concentration, and then use it to find pH.
pH = -log[H$^+$]

anonymous · Answer

thank you!

anonymous · Answer

so would the answer be 2.024? I set up the equation like this. .0215L*.044M = .1L * M2 THEN I GOT 9.46e-3 and took the -log of that.