Simple pH Problem (If I could remember)

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The discussion focuses on calculating the pH after adding NaOH to a buffer solution of sodium acetate and acetic acid. The initial pH of the mixture is given as 4.7, based on the Henderson-Hasselbalch equation. The main confusion arises regarding which pKa to use, but it's clarified that acetic acid is monoprotic and has a single pKa value. The participant seeks guidance on how to proceed with the calculation after the addition of NaOH. Understanding the role of pKa in this context is essential for solving the problem accurately.
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Homework Statement


If one mixed 100mL of .1M Sodium acetate with 100 mL of .1M acetic acid, the pH of the solution would be 4.7 If 60 mL of .1M NaOH were added to this solution, what would be it's pH?


Homework Equations


Henderson Hasselback
pH=pKa+ log(base/acid)


The Attempt at a Solution


I haven't really made one because I'm not sure how to proceed. The thing that really confuses me is the pKa part of henderson-hasselbach. When we are dealing with solutions having more more than one pkA, which pkA do we use? I know I did a ton of these problems in Gen Chem but can't remember how!
 
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There's only one thing (ignoring water) that has a pKa: the acetic acid. Since acetic acid is monoprotic, it has only one pKa.
 
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