The buffer from Part A is diluted to 1.00L. To half of it (500.mL), you add 0.02

ID: 793307 • Letter: T

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The buffer from Part A is diluted to 1.00L. To half of it (500.mL), you add 0.0250mol of hydrogen ions without changing the volume. What is the pH of the final solution?

This was the question from Part A (I do not need this answered, as I have already answered it, it is just here for reference): What volume of 10.0M NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52g of TrisHCl? And the answer I got was 6.7mL.

Here is some other handy information that came with the question: In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH2)3CNH2, often abbreviated as Tris. At 25 degrees Celcius, Tris has a pK b of 5.91.
The hydrochloride of Tris is (HOCH2)3CNH3Cl which can be abbreviated as TrisHCl.

I'm having a pretty tough time with this question, so please elaborate when explaining. Do not just give the answer; I'd like to see how it is worked out. Thank you in advance.

Explanation / Answer

7.05

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The buffer bis-Tris is a commonly used in biochemistry labs. It has a Ka = 3.16

The buffer or solution is used to move the compounds from a column is called voi

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The buffer from Part A is diluted to 1.00L. To half of it (500.mL), you add 0.02

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