Part 2: Titration of Acetate Buffer with HCl and NaOH 1. How do the graphs diffe

Question

Part 2: Titration of Acetate Buffer with HCl and NaOH 1. How do the graphs differ between the titration of buffer with NaOH and the titration of water 2. How do the graphs differ between the titration of buffer with HCl and the titration of water with 3. Which solution (HCI or NaOH) required the largest volume to reach equivalence point when 4. How do you hypothesize that these results would differ if a basic buffer was titrated (vs. an 5. Does the buffer action of acetate last over the entire pH range? Why or why not? What with NaOH? Why? HCI? Why? titrating the acetate buffer? Why do you think this is the case? acidic one)? evidence do you have of this?

Explanation / Answer

Answers for 1 and 2:

The acetate buffer has an initial pH around 5.   (pH = pKa = 4.75)

Your pictures are in order of appearance (from top to down)

-buffer titration with NaOH (for more than 100 added drops, the variation of pH is small)

-water titration with NaOH (immediately after addition of a few drops, pH rise in alkaline range)

-buffer titration with HCl (for more than 100 added drops, the variation of pH is small)

-water titration with HCl (immediately after addition of a few drops, pH become highly acidic, <2)

3.

120 drops of NaOH until EP (equivqlence point) is reached

240 drops of HCL until EP is reached

The buffer contains CH2COOH and CH3COO- in 1:2 proportion (more acetate).

4.

The situation is similar, but before EP the pH will be   >7 (basic)

5.

For any buffer the pH range of action is limited to:

   pKa-1 to pKa +1     or

pKb-1 to pKb +1

(not more than 2 pH units).

Don’t use your last picture for answer. These are not graphs.

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