You decided to take the pH after each addition of 5.0 mL of NaOH rather than after every 0.5 mL during the neutralization of your acid sample. The pH buffers used to calibrate the pH meter were each 0.5 pH units high (4.5 and 7.5 rather than 4.0 and 1. pKa would be unchanged. 7.0 respectively). 2. pKa would be too high. While using the Half Volume method, your solution was dark pink (you overshot the endpoint) and added the unreacted 3. pka would be too low. you acid to this solution. You refilled your buret between titrations of your unknown acid. Instead of using 0.1 M NAOH as you did for the first titration, you used 0.2 M NaOH.

You decided to take the pH after each addition of 5.0 mL of NaOH rather than after every 0.5 mL during the neutralization of your acid sample. The pH buffers used to calibrate the pH meter were each 0.5 pH units high (4.5 and 7.5 rather than 4.0 and 1. pKa would be unchanged. 7.0 respectively). 2. pKa would be too high. While using the Half Volume method, your solution was dark pink (you overshot the endpoint) and added the unreacted 3. pka would be too low. you acid to this solution. You refilled your buret between titrations of your unknown acid. Instead of using 0.1 M NAOH as you did for the first titration, you used 0.2 M NaOH.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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You decided to take the pH
after each addition of 5.0
mL of NaOH rather than
after every 0.5 mL during
the neutralization of your
acid sample.
The pH buffers used to
calibrate the pH meter were
each 0.5 pH units high (4.5
and 7.5 rather than 4.0 and
1. pka would be unchanged.
7.0 respectively).
2. pKa would be too high.
While using the Half
Volume method, your
solution was dark pink (you
overshot the endpoint) and
you added the unreacted
acid to this solution.
3. pka would be too low.
You refilled your buret
between titrations of your
unknown acid. Instead of
using 0.1 M NaOH as you
did for the first titration,
you used 0.2 M NaOH.

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