Part C For 500.0 mL of a buffer solution that is 0.185 M in CHCH,NH2 and 0.135 M in CH3CH2NH3CI, calculate the initial pH and the final pH after adding 2.0x10-2 mol of HCL (K,(CH3CH2NH2) =5.6 x 104) Express your answers using two decimal places separated by a comma.

Part C For 500.0 mL of a buffer solution that is 0.185 M in CHCH,NH2 and 0.135 M in CH3CH2NH3CI, calculate the initial pH and the final pH after adding 2.0x10-2 mol of HCL (K,(CH3CH2NH2) =5.6 x 104) Express your answers using two decimal places separated by a comma.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 80QAP

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Question

OpenVellumHMAC=defce5f03204e95efa2fcf11b1ecff98#10001
I Review | Constants | Periodic Table
[base]
pH = pK, + log
Tacid
3.5 x 10 2
-log(1.8 x 10-5)+ log
0.1025
4.74 – 0.467
4.28
Part C
For 500.0 mL of a buffer solution that is 0.185 M in CH,CH,NH, and 0.135 M in CH3CH,NH CI, calculate the initial pH
and the final pH after adding 2.0x10-2 mol of HCl (K,(CH CH,NH,) = 5.6 x 10 4)
Express your answers using two decimal places separated by a comma.
pHinitial. pHrinal
10.89, 11.12
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