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

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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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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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