(2)Calculate the pH for a buffer solution that is 0.05 M in ethyl amine (CH3CH2NH2) and 0.137 M in ethyl ammonium chloride (Cl- CH3CH2NH3+). Ka for ethyl ammonium chloride = 2.31 X10-11 Select one: a. 10.2 b. 12.3 c. 11.6 d. 13.0

(2)Calculate the pH for a buffer solution that is 0.05 M in ethyl amine (CH3CH2NH2) and 0.137 M in ethyl ammonium chloride (Cl- CH3CH2NH3+). Ka for ethyl ammonium chloride = 2.31 X10-11 Select one: a. 10.2 b. 12.3 c. 11.6 d. 13.0

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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Question

Solve question 2 and question 3 by clarifying the steps

(2)Calculate the pH for a buffer solution that is
0.05 M in ethyl amine (CH3CH2NH2) and 0.137
M in ethyl ammonium chloride (Cl-
CH3CH2NH3+).
Ka for ethyl ammonium chloride = 2.31 X10-11
Select one:
а. 10.2
b. 12.3
C. 11.6
d. 13.0
(3)Calculate the pH of a 0.1 M weak acid HA
solution; Ka = 3.0 X10-8
Select one:
а. 4.26
b. 2.20
С. 5.15
d. 6.11
е. 3.08

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