-0.763 V) immersed inCalculate the potential of a zinc electrode (E2+ 1Za 0.0130 M in2+Zn (NH3),and 0.440 M inNH3 (Ba for2+Zn (NH3), is7.76 x 10°).Potential =Vba solution in which the molar analytical concentration ofZn (NO3)2 is2.70 x 10-3 M, that forH2Y- (Kzy = 3.2 x 1016) is 0.0330 M, and the pH is fixed at 9.0o.%3DThe dissociation constants for the acidic groups in EDTA areK1 = 1.02 x 10-2,K2 = 2.14 x 10-3K3 = 6.92 x 10, and%3D%3D%3DKA = 5.50 x 10-".Potential =V

To calculate the potential of Zn electrode.

Answered: = -0.763 V) immersed in Calculate the…

= -0.763 V) immersed in Calculate the potential of a zinc electrode (E+ /Zn a 0.0130 M in 2+ Zn (NH3)4 NH3 ( and 0.440 M in B. for

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

-0.763 V) immersed in
Calculate the potential of a zinc electrode (E2+ 1Z
a 0.0130 M in
2+
Zn (NH3),
and 0.440 M in
NH3 (
Ba for
2+
Zn (NH3), is
7.76 x 10°).
Potential =
V
ba solution in which the molar analytical concentration of
Zn (NO3)2 is
2.70 x 10-3 M, that for
H2Y- (
Kzy = 3.2 x 1016) is 0.0330 M, and the pH is fixed at 9.0o.
%3D
The dissociation constants for the acidic groups in EDTA are
K1 = 1.02 x 10-2,
K2 = 2.14 x 10-3
K3 = 6.92 x 10, and
%3D
%3D
%3D
KA = 5.50 x 10-".
Potential =
V

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