3. Metal ion complexation is known to affect the half-wave potential for the reduction of a metal ion. M++Hg+ne → M(Hg) MxAMAX (n-x)+ [1] [2] The relationship between the molar concentrations of the ligand CL and the shift in the half-wave potential is: = (E) E (-0.0592/n)logK - (0.0592x/n)logcL - [3] Where (E) and E½ are half-wave potentials for the complexed and uncomplexed
3. Metal ion complexation is known to affect the half-wave potential for the reduction of a metal ion. M++Hg+ne → M(Hg) MxAMAX (n-x)+ [1] [2] The relationship between the molar concentrations of the ligand CL and the shift in the half-wave potential is: = (E) E (-0.0592/n)logK - (0.0592x/n)logcL - [3] Where (E) and E½ are half-wave potentials for the complexed and uncomplexed
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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![3. Metal ion complexation is known to affect the half-wave potential for the reduction of
a metal ion.
M+ + Hg+ne → M(Hg)
MxAMAX (n-x)+
[1]
[2]
The relationship between the molar concentrations of the ligand CL and the shift in the
half-wave potential is:
=
(E) E (-0.0592/n)logK - (0.0592x/n)logcL
[3]
Where (E) and E½ are half-wave potentials for the complexed and uncomplexed
cation, respectively, K, is the formation constant for the complex, and x is the molar
combining ratio of the complexing agent to cation.
The following polarographic data were obtained for the reduction of Pb2+ to its
amalgam from solutions that were 2.00 x 10-3 M in Pb2+, 0.100 M in KNO3, and
different concentrations of the anion A. From the half-wave potentials, find (i) the
formula of the complex, and (ii) its formation constant Kſ.
Concentration A, M
0.0000
E vs. SCE, V
-0.405
0.0200
-0.473
0.0600
-0.507
0.1007
-0.516
0.3000
-0.547
0.5000
-0.558](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F55ad1c89-e77a-4c6d-aab4-0bb0be0d85c7%2Ffd7523c7-d2da-409c-bf18-227ad53e1414%2Fwkxestg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3. Metal ion complexation is known to affect the half-wave potential for the reduction of
a metal ion.
M+ + Hg+ne → M(Hg)
MxAMAX (n-x)+
[1]
[2]
The relationship between the molar concentrations of the ligand CL and the shift in the
half-wave potential is:
=
(E) E (-0.0592/n)logK - (0.0592x/n)logcL
[3]
Where (E) and E½ are half-wave potentials for the complexed and uncomplexed
cation, respectively, K, is the formation constant for the complex, and x is the molar
combining ratio of the complexing agent to cation.
The following polarographic data were obtained for the reduction of Pb2+ to its
amalgam from solutions that were 2.00 x 10-3 M in Pb2+, 0.100 M in KNO3, and
different concentrations of the anion A. From the half-wave potentials, find (i) the
formula of the complex, and (ii) its formation constant Kſ.
Concentration A, M
0.0000
E vs. SCE, V
-0.405
0.0200
-0.473
0.0600
-0.507
0.1007
-0.516
0.3000
-0.547
0.5000
-0.558
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