Consider the voltaic cell made from the following redox couples: TiOH3+(aq) / Ti3+(aq) E°red = -0.060 V & Zn(OH)42-(aq) / Zn(s) E°red = -1.36 V a) Write the balanced half-reaction that occurs in the anodeunder basic conditions. Use the 1/2 reaction method to balance. b) Write the balanced half-reaction that occurs in the cathodeunder basic conditions. Use the 1/2 reaction method to balance. c) Write the balanced overall cell reaction for basic conditions
Consider the voltaic cell made from the following redox couples: TiOH3+(aq) / Ti3+(aq) E°red = -0.060 V & Zn(OH)42-(aq) / Zn(s) E°red = -1.36 V a) Write the balanced half-reaction that occurs in the anodeunder basic conditions. Use the 1/2 reaction method to balance. b) Write the balanced half-reaction that occurs in the cathodeunder basic conditions. Use the 1/2 reaction method to balance. c) Write the balanced overall cell reaction for basic conditions
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 9P
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Consider the voltaic cell made from the following redox couples:
TiOH3+(aq) / Ti3+(aq) E°red = -0.060 V &
Zn(OH)42-(aq) / Zn(s) E°red = -1.36 V
a) Write the balanced half-reaction that occurs in the anodeunder basic conditions. Use the 1/2 reaction method to balance.
b) Write the balanced half-reaction that occurs in the cathodeunder basic conditions. Use the 1/2 reaction method to balance.
c) Write the balanced overall cell reaction for basic conditions.
d) Calculate the standard cell potential.
e) Calculate the cell potential at 25oC when the cathode and anode are at pH = 8.00 and the [TiOH3+] = [Ti3+] = [Zn(OH)42-] = 0.0025 M. (Hint: What concentrations can you find given pH?)
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