A cell was set up having the following reaction Mg(s) + Cd2+ (aq) → Mg2+ (aq) + Cd (s) E°cell = 1.98 V The Magnesium electrode was dipped in a 1.00 M solution of MgSO4 and the Cadmium electrode was dipped in a solution of unknown Cd2+ concentration. The cell potential was measured to be 1.54 V. What is the unknown Cd2+ concentration?
A cell was set up having the following reaction Mg(s) + Cd2+ (aq) → Mg2+ (aq) + Cd (s) E°cell = 1.98 V The Magnesium electrode was dipped in a 1.00 M solution of MgSO4 and the Cadmium electrode was dipped in a solution of unknown Cd2+ concentration. The cell potential was measured to be 1.54 V. What is the unknown Cd2+ concentration?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section: Chapter Questions
Problem 84GQ
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A cell was set up having the following reaction
Mg(s) + Cd2+ (aq) → Mg2+ (aq) + Cd (s) E°cell = 1.98 V
The Magnesium electrode was dipped in a 1.00 M solution of MgSO4 and the Cadmium electrode was dipped in a solution of unknown Cd2+ concentration. The cell potential was measured to be 1.54 V.
What is the unknown Cd2+ concentration?
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