When the Ag+ concentration is 1.36×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is2.937V. What is the Mg2+ concentration?2Ag*(aq) + Mg(s)2Ag(s) + Mg²+ (aq)Answer: 0.66 M Consider the following cell reaction:Ni(s) + 2 H*(? M) →Ni²+(1.00 M) + H₂(g)(1.00 atm)If the cell potential at 298 K is 0.100 volts, what is the pH of the hydrogen electrode?pH = 2.65|

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When the Ag* concentration is 1.36x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.937V. What is the Mg2+ concentration? 2Ag (aq) + Mg(s) →2Ag(s) + Mg2+(aq) Answer: 0.66 M

When the Ag* concentration is 1.36x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.937V. What is the Mg2+ concentration? 2Ag (aq) + Mg(s) →2Ag(s) + Mg2+(aq) Answer: 0.66 M

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

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Question

When the Ag+ concentration is 1.36×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is
2.937V. What is the Mg2+ concentration?
2Ag*(aq) + Mg(s)2Ag(s) + Mg²+ (aq)
Answer: 0.66 M

Consider the following cell reaction:
Ni(s) + 2 H*(? M) →Ni²+(1.00 M) + H₂(g)(1.00 atm)
If the cell potential at 298 K is 0.100 volts, what is the pH of the hydrogen electrode?
pH = 2.65|

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