The cell in Figure could be used to provide a measureof the pH in the cathode half-cell. Calculate the pHof the cathode half-cell solution if the cell emf at 298 Kis measured to be +0.684 V when [Zn2+] = 0.30 M andPH2 = 0.90 atm. 0.76 VVoltmeterZn- NO, Na*-anode- H2(g)Cathodehalf-cell(standardhydrogen-electrode, SHE)NO3Zn2+NO,AnodeNO,H+half-cellZn(s)Zn2+(aq) + 2 e-2H*(aq) + 2 e → H2(g)

In the given cell, Cathode (Reduction half): 2H+(aq) + 2e- → H2(g)Anode (Oxidation half): Zn(s) →…

Answered: 0.76 V Voltmeter Zn - NO, Na*- anode -…

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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The cell in Figure could be used to provide a measure
of the pH in the cathode half-cell. Calculate the pH
of the cathode half-cell solution if the cell emf at 298 K
is measured to be +0.684 V when [Zn²⁺] = 0.30 M and
P_H2 = 0.90 atm.

0.76 V
Voltmeter
Zn
- NO, Na*-
anode
- H2(g)
Cathode
half-cell
(standard
hydrogen
-electrode, SHE)
NO3
Zn2+
NO,
Anode
NO,
H+
half-cell
Zn(s)
Zn2+(aq) + 2 e-
2H*(aq) + 2 e → H2(g)

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