A concentration cell consisting of two hydrogen electrodes (PH₂ = 1 atm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.186 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. pH =
A concentration cell consisting of two hydrogen electrodes (PH₂ = 1 atm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.186 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. pH =
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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Transcribed Image Text:A concentration cell consisting of two hydrogen electrodes (PH₂ = 1 atm), where the cathode is a standard
hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.186 V. What is the pH in
the unknown solution? Assume the temperature of the solutions is 298 K.
pH =
![When [Cu²+] = 1.03 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown
below is 1.192 V. What is the Zn2+ concentration in this cell?
Cu²+ (aq) + Zn(s) →→→ Cu(s) + Zn²+ (aq)
[Zn²+] =
mol/L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2Fa204ec7d-5b52-4ba3-a509-46321bb75674%2Fb9oivms_processed.jpeg&w=3840&q=75)
Transcribed Image Text:When [Cu²+] = 1.03 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown
below is 1.192 V. What is the Zn2+ concentration in this cell?
Cu²+ (aq) + Zn(s) →→→ Cu(s) + Zn²+ (aq)
[Zn²+] =
mol/L
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