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13 Dec 2019

A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ()= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.216 V, what is the pH of the unknown solution at 298 K? pH =

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Bunny Greenfelder
Bunny GreenfelderLv2
17 Dec 2019

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Related questions

A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]^{2+}. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.075 V at 298 K.
Half reaction of Cu = .337 V
Half reaction of H = .000 V

Based on the cell potential, what is the concentration of Cu^{2+} in this solution?

[Cu2+]____ with units


A voltaic cell consists of a copper electrode in a solution of copper(II) ions with unknown concentration, and a palladium electrode in a 0.1 M solution of palladium(II) ions. The palladium electrode is the cathode and its reduction potential is 0.951 V, the Cu electrode is the anode. (7 points)

(a) Write the half-reaction that occurs at the anode and the cathode, as well as the overall cell reaction.

b) What is the concentration of Cu2+ ions in the anode if the cell potential is 0.584 V? What is the error in the Cu2+ concentration if the cell potential measurement has an error of ±2 mV?

(c) What is the equilibrium constant (Keq) for this reaction?


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