An Ag/AgCl electrode dipping into 1.00 M HCI has a standard reduction potential of +0.2223 V. The half-reaction is AgCI(s) +e = Ag(s) +Cl'(aq) A second Ag/AgCl electrode is dipped into a solution containing Cl at an unknown concentration. The cell generates a potential of 0.0481 V, with the electrode in the solution of unknown concentration having a negative charge. What is the molar concentration of Cl' in the unknown solution? [CI]= i M

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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.125QP: An electrochemical cell is made by placing a zinc electrode in 1.00 L of 0.200 M ZnSO4 solution and...
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An Ag/AgCl electrode dipping into 1.00 M HCI has a standard reduction potential of +0.2223 V.
The half-reaction is
ABCI(s) + e = Ag(s) +Cl(aq)
A second Ag/AgCl electrode is dipped into a solution containing Cl at an unknown concentration.
The cell generates a potential of 0.0481 V, with the electrode in the solution of unknown concentration having a negative charge.
What is the molar concentration of Cl' in the unknown solution?
[CI]= i
M
Transcribed Image Text:An Ag/AgCl electrode dipping into 1.00 M HCI has a standard reduction potential of +0.2223 V. The half-reaction is ABCI(s) + e = Ag(s) +Cl(aq) A second Ag/AgCl electrode is dipped into a solution containing Cl at an unknown concentration. The cell generates a potential of 0.0481 V, with the electrode in the solution of unknown concentration having a negative charge. What is the molar concentration of Cl' in the unknown solution? [CI]= i M
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