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A laboratory was assigned the job of determining the copper(II) ion concentration in thousands of water samples. To make these measurements an electrochemical cell was assembled that consists of a silver electrode, dipping into a 0.225 M solution of AgNO3, connected by a salt bridge to a second half-cell containing a copper electrode. The copper half-cell was then filled with one water sample after another, with the cell potential measured for each sample. In the analysis of two other water samples, cell potentials (Ecell) of 0.55 V and 0.64 V were obtained. Calculate the Cu²+ ion concentration in each of these samples. [Cu²+] = i M when Ecell = 0.55 V M when Ecell = 0.64 V [Cu²+] = i

A laboratory was assigned the job of determining the copper(II) ion concentration in thousands of water samples. To make these measurements an electrochemical cell was assembled that consists of a silver electrode, dipping into a 0.225 M solution of AgNO3, connected by a salt bridge to a second half-cell containing a copper electrode. The copper half-cell was then filled with one water sample after another, with the cell potential measured for each sample. In the analysis of two other water samples, cell potentials (Ecell) of 0.55 V and 0.64 V were obtained. Calculate the Cu²+ ion concentration in each of these samples. [Cu²+] = i M when Ecell = 0.55 V M when Ecell = 0.64 V [Cu²+] = i

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.49QE: A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt...
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A laboratory was assigned the job of determining the copper(II) ion concentration in thousands of water samples. To make these measurements an electrochemical cell was assembled that consists of a silver electrode, dipping into a 0.225 M solution of AgNO3, connected by a salt bridge to a second half-cell containing a copper electrode. The copper half-cell was then filled with one water sample after another, with the cell potential measured for each sample. In the analysis of two other water samples, cell potentials (Ecell) of 0.55 V and 0.64 V were obtained. Calculate the Cu²+ ion concentration in each of these samples. [Cu²+] = i M when Ecell = 0.55 V M when Ecell = 0.64 V [Cu²+] = i
Transcribed Image Text:A laboratory was assigned the job of determining the copper(II) ion concentration in thousands of water samples. To make these measurements an electrochemical cell was assembled that consists of a silver electrode, dipping into a 0.225 M solution of AgNO3, connected by a salt bridge to a second half-cell containing a copper electrode. The copper half-cell was then filled with one water sample after another, with the cell potential measured for each sample. In the analysis of two other water samples, cell potentials (Ecell) of 0.55 V and 0.64 V were obtained. Calculate the Cu²+ ion concentration in each of these samples. [Cu²+] = i M when Ecell = 0.55 V M when Ecell = 0.64 V [Cu²+] = i
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