a concentration cell is constructed using Cu oxalate (made from 50ml 0.1 M oxalic acid and 0.05 M Cu sulfate) and Cu sulfate. both electrodes are copper which are connected using a multimeter. temperature reading was 23.0°C for the solution of Cu oxalate before the electrodes was placed.Since the copper concentration in the dilute half-cell changes as the experiment proceeds, we can calculate the concentration of dissolved copper ions using the Nernst equation.The two electrodes are the same in a concentration cell, so the standard electrode potential is 0. The potential difference is the voltage that we measured, and it is due to the difference in copper concentration between the two cells. After plugging in the known values, we can then solve for the concentration of the copper ion in the dilute cell. Here, the concentration of copper ions was 7.9 x 10-7 M. Show the solution. Constructing a Concentration CellA concentration cell is a galvanic cell with the same electrode and substance in the solution.The two half-reactions differ in the concentrations of copper ions in the solution.In this experiment, we constructed a galvanic cell using a solution of dilute copper oxalate andanother solution of concentrated copper sulfate. For the cell to achieve equilibrium, the concentrationof copper oxalate must go up while the concentration of copper sulfate must go down. We know thatelectrons flow from the anode to the cathode. So, in a concentration cell, electrons from the solutionwith a lower concentration must flow through its electrode towards the electrode immersed in thesolution with a higher concentration.This means that the copper ions in the electrode submerged in the dilute copper oxalate mustoccurred, so its electrode has.to be the anode. On the other hand, the concentration of concentratedcopper sulfate must decrease by depositing itself to its electrode (cathode), where reduction occurs(Cu + 2e → Cu,).Table 3. Concentration CellCu-Cu CellAnode (Oxidation)Cathode (Reduction) Cư".Reduction Half-ReactionStandard Reduction Potential (E°), VCu- Cư" n +2€-0.342e- Cu+0.34E°cell = E°red (cathode) -E°cell = -0.34 V –(-0.34V)E°cell = 0E°red (anode)Due to the difference in their concentration, we have recorded a voltage reading of -0.141 V,their potential difference. To determine the concentration of the copper ion in the dilute cell, we can usethe Nernst equation.

Given data, [Cu2+]cathode = 7.9 x 10-7M EMF = -0.141 V Eocell = 0 (since it is a concentration cell)

Answered: a concentration cell is constructed…

Chemistry

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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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a concentration cell is constructed using Cu oxalate (made from 50ml 0.1 M oxalic acid and 0.05 M Cu sulfate) and Cu sulfate. both electrodes are copper which are connected using a multimeter. temperature reading was 23.0°C for the solution of Cu oxalate before the electrodes was placed. Since the copper concentration in the dilute half-cell changes as the experiment proceeds, we can calculate the concentration of dissolved copper ions using the Nernst equation. The two electrodes are the same in a concentration cell, so the standard electrode potential is 0. The potential difference is the voltage that we measured, and it is due to the difference in copper concentration between the two cells. After plugging in the known values, we can then solve for the concentration of the copper ion in the dilute cell. Here, the concentration of copper ions was 7.9 x 10-7 M. Show the solution.

Constructing a Concentration Cell
A concentration cell is a galvanic cell with the same electrode and substance in the solution.
The two half-reactions differ in the concentrations of copper ions in the solution.
In this experiment, we constructed a galvanic cell using a solution of dilute copper oxalate and
another solution of concentrated copper sulfate. For the cell to achieve equilibrium, the concentration
of copper oxalate must go up while the concentration of copper sulfate must go down. We know that
electrons flow from the anode to the cathode. So, in a concentration cell, electrons from the solution
with a lower concentration must flow through its electrode towards the electrode immersed in the
solution with a higher concentration.
This means that the copper ions in the electrode submerged in the dilute copper oxalate must
occurred, so its electrode has.to be the anode. On the other hand, the concentration of concentrated
copper sulfate must decrease by depositing itself to its electrode (cathode), where reduction occurs
(Cu + 2e → Cu,).
Table 3. Concentration Cell
Cu-Cu Cell
Anode (Oxidation)
Cathode (Reduction) Cư".
Reduction Half-Reaction
Standard Reduction Potential (E°), V
Cu- Cư" n +2€
-0.34
2e- Cu
+0.34
E°cell = E°red (cathode) -
E°cell = -0.34 V –(-0.34V)
E°cell = 0
E°red (anode)
Due to the difference in their concentration, we have recorded a voltage reading of -0.141 V,
their potential difference. To determine the concentration of the copper ion in the dilute cell, we can use
the Nernst equation.

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