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Write the half reactions and the overall reaction for the concentration cell.     2.  Calculate the unknown concentration using the Nernst equation.

Write the half reactions and the overall reaction for the concentration cell.     2.  Calculate the unknown concentration using the Nernst equation.

Chemistry
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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  1. Write the half reactions and the overall reaction for the concentration cell.

    2.  Calculate the unknown concentration using the Nernst equation.

Unknown Number Cell Voltage #2 0.02V Identify the anode and cathode Anode Cu diluted Cathode Cu Concentrated
Transcribed Image Text:Unknown Number Cell Voltage #2 0.02V Identify the anode and cathode Anode Cu diluted Cathode Cu Concentrated
Studying a Copper Concentration Cell 1. Add 1 mL of 0.10 M Cu(NO3)2 from a 5-mL or 10-mL graduated cylinder to a clean, dry 100-mL graduated cylinder. Add enough distilled water to bring the volume up to the 100-mL mark. Pour this solution into a clean beaker, and swirl or stir to obtain a homogeneous solution. 2. Clean the surfaces of two copper electrodes with 6 MHNO3. Wash the electrodes with distilled water and dry them. 3. 4. 5. 6. 7. Place an appropriate quantity of the diluted solution from Step 1 in one compartment of a voltaic cell and an appropriate quantity of 0.10 M Cu(NO3)2 in the other compartment. Insert the copper electrodes into these solutions. Use the voltmeter to identify the anode and cathode and to measure the cell potential. Record your results. Add 10 drops of 0.10 M Cu(NO3)2 to the more dilute solution in the cell. Stir and repeat Step 5. Remove the tape from the voltmeter when you are sure that you do not need to repeat any part of this experiment.
Transcribed Image Text:Studying a Copper Concentration Cell 1. Add 1 mL of 0.10 M Cu(NO3)2 from a 5-mL or 10-mL graduated cylinder to a clean, dry 100-mL graduated cylinder. Add enough distilled water to bring the volume up to the 100-mL mark. Pour this solution into a clean beaker, and swirl or stir to obtain a homogeneous solution. 2. Clean the surfaces of two copper electrodes with 6 MHNO3. Wash the electrodes with distilled water and dry them. 3. 4. 5. 6. 7. Place an appropriate quantity of the diluted solution from Step 1 in one compartment of a voltaic cell and an appropriate quantity of 0.10 M Cu(NO3)2 in the other compartment. Insert the copper electrodes into these solutions. Use the voltmeter to identify the anode and cathode and to measure the cell potential. Record your results. Add 10 drops of 0.10 M Cu(NO3)2 to the more dilute solution in the cell. Stir and repeat Step 5. Remove the tape from the voltmeter when you are sure that you do not need to repeat any part of this experiment.
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