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a) Construction of Cu(s) | Cu(NO3)2 (0.001 M) || Cu(NO3)2 (0.1 M) | Cu(s) NOTE: different than above → Electrode cup || porous cup Measure out 1 mL of the 0.1 M Cu2+ solution with a 10 mL graduated cylinder. Transfer this solution to a clean 100 mL graduated cylinder and dilute with water to obtain 100 mL of an approximately 0.001 M solution. Pour 40 mL of this solution into a clean electrode cup and place a clean porous cup inside. Transfer 15 mL of the 0.1 M Cu2+ solution to the porous cup. Place a copper electrode in each half-cell, attach the electrodes to the terminals of the voltmeter, and record the magnitude of the potential of the cell. 11. The diagram below is the concentration cell prepared in the laboratory experiment. On the diagram, label the anode and cathode, the direction of electron flow and indicate the initial [Cu2+] for each solution. Voltmeter V Copper Copper Cu2+, NO3 Cu 2+, NO3 12. Calculate the concentration of Cu2+ in the electrode cup after the addition of ammonia.

a) Construction of Cu(s) | Cu(NO3)2 (0.001 M) || Cu(NO3)2 (0.1 M) | Cu(s) NOTE: different than above → Electrode cup || porous cup Measure out 1 mL of the 0.1 M Cu2+ solution with a 10 mL graduated cylinder. Transfer this solution to a clean 100 mL graduated cylinder and dilute with water to obtain 100 mL of an approximately 0.001 M solution. Pour 40 mL of this solution into a clean electrode cup and place a clean porous cup inside. Transfer 15 mL of the 0.1 M Cu2+ solution to the porous cup. Place a copper electrode in each half-cell, attach the electrodes to the terminals of the voltmeter, and record the magnitude of the potential of the cell. 11. The diagram below is the concentration cell prepared in the laboratory experiment. On the diagram, label the anode and cathode, the direction of electron flow and indicate the initial [Cu2+] for each solution. Voltmeter V Copper Copper Cu2+, NO3 Cu 2+, NO3 12. Calculate the concentration of Cu2+ in the electrode cup after the addition of ammonia.

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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a) Construction of Cu(s) | Cu(NO3)2 (0.001 M) || Cu(NO3)2 (0.1 M) | Cu(s) NOTE: different than above → Electrode cup || porous cup Measure out 1 mL of the 0.1 M Cu2+ solution with a 10 mL graduated cylinder. Transfer this solution to a clean 100 mL graduated cylinder and dilute with water to obtain 100 mL of an approximately 0.001 M solution. Pour 40 mL of this solution into a clean electrode cup and place a clean porous cup inside. Transfer 15 mL of the 0.1 M Cu2+ solution to the porous cup. Place a copper electrode in each half-cell, attach the electrodes to the terminals of the voltmeter, and record the magnitude of the potential of the cell.
Transcribed Image Text:a) Construction of Cu(s) | Cu(NO3)2 (0.001 M) || Cu(NO3)2 (0.1 M) | Cu(s) NOTE: different than above → Electrode cup || porous cup Measure out 1 mL of the 0.1 M Cu2+ solution with a 10 mL graduated cylinder. Transfer this solution to a clean 100 mL graduated cylinder and dilute with water to obtain 100 mL of an approximately 0.001 M solution. Pour 40 mL of this solution into a clean electrode cup and place a clean porous cup inside. Transfer 15 mL of the 0.1 M Cu2+ solution to the porous cup. Place a copper electrode in each half-cell, attach the electrodes to the terminals of the voltmeter, and record the magnitude of the potential of the cell.
11. The diagram below is the concentration cell prepared in the laboratory experiment. On the diagram, label the anode and cathode, the direction of electron flow and indicate the initial [Cu2+] for each solution. Voltmeter V Copper Copper Cu2+, NO3 Cu 2+, NO3 12. Calculate the concentration of Cu2+ in the electrode cup after the addition of ammonia.
Transcribed Image Text:11. The diagram below is the concentration cell prepared in the laboratory experiment. On the diagram, label the anode and cathode, the direction of electron flow and indicate the initial [Cu2+] for each solution. Voltmeter V Copper Copper Cu2+, NO3 Cu 2+, NO3 12. Calculate the concentration of Cu2+ in the electrode cup after the addition of ammonia.
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