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The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn2* (0.80 M) || H† (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn2+ is -0.76 V. (Enter your answer to two significant figures.) pH=

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn2* (0.80 M) || H† (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn2+ is -0.76 V. (Enter your answer to two significant figures.) pH=

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.128QP: a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4...
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The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.80 M) || H† (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn2+ is –0.76 V. (Enter your answer to two significant figures.) pH =
Transcribed Image Text:The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.80 M) || H† (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn2+ is –0.76 V. (Enter your answer to two significant figures.) pH =
Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) 2H, O(1) + 2e = H2 (g) + 20H (aq) -0.83 Cu²+ (aq) + e¯ = Cu*(aq) 0.16 Cu?+ (ag) + 2e = Cu(s) 0.34 O2 (g) + 4H* (aq) + 4e¯ = 2H2O(1) 1.23 Cl2 (g) + 2e = 2C1¯ (ag) 1.36 F2 (g) + 2e = 2F¯(aq) 2.87 Write the overall reactions that you would expect to happen when the following solutions are electrolyzed: (Use the lowest possible coefficients. Be sure to to specify states such as (aq) or (s). If a box is not needed, leave it blank. Add H,O, H", or OH to any side of the reaction if it is needed.) a. Aqueous CuF2. + + + b. Aqueous CuSO4. The sulfate ion is not oxidized. + +
Transcribed Image Text:Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) 2H, O(1) + 2e = H2 (g) + 20H (aq) -0.83 Cu²+ (aq) + e¯ = Cu*(aq) 0.16 Cu?+ (ag) + 2e = Cu(s) 0.34 O2 (g) + 4H* (aq) + 4e¯ = 2H2O(1) 1.23 Cl2 (g) + 2e = 2C1¯ (ag) 1.36 F2 (g) + 2e = 2F¯(aq) 2.87 Write the overall reactions that you would expect to happen when the following solutions are electrolyzed: (Use the lowest possible coefficients. Be sure to to specify states such as (aq) or (s). If a box is not needed, leave it blank. Add H,O, H", or OH to any side of the reaction if it is needed.) a. Aqueous CuF2. + + + b. Aqueous CuSO4. The sulfate ion is not oxidized. + +
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