immersed in a solution where [Cu²+] = 1.00 M, is 0.340 V. The positive voltage indicates that the following reaction is spontaneous. H₂(g) + Cu²+(aq) → 2H+(aq) + Cu(s) What would be the Cu²+ reduction potential if the standard hydrogen electrode was kept the same, but copper electrode were instead immersed in a solution of 0.850 M NaOH that was saturated with Cu(OH)₂? (The Ksp of Cu(OH)₂ is 2.20 × 10-²0)
immersed in a solution where [Cu²+] = 1.00 M, is 0.340 V. The positive voltage indicates that the following reaction is spontaneous. H₂(g) + Cu²+(aq) → 2H+(aq) + Cu(s) What would be the Cu²+ reduction potential if the standard hydrogen electrode was kept the same, but copper electrode were instead immersed in a solution of 0.850 M NaOH that was saturated with Cu(OH)₂? (The Ksp of Cu(OH)₂ is 2.20 × 10-²0)
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
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 120AE
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![The standard reduction potential for Cu²+,
the voltage measured between a standard
hydrogen electrode and a Cu electrode
immersed in a solution where [Cu²+] = 1.00
M, is 0.340 V. The positive voltage indicates
that the following reaction is spontaneous.
H₂(g) + Cu²+(aq) → 2H*(aq) + Cu(s) What
would be the Cu²+ reduction potential if the
standard hydrogen electrode was kept the
same, but copper electrode were instead
immersed in a solution of 0.850 M NaOH
that was saturated with Cu(OH)₂? (The Ksp
of Cu(OH)2 is 2.20 × 10-²⁰.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc616abe4-3727-4750-bcbf-87fddf54e9f2%2Fda95dc03-1259-4321-a9fe-50e660f0cfc5%2Frs1wa9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The standard reduction potential for Cu²+,
the voltage measured between a standard
hydrogen electrode and a Cu electrode
immersed in a solution where [Cu²+] = 1.00
M, is 0.340 V. The positive voltage indicates
that the following reaction is spontaneous.
H₂(g) + Cu²+(aq) → 2H*(aq) + Cu(s) What
would be the Cu²+ reduction potential if the
standard hydrogen electrode was kept the
same, but copper electrode were instead
immersed in a solution of 0.850 M NaOH
that was saturated with Cu(OH)₂? (The Ksp
of Cu(OH)2 is 2.20 × 10-²⁰.)
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