Question

A copper, Cu(s), the electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraammine copper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.067 V at 298 K. [Cu2+] = 2×10^−14 M Based on these data, what is the value of the formation constant, Kf, of [Cu(NH3)4]2+?

Name: a copper cus the electrode is immersed in a solution that is 100 m in ammonia nh3 and 100 m in tetraammine copperii cunh342 if a standard hydrogen electrode is used as the cathode the cell p 84633
Uploaded: 2022-03-17T01:42:17-08:00
Duration: 2 min 3 s
Channel: Caryl Abrenica
Description: a copper cus the electrode is immersed in a solution that is 100 m in ammonia nh3 and 100 m in tetraammine copperii cunh342 if a standard hydrogen electrode is used as the cathode the cell p 84633

          A copper, Cu(s), the electrode is immersed in a solution that is
1.00 M in ammonia, NH3, and 1.00 M in tetraammine copper(II),
[Cu(NH3)4]2+. If a standard hydrogen electrode is used as the
cathode, the cell potential, Ecell, is found to be 0.067 V at 298
K.
[Cu2+] = 2×10^−14 M
Based on these data, what is the value of the formation
constant, Kf, of [Cu(NH3)4]2+?

Added by Jennifer S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Caryl Abrenica

03/17/2022

Step 1

Step 1: Calculate the concentration of [Cu2+] in the solution using the given information that [Cu2+] = 2×10^−14 M. Show more…

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A copper, Cu(s), the electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraammine copper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.067 V at 298 K. [Cu2+] = 2×10^−14 M Based on these data, what is the value of the formation constant, Kf, of [Cu(NH3)4]2+?