A. If the measured cell potential is 1.800V, what is the concentration of Au3+?B. How long will it take to electroplate the katana assuming that all gold ions are converted to solid gold?C. What is the mass of the electroplated gold? Au³+₁(aq)Ni²+E° +1.520VE° = -0.230VGiven:[Ni²+] = 0.050 MFMAU = 196.97 g/molFMNi = 58.69 g/molAfter determining the gold ion concentration, Tanjiro then proceeded with theelectrolysis process. He electroplated the katana using 250.0 mL of the gold solutionwith a current of 3.20A.+ 3e → Au(s)*(aq) + 2e → Ni(s)

Here we have to determine the concentration of Au+3 of the galvanic cell and mass of gold…

A. If the measured cell potential is 1.800V, what is the concentration of Au3+? B. How long will it take to electroplate the katana assuming that all gold ions are converted to solid gold? C. What is the mass of the electroplated gold?

A. If the measured cell potential is 1.800V, what is the concentration of Au3+? B. How long will it take to electroplate the katana assuming that all gold ions are converted to solid gold? C. What is the mass of the electroplated gold?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.26QAP

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Question

A. If the measured cell potential is 1.800V, what is the concentration of Au3+?

B. How long will it take to electroplate the katana assuming that all gold ions are converted to solid gold?

C. What is the mass of the electroplated gold?

Au³+₁
(aq)
Ni²+
E° +1.520V
E° = -0.230V
Given:
[Ni²+] = 0.050 M
FMAU = 196.97 g/mol
FMNi = 58.69 g/mol
After determining the gold ion concentration, Tanjiro then proceeded with the
electrolysis process. He electroplated the katana using 250.0 mL of the gold solution
with a current of 3.20A.
+ 3e → Au(s)
*(aq) + 2e → Ni(s)

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