The titration solution in the cell below had a total volume of 50.0 mL and contained 0.100 M Mg2+ and 1.00 x 10-5 M Zn(EDTA)2- at a pH of 10.00 S.C.E. || Zn(s) | titration solution Zn2* + 2e- Zn(s) E = -0.762 v MgY2: Kf = 6.2 x 108; Zny2-: Kf = 3.2 x 1016. What will be the cell voltage when 10.0 mL of 0.100 M EDTA has been added? (Hint: See Exercise 15-B.) i) Total mmoles of Mg*2 ii) mmoles of EDTA added is iii) mmoles of Mg*2 reacting with EDTA

The titration solution in the cell below had a total volume of 50.0 mL and contained 0.100 M Mg2+ and 1.00 x 10-5 M Zn(EDTA)2- at a pH of 10.00 S.C.E. || Zn(s) | titration solution Zn2* + 2e- Zn(s) E = -0.762 v MgY2: Kf = 6.2 x 108; Zny2-: Kf = 3.2 x 1016. What will be the cell voltage when 10.0 mL of 0.100 M EDTA has been added? (Hint: See Exercise 15-B.) i) Total mmoles of Mg2 ii) mmoles of EDTA added is iii) mmoles of Mg2 reacting with EDTA

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.21QAP

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