A 36.0 mL solution of 0.0150 M Rh3+ in 1 M HClO4 was titrated with 0.0900 M Ce4+ to give Rh6+ and Ce3+. The reference electrode used is silver-silver chloride in saturated KCl. e) Calculate the potential (vs. Ag | AgCI) when 10.8 mL of titrant is added.E =Vf) Calculate the potential (vs. Ag | AGCI) at the equivalence point.E =Vg) Calculate the potential (vs. Ag | AgCl) when 19.2 mL of titrant is added.E =Vh) At what volume of titrant will the potential be equal to the standard potential of the Ce half-reaction (ignoring the Ag | AgCl electrode)?V =mL

e) Calculate the potential (vs. Ag | AgCI) when 10.8 mL of titrant is added. E = ) Calculate the potential (vs. Ag | AgCI) at the equivalence point. E = 3) Calculate the potential (vs. Ag|AgCI) when 19.2 mL of titrant is added. E = V

e) Calculate the potential (vs. Ag | AgCI) when 10.8 mL of titrant is added. E = ) Calculate the potential (vs. Ag | AgCI) at the equivalence point. E = 3) Calculate the potential (vs. Ag|AgCI) when 19.2 mL of titrant is added. E = V

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 147CP: The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a...

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Question

A 36.0 mL solution of 0.0150 M Rh³⁺ in 1 M HClO₄ was titrated with 0.0900 M Ce⁴⁺ to give Rh⁶⁺ and Ce³⁺. The reference electrode used is silver-silver chloride in saturated KCl.

e) Calculate the potential (vs. Ag | AgCI) when 10.8 mL of titrant is added.
E =
V
f) Calculate the potential (vs. Ag | AGCI) at the equivalence point.
E =
V
g) Calculate the potential (vs. Ag | AgCl) when 19.2 mL of titrant is added.
E =
V
h) At what volume of titrant will the potential be equal to the standard potential of the Ce half-reaction (ignoring the Ag | AgCl electrode)?
V =
mL

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