Based on the following three half-reactions, answer the questions below:AsO43- + 2 H+ + 2 e - = AsO33- + H2 O pe° = 2.64Fe(OH) 3 (s) + 3 H+ + e - → Fe 2+ + 3 H2 O pe° = 16.2MnO2 (s) + 4 H+ + 2 e - → Mn2+ + 2 H2 O pe° = 21.8 In the laboratory, a solution is initially prepared with 1.0×10 -5 M Na 3 AsO3 and 1.0×10-5 MNa 3 AsO4 and is buffered at pH 7.0. Then, 1.0×10-4 M FeCl 2 is added. Will reduction ofAsO43- by Fe 2+ occur (assume Fe(OH) 3 (s) is the iron product)?
Based on the following three half-reactions, answer the questions below:AsO43- + 2 H+ + 2 e - = AsO33- + H2 O pe° = 2.64Fe(OH) 3 (s) + 3 H+ + e - → Fe 2+ + 3 H2 O pe° = 16.2MnO2 (s) + 4 H+ + 2 e - → Mn2+ + 2 H2 O pe° = 21.8 In the laboratory, a solution is initially prepared with 1.0×10 -5 M Na 3 AsO3 and 1.0×10-5 MNa 3 AsO4 and is buffered at pH 7.0. Then, 1.0×10-4 M FeCl 2 is added. Will reduction ofAsO43- by Fe 2+ occur (assume Fe(OH) 3 (s) is the iron product)?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 26QAP: For the following half-reactions, answer the questions below....
Related questions
Question
Based on the following three half-reactions, answer the questions below:
AsO43- + 2 H+ + 2 e - = AsO33- + H2 O pe° = 2.64
Fe(OH) 3 (s) + 3 H+ + e - → Fe 2+ + 3 H2 O pe° = 16.2
MnO2 (s) + 4 H+ + 2 e - → Mn2+ + 2 H2 O pe° = 21.8
In the laboratory, a solution is initially prepared with 1.0×10 -5 M Na 3 AsO3 and 1.0×10-5 M
Na 3 AsO4 and is buffered at pH 7.0. Then, 1.0×10-4 M FeCl 2 is added. Will reduction of
AsO43- by Fe 2+ occur (assume Fe(OH) 3 (s) is the iron product)?
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