By suitable combination of redox half-equations, under acidic conditions, determine a redox potential for the oxidation of nitrite (NO2–) to nitrate (NO3–). NO3– → NO2– E, = 0.94 V O2 → H2O E, = 1.23 V
By suitable combination of redox half-equations, under acidic conditions, determine a redox potential for the oxidation of nitrite (NO2–) to nitrate (NO3–). NO3– → NO2– E, = 0.94 V O2 → H2O E, = 1.23 V
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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(a) The concentration of nitrites can be estimated by oxidation with ceric sulfate, Ce(SO4)2. However, nitrites cannot be titrated with ceric sulfate solutions directly, owing to oxidation by air.
(i) By suitable combination of redox half-equations, under acidic conditions, determine a redox potential for the oxidation of nitrite (NO2–) to nitrate (NO3–).
NO3– → NO2– E, = 0.94 V
O2 → H2O E, = 1.23 V
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