Explanation In order to show the steps required to balance any redox reaction. For representing the balancing steps of a redox reaction, a reaction is to be considered as given below. HNO 3 ( aq ) + H 3 AsO 3 ( aq ) → NO ( g ) + H 3 AsO 4 ( aq ) + H 2 O ( l ) (1) Step 1: Identify oxidation state of every atom on both reaction sides. Each atom’s oxidation state on left hand side is shown below. H = +1 N = +5 O = − 2 As = +3 Each atom’s oxidation state on right hand side is shown below. H = +1 N = +2 O = − 2 As = +5 Step 2 : Find the change in oxidation of atoms if any. The oxidation state of N changes from + 5 to + 2 and the oxidation state of As changes from + 3 to + 5 . The oxidation state of all other atoms remains the same. Step 3 : Find the number of N and As atoms that should be involved so that the increase in oxidation state of As becomes equal to the decrease in oxidations state of N . The increase in oxidation state of As is 2 and the decrease in oxidations state of N is 3 . Therefore, in order to balance the oxidation state change. The number of N atoms taken should be 2 and the number of As atoms taken should be 3

8th Edition

ISBN: 9781305581982

Author: Steven S. Zumdahl, Donald J. DeCoste

Publisher: Cengage Learning

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Redox Reactions

Redox reactions are considered to be the chemical reactions involving both oxidation and reduction processes. They are actually oxidation-reduction reactions. The term redox is made from two words where “red” comes from reduction and “ox” comes from oxid…

Question

Chapter 4, Problem 74E

Interpretation Introduction

Interpretation: The steps for balancing any redox reaction by oxidation state method are to be stated.

Concept introduction: All redox reactions are associated with one species’ oxidation and other species’ reduction. This reduction or oxidation also alters the oxidation state of involved species. For a balanced redox reaction, the increment oxidation state of one species must always be equal to decrement in oxidation state of other species. This is done to equalize the electrons gained and lost.

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Chapter 4 Solutions

Chemical Principles

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The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
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