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1. The yellow dioxovanadium(V) ion, VO 2 + (aq), is reduced by zinc metal in three steps. The first step reduces it to blue VO 2 + (aq). This ion is further reduced to green V 3+ (aq) in the second step, and V 3+ can be reduced to violet V 2+ (aq) in a third step. In each step, zinc is oxidized to Zn 2+ (aq). Write balanced net ionic equations for Steps 2 and 3. (This reduction sequence is shown in Figure 193.) 2. A common laboratory analysis for iron is to titrate aqueous iron(ll) ion with a solution of potassium permanganate of precisely known concentration. Use the half-reaction method to write the balanced net ionic equation for the reaction in acid solution. MnO 4 − (aq) + Fe 2+ (aq) → Mn 2+ (aq) + Fe 3+ (aq) Identify the oxidizing agent, the reducing agent, the substance oxidized, and the substance reduced (see Figure 19.4).

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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 19.1, Problem 2CYU
Textbook Problem
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  1. 1. The yellow dioxovanadium(V) ion, VO2+ (aq), is reduced by zinc metal in three steps. The first step reduces it to blue VO2+ (aq). This ion is further reduced to green V3+(aq) in the second step, and V3+ can be reduced to violet V2+(aq) in a third step. In each step, zinc is oxidized to Zn2+ (aq). Write balanced net ionic equations for Steps 2 and 3. (This reduction sequence is shown in Figure 193.)
  2. 2. A common laboratory analysis for iron is to titrate aqueous iron(ll) ion with a solution of potassium permanganate of precisely known concentration. Use the half-reaction method to write the balanced net ionic equation for the reaction in acid solution.

MnO4(aq) + Fe2+(aq) → Mn2+(aq) + Fe3+(aq)

Identify the oxidizing agent, the reducing agent, the substance oxidized, and the substance reduced (see Figure 19.4).

1.

Interpretation Introduction

Interpretation:

The net ionic equation for step 2 and 3 reduction reactions of dioxovanadium ion by zinc metal is to be determined.

Concept Introduction:

  • The substance that easily be reduced in a reaction is represented as an oxidizing agent. The substance that easily be oxidized in a reaction is represented as an reducing agent.
  • Redox reaction: In a reaction both oxidation and reduction occurs at the same time.

Steps followed to balance a redox (reduction-oxidation) reaction occurs in acidic medium,

  • Redox reacions can be sperated into two half-reactions, such as oxidation reaction and reduction reaction.
  • Balancing of oxygen and hydrogen are carried out by adding water and H+ions in the half-reactions, and balance the number of elctrons then make the number of electrons in oxidation and reduction reactions equal by multiplying by integers.
  • Club the both half-reactions.

Explanation of Solution

The given redox equation is as follows.

VO2+(aq) + Zn(s) V3+(aq) + Zn2+(aq)

Steps for balancing redox reactions in acidic solution:

  1. 1. Recognize the reaction as an oxidation and reduction reaction.

    Zn increases their oxidation state from 0to+2 .Therefore, it is an oxidation reaction.

    Vreduces its oxidation state from +4to+3.Therefore, it is a reduction reaction.

  2. 2. Separate two half reactions.

    Oxidation:    Zn(s)  Zn2+(aq)Reduction:     VO2+ (aq)  V3+(aq)

  3. 3. Balance half reactions by mass.

    Balance all atoms except H and O in half reaction.

    Oxidation:    Zn(s)  Zn2+(aq)Reduction:     VO2+ (aq)  V3+(aq)

    Balance O atoms by adding water to the side missing O atoms.

    Oxidation:    Zn(s)  Zn2+(aq)Reduction:     VO2+ (aq)  V3+(aq)+H2Ol

    Balance the H atoms by adding H+to the side missing Hatoms.

    Oxidation:    Zn(s)  Zn2+(aq)Reduction:     VO2+(aq) +2H+ V3+(aq)+H2Ol

  4. 4. Balance the charge by adding electrons to side with more total positive charge.

    Oxidation:    Zn(s)  Zn2+(aq)+2eReduction:     VO2+(aq) +2H++2e V3+(aq)+H2Ol

  5. 5. Make the number of electrons the same in both half reactions by multiplication, while avoiding fractional number of electrons.

    Oxidation:    Zn(s)  Zn2+(aq)+2eReduction:     2VO2+(aq) +2H++e V3+(aq)+H2Ol

  6. 6. Add the half reaction together and than simplyfy by cancelling out species that show up on both sides

2.

Interpretation Introduction

Interpretation:

The net ionic equation for step 2 and 3 reduction reactions of dioxovanadium ion by zinc metal is to be determined. Also the net ionic equation oxidizing agent, reducing agent, the oxidized substance and reduced substance for the titration of aqueous ion with potassium permanganate is to be identified.

Concept Introduction:

Refer part 1.

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Chapter 19 Solutions

Chemistry & Chemical Reactivity
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