Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 39

Balance these equations for redox reactions in basic solution. (a) \(\mathrm{MnO}_{2}(\mathrm{s})+\mathrm{ClO}_{3}^{-} \longrightarrow \mathrm{MnO}_{4}^{-}+\mathrm{Cl}^{-}\) (b) \(\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{OCl}^{-} \longrightarrow \mathrm{FeO}_{4}^{2-}+\mathrm{Cl}^{-}\) (c) \(\mathrm{ClO}_{2} \longrightarrow \mathrm{ClO}_{3}^{-}+\mathrm{Cl}\) (d) \(\mathrm{Ag}(\mathrm{s})+\mathrm{CrO}_{4}^{2-} \rightarrow \mathrm{Ag}^{+}+\mathrm{Cr}(\mathrm{OH})_{3}(\mathrm{s})\)

Short Answer

Expert verified
The balanced chemical equations are: (a) \(4\, \mathrm{MnO}_2 + 4\, \mathrm{ClO}_3^- + 8\, \mathrm{OH}^- \rightarrow 4\, \mathrm{MnO}_4^- + 4\, \mathrm{Cl}^- + 2\, \mathrm{H}_2\mathrm{O}\), (b) \(2\, \mathrm{Fe(OH)}_3 + 5\, \mathrm{OCl}^- + 8\, \mathrm{H}_2\mathrm{O} \rightarrow 2\, \mathrm{FeO}_4^{2-} + 5\, \mathrm{Cl}^- + 8\, \mathrm{OH}^-\), (c) \(2\, \mathrm{ClO}_2 + 2\, \mathrm{OH}^- \rightarrow \mathrm{ClO}_3^- + 3\, \mathrm{Cl}^- + 2\, \mathrm{H}_2\mathrm{O}\), (d) \(\mathrm{Ag} + \mathrm{CrO}_4^{2-} + 1\, \mathrm{OH}^- \rightarrow \mathrm{Ag}^{+} + \mathrm{Cr(OH)}_3 + 4\, \mathrm{H}_2\mathrm{O}\)

Step by step solution

01

- Identify the oxidation states and which species are reduced and oxidized for each reaction

The oxidation state changes are for reaction (a) Mn (from +4 to +7), Cl (from +5 to -1), for (b) Fe (from +3 to +6), Cl (from +1 to -1), for (c) Cl (from +3 to +5 and from +3 to -1), and for (d) Ag (from 0 to +1), Cr (from +6 to +3).
02

- Balance atoms other than Hydrogen and Oxygen

In (a) the Cl atoms are already balanced and so are the Mn. In (b) the Cl and Fe atoms are already balanced. In (c) there is one ClO2 molecule and one atom each of Chlorine and ClO3-. In (d) there is one atom of Ag on each side and one CrO4 on left and one Cr on right.
03

- Balance Oxygen using H2O

Add, for (a) 4H2O to the right side, for (b) 4H2O to the left side, for (c) 2H2O to the right side, for (d) 4H2O to the right side.
04

- Balance Hydrogen using OH-

Add, for (a) 8OH- to the left side, for (b) 8OH- to the right side, for (c) 2OH- to the left, for (d) 8OH- to the left.
05

- Balance charges with e-

Balance the charges by adding, for (a) 2e- to the right side, for (b) 5e- to the left side, for (c) 2e- to the left of the first half reaction and 4e- to the right of the second half reaction, for (d) 1e- to the left side.
06

- Combine half-reactions

Combine the half reactions by adding, for (a) the reduction and oxidation half-reactions, for (b) the reduction and oxidation half reactions, for (c) the reduction half reaction to the oxidation half reaction multiplied by 2, for (d) the reduction and oxidation half reactions.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Explain the important distinctions between (a) a strong electrolyte and strong acid; (b) an oxidizing agent and reducing agent; (c) precipitation reactions and neutralization reactions; (d) half-reaction and overall reaction.

The exact neutralization of \(10.00 \mathrm{mL}\) of \(0.1012 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\text { aq })\) requires \(23.31 \mathrm{mL}\) of \(\mathrm{NaOH}\). What must be the molarity of the \(\mathrm{NaOH}(\mathrm{aq}) ?\) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{NaOH}(\mathrm{aq}) \longrightarrow\) \(\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(1)\)

To precipitate \(\mathrm{Zn}^{2+}\) from \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}),\) add (a) \(\mathrm{NH}_{4} \mathrm{Cl} ;\) (b) \(\mathrm{MgBr}_{2} ;\) (c) \(\mathrm{K}_{2} \mathrm{CO}_{3} ;\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\).

Which solutions would you use to precipitate \(\mathrm{Mg}^{2+}\) from an aqueous solution of \(\mathrm{MgCl}_{2} ?\) Explain your choice. (a) \(\mathrm{KNO}_{3}(\mathrm{aq}) ;\) (b) \(\mathrm{NH}_{3}(\mathrm{aq}) ;\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq});\) (d) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(\mathrm{aq})\).

What volume of \(0.248 \mathrm{M} \mathrm{CaCl}_{2}\) must be added to \(335 \mathrm{mL}\) of \(0.186 \mathrm{M} \mathrm{KCl}\) to produce a solution with a concentration of \(0.250 \mathrm{M} \mathrm{Cl}^{-2}\) Assume that the solution volumes are additive.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free