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Ch.20 - Electrochemistry
All textbooksTro 6th EditionCh.20 - ElectrochemistryProblem 42b
Chapter 20, Problem 42b

Balance each redox reaction occurring in basic aqueous solution. b. Ag(s) + CN–(aq) + O2(g) → Ag(CN)2–(aq)

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Identify the oxidation and reduction half-reactions. In this case, Ag(s) is oxidized to Ag(CN)_2^-(aq), and O_2(g) is reduced.
Write the oxidation half-reaction: Ag(s) → Ag(CN)_2^-(aq). Balance the silver atoms and add CN^- to balance the cyanide ions.
Write the reduction half-reaction: O_2(g) → OH^-(aq). Balance the oxygen atoms by adding H_2O, and then balance the hydrogen atoms by adding OH^-.
Balance the charge in each half-reaction by adding electrons. The oxidation half-reaction will have electrons on the right, and the reduction half-reaction will have electrons on the left.
Combine the balanced half-reactions, ensuring that the electrons cancel out. Adjust coefficients as necessary to ensure mass and charge balance in the basic solution.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Redox Reactions

Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between two species. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the oxidation states of the elements involved is crucial for identifying which species undergo oxidation and reduction.
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Balancing Redox Reactions in Basic Solution

Balancing redox reactions in basic solutions requires a systematic approach that includes separating the reaction into half-reactions for oxidation and reduction. After balancing the atoms and charges in each half-reaction, hydroxide ions (OH-) are added to neutralize any hydrogen ions (H+) that may form, ensuring the reaction adheres to the basic conditions.
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Half-Reaction Method

The half-reaction method is a technique used to balance redox reactions by focusing on the individual oxidation and reduction processes. Each half-reaction is balanced for mass and charge, and then combined to form the overall balanced equation. This method is particularly useful in complex reactions, such as those occurring in aqueous solutions.
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Related Practice
Textbook Question

Balance each redox reaction occurring in basic aqueous solution. a. H2O2(aq) + ClO2(aq) → ClO2–(aq) + O2(g)

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Balance each redox reaction occurring in basic aqueous solution. a. MnO4–(aq) + Br–(aq) → MnO2(s) + BrO3–(aq)

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Balance each redox reaction occurring in basic aqueous solution. c. NO2–(aq) + Al(s) → NH3(g) + AlO2–(aq)

Textbook Question

Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. Ni2+(aq) + Mg(s) → Ni(s) + Mg2+(aq)

Textbook Question

Calculate the standard cell potential for each of the electro- chemical cells in Problem 43.