Textbook Question
Balance each redox reaction occurring in basic aqueous solution. b. Al(s) + MnO4–(aq) → MnO2(s) + Al(OH)4–(aq)
Ch.19 - Electrochemistry
Chapter 19, Problem 42b
Balance each redox reaction occurring in basic aqueous solution. b. Ag(s) + CN–(aq) + O2(g) → Ag(CN)2–(aq)
Verified step by step guidance1
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.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
13mWas this helpful?
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.
Recommended video:
Guided course
03:12
Identifying Redox Reactions
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.
Recommended video:
Guided course
01:04Balancing Basic Redox Reactions
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.
Recommended video:
Guided course
01:49Method 1 of Radioactive Half-Life
Related Practice
Textbook Question
Balance each redox reaction occurring in basic aqueous solution. c. Cl2(g) → Cl–(aq) + ClO–(aq)
Textbook Question
Balance each redox reaction occurring in basic aqueous solution. a. MnO4–(aq) + Br–(aq) → MnO2(s) + BrO3–(aq)
Textbook Question
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. 2 Ag+(aq) + Pb(s) → 2 Ag(s) + Pb2+(aq)
b. 2 ClO2(g) + 2 I–(aq) → 2 ClO2–(aq) + I2(s)
c. O2(g) + 4 H+(aq) + 2 Zn(s) → 2 H2O(l) + 2 Zn2+(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)