Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
Solutions
Molarity
Osmolarity
Dilutions
Solubility Rules
Electrolytes
Molecular Equations
Gas Evolution Equations
Solution Stoichiometry
Complete Ionic Equations
Calculate Oxidation Numbers
Redox Reactions
Balancing Redox Reactions: Acidic Solutions
Balancing Redox Reactions: Basic Solutions
Activity Series
Additional Practice
Types of Chemical Reactions
Normality & Equivalent Weight
Additional Guides
Oxidation Reduction (Redox) Reactions
Oxidation Number
Net Ionic Equation
LearnAdditional Practice
Next SectionActivity Series

Balancing Basic Redox Reactions requires all the same steps as balancing in an acidic solution plus an additional step.

Balancing Basic Redox Reactions

Concept #1: Balancing Redox Reactions: Basic Solutions

Basic Redox Reactions generally have the presence of an OH– ion.

Example #1: Balance the following redox reaction if it is found to be in a basic solution.

Practice: Balance the following redox reaction in a basic solution

H2O2 (aq) + ClO2 (aq) → ClO2- (aq) + O2 (g)

Practice: Balance the following redox reaction in a basic solution.

ClO2- (aq) → Cl- (aq) + ClO4- (aq)

Previous SectionBalancing Redox Reactions: Acidic Solutions
Next SectionActivity Series
Additional Problems
What is the coefficient of the oxidizing agent when it is balanced within a basic solution? Cl2(g) + S2O3 2- (aq)      →       Cl- (aq) + SO4 2- (aq)   a) 1                b) 2                c) 3                d) 4
Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Br2 and OH- in the balanced reaction? Br2(l) → BrO3-(aq) + Br-(aq) A) Br2 = 3, OH - = 6 B) Br2 = 3, OH - = 3 C) Br2 = 2, OH - = 5 D) Br2 = 1, OH - = 2 E) Br2 = 1, OH - = 6
Balance the following redox reactions occurring in basic solution.MnO4−(aq) + Br -(aq) → MnO2(s) + BrO3−(aq)a. MnO4−(aq) + H2O(l) + Br−(aq) → MnO2(s) + 2OH−(aq) + BrO3−(aq)b. 2MnO4−(aq) +  H2O(l) + Br−(aq) → 2MnO2(s) + 2OH−(aq) + BrO3−(aq)c. 2MnO4−(aq) +  H2O(l) + Br−(aq) → 2MnO2(s) + OH−(aq) + BrO3−(aq)d. MnO4−(aq) +  H2O(l) + 2Br−(aq) → MnO2(s) + OH−(aq) + 2BrO3−(aq)
Balance the following redox reactions occurring in basic solution.NO2−(aq) + Al(s) → NH 3(g) + AlO2−(aq)a. NO2−(aq) + H2O(l) + 2Al(s) + OH−(aq) → NH3(g) + 2AlO2−(aq)b. NO2−(aq) + H2O(l) + 2Al(s) + OH−(aq) → 2NH3(g) + 2AlO2−(aq)c. NO2−(aq) + H2O(l) + Al(s) + 2OH−(aq) → 2NH3(g) + AlO2−(aq)d. NO2−(aq) + 2H2O(l) + Al(s) + 2OH−(aq) → NH3(g) + AlO2−(aq)