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

Solution: The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a __________ process.a. 2-electronb. 3-electronc. 4-electrond. 6-electrone. 1-electron


The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a __________ process.

a. 2-electron

b. 3-electron

c. 4-electron

d. 6-electron

e. 1-electron


We’re being asked to determine how many electrons are involved in the half-reaction of conversion of sulfate (SO42-) to sulfite ion (SO32-)

In this case, we have to balance the redox reaction for this half-reaction.

SO42- → SO32-

Follow the steps below:

Step 1: Balance the non-hydrogen and non-oxygen elements first

Step 2: Balance oxygen by adding H2O to the side that needs oxygen (1 O: 1 H2O)

Step 3: Balance hydrogen by adding Hto the side that needs hydrogen (1 H: 1 H+)

Step 4: Balance the charges: add electrons to the more positive side (or less negative side)

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