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: Classify the following as acid-base reactions or oxidation-reduction reactions:(e) K3P(s) + 2O2(g) ⟶ K3PO4(s)

Solution: Classify the following as acid-base reactions or oxidation-reduction reactions:(e) K3P(s) + 2O2(g) ⟶ K3PO4(s)

Problem

Classify the following as acid-base reactions or oxidation-reduction reactions:

(e) K3P(s) + 2O2(g) ⟶ K3PO4(s)

Solution

Recall: An acid-base reaction is also called a neutralization reaction. An acid and a base reacts together, forming a salt and water.

On the other hand, oxidation-reduction reactions involve a change in the oxidation states of the reactants.

For the reaction K3P(s) + 2 O2(g K3PO4(s), we can see that water isn't formed, which means this isn't an acid-base reaction. To confirm, we can check the oxidation states of the reactants vs. oxidation states of the products.

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