Ch.15 - Acid and Base EquilibriumWorksheetSee 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: Given the balanced equation representing a reaction: HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq) According to one acid-base theory, the H2O(l) molecules act as a. a base because they accept H+ ions b. a base because they donate H+ ions c. an acid because they accept H+ ions d. an acid because they donate H+ ions

Solution: Given the balanced equation representing a reaction: HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq) According to one acid-base theory, the H2O(l) molecules act as a. a base because they accept H+ ions b. a

Problem

Given the balanced equation representing a reaction: 

HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq) 

According to one acid-base theory, the H2O(l) molecules act as 

a. a base because they accept H+ ions 

b. a base because they donate H+ ions 

c. an acid because they accept H+ ions 

d. an acid because they donate H+ ions