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: Give the conjugate acid of the following Bronsted-Lowry base: H2PO4-.

Solution: Give the conjugate acid of the following Bronsted-Lowry base: H2PO4-.

Problem

Give the conjugate acid of the following Bronsted-Lowry base: H2PO4-.

Solution

We’re being asked to determine the conjugate acids and bases of each of the given compound.

According to Brønsted and Lowry, an acid was classified as a proton (H+) donor while a base was a proton (H+) acceptor


When an acid loses an H+ the resulting species is called its conjugate base.

***Note: The compound gains 1 negative charge for each proton removed

Solution BlurView Complete Written Solution