Ch.15 - Acid and Base EquilibriumSee 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 reason HI is a stronger acid than HCl is because      A) the difference in electronegativity gets larger as the atoms get farther apart on the periodic table. B) electronegativity increases as you go up the periodic table. C) the bond strength decreases down a group in the periodic table. D) anion radius decreases as you go down the periodic table. E) HI is an Arrehnius acid and HCl is not.

Problem

The reason HI is a stronger acid than HCl is because     

A) the difference in electronegativity gets larger as the atoms get farther apart on the periodic table.

B) electronegativity increases as you go up the periodic table.

C) the bond strength decreases down a group in the periodic table.

D) anion radius decreases as you go down the periodic table.

E) HI is an Arrehnius acid and HCl is not.