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

Arrange the acids H2S, HCl, and HBr in order of increasing acid strength.

A. H2S < HBr < HCl 

B. HCl < HBr < H2S

C. HCl < H2S < HBr 

D. HBr < H2S < HCl

E. H2S < HCl < HBr


We're being asked to rank the following acids in increasing acid strength

Recall that the strengths of binary acids is based on the electronegativity or size of the nonmetal.

Given: H2S, HCl, HBr

Recall that HCl, HBr and HI are the most common strong binary acids

Solution BlurView Complete Written Solution