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
Problem

The following acids are listed in order of their increasing acidity. Provide a brief explanation for the observed trends. Note: The Pauling electronegativity values for selected elements are given in Table 1.

HIO < HBrO < HClO

Solution

We are asked to provide an explanation for the observed trend where the compounds are arranged in increasing acidity. 

HIO < HBrO < HClO

It can be observed that all of the acids have an O meaning they are oxyacids. 

The strengths of oxyacids is based on the number of oxygens or the electronegativity of the nonmetal in the oxyacid. An oxyacid is considered strong when there are at least 2 or more O than H.

Given:

HIO < HBrO < HClO


The three oxyacids given have an equal number of oxygens. We’ll rank their strength based on the electronegativity of the nonmetal in each oxyacid.


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