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: Percent ionization for a weak acid (HA) is determined by the following formula:Percent ionization=[HA] ionized / [HA] initial × 100%For strong acids, ionization is nearly complete (100%) at most conce

Solution: Percent ionization for a weak acid (HA) is determined by the following formula:Percent ionization=[HA] ionized / [HA] initial × 100%For strong acids, ionization is nearly complete (100%) at most conce

Problem

Percent ionization for a weak acid (HA) is determined by the following formula:

Percent ionization=[HA] ionized / [HA] initial × 100%

For strong acids, ionization is nearly complete (100%) at most concentrations. However, for weak acids, the percent ionization changes significantly with concentration. The more diluted the acid is, the greater percent ionization.

A certain weak acid, HA, has a Ka value of 7.6×10 −7.

A) Calculate the percent ionization of HA in a 0.10 M solution. Express your answer as a percent using two significant figures.

B) Calculate the percent ionization of HA in a 0.010 M solution. Express your answer as a percent using two significant figures.