Textbook Question
Calculate the percent ionization of a formic acid solution having the given concentration. b. 0.500 M
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Ch.16 - Acids and Bases
Chapter 16, Problem 75
A 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Monoprotic Acid
A monoprotic acid is an acid that can donate only one proton (H+) per molecule during the ionization process. This characteristic simplifies the calculation of its ionization constant, as the equilibrium expression involves only one dissociation step. Common examples include acetic acid and hydrochloric acid.
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Binary Acids
Percent Ionization
Percent ionization is a measure of the extent to which an acid dissociates in solution, expressed as a percentage of the initial concentration that has ionized. It is calculated using the formula: (concentration of ionized acid / initial concentration) × 100%. This concept helps in understanding the strength of the acid and its behavior in solution.
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06:08Percent Ionization Example
Acid Ionization Constant (Ka)
The acid ionization constant (Ka) quantifies the strength of an acid in solution, representing the equilibrium constant for the dissociation of the acid into its ions. It is calculated using the formula: Ka = [H+][A-] / [HA], where [H+] is the concentration of hydrogen ions, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the undissociated acid. A higher Ka value indicates a stronger acid.
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03:50Characteristics of Ka and Kb
Related Practice
Textbook Question
Calculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M
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Textbook Question
Calculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M
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Open Question
A 0.085 M solution of a monoprotic acid has a percent ionization of 0.59%. Determine the acid ionization constant (Ka) for the acid.
Open Question
Find the pH and percent ionization of each HF solution. (Ka for HF is 6.8 * 10^-4.) a. 0.250 M HF b. 0.100 M HF c. 0.050 M HF.
Open Question
Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid given the following Ka values: a. Ka = 1.0 * 10^-5, b. Ka = 1.0 * 10^-3, c. Ka = 1.0 * 10^-1.