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Calculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M
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Ch.17 - Acids and Bases
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
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Capitolo 17, Problema 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.
Guida verificata passo dopo passo1
Identify the given information: the concentration of the acid \([HA]\) is 0.148 M, and the percent ionization is 1.55%.
Calculate the concentration of ionized acid \([H^+]\) using the percent ionization: \([H^+] = \frac{\text{percent ionization}}{100} \times [HA]\).
Since the acid is monoprotic, the concentration of \([A^-]\) is equal to \([H^+]\).
Write the expression for the acid ionization constant \(K_a\): \(K_a = \frac{[H^+][A^-]}{[HA] - [H^+]}\).
Substitute the values of \([H^+]\), \([A^-]\), and \([HA]\) into the \(K_a\) expression and simplify to find \(K_a\).
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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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Percorso guidato
01:03
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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Percorso guidato
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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Percorso guidato
03:50Characteristics of Ka and Kb