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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
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
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Capitolo 17, Problema 78c
Calculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M
Guida verificata passo dopo passo1
Identify the chemical formula for formic acid, which is \( \text{HCOOH} \).
Write the ionization equation for formic acid: \( \text{HCOOH} \rightleftharpoons \text{H}^+ + \text{HCOO}^- \).
Use the expression for the acid dissociation constant \( K_a \) for formic acid: \( K_a = \frac{[\text{H}^+][\text{HCOO}^-]}{[\text{HCOOH}]} \).
Assume initial concentration of formic acid is \( 0.100 \text{ M} \) and let \( x \) be the concentration of \( \text{H}^+ \) ions at equilibrium. Set up the expression: \( K_a = \frac{x^2}{0.100 - x} \).
Calculate the percent ionization using the formula: \( \text{Percent Ionization} = \left( \frac{x}{0.100} \right) \times 100 \% \).
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Ionization of Weak Acids
Weak acids, like formic acid, do not completely dissociate in solution. Instead, they establish an equilibrium between the undissociated acid and its ions. The degree of ionization is crucial for understanding the acid's strength and its behavior in solution.
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01:15
Calculating Percent Ionization of Weak Acids
Equilibrium Constant (Ka)
The acid dissociation constant (Ka) quantifies the strength of a weak acid by measuring the extent of ionization at equilibrium. For formic acid, the Ka value helps determine how much of the acid will ionize in a given concentration, which is essential for calculating percent ionization.
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01:14Equilibrium Constant K
Percent Ionization Calculation
Percent ionization is calculated by taking the ratio of the concentration of ionized acid to the initial concentration of the acid, multiplied by 100. This metric provides insight into the strength of the acid and its effectiveness in solution, particularly in dilute concentrations.
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01:15Calculating Percent Ionization of Weak Acids
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