Domanda del libro di testo
If a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate the concentration of hydrofluoric acid.
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Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 53
A 0.100 M solution of chloroacetic acid 1ClCH2COOH2 is 11.0% ionized. Using this information, calculate 3ClCH2COO-4, 3H+4, 3ClCH2COOH4, and Ka for chloroacetic acid.
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Identify the initial concentration of chloroacetic acid, \([\text{ClCH}_2\text{COOH}]_0 = 0.100\, \text{M}\).
Determine the concentration of ionized chloroacetic acid using the ionization percentage: \(0.100\, \text{M} \times 0.110 = [\text{ClCH}_2\text{COO}^-] = [\text{H}^+]\).
Calculate the concentration of non-ionized chloroacetic acid: \([\text{ClCH}_2\text{COOH}] = 0.100\, \text{M} - [\text{ClCH}_2\text{COO}^-]\).
Write the expression for the acid dissociation constant, \(K_a = \frac{[\text{ClCH}_2\text{COO}^-][\text{H}^+]}{[\text{ClCH}_2\text{COOH}]}\).
Substitute the concentrations into the \(K_a\) expression to solve for \(K_a\).
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Ionization of Weak Acids
Weak acids, like chloroacetic acid, do not fully dissociate in solution. The degree of ionization indicates how much of the acid has converted to its ions. In this case, an 11.0% ionization means that 11% of the chloroacetic acid molecules have dissociated into ions, which is crucial for calculating concentrations of the species in solution.
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01:15
Calculating Percent Ionization of Weak Acids
Equilibrium Concentrations
To find the concentrations of the ions and the undissociated acid at equilibrium, we use the initial concentration and the degree of ionization. For a 0.100 M solution that is 11.0% ionized, we can calculate the concentrations of ClCH2COO-, H+, and ClCH2COOH by applying the percentage to the initial concentration, which is essential for determining the acid dissociation constant (Ka).
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02:35Thermal Equilibrium
Acid Dissociation Constant (Ka)
The acid dissociation constant (Ka) quantifies the strength of an acid in solution. It is calculated using the equilibrium concentrations of the products and reactants from the ionization reaction. For chloroacetic acid, Ka can be determined using the formula Ka = [H+][ClCH2COO-] / [ClCH2COOH], where the concentrations are derived from the ionization data provided.
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03:50Characteristics of Ka and Kb
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Domanda del libro di testo
Write the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+(a)q as a product and then with the hydronium ion: (a) C6H5COOH (b) HCO3-
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Domanda del libro di testo
A 0.100 M solution of bromoacetic acid 1BrCH2COOH2 is 13.2% ionized. Calculate 3H+4, 3BrCH2COO-4, 3BrCH2COOH4 and Ka for bromoacetic acid.
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Domanda del libro di testo
Phenylacetic acid 1C6H5CH2COOH2 is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. A 0.085 M solution of C6H5CH2COOH has a pH of 2.68. Calculate the Ka value for this acid.
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