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
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 58
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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Identify the initial concentration of bromoacetic acid, which is 0.100 M.
Determine the concentration of ionized bromoacetic acid using the given ionization percentage: 13.2% of 0.100 M.
Calculate the concentrations of \([\text{H}^+]\) and \([\text{BrCH}_2\text{COO}^-]\) since they are equal to the concentration of ionized bromoacetic acid.
Find the concentration of the non-ionized bromoacetic acid \([\text{BrCH}_2\text{COOH}]\) by subtracting the ionized concentration from the initial concentration.
Use the expression for the acid dissociation constant \(K_a = \frac{[\text{H}^+][\text{BrCH}_2\text{COO}^-]}{[\text{BrCH}_2\text{COOH}]}\) to calculate \(K_a\).
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Ionization of Weak Acids
Weak acids, like bromoacetic acid, do not fully dissociate in solution. The degree of ionization indicates how much of the acid has converted to its ions, which is crucial for calculating concentrations of the species in solution. In this case, a 13.2% ionization means that 13.2% of the bromoacetic acid molecules have dissociated into H+ and BrCH2COO- ions.
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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 in solution. It is calculated using the concentrations of the products and reactants at equilibrium. For bromoacetic acid, Ka can be determined from the concentrations of H+, BrCH2COO-, and BrCH2COOH at equilibrium, reflecting the extent of ionization.
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01:14Equilibrium Constant K
Concentration Calculations
To find the concentrations of H+, BrCH2COO-, and BrCH2COOH, one must apply the initial concentration and the degree of ionization. For a 0.100 M solution that is 13.2% ionized, the concentration of H+ and BrCH2COO- can be calculated as 0.0132 M, while the remaining concentration of BrCH2COOH can be found by subtracting the ionized amount from the initial concentration.
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07:35Calculate Concentration of the Basic Form
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Domanda del libro di testo
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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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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