Domanda del libro di testo
Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.
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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 51
Lactic acid CH3CH(OH)COOH has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate Ka.
Guida verificata passo dopo passo1
Identify the given information: The concentration of lactic acid is 0.10 M, and the pH of the solution is 2.44.
Calculate the concentration of hydrogen ions [H⁺] using the pH value: [H⁺] = 10^(-pH). Substitute the given pH value to find [H⁺].
Write the expression for the acid dissociation constant (Ka) for lactic acid: Ka = [H⁺][A⁻]/[HA], where [A⁻] is the concentration of the conjugate base and [HA] is the concentration of the undissociated acid.
Assume that the initial concentration of lactic acid [HA] is 0.10 M and that the change in concentration due to dissociation is equal to [H⁺]. Therefore, [A⁻] = [H⁺] and [HA] = 0.10 - [H⁺].
Substitute the values of [H⁺], [A⁻], and [HA] into the Ka expression and solve for Ka.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Acid-Base Equilibrium
Acid-base equilibrium refers to the balance between the concentrations of an acid and its conjugate base in a solution. For weak acids like lactic acid, this equilibrium can be described by the dissociation reaction, where the acid donates a proton (H+) to water, forming its conjugate base and hydronium ions. Understanding this concept is crucial for calculating the acid dissociation constant (Ka).
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Percorso guidato
6:47
Triprotic Acid Equilibrium
pH and Hydronium Ion Concentration
pH is a measure of the acidity of a solution, defined as the negative logarithm of the hydronium ion concentration (H3O+). A lower pH indicates a higher concentration of H3O+. In this case, the pH of 2.44 corresponds to a specific concentration of hydronium ions, which is essential for determining the degree of dissociation of lactic acid and subsequently calculating Ka.
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Percorso guidato
06:25Hydronium Ion Concentration Example
Acid Dissociation Constant (Ka)
The acid dissociation constant (Ka) quantifies the strength of a weak acid in solution. It is defined as the ratio of the concentration of the products (the conjugate base and hydronium ions) to the concentration of the undissociated acid at equilibrium. Calculating Ka involves using the concentrations derived from the initial concentration of the acid and the change in concentration due to dissociation, which is influenced by the pH of the solution.
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Percorso guidato
03:50Characteristics of Ka and Kb
Pratica correlata
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
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-
899
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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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