Domanda del libro di testo
(a) Write the net ionic equation for the reaction that occurs when a solution of hydrochloric acid (HCl) is mixed with a solution of sodium formate 1NaCHO22.
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Ch.17 - Additional Aspects of Aqueous 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
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Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 111b
Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 111bCapitolo 17, Problema 111b
(b) As the acid is titrated, the pH of the solution after the addition of 11.05 mL of the base is 4.89. What is the Ka for the acid?
Guida verificata passo dopo passo1
Identify the type of titration: Since the pH is given after adding a base to an acid, this is an acid-base titration.
Use the Henderson-Hasselbalch equation: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \), where \([\text{A}^-]\) is the concentration of the conjugate base and \([\text{HA}]\) is the concentration of the acid.
Rearrange the equation to solve for \( \text{pK}_a \): \( \text{pK}_a = \text{pH} - \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \).
Convert \( \text{pK}_a \) to \( K_a \) using the relationship \( K_a = 10^{-\text{pK}_a} \).
Determine the concentrations of \([\text{A}^-]\) and \([\text{HA}]\) using the initial concentrations and volumes of the acid and base to find \( K_a \).
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Acid-Base Titration
An acid-base titration is a quantitative analytical method used to determine the concentration of an acid or base in a solution. During the titration, a base is gradually added to an acid (or vice versa) until the reaction reaches the equivalence point, where the amount of acid equals the amount of base. The pH of the solution changes throughout the process, and specific pH values can indicate the strength of the acid or base involved.
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03:04
Acid-Base Titration
pH and pKa Relationship
The pH of a solution is a measure of its acidity or basicity, defined as the negative logarithm of the hydrogen ion concentration. The pKa is the negative logarithm of the acid dissociation constant (Ka) and indicates the strength of an acid; lower pKa values correspond to stronger acids. The Henderson-Hasselbalch equation relates pH, pKa, and the concentrations of the acid and its conjugate base, allowing for the calculation of Ka when pH and concentrations are known.
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02:09pH and pOH Calculations
Acid Dissociation Constant (Ka)
The acid dissociation constant (Ka) quantifies the strength of an acid in solution, representing the equilibrium constant for the dissociation of the acid into its ions. A higher Ka value indicates a stronger acid that dissociates more completely in solution. The Ka can be calculated using the concentrations of the products and reactants at equilibrium, which is essential for determining the strength of the acid in the titration scenario presented.
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03:50Characteristics of Ka and Kb
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