Domanda del libro di testo
Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (c) Calculate the pH of a 0.050 M solution of sodium butyrate.
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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 109a
Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (a) Calculate the pKb for the butyrate ion.
Guida verificata passo dopo passo1
Identify the relationship between pKa and pKb in the context of the acid-base conjugate pair. The formula to use is: pKa + pKb = 14. This equation is derived from the ion product constant of water at 25°C, which is Kw = 10^{-14}.
Recognize that butyric acid (CH3CH2CH2COOH) dissociates to form the butyrate ion (CH3CH2CH2COO-) and a hydrogen ion (H+).
Use the given pKa value of butyric acid, which is 4.84, to find the pKb of the conjugate base, the butyrate ion.
Substitute the pKa value into the formula from step 1: pKb = 14 - pKa.
Calculate pKb using the substituted values to find the strength of the butyrate ion as a base.
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pKa and pKb Relationship
The pKa and pKb values are related through the equation pKa + pKb = 14 at 25°C. This relationship allows us to convert between the acidity of a weak acid and the basicity of its conjugate base. In this case, butyric acid has a pKa of 4.84, which can be used to find the pKb of the butyrate ion.
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Percorso guidato
03:01
Ka and Kb Relationship
Acid-Base Equilibrium
Acid-base equilibrium describes the balance between an acid and its conjugate base in solution. For butyric acid, the equilibrium can be represented as HA ⇌ H⁺ + A⁻, where HA is the acid and A⁻ is the conjugate base (butyrate ion). Understanding this equilibrium is essential for calculating pKb from pKa.
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Percorso guidato
6:47Triprotic Acid Equilibrium
Conjugate Acid-Base Pairs
Conjugate acid-base pairs consist of an acid and its corresponding base that differ by a proton (H⁺). In this scenario, butyric acid (the acid) and butyrate ion (the base) form a conjugate pair. Recognizing these pairs is crucial for applying the pKa and pKb relationship effectively.
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Percorso guidato
01:30Conjugate Acid-Base Pairs
Pratica correlata
Domanda del libro di testo
Arrange the following 0.10 M solutions in order of increasing acidity: (i) NH4NO3, (ii) NaNO3, (iii) CH3COONH4, (iv) NaF, (v) CH3COONa.
Domanda del libro di testo
Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (b) Calculate the pH of a 0.050 M solution of butyric acid.
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