Domanda del libro di testo
Given that pH + pOH = 14 and that the concentration of water in a solution of water is 55.5 M, show that the pKa of water is 15.7. (Hint: pOH=−log [HO−])
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Ch. 2 - Acids and Bases: Central to Understanding Organic Chemistry
Bruice8th EditionOrganic ChemistryISBN: 9780135213711
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TOC.tableOfContents
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding31
- Ch. 2 - Acids and Bases: Central to Understanding Organic Chemistry84
- Ch. 3 - An Introduction to Organic Compounds: Nomenclature, Physical Properties, and Structure183
- Ch. 4 - Isomers: The Arrangement of Atoms in Space121
- Ch. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and Kinetics83
- Ch. 6 - The Reactions of Alkenes • The Stereochemistry of Addition Reactions175
- Ch. 7 - The Reactions of Alkynes • An Introduction to Multistep Synthesis119
- Ch. 8 - Delocalized Electrons: Their Effect on Stability, pKa, and the Products of a Reaction • Aromaticity and Electronic Effects: An Introduction to the Reactions of Benzene148
- Ch. 9 - Substitution and Elimination Reactions of Alkyl Halides212
- Ch. 10 - Reactions of Alcohols, Ethers, Epoxides, Amines, and Sulfur-Containing Compounds131
- Ch. 11 - Organometallic Compounds60
- Ch. 12 - Radicals90
- Ch. 13 - Mass Spectrometry; Infrared Spectroscopy; UV/Vis Spectroscopy62
- Ch. 14 - NMR Spectroscopy95
- Ch. 15 - Reactions of Carboxylic Acids and Carboxylic Acid Derivatives123
- Ch. 16 - Reactions of Aldehydes and Ketones • More Reactions of Carboxylic Acid Derivatives141
- Ch. 17 - Reactions at the Alpha-Carbon101
- Ch. 18 - Reactions of Benzene and Substituted Benzenes144
- Ch. 19 - More About Amines • Reactions of Heterocyclic Compounds49
- Ch. 20 - The Organic Chemistry of Carbohydrates80
- Ch. 21 - Amino Acids, Peptides, and Proteins57
- Ch. 22 - Catalysis in Organic Reactions and in Enzymatic Reactions35
- Ch. 23 - The Organic Chemistry of the Coenzymes—Compounds Derived from Vitamins1
- Ch. 28 - Pericyclic Reactions58
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Bruice 8th EditionCh. 2 - Acids and Bases: Central to Understanding Organic ChemistryProblema 76b
Bruice 8th EditionCh. 2 - Acids and Bases: Central to Understanding Organic ChemistryProblema 76bCapitolo 2, Problema 76b
At what pH does 80% of the acid exist in its acidic form?
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Identify the relationship between the acidic form (HA) and its conjugate base (A⁻) using the Henderson-Hasselbalch equation: \( \text{pH} = \text{pKa} + \log \left( \frac{[A^-]}{[HA]} \right) \).
Determine the ratio of \([A^-]\) to \([HA]\) based on the problem statement. If 80% of the acid exists in its acidic form (HA), then \([HA] = 0.8\) and \([A^-] = 0.2\). The ratio \( \frac{[A^-]}{[HA]} \) is \( \frac{0.2}{0.8} = 0.25 \).
Substitute the ratio \( \frac{[A^-]}{[HA]} = 0.25 \) into the Henderson-Hasselbalch equation: \( \text{pH} = \text{pKa} + \log(0.25) \).
Simplify \( \log(0.25) \) using logarithmic properties: \( \log(0.25) = \log(1/4) = \log(1) - \log(4) = 0 - \log(4) = -\log(4) \).
Combine the simplified logarithmic term with the \( \text{pKa} \) to express the pH: \( \text{pH} = \text{pKa} - \log(4) \). This is the pH at which 80% of the acid exists in its acidic form.
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Acid-Base Equilibrium
Acid-base equilibrium refers to the balance between the concentrations of an acid and its conjugate base in a solution. This equilibrium is influenced by the pH of the solution, which determines the degree of ionization of the acid. Understanding this concept is crucial for determining the proportions of acidic and basic forms of a substance at a given pH.
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Determining Acid/Base Equilibrium
Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation is a mathematical formula that relates the pH of a solution to the pKa of an acid and the ratio of the concentrations of its deprotonated (base) and protonated (acid) forms. It is expressed as pH = pKa + log([A-]/[HA]). This equation is essential for calculating the pH at which a specific percentage of an acid exists in its acidic form.
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Percent Ionization
Percent ionization is a measure of the extent to which an acid dissociates into its ions in solution. It is calculated as the ratio of the concentration of ionized acid to the initial concentration of the acid, multiplied by 100. Knowing the percent ionization helps in understanding how much of the acid exists in its acidic form versus its ionized form at a specific pH.
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04:28Ionization Potentials
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