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At what pH does 80% of the acid exist in its acidic form?
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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 76a
Bruice 8th EditionCh. 2 - Acids and Bases: Central to Understanding Organic ChemistryProblema 76aCapitolo 2, Problema 76a
If an acid with a pKa of 5.3 is in an aqueous solution of pH 5.7, what percentage of the acid is present in its acidic form?
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Identify the relationship between pH, pKa, and the ratio of the acidic form (HA) to the conjugate base (A⁻) using the Henderson-Hasselbalch equation: \( \text{pH} = \text{pKa} + \log \left( \frac{[A^-]}{[HA]} \right) \).
Rearrange the Henderson-Hasselbalch equation to solve for the ratio \( \frac{[A^-]}{[HA]} \): \( \frac{[A^-]}{[HA]} = 10^{\text{pH} - \text{pKa}} \).
Substitute the given values for pH (5.7) and pKa (5.3) into the equation: \( \frac{[A^-]}{[HA]} = 10^{5.7 - 5.3} \).
Once the ratio \( \frac{[A^-]}{[HA]} \) is determined, calculate the fraction of the acid in its acidic form (HA) using the formula: \( \text{Fraction of HA} = \frac{1}{1 + \frac{[A^-]}{[HA]}} \).
Convert the fraction of HA into a percentage by multiplying by 100: \( \text{Percentage of HA} = \text{Fraction of HA} \times 100 \).
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pKa and pH Relationship
The pKa of an acid is a measure of its strength, indicating the pH at which half of the acid is dissociated. A lower pKa value means a stronger acid. The pH of a solution reflects the concentration of hydrogen ions; when pH is higher than pKa, the acid is more likely to be in its deprotonated (conjugate base) form.
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Identifying pKa values
Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation relates pH, pKa, and the ratio of the concentrations of the deprotonated and protonated forms of an acid. It is expressed as pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the acid. This equation is essential for calculating the proportions of the acid in different forms at a given pH.
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Percentage of Acidic Form
To determine the percentage of an acid present in its acidic form, one can use the ratio derived from the Henderson-Hasselbalch equation. By calculating the ratio of [HA] to the total concentration of acid ([HA] + [A-]), the percentage of the acid in its protonated form can be expressed as ( [HA] / ([HA] + [A-]) ) × 100%. This calculation is crucial for understanding the acid's behavior in solution.
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