Domanda del libro di testo
Rank the ions (−CH3, −NH2, HO−, and F−) from most basic to least basic.
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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 19c,d
Bruice 8th EditionCh. 2 - Acids and Bases: Central to Understanding Organic ChemistryProblema 19c,dCapitolo 2, Problema 19c,d
Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs:
c. CH3NH2 + H2O
d. CH3N+H3 + H2O
Guida verificata passo dopo passo1
Identify the acid and base in the reaction. For part (c), CH3NH2 (methylamine) acts as a base, and H2O (water) acts as an acid. For part (d), CH3NH3+ (methylammonium ion) acts as an acid, and H2O acts as a base.
Write the chemical equations for the reactions. For part (c), the reaction is CH3NH2 + H2O ⇌ CH3NH3+ + OH⁻. For part (d), the reaction is CH3NH3+ + H2O ⇌ CH3NH2 + H3O⁺.
Determine the equilibrium constant expression (K_eq) for each reaction. For part (c), K_eq = ([CH3NH3+][OH⁻]) / ([CH3NH2][H2O]). For part (d), K_eq = ([CH3NH2][H3O⁺]) / ([CH3NH3+][H2O]).
Simplify the equilibrium constant expressions by recognizing that the concentration of water ([H2O]) is constant in dilute aqueous solutions. This allows you to use the base dissociation constant (K_b) for part (c) and the acid dissociation constant (K_a) for part (d).
Use the relationship between K_a and K_b for conjugate acid-base pairs: K_a × K_b = K_w, where K_w is the ionization constant of water (1.0 × 10⁻¹⁴ at 25°C). If needed, calculate K_a or K_b using this relationship to find the equilibrium constant for the given reactions.
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Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H+) between reactants. In these reactions, acids donate protons while bases accept them. Understanding the nature of the reactants, such as whether they are strong or weak acids or bases, is crucial for predicting the direction of the reaction and calculating the equilibrium constant.
Video consigliato:
02:49
The Lewis definition of acids and bases.
Equilibrium Constant (K)
The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is calculated using the formula K = [products]/[reactants], where the concentrations are raised to the power of their coefficients in the balanced equation. A higher K value indicates a greater tendency for the reaction to favor products.
Video consigliato:
02:19The relationship between equilibrium constant and pKa.
pKa and pKb Values
pKa and pKb values are measures of the strength of acids and bases, respectively. The pKa indicates the acidity of a compound, while pKb indicates the basicity. These values are essential for determining the equilibrium position of acid-base reactions, as they help predict which species will be favored at equilibrium based on their relative strengths.
Video consigliato:
07:45Identifying pKa values
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Ethyne (HC≡CH) has a pKa value of 25, water has a pKa value of 15.7, and ammonia (NH3) has a pKa value of 36. Draw the equation, showing equilibrium arrows that indicate whether reactants or products are favored, for the acid–base reaction of ethyne with
b. −NH2.
c. Which would be a better base to use if you wanted to remove a proton from ethyne, HO− or -NH2?
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Rank the carbanions shown in the margin from most basic to least basic.
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Domanda del libro di testo
Ethyne (HC≡CH) has a pKa value of 25, water has a pKa value of 15.7, and ammonia (NH3) has a pKa value of 36. Draw the equation, showing equilibrium arrows that indicate whether reactants or products are favored, for the acid–base reaction of ethyne with
a. HO-.
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Which of the following bases can remove a proton from acetic acid in a reaction that favors products?
HO− CH3NH2 HC≡C− CH3OH H2O Cl−
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Which is a stronger acid?
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