Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(c)
1242
views
Ch. 4 - Acids and Bases: Electron Flow
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch. 2 - General Chemistry Translated: Finding the Electrons114
- Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis109
- Ch. 4 - Acids and Bases: Electron Flow144
- Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics118
- Ch. 6 - Stereoisomerism: Arrangement of Atoms in Space112
- Ch. 7 - Principles of Green (Organic) Chemistry3
- Ch. 8 - Alkenes I: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes II: Oxidation and Reduction150
- Ch. 10 - Alkynes: Electrophilic Addition and Redox Reactions101
- Ch. 11 - Properties and Synthesis of Alkyl Halides: Radical Reactions108
- Ch. 12 - Substitution and Elimination: Reactions of Haloalkanes172
- Ch. 13 - Alcohols, Ethers and Related Compounds: Substitution and Elimination239
- Ch. 14 - Structural Identification I: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification II: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution I: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution II: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems I: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems II: Pericyclic Reactions54
- Ch. 23 - Benzene I: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene II: Reactions Influenced by the Aromatic Ring62
- Ch. 25 - Amines: Structure, Reactions, and Synthesis27
- Ch. 26 - Amino Acids, Proteins, and Peptide Synthesis9
- Ch. 27 - Carbohydrates, Nucleic Acids, and Lipids54
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Not the one you use?Change textbook
Chapter 3, Problem 8a
Sulfuric acid is a very strong acid. Show how the following equation can be used to explain that sulfuric acid is at once an Arrhenius, Brønsted–Lowry, and Lewis acid.
Verified step by step guidance1
Step 1: Analyze the chemical equation provided. Sulfuric acid (H₂SO₄) reacts with water (H₂O) to produce hydronium ion (H₃O⁺) and bisulfate ion (HSO₄⁻). This reaction demonstrates the acid dissociation process.
Step 2: Explain sulfuric acid as an Arrhenius acid. According to Arrhenius theory, an acid increases the concentration of H⁺ ions in aqueous solution. In this reaction, sulfuric acid donates a proton (H⁺) to water, forming H₃O⁺, which increases the H⁺ concentration in the solution.
Step 3: Explain sulfuric acid as a Brønsted–Lowry acid. According to Brønsted–Lowry theory, an acid is a proton donor. Sulfuric acid donates a proton (H⁺) to water, which acts as a Brønsted–Lowry base by accepting the proton, forming H₃O⁺.
Step 4: Explain sulfuric acid as a Lewis acid. According to Lewis theory, an acid is an electron pair acceptor. In this reaction, sulfuric acid accepts an electron pair from water during the formation of the hydronium ion (H₃O⁺), demonstrating its role as a Lewis acid.
Step 5: Summarize the versatility of sulfuric acid. The reaction shows that sulfuric acid fulfills the criteria for being an Arrhenius acid (increases H⁺ concentration), a Brønsted–Lowry acid (proton donor), and a Lewis acid (electron pair acceptor), highlighting its strong acidic nature.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Arrhenius Acid
An Arrhenius acid is defined as a substance that increases the concentration of hydrogen ions (H⁺) in aqueous solution. In the case of sulfuric acid (H₂SO₄), it dissociates in water to produce H₃O⁺ ions, demonstrating its role as an Arrhenius acid. This definition emphasizes the acid's ability to release protons when dissolved in water.
Recommended video:
Guided course
02:23
Using factors affecting acidity to rank acids
Brønsted–Lowry Acid
According to the Brønsted–Lowry theory, an acid is a proton donor. Sulfuric acid donates a proton (H⁺) to water, forming hydronium ions (H₃O⁺) and bisulfate ions (HSO₄⁻). This interaction illustrates sulfuric acid's behavior as a Brønsted–Lowry acid, highlighting its role in proton transfer reactions.
Recommended video:
Guided course
00:54The Bronsted-Lowry definition of acids and bases.
Lewis Acid
A Lewis acid is defined as an electron pair acceptor. In the context of sulfuric acid, it can act as a Lewis acid by accepting an electron pair from a base during chemical reactions. This property allows sulfuric acid to participate in various reactions beyond simple proton donation, showcasing its versatility as a Lewis acid.
Recommended video:
Guided course
02:49The Lewis definition of acids and bases.
Related Practice
Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(a)
1128
views
Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(d)
1157
views
Textbook Question
Sodium amide (NaNH₂) dissociates to give a sodium cation (Na+) and amide ion (NH2–) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(b)
1047
views
Textbook Question
Sodium amide (NaNH2) dissociates to give a sodium cation (Na+) and amide ion (NH2-) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(c)
1327
views
Textbook Question
Sodium amide (NaNH2) dissociates to give a sodium cation (Na+) and amide ion (NH2-) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(a)
1763
views