The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The p K a value of the conjugate acid is to be calculated. Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it. The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure. To determine: The possible structures of the conjugate acids of acetic acid, p K a value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Question

Want to see the full answer?

Answer 1

Question

Chapter 2.12, Problem 2.20P

Interpretation Introduction

Interpretation: The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The pKa value of the conjugate acid is to be calculated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it.

The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure.

To determine: The possible structures of the conjugate acids of acetic acid, pKa value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Indicate the formula of the product obtained by reacting methyl 5-chloro-5-oxopentanoate with 1 mole of 4-penten-1-ylmagnesium bromide.

In the two chair conformations of glucose, the most stable is the one with all the OH groups in the equatorial position. Is this correct?

Indicate the formula of the product obtained by reacting D-Galactose with hydroxylamine.

Answer 2

Question

Chapter 2.12, Problem 2.20P

Interpretation Introduction

Interpretation: The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The pKa value of the conjugate acid is to be calculated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it.

The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure.

To determine: The possible structures of the conjugate acids of acetic acid, pKa value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 2.12, Problem 2.20P

Interpretation Introduction

Interpretation: The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The pKa value of the conjugate acid is to be calculated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it.

The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure.

To determine: The possible structures of the conjugate acids of acetic acid, pKa value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 2.12, Problem 2.20P

Interpretation Introduction

Interpretation: The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The pKa value of the conjugate acid is to be calculated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it.

The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure.

To determine: The possible structures of the conjugate acids of acetic acid, pKa value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 2.12, Problem 2.20P

Interpretation Introduction

Interpretation: The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The pKa value of the conjugate acid is to be calculated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it.

The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure.

To determine: The possible structures of the conjugate acids of acetic acid, pKa value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Answer 6

Chapter 2.12, Problem 2.20P

Interpretation Introduction

Interpretation: The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The pKa value of the conjugate acid is to be calculated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it.

The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure.

To determine: The possible structures of the conjugate acids of acetic acid, pKa value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Answer 7

Chapter 2.12, Problem 2.20P

Interpretation Introduction

Interpretation: The possible structures of the conjugate acids of acetic acid are to be drawn. An explanation corresponding to the fact that in acetic acid the correct conjugate acid more stable is to be explained. The pKa value of the conjugate acid is to be calculated.

Concept introduction: According to Bronsted-Lowry theory, when an acid donates a proton the species formed is known as conjugate base and when the base accepts a proton the species formed is known as conjugate acid. The conjugate base has negative charge or lone pair of electrons present over it.

The acidity and basicity of a compound is influenced by the resonance. The amount of stability depends on the delocalization of the charge through the resonance. The delocalization of electrons due to presence of lone pair and double bond is called resonating structure.

To determine: The possible structures of the conjugate acids of acetic acid, pKa value of the conjugate acid and an explanation corresponding to the fact in acetic acid the correct conjugate acid more stable.

Answer 8

Expert Solution & Answer

Answer 9

Expert Solution & Answer

Answer 10

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 11

Ch. 2.1A - Prob. 2.1P Ch. 2.1B - The NF bond is more polar than the NH bond: but...Ch. 2.1B - For each of the following compounds 1. Draw the...Ch. 2.1B - Two isomers of 1,2-dichloroethene are known One...Ch. 2.2C - Prob. 2.5P Ch. 2.2C - Prob. 2.6P Ch. 2.3 - Prob. 2.7P Ch. 2.4 - Calculate the pH of the following solutions a....Ch. 2.6A - Ammonia appears in Table 2-2 as both an acid and a...Ch. 2.7 - Write equations for the following acid-base...

Solution Summary: The author explains the possible structures of the conjugate acids of acetic acid.

Want to see the full answer?

Chapter 2 Solutions