Chapter 2, Problem 33P

(i)

Interpretation Introduction

Interpretation: The Bronsted acid or base present in the below reaction should be identified.

  

Concept introduction: In accordance with Bronsted definition an acid act as proton donor and a base can act as proton acceptor. Thus in a typical acid-base reaction, the fundamental principle is a lone pair of base reaches out for an acidic proton. Similarly, curved arrows are used for departing conjugate base. After deprotonation, the species left with negative charge is refers as conjugate base of acid while the other with positive charge is termed conjugate acid of given base. For example,

  

The strength of various conjugate acid-base pairs varies inversely to one another; the strong acid has a weak conjugate base and the strong base has weak conjugate acid and vice-versa.

(ii)

Interpretation Introduction

Interpretation: Whether the equilibrium is favored to left or right should be identified in below reactions.

  

Concept introduction: In accordance with Bronsted definition an acid act as proton donor and a base can act as proton acceptor. Thus in a typical acid-base reaction, the fundamental principle is a lone pair of base reaches out for an acidic proton. Similarly, curved arrows are used for departing conjugate base. After deprotonation, the species left with negative charge is refers as conjugate base of acid while the other with positive charge is termed conjugate acid of given base. For example,

  

The strength of various conjugate acid-base pairs varies inversely to one another; the strong acid has a weak conjugate base and the strong base has weak conjugate acid and vice-versa.

Smaller the magnitude of $\text{p}{K}_{\text{a}}$ of an acid, greater is the acidic strength and vice-versa. This is because the relation between $K_{\text{a}}$ from $\text{p}{K}_{\text{a}}$ is inversely related to each other. The acid will smaller $\text{p}{K}_{\text{a}}$ will have more dissociation and thus would act as a stronger acid.

(iii)

Interpretation Introduction

Interpretation: The value of $K_{\text{a}}$ for below equation should be estimated.

  

Concept introduction: In accordance with Bronsted definition an acid act as proton donor and a base can act as proton acceptor. Thus in a typical acid-base reaction, the fundamental principle is a lone pair of base reaches out for an acidic proton. Similarly, curved arrows are used for departing conjugate base. After deprotonation, the species left with negative charge is refers as conjugate base of acid while the other with positive charge is termed conjugate acid of given base. For example,

  

The strength of various conjugate acid-base pairs varies inversely to one another; the strong acid has a weak conjugate base and strong base has weak conjugate acid and vice-versa.

Smaller the magnitude of $\text{p}{K}_{\text{a}}$ of an acid, greater is the acidic strength and vice-versa. This is because the relation between $K_{\text{a}}$ from $\text{p}{K}_{\text{a}}$ is inversely related to each other. The acid will smaller $\text{p}{K}_{\text{a}}$ will have more dissociation and thus would act as a stronger acid.