Chapter 2, Problem 71P

(a)

Interpretation Introduction

Interpretation:

The $p{K}_a$ value ranges of the following acids are to be determined without using a calculator. The exact $p{K}_a$ values of the following acids are to be determined by using a calculator. The stronger acid among the following is to be determined.

Concept introduction:

Mixture of acid and base undergoes equilibrium reaction and it’s ${\text{pk}}_{\text{a}}$-values determine their direction of reaction.

Weak acids are more stable and less reactive, so equilibrium follows the direction of formation weak acids in a reaction.

Lesser the ${\text{pk}}_{\text{a}}$- value of compound will be more acidic. So the equilibrium follows the direction of compounds having low ${\text{pk}}_{\text{a}}$-value to the products of high ${\text{pk}}_{\text{a}}$ value

Acid dissociation constant ${\text{K}}_{\text{a}}$ represents how strong the acid is in a solution. The strength of acid decreases as the value of $p{K}_a$ increases

$p{K}_a=-\log K_a$

$p{K}_a$ represents the chance of losing proton from a compound.

(b)

Interpretation Introduction

Interpretation: The $p{K}_a$ value ranges of the following acids are to be determined without using a calculator. The exact $p{K}_a$ values of the following acids are to be determined by using a calculator. The stronger acid among the following is to be determined.

Concept introduction:

Mixture of acid and base undergoes equilibrium reaction and it’s ${\text{pk}}_{\text{a}}$-values determine their direction of reaction.

Weak acids are more stable and less reactive, so equilibrium follows the direction of formation weak acids in a reaction.

Lesser the ${\text{pk}}_{\text{a}}$- value of compound will be more acidic. So the equilibrium follows the direction of compounds having low ${\text{pk}}_{\text{a}}$-value to the products of high ${\text{pk}}_{\text{a}}$ value

Acid dissociation constant ${\text{K}}_{\text{a}}$ represents how strong the acid is in a solution. The strength of acid decreases as the value of $p{K}_a$ increases

$p{K}_a=-\log K_a$

$p{K}_a$ represents the chance of losing proton from a compound.