Chapter 2, Problem 3P

(a)

Interpretation Introduction

Interpretation:

The product of the acid-base reaction of $C{H}_3\stackrel{+}{N}{H}_{3}with{H}_{2}O$ has to be drawn.

Concept introduction:

According to the explanations by Bronsted-Lowry, if a species loses a proton then it is an acid whereas if a species receives one proton, then it is base.

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

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

(b)

Interpretation Introduction

Interpretation:

The product of the acid-base reaction of $HBrwithC{H}_{3}OH$ has to be drawn.

Concept introduction:

According to the explanations by Bronsted-Lowry, if a species loses a proton then it is an acid whereas if a species receives one proton, then it is base.

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

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

(c)

Interpretation Introduction

Interpretation:

The product of the acid-base reaction of $C{H}_3\stackrel{+}{N}{H}_{3}withO{H}^{-}$ has to be drawn.

Concept introduction:

According to the explanations by Bronsted-Lowry, if a species loses a proton then it is an acid whereas if a species receives one proton, then it is base.

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

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

(d)

Interpretation Introduction

Interpretation:

The product of the acid-base reaction of $C{H}_{3}N{H}_{2}withC{H}_{3}OH$ has to be drawn.

Concept introduction:

According to the explanations by Bronsted-Lowry, if a species loses a proton then it is an acid whereas if a species receives one proton, then it is base.

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.

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