Chapter 23, Problem 23.30P

(a)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

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.

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, acetate anion is the weaker acid and equilibrium lies towards the right.

(b)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

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.

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, triethylammonium cation is the weaker acid and equilibrium lies towards the right.

(c)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

  $\begin{array}{l}PhC\equiv CH{\text{ + NH}}_3\underset{}{\overset{}{\rightleftharpoons }}\\ \text{Phenylacetylene Ammonia}\end{array}$

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.

$\begin{array}{l}PhC\equiv CH{\text{ + NH}}_3\underset{}{\underset{\leftharpoondown }{\rightharpoonup }}PhC\equiv C^{-}{\text{ + NH}}_4^{+}\\ pKa\sim \text{25 }\text{pKa 9}\text{.26}\end{array}$

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, phenyl acetylene is the weaker acid and equilibrium lies towards the left.

(d)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

  $\begin{array}{l}PhC\equiv CH{\text{ + iPr}}_2{N}^{-}L{i}^{+}\underset{}{\overset{}{\rightleftharpoons }}\\ Phenylacetylene\text{ LDA}\end{array}$

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.

$\begin{array}{l}PhC\equiv CH{\text{ + iPr}}_2{N}^{-}L{i}^{+}\underset{}{\overset{}{\rightleftharpoons }}PhC\equiv C^{-}{\text{ + iPr}}_{2}NH\\ pKa\sim \text{25}\text{ pKa }\sim \text{40}\end{array}$

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, amine is the weaker acid and equilibrium lies towards the right.

(e)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

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.

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, triethylammonium chloride is the weaker acid and equilibrium lies towards the left.

(f)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

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.

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, 1-phenyl-2-propanammonium ion is the weaker acid and equilibrium lies towards the right.

(g)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

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.

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, amphetamine hydrochloride is the weaker acid and equilibrium lies towards the left.

(h)

Interpretation Introduction

Interpretation:

Given acid-base reaction has to be completed and the direction of equilibrium has to be predicted.

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

Explanation of Solution

Given reaction is shown below,

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.

Weak acid is more stable, equilibrium follows the direction of formation weak acids in a reaction. Long arrow indicates the direction where equilibrium favors.

Here, water is the weaker acid and equilibrium lies towards the right.