Chapter 19, Problem 19.36P

Draw the products of each acid-base reaction, and using the $\text{p}{K}_{\text{a}}$ table in Appendix A, determine if equilibrium favors the reactants or products.

a. d.

b. e. ${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}{\text{CHCH}}_{\text{2}}\text{OH}+\text{NaH}\rightleftarrows$

c. f..

Interpretation Introduction

(a)

Interpretation: The products of the given acid-base reaction are to be drawn. Whether the equilibrium favors the reactants or the product is to be determined.

Concept introduction: An acidic substance in a reaction donates a proton, whereas base in a reaction accepts a proton. The $\text{pH}$ value determines whether the compound is acidic or basic. Water has a neutral $\text{pH}$. The number of dissociated hydrogen ions determine the acidic strength of the compound. The elimination of a proton leads to the formation of a conjugate base.

Answer to Problem 19.36P

The products of the given acid-base reaction are,

The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors formation of products.

Explanation of Solution

The products of the given acid-base reaction are shown below.

Figure 1

The ${\text{pK}}_{\text{a}}$ values of ${\left({\text{CH}}_{\text{3}}\right)}_{\text{3}}\text{COH}$ and ${\text{C}}_{\text{6}}{\text{H}}_{\text{5}}\text{COOH}$ in the above reaction are $18$ and $4.2$ respectively, which indicates that ${\text{pK}}_{\text{a}}$ value is more on the right side. Therefore, the equilibrium favors the formation of products.

Conclusion

The products of the given acid-base reaction are shown in Figure 1. The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors formation of products.

Interpretation Introduction

(b)

Interpretation: The products of the given acid-base reaction are to be drawn. The equilibrium favors the reactants or a product is to be determined.

Concept introduction: An acidic substance in a reaction donates a proton, whereas base in a reaction accepts a proton. The $\text{pH}$ value determines that whether the compound is acidic or basic. Water has neutral $\text{pH}$. The number of dissociated hydrogen ions determine the acidic strength of the compound. The elimination of a proton leads to the formation of a conjugate base.

Answer to Problem 19.36P

The products of the given acid-base reaction are,

The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the reactants.

Explanation of Solution

The products of the given acid-base reaction are shown below.

Figure 2

The ${\text{pK}}_{\text{a}}$ values of acid and conjugate acid in the above reaction are $18$ and $9.4$ respectively, which indicates that ${\text{pK}}_{\text{a}}$ value is more on the left side. Therefore, the equilibrium favors the formation of reactants.

Conclusion

The products of the given acid-base reaction are shown in Figure 2. The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the formation of reactants.

Interpretation Introduction

(c)

Interpretation: The products of the given acid-base reaction are to be drawn. Whether the equilibrium favors the reactants or the product is to be determined.

Concept introduction: An acidic substance in a reaction donates a proton, whereas base in a reaction accepts a proton. The $\text{pH}$ value determines whether the compound is acidic or basic. Water has a neutral $\text{pH}$. The number of dissociated hydrogen ions determine the acidic strength of the compound. The elimination of a proton leads to the formation of a conjugate base.

Answer to Problem 19.36P

The products of the given acid-base reaction are,

The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the products.

Explanation of Solution

The products of the given acid-base reaction are shown below.

Figure 3

The ${\text{pK}}_{\text{a}}$ values of acid and conjugate acid in the above reaction are $10$ and $38$ respectively, which indicates that ${\text{pK}}_{\text{a}}$ value is more on the right side. Therefore, the equilibrium favors the formation of products.

Conclusion

The products of the given acid-base reaction are shown in Figure 3. The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the products.

Interpretation Introduction

(d)

Interpretation: The products of the given acid-base reaction are to be drawn. Whether the equilibrium favors the reactants or the product is to be determined.

Concept introduction: An acidic substance in a reaction donates a proton, whereas base in a reaction accepts a proton. The $\text{pH}$ value determines whether the compound is acidic or basic. Water has a neutral $\text{pH}$. The number of dissociated hydrogen ions determine the acidic strength of the compound. The elimination of a proton leads to the formation of a conjugate base.

Answer to Problem 19.36P

The products of the given acid-base reaction are,

The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the products.

Explanation of Solution

The products of the given acid-base reaction are shown below.

Figure 3

The ${\text{pK}}_{\text{a}}$ values of acid and conjugate acid in the above reaction are $4.5$ and $50$ respectively, which indicates that ${\text{pK}}_{\text{a}}$ value is more on the right side. Therefore, the equilibrium favors the formation of products.

Conclusion

The products of the given acid-base reaction are shown in Figure 3. The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the products.

Interpretation Introduction

(e)

Interpretation: The products of the given acid-base reaction are to be drawn. Whether the equilibrium favors the reactants or the product is to be determined.

Concept introduction: An acidic substance in a reaction donates a proton, whereas base in a reaction accepts a proton. The $\text{pH}$ value determines whether the compound is acidic or basic. Water has a neutral $\text{pH}$. The number of dissociated hydrogen ions determine the acidic strength of the compound. The elimination of a proton leads to the formation of a conjugate base.

Answer to Problem 19.36P

The products of the given acid-base reaction are ${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}{\text{CHCH}}_{\text{2}}\stackrel{-}{\text{O}}\stackrel{+}{\text{Na}}$ and ${\text{H}}_{\text{2}}$.

The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the formation of products.

Explanation of Solution

The products of the given acid-base reaction are,

${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}{\text{CHCH}}_{\text{2}}\text{OH}+\text{NaH}\rightleftarrows {\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}{\text{CHCH}}_{\text{2}}\stackrel{-}{\text{O}}\stackrel{+}{\text{Na}}{\text{+H}}_{\text{2}}$

The ${\text{pK}}_{\text{a}}$ values of ${\text{H}}_{\text{2}}$ and ${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}{\text{CHCH}}_{\text{2}}\text{OH}$ in the above reaction are $35$ and $16$ respectively, which indicates that ${\text{pK}}_{\text{a}}$ value is more on the right side. Therefore, the equilibrium favors the formation of products.

Conclusion

The products of the given acid-base reaction are ${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}{\text{CHCH}}_{\text{2}}\stackrel{-}{\text{O}}\stackrel{+}{\text{Na}}$ and ${\text{H}}_{\text{2}}$. The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the products.

Interpretation Introduction

(f)

Interpretation: The products of the given acid-base reaction are to be drawn. Whether the equilibrium favors the reactants or the product is to be determined.

Concept introduction: An acidic substance in a reaction donates a proton, whereas base in a reaction accepts a proton. The $\text{pH}$ value determines whether the compound is acidic or basic. Water has a neutral $\text{pH}$. The number of dissociated hydrogen ions determine the acidic strength of the compound. The elimination of a proton leads to the formation of a conjugate base.

Answer to Problem 19.36P

The products of the given acid-base reaction are,

The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the reactants.

Explanation of Solution

The products of the given acid-base reaction are shown below.

Figure 4

The ${\text{pK}}_{\text{a}}$ values of acid and conjugate acid in the above reaction are $10.2$ and $6.4$ respectively, which indicates that ${\text{pK}}_{\text{a}}$ value is more on the left side. Therefore, the equilibrium favors the formation of reactants.

Conclusion

The products of the given acid-base reaction are shown in Figure 4. The ${\text{pK}}_{\text{a}}$ values imply that equilibrium favors the reactants.