Chapter 16, Problem 33E

Interpretation Introduction

(a)

Interpretation:

The direction of the equilibrium on increasing concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$ is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

On increasing the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$, equilibrium shifts to the right.

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On increasing the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$, the equilibrium shifts to the right. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on increasing the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$, the equilibrium shifts to the right to decrease the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$.

Conclusion

The effect of increasing concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$ has been stated above.

Interpretation Introduction

(b)

Interpretation:

The effect of increasing concentration of hydrogen ion is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

The equilibrium shifts to the left on increasing concentration of hydrogen ion.

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On increasing the concentration of ${\text{H}}^{+}$, the equilibrium shifts to the left. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on increasing the concentration of ${\text{H}}^{+}$, the equilibrium shifts to the left to decrease the concentration of ${\text{H}}^{+}$.

Conclusion

The effect of increasing concentration of ${\text{H}}^{+}$ has been stated above.

Interpretation Introduction

(c)

Interpretation:

The direction of the equilibrium on decreasing concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$ is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

On decreasing the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$, equilibrium shifts to the left.

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On decreasing the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$, the equilibrium shifts to the left. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on decreasing the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$, the equilibrium shifts to the left to increase the concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$.

Conclusion

The effect of decreasing concentration of ${\text{HC}}_2{\text{H}}_3{\text{O}}_2$ has been stated above.

Interpretation Introduction

(d)

Interpretation:

The direction of the equilibrium on increasing concentration of ${\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}$ is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

On increasing the concentration of ${\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}$, equilibrium shifts to the left

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On increasing the concentration of ${\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}$, the equilibrium shifts to the left. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on increasing the concentration of ${\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}$, the equilibrium shifts to the left to decrease the concentration of ${\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}$.

Conclusion

The effect of increasing concentration of ${\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}$ has been stated above.

Interpretation Introduction

(e)

Interpretation:

The direction of the equilibrium on adding solid ${\text{NaC}}_2{\text{H}}_3{\text{O}}_2$ is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

On adding solid ${\text{NaC}}_2{\text{H}}_3{\text{O}}_2$ equilibrium shifts to the left.

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On adding solid ${\text{NaC}}_2{\text{H}}_3{\text{O}}_2$, the concentration of acetate ion increases in the reaction mixture. Therefore, according to Le Chatelier’s principle, the equilibrium shifts to the left to decrease the concentration of ${\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}$.

Conclusion

The effect of adding solid ${\text{NaC}}_2{\text{H}}_3{\text{O}}_2$ has been stated above.

Interpretation Introduction

(f)

Interpretation:

The direction of the equilibrium on adding gaseous $\text{NaCl}$ is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

There is no effect on equilibrium on adding solid $\text{NaCl}$.

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On adding solid $\text{KCl}$, there is no effect on the equilibrium as the ions produced by $\text{NaCl}$ will not alter the contents of reaction mixture.

Conclusion

The effect of adding solid $\text{NaCl}$ has been stated above.

Interpretation Introduction

(g)

Interpretation:

The direction of the equilibrium on adding solid $\text{NaOH}$ is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

On adding solid $\text{NaOH}$ equilibrium shifts to the right.

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On adding solid $\text{NaOH}$, hydroxide ions are produced which will neutralize the hydrogen ion concentration. Due to the neutralization reaction, the concentration of hydrogen ion will decrease and equilibrium will shift towards right to produce more hydrogen ion concentration.

Conclusion

The effect of adding solid $\text{NaOH}$ has been stated above.

Interpretation Introduction

(h)

Interpretation:

The direction of the equilibrium on increasing $\text{pH}$ is to be stated.

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s Principle, it states that the equilibrium shifts in such a way or a direction that it can reduce the effect of change.

Answer to Problem 33E

On increasing $\text{pH}$ equilibrium shifts to the right.

Explanation of Solution

The given reaction is shown below.

${\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2^{-}\left(aq\right)$

On increasing $\text{pH}$, the concentration of hydrogen ions decreases and therefore the equilibrium shifts to the right to increase the hydrogen ion concentration.

Conclusion

The effect of increasing $\text{pH}$ has been stated above.