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Chapter 16: Problem 109

The reaction of \(\mathrm{CH}_{3} \mathrm{COOH}(\) aq) proceeds furthest toward completion with a base when that base is (a) \(\mathrm{H}_{2} \mathrm{O} ;\) (b) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+} ;\) (c) \(\mathrm{NH}_{4}^{+} ;\) (d) \(\mathrm{Cl}^{-} ;\) (e) \(\mathrm{CO}_{3}^{2-}\).

Short Answer

Expert verified
The base that will make the reaction of \(\mathrm{CH}_{3} \mathrm{COOH}\) proceed furthest toward completion is \(\mathrm{CO}_{3}^{2-}\).

Step by step solution

01

Analyze the Bases

We have five substances that can act as bases. Water (\(\mathrm{H}_{2} \mathrm{O}\)) is a weak base, \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) and \(\mathrm{NH}_{4}^{+}\) are weak because of their positively charged ammonium group. Chloride ions (\(\mathrm{Cl}^{-}\)) can act as bases but are extremely weak due to their complete electronic shell. The carbonate ion (\(\mathrm{CO}_{3}^{2-}\)) is a moderate-strong base due its extra lone pairs.
02

Reaction capabilities

Now that we have analyzed the bases, we understand that moderate to strong bases can make the reaction proceed further. \(\mathrm{NH}_{4}^{+}\), \(\mathrm{Cl}^{-}\) and \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) cannot accept protons effectively due to their positive charge or complete electronic shell, so they will be less efficient in reacting with the acid.
03

Determine the most effective base

Given that \(\mathrm{CO}_{3}^{2-}\) is the only moderate-strong base (and thus more capable of reacting with the acid than the others) in this list, we can say that it will react most effectively, making the reaction proceed furthest.

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Most popular questions from this chapter

Explain why trichloroacetic acid, \(\mathrm{CCl}_{3} \mathrm{COOH},\) is a stronger acid than acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}\).

Show that when \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) is reduced to half its original value, the \(\mathrm{pH}\) of a solution increases by 0.30 unit, regardless ofthe initial \(p H .\) Is it also true that when any solution is diluted to half its original concentration, the pH increases by 0.30 unit? Explain.

\(\mathrm{CO}_{2}(\mathrm{g})\) can be removed from confined quarters (such as a spacecraft) by allowing it to react with an alkali metal hydroxide. Show that this is a Lewis acid-base reaction. For example, $$\mathrm{CO}_{2}(\mathrm{g})+\mathrm{LiOH}(\mathrm{s}) \longrightarrow \mathrm{LiHCO}_{3}(\mathrm{s})$$

A 625 mL sample of an aqueous solution containing 0.275 mol propionic acid, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H},\) has \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=0.00239 \mathrm{M} .\) What is the value of \(K_{\mathrm{a}}\) for propionic acid? $$\begin{aligned} &\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}\\\ &&K_{\mathrm{a}}=? \end{aligned}$$

Phosphorous acid is listed in Appendix D as a diprotic acid. Propose a Lewis structure for phosphorous acid that is consistent with this fact.
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