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Chapter 8: Problem 60

Ammonium ions \(\left(\mathrm{NH}_{4}^{+}\right)\) behave as an acid. (a) Write an equation that shows \(\mathrm{NH}_{4}{ }^{+}(a q)\) behaving as an acid when it reacts with aqueous hydroxide ion. (b) What are the products of neutralizing an aqueous solution of \(\mathrm{NH}_{4} \mathrm{Cl}\) with \(\mathrm{NaOH}\) ?

Short Answer

Expert verified
(a) \(\mathrm{NH}_{4}^{+}(aq) + \mathrm{OH}^{-}(aq) \rightarrow \mathrm{NH}_{3}(aq) + \mathrm{H}_{2}\mathrm{O}(l)\) (b) \(\mathrm{NH}_{4}\mathrm{Cl}(aq) + \mathrm{NaOH}(aq) \rightarrow \mathrm{NH}_{3}(aq) + \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{NaCl}(aq)\)

Step by step solution

01

Write the chemical reaction for the ammonium ion and hydroxide ion.

When an ammonium ion \(\left(\mathrm{NH}_{4}^{+}\right)\) reacts with a hydroxide ion \(\left(\mathrm{OH}^{-}\right)\), it donates a proton (H\(^{+}\)) to the hydroxide ion, forming water (H\(_2\)O) and ammonia (NH\(_3\)). The balanced chemical equation is: \[\mathrm{NH}_{4}^{+}(aq) + \mathrm{OH}^{-}(aq) \rightarrow \mathrm{NH}_{3}(aq) + \mathrm{H}_{2}\mathrm{O}(l)\] (b) Neutralization reaction of \(\mathrm{NH}_{4} \mathrm{Cl}\) with \(\mathrm{NaOH}\)
02

Write the ionic dissociation of \(\mathrm{NH}_{4}\mathrm{Cl}\) and \(\mathrm{NaOH}\) in water.

The ionic dissociation of ammonium chloride (NH\(_4\)Cl) and sodium hydroxide (NaOH) in water can be written as: \[ \mathrm{NH}_{4}\mathrm{Cl}(aq) \rightarrow \mathrm{NH}_{4}^{+}(aq) + \mathrm{Cl}^{-}(aq) \] \[ \mathrm{NaOH}(aq) \rightarrow \mathrm{Na}^{+}(aq) + \mathrm{OH}^{-}(aq) \]
03

Identify which neutralization reaction is going on.

In the neutralization reaction, the ammonium ion \(\left(\mathrm{NH}_{4}^{+}\right)\) reacts with hydroxide ion \(\left(\mathrm{OH}^{-}\right)\) as shown in the equation in part (a). At the same time, sodium ions \(\left(\mathrm{Na}^{+}\right)\) and chloride ions \(\left(\mathrm{Cl}^{-}\right)\) remain in the solution.
04

Write the balanced equation for the neutralization reaction.

When ammonium chloride is neutralized with sodium hydroxide, the resulting products are ammonia, water, sodium ions, and chloride ions. The balanced chemical equation is: \[\mathrm{NH}_{4}^{+}(aq) + \mathrm{OH}^{-}(aq) + \mathrm{Na}^{+}(aq) + \mathrm{Cl}^{-}(aq) \rightarrow \mathrm{NH}_{3}(aq) + \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Na}^{+}(aq) + \mathrm{Cl}^{-}(aq)\] Since sodium and chloride ions are unchanged during the reaction, we can rewrite the equation as: \[ \mathrm{NH}_{4}\mathrm{Cl}(aq) + \mathrm{NaOH}(aq) \rightarrow \mathrm{NH}_{3}(aq) + \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{NaCl}(aq) \]
05

Identify the products of the neutralization.

The products of neutralizing an aqueous solution of \(\mathrm{NH}_{4}\mathrm{Cl}\) with \(\mathrm{NaOH}\) are ammonia (NH\(_3\)), water (H\(_2\)O), and sodium chloride (NaCl).

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Most popular questions from this chapter

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