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Chapter 15: Problem 13

In Reaction \(15.7\), water is shown acting as a base. How is water behaving in the following reaction? $$ \mathrm{NH}_{2}^{-}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NH}_{3}+\mathrm{OH}^{-} $$ Explain your answer.

Short Answer

Expert verified
In the reaction \(\mathrm{NH}_{2}^{-}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NH}_{3}+\mathrm{OH}^{-}\), water is behaving as an acid because it donates a hydrogen ion (H+) to the \(\mathrm{NH}_{2}^{-}\) ion, resulting in the formation of \(\mathrm{NH}_{3}\) and \(\mathrm{OH}^{-}\).

Step by step solution

01

Understand the role of acids and bases

Acids are substances that donate a hydrogen ion (H+), while bases are substances that accept a hydrogen ion. In a reaction, when a molecule accepts a hydrogen ion, it is functioning as a base; while if it donates a hydrogen ion, it is functioning as an acid.
02

Identify the reactants and products of the reaction

In the given reaction: $$ \mathrm{NH}_{2}^{-}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NH}_{3}+\mathrm{OH}^{-} $$ The reactants are \(\mathrm{NH}_{2}^-\) and \(\mathrm{H}_{2} \mathrm{O}\), while the products are \(\mathrm{NH}_{3}\) and \(\mathrm{OH}^{-}\).
03

Study the water molecule in the reaction

In the reaction: $$ \mathrm{NH}_{2}^{-}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NH}_{3}+\mathrm{OH}^{-} $$ Water is one of the reactants and participates by giving away one of its hydrogen ions (H+) to the \(\mathrm{NH}_{2}^-\) ion.
04

Determine how water is behaving in the reaction

When \(\mathrm{H}_{2}\mathrm{O}\) donates a hydrogen ion to \(\mathrm{NH}_{2}^{-}\) to form \(\mathrm{NH}_{3}\), it leaves behind an \(\mathrm{OH}^{-}\) ion. Since water is donating a hydrogen ion (H+) in the reaction, it is functioning as an acid.
05

Provide the explanation

In the given reaction, water is behaving as an acid because it donates a hydrogen ion (H+) to the \(\mathrm{NH}_{2}^{-}\) ion, resulting in the formation of \(\mathrm{NH}_{3}\) and \(\mathrm{OH}^{-}\).

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Most popular questions from this chapter

Solid ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl}\), reacts with solid sodium hydroxide to produce ammonia gas, water, and sodium chloride, \(\mathrm{NaCl}\). (a) Write a balanced equation for this reaction. (b) According to the Bronsted-Lowry definition, which species is the acid and which species is the base? Explain.

When ammonia gas is dissolved in water, is the water behaving as an acid, as a base, or neither? Explain.

An ionic compound with the formula \(\operatorname{NaX}(\mathrm{X}\) is an unknown anion) is dissolved in water, and the resulting solution is basic. Is HX a strong acid or a weak acid? Explain.

What is the pH of a \(0.010 \mathrm{M}\) aqueous solution of \(\mathrm{NaOH}\) ?

The equilibrium constant for the reaction \(\mathrm{NH}_{4}^{+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{NH}_{3}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)\) is \(5.6 \times 10^{-10}\) (a) Is a solution of ammonium ion very acidic or only slightly acidic? (b) Is water acting as an acid or a base according to the Bronsted-I owry definition? Explain.
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