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Chapter 8: Problem 141

Ammonia, \(\mathrm{NH}_{3}\), is a gas, but it is very soluble in water, so when you bubble ammonia gas into water you produce an aqueous solution of ammonia. Interestingly, this solution is basic (hydroxide ions are formed). Postulate a reaction that occurs between ammonia and water to make the solution basic, and classify the reaction type.

Short Answer

Expert verified
The balanced chemical equation for the reaction between ammonia (NH3) and water (H2O) is: \[NH_{3(g)} + H_{2}O_{(l)} \rightleftharpoons NH_{4^{+}}_{(aq)} + OH^{-}_{(aq)}\] This reaction is classified as a Brønsted-Lowry acid-base reaction, with ammonia acting as a base gaining a proton (H+) and water acting as an acid donating a proton (H+) to form hydroxide ions (OH-) and ammonium ions (NH4+).

Step by step solution

01

Identify the reactants

The given reactants are ammonia (NH3) and water (H2O).
02

Determine the possible products

Ammonia is a weak base, and water can act as both an acid and a base. When ammonia and water react, they form hydroxide ions (OH-) and ammonium ions (NH4+).
03

Write the balanced chemical equation

By combining the reactants and products, we have the balanced chemical equation for the reaction: \[NH_{3(g)} + H_{2}O_{(l)} \rightleftharpoons NH_{4^{+}}_{(aq)} + OH^{-}_{(aq)}\]
04

Classify the reaction type

The reaction between ammonia and water is classified as a Brønsted-Lowry acid-base reaction. Specifically, ammonia works as a Brønsted-Lowry base that can gain a proton (H+), and water acts as a Brønsted-Lowry acid which donates a proton (H+) to form hydroxide ions (OH-) and ammonium ions (NH4+).

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Most popular questions from this chapter

Aqueous solutions of calcium chloride and potassium carbonate are combined. Does a precipitate form? If yes, write a net ionic equation for the precipitation reaction.

Which equations represent chemical reactions: (a) \(\mathrm{CO}_{2}(\mathrm{~s}) \rightarrow \mathrm{CO}_{2}(g)\) (b) \(3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{O}_{3}(g)\) (c) \(\mathrm{NaCl}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{NaOH}(a q)+\mathrm{HCl}(a q)\) (d) \(\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CH}_{4}(g) \rightarrow \mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)

Draw dot diagrams for the reactants and products in each equation, and indicate which bonds are broken and which bonds are formed: (a) \(\mathrm{CH}_{4}+\mathrm{I}_{2} \rightarrow \mathrm{CH}_{3} \mathrm{I}+\mathrm{HI}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{F}_{2} \rightarrow \mathrm{FCH}_{2} \mathrm{CH}_{2} \mathrm{~F}\)

Translate this balanced chemical equation into words: \(\mathrm{CH}_{4}+2 \mathrm{O}_{2} \rightarrow \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) Methane

Which anions form compounds that are generally soluble in water: \(\mathrm{CO}_{3}^{2-}, \mathrm{NO}_{3}^{-}, \mathrm{Br}^{-}, \mathrm{SO}_{4}^{2-}, \mathrm{OH}^{-}, \mathrm{PO}_{4}^{3-} ?\)
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