Write the formulas of the products expected to form in the...

Write the formulas of the products expected to form in the following situations. If no reaction occurs, write N.R. (a) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow$ (b) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}(\mathrm{aq})+\mathrm{HBr}(\mathrm{aq}) \longrightarrow$ (c) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \longrightarrow$ (d) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \longrightarrow$

Write the formulas of the products expected to form in the following situations. If no reaction occurs, write N.R.
(a) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow$
(b) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}(\mathrm{aq})+\mathrm{HBr}(\mathrm{aq}) \longrightarrow$
(c) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \longrightarrow$
(d) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \longrightarrow$

Key Concepts

Neutralization Reactions

Neutralization reactions involve an acid reacting with a base to produce a salt and, typically, water. In aqueous systems, the reaction between an ammonium ion and a base, such as hydroxide, can lead to deprotonation of the ammonium ion, regenerating the original amine and forming water. Understanding this process is key to predicting the outcome of reactions where protonated amines interact with bases.

Proton Transfer Equilibria

Proton transfer equilibria describe the reversible exchange of protons between acids and bases. The position of this equilibrium is determined by the relative strengths of the acids and bases involved. In reactions featuring amines and their conjugate acids, subtle shifts in equilibrium dictate whether protonation or deprotonation is favored, which is essential for predicting the products of mixtures involving species like hydronium ions or hydroxide ions.

Acid–Base Reactions

Acid–base reactions are fundamental processes involving the transfer of protons between species. In these reactions, a base (such as an amine with a lone pair on nitrogen) accepts a proton from an acid (like HCl or HBr), resulting in the formation of its conjugate acid. This concept explains why amines form ammonium salts when mixed with strong acids, as the proton is transferred to the nitrogen center.

Amines and Their Conjugate Acids

Amines act as bases due to the presence of a lone electron pair on the nitrogen atom. When protonated by an acid, they convert into ammonium ions. The nature of the amine—whether it is primary, secondary, or tertiary—can affect the reaction, as steric hindrance may influence the ease of protonation. This concept underpins the formation of ammonium salts in acid–base reactions involving amines.

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