State whether each of the following reactions is an acidbase...

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted-Lowry, and Lewis. (a) $\mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})$ (b) $\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NaOH}(\mathrm{s}) \rightarrow \mathrm{NaHSO}_{3}(\mathrm{~s})$

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted-Lowry, and Lewis.
(a) $\mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})$
(b) $\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NaOH}(\mathrm{s}) \rightarrow \mathrm{NaHSO}_{3}(\mathrm{~s})$

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Key Concepts

Arrhenius Acid-Base Theory

This theory defines acids as substances that increase the concentration of H+ ions (or hydronium ions) in aqueous solutions, and bases as substances that increase the concentration of OH- ions. It is mainly applicable to reactions taking place in water and provides a simple framework to identify acid-base reactions by the formation or consumption of these ions.

Brønsted-Lowry Acid-Base Theory

According to this theory, acids are proton donors and bases are proton acceptors. This concept broadens the scope of acid-base reactions beyond those strictly involving water, allowing the classification of a wider variety of chemical reactions based on the transfer of protons between reactants.

Lewis Acid-Base Theory

This theory defines acids as species that can accept an electron pair, while bases are species that can donate an electron pair. This perspective generalizes the acid-base concept even further, including reactions that do not involve proton transfer, and is particularly useful in explaining reactions involving complex formation and other electron pair interactions.

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