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) $\mathrm{LiH}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{LiOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$ (b) $\mathrm{HSO}_{4}^{-}(\mathrm{aq})+\mathrm{F}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{HF}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}$

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted-Lowry, and Lewis.
(a) $\mathrm{LiH}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{LiOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
(b) $\mathrm{HSO}_{4}^{-}(\mathrm{aq})+\mathrm{F}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{HF}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}$

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Key Concepts

Arrhenius Acid-Base Concept

The Arrhenius concept defines acids as substances that increase the concentration of hydrogen ions (H+) in aqueous solution, while bases increase the concentration of hydroxide ions (OH–). This definition is useful for classifying reactions in water, where the formation or consumption of H+ or OH– ions indicates acid-base behavior.

Brønsted-Lowry Acid-Base Concept

The Brønsted-Lowry theory expands the definition of acids and bases by defining acids as proton donors and bases as proton acceptors. This definition is more general than Arrhenius', as it applies to reactions in both aqueous and non-aqueous environments and focuses on the transfer of protons between species.

Lewis Acid-Base Concept

The Lewis acid-base theory characterizes acids as electron pair acceptors and bases as electron pair donors. This concept broadens the scope of acid-base reactions beyond proton transfer, including reactions where the interaction involves the formation of a coordinate covalent bond through electron pair sharing.

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