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) $\cdot \mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$ (b) $\mathrm{Zn}(\mathrm{OH})_{3}^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Zn}(\mathrm{OH})_{4}^{2-}(\mathrm{aq})$

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted-Lowry, and Lewis.
(a) $\cdot \mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$
(b) $\mathrm{Zn}(\mathrm{OH})_{3}^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Zn}(\mathrm{OH})_{4}^{2-}(\mathrm{aq})$

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Key Concepts

Lewis Acid?Base Theory

This theory defines acids as electron pair acceptors and bases as electron pair donors. It further generalizes the concept of acid-base reactions by focusing on the transfer of electron pairs rather than protons, which is particularly useful in understanding reactions that do not involve protons at all.

Arrhenius Acid?Base Theory

This theory defines acids as substances that increase the concentration of hydrogen ions (H+) in aqueous solution and bases as substances that increase the concentration of hydroxide ions (OH?) in aqueous solution. It is one of the earliest acid-base theories and is most applicable to reactions that occur in water.

Brønsted?Lowry Acid?Base Theory

In this theory, acids are considered proton donors while bases are proton acceptors. It expands the concept of acid-base reactions beyond aqueous solutions to include any reaction where a proton transfer occurs, allowing for a broader range of chemical reactions to be classified as acid-base reactions.

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