For each of the following reactions, identify the acid and the base. Also indicate which acid–base definition (Lewis, Brønsted–Lowry) applies. In some cases, more than one definition may apply. XeO3 + OH−→ [HXeO4]− Pt + XeF4 → PtF4 + Xe C2H5OH + H2SeO4 → C2H5OH2+ + HSeO4− [CH3Hg(H2O)]+ + SH− ⇌ [CH3HgS]− + H3O+ (benzyl)3 N + CH3COOH → (benzyl)3 NH+ + CH3COO− SO2 + HCl → OSO ··· HCl

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For each of the following reactions, identify the acid and the base. Also indicate which acid–base definition (Lewis, Brønsted–Lowry) applies. In some cases, more than one definition may apply.

XeO3 + OH−→ [HXeO4]−

Pt + XeF4 → PtF4 + Xe

C2H5OH + H2SeO4 → C2H5OH2+ + HSeO4−

[CH3Hg(H2O)]+ + SH− ⇌ [CH3HgS]− + H3O+

(benzyl)3 N + CH3COOH → (benzyl)3 NH+ + CH3COO−

SO2 + HCl → OSO ··· HCl

Expert Solution
Step 1: Lewis acid-base theory and Bronsted-Lowry theory

The Lewis acid-base theory, named after chemist Gilbert N. Lewis, defines an acid as an electron pair acceptor and a base as an electron pair donor. According to this theory, a Lewis acid is a chemical species that can accept a pair of electrons to form a covalent bond, while a Lewis base is a chemical species that can donate a pair of electrons to form a covalent bond. This definition of acid and base is more general than the Brønsted-Lowry theory, which defines an acid as a proton (H+) donor and a base as a proton acceptor.

According to the Brønsted-Lowry acid-base theory, the key factor in acid-base reactions is the transfer of a proton from an acid to a base. In other words, a Brønsted acid is a species that has a hydrogen ion (H+) that can be donated to a base, while a Brønsted base is a species that has a lone pair of electrons that can accept a proton.

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