Identify the reactant that is a Bronsted-Lowry acid and the...

Identify the reactant that is a Bronsted-Lowry acid and the reactant that is a Bronsted-Lowry base in each of the following: a. $\mathrm{HI}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{I}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)$ b. $\mathrm{F}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{HF}(a q)+\mathrm{OH}^{-}(a q)$

Identify the reactant that is a Bronsted-Lowry acid and the reactant that is a Bronsted-Lowry base in each of the following:
a. $\mathrm{HI}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{I}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)$
b. $\mathrm{F}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{HF}(a q)+\mathrm{OH}^{-}(a q)$

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Key Concepts

Bronsted-Lowry Acid

A Bronsted-Lowry acid is defined as a substance that donates a proton (H? ion) to another substance during a chemical reaction. This concept is broader than classical definitions of acids because it allows the identification of acids based on their proton-donating ability rather than their composition or traditional properties.

Bronsted-Lowry Base

A Bronsted-Lowry base is characterized as a substance that accepts a proton (H? ion) during a chemical reaction. This definition expands the idea of bases to include any species that can accept a proton, rather than those traditionally recognized based on their basic properties.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs are formed when a Bronsted-Lowry acid donates a proton to a Bronsted-Lowry base, resulting in a pair of species that differ by just one proton. The acid, after donating a proton, becomes its conjugate base, while the base, after accepting the proton, becomes its conjugate acid. This concept is central to understanding equilibrium and reaction mechanisms in acid-base chemistry.

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