Identify the Bronsted-Lowry acid and base in each of the...

Identify the Bronsted-Lowry acid and base in each of the following neutralization reactions: (a) $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{LiOH}(a q) \longrightarrow \mathrm{LiC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ (b) $2 \mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)$

Identify the Bronsted-Lowry acid and base in each of the following neutralization reactions:
(a) $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{LiOH}(a q) \longrightarrow \mathrm{LiC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$
(b) $2 \mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)$

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Key Concepts

Conjugate Acid-Base Pairs

When a Bronsted-Lowry acid donates a proton, it forms its conjugate base, and when a Bronsted-Lowry base accepts a proton, it forms its conjugate acid. Understanding these pairs is essential to track the changes in protonation states during acid-base reactions and to apply the acid-base equilibrium concepts effectively.

Neutralization Reaction

A neutralization reaction is a specific type of acid-base reaction in which an acid and a base react to form water and a salt. This reaction is characterized by the transfer of a proton from the acid to the base, resulting in the formation of a conjugate acid and a conjugate base that together comprise the salt.

Bronsted-Lowry Acid-Base Theory

This theory defines acids as substances that donate protons (H? ions) and bases as substances that accept protons. It provides a framework for understanding reactions as transfers of protons between molecules rather than just as reactions between acids and bases in a general sense.

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