For each of the following reactions, indicate the...

For each of the following reactions, indicate the Brønsted-Lowry acids and bases. What are the conjugate acid/base pairs? $$ \begin{array}{l} \text { (a) } \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{H}_{2} \mathrm{O} \\ \text { (b) } \mathrm{HNO}_{2}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{NO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O} \\ \text { (c) } \mathrm{HCHO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{CHO}_{2}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \end{array} $$

For each of the following reactions, indicate the Brønsted-Lowry acids and bases. What are the conjugate acid/base pairs?
$$
\begin{array}{l}
\text { (a) } \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{H}_{2} \mathrm{O} \\
\text { (b) } \mathrm{HNO}_{2}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{NO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O} \\
\text { (c) } \mathrm{HCHO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{CHO}_{2}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)
\end{array}
$$

Key Concepts

Proton Transfer Reaction

Proton transfer reactions are processes in which a proton moves from one species to another, altering the protonation states of the involved molecules. These reactions are the basis of the Brønsted-Lowry acid-base theory and are key to understanding how acids and bases interact to form conjugate pairs and establish chemical equilibrium in solution.

Conjugate Acid-Base Pair

A conjugate acid-base pair consists of two species that differ by one proton. When an acid donates a proton, it becomes its conjugate base; conversely, a base that accepts a proton becomes its conjugate acid. This relationship is fundamental to understanding the reversibility of proton transfer reactions and the dynamic equilibrium present in acid-base systems.

Brønsted-Lowry Acid

The Brønsted-Lowry acid is defined as a species that donates a proton (H?) during a chemical reaction. This concept frames acid-base reactions in terms of proton transfer rather than electron pair donation, which distinguishes it from other acid-base theories. Understanding this idea is crucial because it allows the prediction of how species will interact in aqueous solutions and the formation of conjugate pairs.

Brønsted-Lowry Base

The Brønsted-Lowry base is a species that accepts a proton (H?) from an acid. In a reaction, bases gain a proton, and through this transfer, they are paired with their corresponding conjugate acids. Recognizing bases using the Brønsted-Lowry definition helps in analyzing and predicting the behavior of substances in various chemical reactions, especially in acid-base equilibria.

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