Write an equation to describe the proton transfer that...

Write an equation to describe the proton transfer that occurs when each of these acids is added to water.
(a) $\mathrm{HCO}_{3}^{-}$
(b) $\mathrm{HCl}$
(c) $\mathrm{CH}_{3} \mathrm{COOH}$
(d) $\mathrm{HCN}$

Key Concepts

Conjugate Acid-Base Pairs

In every acid-base reaction, the acid and its conjugate base form a conjugate pair, as do the base and its conjugate acid. These pairs are interrelated; when an acid donates a proton, its conjugate base is formed, and when a base accepts a proton, its conjugate acid is produced. This concept is crucial for understanding reaction reversibility and the equilibrium established in acid-base reactions.

Proton Transfer

Proton transfer is the movement of a proton (H+) from one species to another, which is a core aspect of acid-base reactions. It is the mechanism by which acids donate protons to water, forming hydronium ions, while bases accept these protons to form their conjugate acids, establishing the dynamic equilibrium in aqueous systems.

Bronsted-Lowry Acid-Base Theory

This theory defines acids as proton donors and bases as proton acceptors. In water, an acid donates a proton to the water molecule, forming hydronium ions and its conjugate base. It provides the fundamental explanation for proton transfer reactions in aqueous solutions.

Acid Dissociation Reaction

An acid dissociation reaction describes the process in which an acid donates a proton to water, resulting in the formation of hydronium ions (H3O+) and the corresponding conjugate base. This type of reaction is essential for understanding how acids behave in water, governing factors like acid strength and ionization equilibria.

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