Write the chemical equation and the K_a expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H⁺(a)q as a product and then with the hydronium ion: (a) C₆H₅COOH (b) HCO₃^-

Acid dissociation refers to the process by which an acid donates a proton (H+) to a water molecule, resulting in the formation of a hydronium ion (H3O+). This process is fundamental in understanding the behavior of acids in aqueous solutions, as it determines the strength of the acid and its ability to increase the concentration of H3O+ in the solution.

The acid dissociation constant (Ka) is a quantitative measure of the strength of an acid in solution. It is defined as the ratio of the concentration of the products (hydronium ion and the conjugate base) to the concentration of the undissociated acid at equilibrium. The Ka expression provides insight into how readily an acid donates protons, with larger values indicating stronger acids.

A chemical equation represents the reactants and products of a chemical reaction using their chemical formulas. In the context of acid dissociation, the equation illustrates how an acid, such as benzoic acid (C6H5COOH), dissociates in water to form hydronium ions and its conjugate base. Writing these equations correctly is essential for understanding the reaction dynamics and calculating related properties like pH.