The hydrated cation M1H2O26 3 + has Ka = 10-4, and the acid HA has Ka = 10-5. Identify the principal reaction in an aqueous solution of each of the following salts, and classify each solution as acidic, basic, or neutral. (a) NaA

Hydrated cations, such as M1H2O26 3+, can act as acids in solution by donating protons (H+) to water, leading to the formation of hydronium ions (H3O+). The strength of this acidic behavior is quantified by the acid dissociation constant (Ka), which indicates how readily the cation donates protons. A higher Ka value signifies a stronger acid, influencing the pH of the solution.

Acid-base equilibria describe the balance between acids and bases in a solution, governed by their respective Ka values. In this context, the acid HA with a Ka of 10-5 is weaker than the hydrated cation M1H2O26 3+ with a Ka of 10-4. This difference in strength determines the predominant species in solution and helps classify the resulting solution as acidic, basic, or neutral based on the concentration of H3O+ ions.

Salt hydrolysis occurs when a salt dissolves in water and its constituent ions interact with water molecules, potentially altering the pH of the solution. For example, the salt NaA dissociates into Na+ and A- ions. The A- ion, being the conjugate base of the weak acid HA, can accept protons from water, leading to an increase in hydroxide ions (OH-) and resulting in a basic solution.