Occurs when solid sodium acetate, NaC2H3O2(s), is added to water — Acids and Bases Chemistry Question

STEPS:

1. Identify the nature of the solute: Sodium acetate ($NaC_2H_3O_2$) is an ionic salt composed of sodium cations ($Na^+$) and acetate anions ($C_2H_3O_2^-$).
2. Determine the process of dissolution: When solid sodium acetate is added to water, it dissociates completely into its constituent ions: $Na^+(aq)$ and $C_2H_3O_2^-(aq)$.
3. Analyze ion reactivity (Hydrolysis): The $Na^+$ ion is the conjugate of a strong base ($NaOH$) and is therefore a spectator ion that does not react with water. The acetate ion ($C_2H_3O_2^-$), however, is the conjugate base of a weak acid (acetic acid).
4. Apply the Brønsted^-Lowry definition: A Brønsted^-Lowry reaction is defined by the transfer of a proton ($H^+$). Because the acetate ion is a conjugate base, it will react with water molecules by accepting a proton.
5. Write the chemical equation: The resulting hydrolysis reaction is:
$$C_2H_3O_2^-(aq) + H_2O(l) \rightleftharpoons HC_2H_3O_2(aq) + OH^-(aq)$$
Since this process fundamentally involves a proton transfer from water (acting as the acid) to the acetate ion (acting as the base), it is classified as a Brønsted^-Lowry acid-base reaction.

WHY_OTHERS_WRONG:

• Oxidation-reduction reaction (A): There is no change in oxidation states for any of the atoms involved. The process is a redistribution of protons, not a transfer of electrons.
• Sublimation (C): Sublimation is a physical phase change where a solid turns directly into a gas (such as $CO_2(s) \rightarrow CO_2(g)$); it does not describe a salt dissolving in and reacting with a solvent.
• Dehydration (D): Dehydration involves the removal of water from a compound (often by heating a hydrate). Adding a solid to water is the opposite of this process.
• Precipitation (E): Precipitation occurs when ions in solution combine to form an insoluble solid. Sodium acetate is highly soluble in water, so it dissolves rather than forming a precipitate.