Consider the following reaction equation H3O+(aq) + OH(aq) $\rightarrow$ 2H2O(1) The reaction represents

Step 1: Analyze the question We are given H₃O⁺(aq) + OH⁻(aq) → 2H₂O(l) and asked what type of reaction it is.

Step 2: Key concept

• H₃O⁺ (hydroxonium ion) is the form in which an acid's H⁺ exists in water.
• OH⁻ (hydroxide ion) comes from a base (alkali).
• When an acid and a base react to form water (and usually a salt), the reaction is neutralization.

Step 3: Check each option

• A. Esterification: this is a reaction between an alcohol and a carboxylic acid that produces an ester and water. No alcohol or organic acid is present here, so it is not esterification.
• B. Hydrolysis: this is the breakdown of a compound by water, for example an ester or a salt reacting with water. Here water is the product, not a reactant that breaks something down, so it is not hydrolysis.
• C. Neutralization: the acid species (H₃O⁺) reacts with the base species (OH⁻) to form water only. This is the net ionic equation of neutralization (H⁺ + OH⁻ → H₂O).
• D. Redox: no oxidation numbers change (H stays +1, O stays -2), so electrons are not transferred. It is not redox.

Step 4: Answer The reaction represents neutralization, which is option C.

Exam tip: Whenever you see H⁺ or H₃O⁺ reacting with OH⁻ to give water, think "neutralization." For redox, always check whether oxidation numbers change. For hydrolysis, water must be a reactant that splits something apart.