Write balanced ionic equations for the following reactions. (b) Aqueous sodium hydroxide is neutralized by aqueous acetic acid.

검증된 단계별 안내

Identify the reactants: Sodium hydroxide (NaOH) and acetic acid (CH₃COOH).

Write the molecular equation for the reaction: NaOH(aq) + CH₃COOH(aq) → CH₃COONa(aq) + H₂O(l).

Dissociate the strong electrolytes into ions: NaOH(aq) → Na⁺(aq) + OH⁻(aq).

Recognize that acetic acid (CH₃COOH) is a weak acid and does not dissociate completely in solution.

Write the net ionic equation by removing the spectator ions: OH⁻(aq) + CH₃COOH(aq) → CH₃COO⁻(aq) + H₂O(l).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

도움이 되었나요?

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, acetic acid (a weak acid) reacts with sodium hydroxide (a strong base) to form water and sodium acetate. Understanding this concept is crucial for predicting the products of the reaction and writing the balanced equation.

Ionic Equations

Ionic equations represent the species involved in a chemical reaction in their ionic forms. In the case of the neutralization of acetic acid by sodium hydroxide, the complete ionic equation shows all soluble ionic compounds as ions. This helps in identifying the actual participants in the reaction, particularly the formation of water from hydrogen and hydroxide ions.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. For the reaction between sodium hydroxide and acetic acid, balancing involves ensuring that the total number of each type of ion is equal before and after the reaction, which is essential for accurately representing the chemical process.