Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous barium hydroxide

Verified step by step guidance

1. Identify the reactants: acetic acid (CH₃COOH) and barium hydroxide (Ba(OH)₂).
2. Write the unbalanced molecular equation: CH₃COOH(aq) + Ba(OH)₂(aq) → Ba(CH₃COO)₂(aq) + H₂O(l).
3. Balance the molecular equation by ensuring the number of atoms of each element is equal on both sides.
4. Write the complete ionic equation by dissociating all strong electrolytes into their ions.
5. Identify and cancel the spectator ions to write the net ionic equation, focusing on the ions that participate in the reaction.

Key Concepts

Neutralization Reactions

Neutralization reactions occur when an acid reacts with a base to produce water and a salt. In this process, the hydrogen ions (H+) from the acid combine with hydroxide ions (OH-) from the base to form water (H2O). Understanding the general form of these reactions is essential for writing balanced equations.

Balanced Molecular Equations

A balanced molecular equation represents the reactants and products of a chemical reaction with their respective coefficients, ensuring that the number of atoms for each element is the same on both sides. This is crucial for accurately depicting the stoichiometry of the reaction and is the first step in deriving the net ionic equation.

Net Ionic Equations

Net ionic equations show only the species that participate in the reaction, omitting spectator ions that do not change during the reaction. This simplification highlights the actual chemical change occurring, which is particularly important in reactions involving strong electrolytes, such as the neutralization of acetic acid by barium hydroxide.