Write balanced complete ionic and net ionic equations for each acid–base reaction.
b. HCHO₂(aq) + NaOH(aq) →
c. HC₂H₃O₂(aq) + LiOH(aq) →

Verified step by step guidance

1. Identify the reactants and products in the given acid-base reaction: HCHO_2 (formic acid) and NaOH (sodium hydroxide).
2. Write the balanced molecular equation for the reaction: HCHO_2(aq) + NaOH(aq) \(\rightarrow\) NaCHO_2(aq) + H_2O(l).
3. Break down all the strong electrolytes into their ions to write the complete ionic equation: HCHO_2(aq) + Na^+(aq) + OH^-(aq) \(\rightarrow\) Na^+(aq) + CHO_2^-(aq) + H_2O(l).
4. Identify the spectator ions, which are ions that appear on both sides of the complete ionic equation and do not participate in the reaction. In this case, Na^+ is the spectator ion.
5. Write the net ionic equation by removing the spectator ions: HCHO_2(aq) + OH^-(aq) \(\rightarrow\) CHO_2^-(aq) + H_2O(l).

Key Concepts

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, HCHO2 (formic acid) acts as an acid, donating a proton, while NaOH (sodium hydroxide) serves as a base, accepting the proton. Understanding the roles of acids and bases is crucial for writing balanced equations.

Complete Ionic Equations

A complete ionic equation represents all the ions present in a solution during a reaction. It shows the reactants and products in their ionic forms, highlighting the dissociation of soluble ionic compounds. This step is essential for identifying the species involved in the reaction before simplifying to the net ionic equation.

Net Ionic Equations

A net ionic equation focuses on the species that actually participate in the reaction, omitting spectator ions that do not change during the reaction. By removing these non-reactive ions, the net ionic equation provides a clearer picture of the chemical change occurring, which is particularly useful in acid-base reactions.