(a) Write the net ionic equation for the reaction that occurs when a solution of hydrochloric acid (HCl) is mixed with a solution of sodium formate 1NaCHO22.

Verified step by step guidance

1. Identify the reactants: Hydrochloric acid (HCl) and sodium formate (NaCHO_2).
2. Write the balanced molecular equation: HCl(aq) + NaCHO_2(aq) \rightarrow NaCl(aq) + HCHO_2(aq).
3. Dissociate all strong electrolytes into their ions: H^+(aq) + Cl^-(aq) + Na^+(aq) + CHO_2^-(aq) \rightarrow Na^+(aq) + Cl^-(aq) + HCHO_2(aq).
4. Identify the spectator ions: Na^+(aq) and Cl^-(aq) are present on both sides of the equation.
5. Write the net ionic equation by removing the spectator ions: H^+(aq) + CHO_2^-(aq) \rightarrow HCHO_2(aq).

Key Concepts

Net Ionic Equations

A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions that do not participate in the reaction. It focuses on the actual chemical change occurring, providing a clearer picture of the reaction's essence. To write a net ionic equation, one must first write the balanced molecular equation, then dissociate the soluble strong electrolytes into their ions, and finally eliminate the spectator ions.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, hydrochloric acid (HCl) acts as a strong acid, fully dissociating in solution to release H+ ions. Sodium formate (NaCHO2) can act as a weak base, accepting protons. Understanding the behavior of acids and bases is crucial for predicting the products of their reactions.

Dissociation of Electrolytes

Dissociation refers to the process by which an ionic compound separates into its constituent ions when dissolved in water. Strong electrolytes, like HCl and NaCHO2, dissociate completely in solution, while weak electrolytes do not. Recognizing which compounds dissociate and how they behave in solution is essential for writing accurate chemical equations and understanding the resulting ionic interactions.