Write balanced complete ionic and net ionic equations for each acid–base reaction. a. HI(aq) + RbOH(aq) →

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Identify the reactants and products in the given acid-base reaction: HI(aq) + RbOH(aq) -> H2O(l) + RbI(aq).

Write the balanced molecular equation for the reaction: HI(aq) + RbOH(aq) -> H2O(l) + RbI(aq).

Break down all the strong electrolytes into their constituent ions to write the complete ionic equation: H^+(aq) + I^-(aq) + Rb^+(aq) + OH^-(aq) -> H2O(l) + Rb^+(aq) + I^-(aq).

Identify and cancel out the spectator ions that appear on both sides of the complete ionic equation: Rb^+(aq) and I^-(aq).

Write the net ionic equation by including only the species that undergo a chemical change: H^+(aq) + OH^-(aq) -> H2O(l).

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주요 개념

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Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, HI (hydroiodic acid) acts as an acid, donating a proton, while RbOH (rubidium hydroxide) acts 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 shows all the ions present in a solution, including spectator ions that do not participate in the reaction. For the reaction between HI and RbOH, the complete ionic equation will include the dissociated forms of the acids and bases, allowing for a clearer view of the reactants and products involved.

Net Ionic Equations

The net ionic equation simplifies the complete ionic equation by removing spectator ions, focusing only on the ions that participate in the reaction. This is essential for understanding the actual chemical change occurring, as it highlights the formation of water in the neutralization of HI and RbOH.