Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

Verified step by step guidance

1. Identify the reactants and products: Hydrobromic acid (HBr) reacts with potassium hydroxide (KOH) to form water (H2O) and potassium bromide (KBr).
2. Write the balanced molecular equation: Combine the reactants to form the products, ensuring that the number of atoms for each element is equal on both sides of the equation.
3. Dissociate all strong electrolytes into their ions: HBr and KOH are strong acids and bases, respectively, so they dissociate completely in water.
4. Write the complete ionic equation: Show all the ions present in the reaction, including spectator ions that do not participate in the reaction.
5. Identify and cancel out the spectator ions to write the net ionic equation: Remove the ions that appear on both sides of the complete ionic equation to find the net ionic equation, which shows only the species that actually change during the reaction.

Key Concepts

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, hydrobromic acid (HBr) acts as an acid, donating a proton, while potassium hydroxide (KOH) serves as a base, accepting the proton. The result is the formation of water and a salt, illustrating the neutralization process typical of acid-base reactions.

Balanced Chemical Equations

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This ensures the law of conservation of mass is upheld. For the reaction between HBr and KOH, the balanced molecular equation shows all reactants and products, while the net ionic equation focuses on the species that undergo change during the reaction.

Ionic Compounds and Solubility

Ionic compounds, such as KBr formed in this reaction, dissociate into their constituent ions in solution. Understanding solubility rules helps predict which compounds will remain in solution and which will precipitate. In the case of the net ionic equation, only the ions that participate in the reaction are included, omitting spectator ions that do not change during the reaction.