Write balanced molecular and net ionic equations for the reaction between hydrochloric acid and rubidium hydroxide.

Verified step by step guidance

1. Identify the reactants and products: Hydrochloric acid (HCl) and rubidium hydroxide (RbOH) react to form water (H2O) and rubidium chloride (RbCl).
2. Write the balanced molecular equation: Combine the reactants to form the products, ensuring that the number of atoms of each element is the same on both sides of the equation.
3. Dissociate all strong electrolytes into their ions for the complete ionic equation: HCl and RbOH are strong electrolytes, so they dissociate completely in water.
4. Cancel out the spectator ions to write the net ionic equation: Identify ions that appear on both sides of the complete ionic equation and remove them.
5. Write the final net ionic equation: The net ionic equation should only include the ions and molecules directly involved in the chemical reaction.

Key Concepts

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, hydrochloric acid (HCl) acts as an acid, donating a proton, while rubidium hydroxide (RbOH) acts as a base, accepting the proton. The result is the formation of water and a salt, which is a typical outcome of neutralization 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 HCl and RbOH, the balanced molecular equation must reflect the stoichiometry of the reactants and products accurately.

Net Ionic Equations

Net ionic equations simplify chemical reactions by removing spectator ions—ions that do not participate in the reaction—from the full ionic equation. This focuses on the actual chemical species that undergo change. In the case of HCl and RbOH, the net ionic equation highlights the formation of water from H+ and OH- ions.