Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (c) Aqueous nitric acid and aqueous ammonia react.

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Identify the reactants and their states. In this case, the reactants are nitric acid (HNO3) which is aqueous, and ammonia (NH3) which is also in aqueous form when dissolved in water.

Write the unbalanced molecular equation for the reaction. Combine the reactants to form the products. For a neutralization reaction involving an acid and a base, the products are typically water (H2O) and a salt. Here, the salt formed would be ammonium nitrate (NH4NO3). The unbalanced equation is: HNO3(aq) + NH3(aq) ightarrow NH4NO3(aq) + H2O(l).

Balance the molecular equation. Ensure that the number of atoms for each element is equal on both sides of the equation. For this reaction, the equation is already balanced as written.

Write the total ionic equation. Break all soluble compounds into their ions. HNO3 and NH4NO3 are strong electrolytes and will dissociate completely into ions: HNO3(aq) ightarrow H+(aq) + NO3-(aq), NH3(aq) + H2O(l) ightarrow NH4+(aq) + OH-(aq), NH4NO3(aq) ightarrow NH4+(aq) + NO3-(aq).

Write the net ionic equation by canceling out the spectator ions (ions that appear on both sides of the equation). The spectator ions in this case are NH4+ and NO3-. The net ionic equation is: H+(aq) + OH-(aq) ightarrow H2O(l).

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Neutralization Reactions

Neutralization reactions occur when an acid reacts with a base to produce water and a salt. In this process, the hydrogen ions (H+) from the acid combine with hydroxide ions (OH-) from the base to form water (H2O). Understanding this concept is crucial for writing balanced equations, as it highlights the fundamental interaction between acids and bases.

Balanced Molecular Equations

A balanced molecular equation represents the reactants and products of a chemical reaction with their respective coefficients, ensuring that the number of atoms for each element is the same on both sides. For the reaction between nitric acid and ammonia, it is essential to correctly identify the products formed and balance the equation to reflect the conservation of mass.

Net Ionic Equations

Net ionic equations focus on the species that actually participate in the reaction, omitting spectator ions that do not change during the reaction. To derive the net ionic equation for the neutralization of nitric acid and ammonia, one must first write the complete ionic equation and then eliminate the spectator ions, highlighting the essential chemical changes occurring in the reaction.