Enter the molecular equation representing aqueous nitric acid and aqueous ammonia reacting. Express your answer as a balanced molecular equation. Identify all of the phases in your answer. ?SF R o ? HNO3(aq) + NH, •H2O(1)?NH, NO2 (aq) +H, O(1) You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers Request Answer Part F Enter the net ionic equation representing aqueous nitric acid and aqueous ammonia reacting. Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.
The Correct Answer and Explanation is :
When aqueous nitric acid (HNO₃) reacts with aqueous ammonia (NH₃), they undergo an acid-base reaction to form ammonium nitrate (NH₄NO₃).
Balanced Molecular Equation:
[ \text{HNO}_3(aq) + \text{NH}_3(aq) \rightarrow \text{NH}_4\text{NO}_3(aq) ]
Balanced Net Ionic Equation:
[ \text{H}^+(aq) + \text{NH}_3(aq) \rightarrow \text{NH}_4^+(aq) ]
Explanation:
In this reaction, nitric acid, a strong acid, dissociates completely in water to produce hydrogen ions (H⁺) and nitrate ions (NO₃⁻). Ammonia, a weak base, partially ionizes in water to form ammonium ions (NH₄⁺) and hydroxide ions (OH⁻). When ammonia and nitric acid are mixed, the hydrogen ion from the acid reacts with the ammonia molecule to form the ammonium ion. The nitrate ion remains unchanged as a spectator ion. Therefore, the net ionic equation focuses on the proton transfer between ammonia and the hydrogen ion from nitric acid, resulting in the formation of the ammonium ion.
This reaction is a classic example of an acid-base neutralization, where the acid (HNO₃) donates a proton to the base (NH₃), leading to the formation of a salt (NH₄NO₃) in aqueous solution.