Question

Write a balanced equation illustrating the reactions that occur between one molecule of ammonia with (a) one molecule of nitric acid and with (b) one molecule of sulfuric acid.

Short answer

(a) \( \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \); (b) \( 2\text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow (\text{NH}_4)_2\text{SO}_4 \).

Step-by-step solution

Identify the Reactants

For part (a), the reactants are ammonia (NH₃) and nitric acid (HNO₃). For part (b), the reactants are ammonia (NH₃) and sulfuric acid (H₂SO₄).

Predict the Products for Each Reaction

In part (a), ammonia (NH₃) reacts with nitric acid (HNO₃) to form ammonium nitrate (NH₄NO₃). In part (b), ammonia (NH₃) reacts with sulfuric acid (H₂SO₄) to form ammonium sulfate ((NH₄)₂SO₄).

Write the Balanced Equation for Reaction (a)

The reaction between ammonia and nitric acid is: \[ \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \]. This equation is already balanced as written.

Write the Balanced Equation for Reaction (b)

The reaction between ammonia and sulfuric acid is: \[ 2\text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow (\text{NH}_4)_2\text{SO}_4 \]. This equation shows that 2 molecules of ammonia react with 1 molecule of sulfuric acid to form 1 molecule of ammonium sulfate.

Key concepts

Balanced Equations

In chemical reactions, a balanced equation is essential because it shows the equal number of atoms for each element on both sides of the reaction. This is in line with the Law of Conservation of Mass, which states that matter cannot be created or destroyed. In the equations we have, you see a balance because the number of atoms of each element remains constant from reactants to products.
To write a balanced chemical equation, follow these steps:

• Identify the reactants and products in the reaction.
• Write the skeletal equation for the process.
• Adjust the coefficients (the numbers in front) to ensure the number of atoms of each element is equal on both sides.

In the given exercises, for ammonia and nitric acid, we start with the reactants: \( \text{NH}_3 + \text{HNO}_3 \) producing \( \text{NH}_4\text{NO}_3 \), which is already balanced. Similarly, for ammonia and sulfuric acid, \( 2\text{NH}_3 + \text{H}_2\text{SO}_4 \) produces \( (\text{NH}_4)_2\text{SO}_4 \), ensuring each atom is equally represented on both sides.

Ammonia Reaction

Ammonia is a colorless gas with a pungent smell, made up of nitrogen and hydrogen \((\text{NH}_3)\). It is a common chemical used in various industrial applications.
When ammonia reacts with acids, it typically forms ammonium salts. The reactions highlighted here involve ammonia reacting with two different acids: nitric acid and sulfuric acid.

• With nitric acid, ammonia forms ammonium nitrate \((\text{NH}_4\text{NO}_3)\), which is used in fertilizers and explosives.
• The reaction with sulfuric acid forms ammonium sulfate \(((\text{NH}_4)_2\text{SO}_4)\), another type of fertilizer.

These reactions are characterized by the transfer of hydrogen ions from the acid to ammonia, transforming it into the ammonium ion \((\text{NH}_4^+)\). This behavior makes ammonia an important chemical in both manufacturing and agriculture.

Acid-Base Reaction

An acid-base reaction is a type of chemical reaction that involves the transfer of protons \((\text{H}^+)\) between an acid and a base. This process leads to the formation of a salt and sometimes water. In our examples, ammonia acts as the base by accepting protons.

• In the case of ammonia and nitric acid, the nitric acid donates a proton to ammonia forming the ammonium ion \((\text{NH}_4^+)\) which combines with the nitrate ion \((\text{NO}_3^-)\) to produce ammonium nitrate.
• For the reaction with sulfuric acid, two protons are transferred to form ammonium ions and the sulfate ion \((\text{SO}_4^{2-})\), resulting in ammonium sulfate.

These reactions typically result in the formation of salts, and in the lab, they're a simple but fundamental illustration of how acids and bases interact with one another. Understanding these interactions is vital for many fields, including chemistry, biology, and environmental science.