Chapter 3: Problem 20
Write a balanced equation illustrating the reactions that occur between one molecule of ammonia and (a) one molecule of nitric acid and (b) one molecule of sulfuric acid.
Short Answer
Expert verified
(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
01
Understanding the problem
We are tasked with writing balanced chemical equations for reactions between ammonia (\( \text{NH}_3 \)) and two different acids: nitric acid (\( \text{HNO}_3 \)) and sulfuric acid (\( \text{H}_2\text{SO}_4 \)). Each part will require us to identify the reactants and predict the formation of ionic compounds, typically a salt and water.
02
Writing the equation for ammonia and nitric acid
Ammonia (\( \text{NH}_3 \)) reacts with nitric acid (\( \text{HNO}_3 \)) to form ammonium nitrate (\( \text{NH}_4\text{NO}_3 \)). The balanced equation for this reaction is:\[ \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \]
03
Writing the equation for ammonia and sulfuric acid
When ammonia (\( \text{NH}_3 \)) reacts with sulfuric acid (\( \text{H}_2\text{SO}_4 \)), the product is ammonium sulfate (\( \text{(NH}_4)_2\text{SO}_4 \)). Because each molecule of sulfuric acid can donate two protons (and ammonia can accept one), two molecules of ammonia react with one molecule of sulfuric acid. The balanced equation is:\[ 2\text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow \text{(NH}_4)_2\text{SO}_4 \]
04
Verifying balance of equations
Both equations should be checked for each element to ensure the same number of atoms appears on each side of the reaction. In the first reaction with nitric acid, we have balanced nitrogen, hydrogen, and oxygen. In the second reaction with sulfuric acid, we have balanced nitrogen, hydrogen, sulfur, and oxygen.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Ammonia
Ammonia is a common chemical you'll encounter in both laboratory and household settings. It's a compound made up of nitrogen and hydrogen, with the chemical formula \( \text{NH}_3 \). Ammonia is well-known for its pungent odor, similar to that found in many household cleaning products.
In chemical terms, ammonia behaves as a base. This means it has the capability to accept protons from acids. In reactions, ammonia's lone pair of electrons on the nitrogen atom allows it to form a bond with a hydrogen ion from an acid. This process is key in forming ammonium ions \( \text{NH}_4^+ \).
The formation of ammonium ions is a crucial part of the reactions in this exercise when ammonia reacts with either nitric acid or sulfuric acid. Understanding ammonia's basic nature and its ability to form bonds with acids is vital for predicting the products of these chemical reactions.
In chemical terms, ammonia behaves as a base. This means it has the capability to accept protons from acids. In reactions, ammonia's lone pair of electrons on the nitrogen atom allows it to form a bond with a hydrogen ion from an acid. This process is key in forming ammonium ions \( \text{NH}_4^+ \).
The formation of ammonium ions is a crucial part of the reactions in this exercise when ammonia reacts with either nitric acid or sulfuric acid. Understanding ammonia's basic nature and its ability to form bonds with acids is vital for predicting the products of these chemical reactions.
Nitric Acid
Nitric acid, with the chemical formula \( \text{HNO}_3 \), is a strong acid that is commonly used in the production of fertilizers, explosives, and in laboratory settings. It is highly corrosive and can cause severe burns, so it must be handled with caution.
In the context of chemical reactions, nitric acid is a source of hydrogen ions \( \text{H}^+ \), which it can donate to bases like ammonia. When nitric acid reacts with ammonia, the hydrogen ions bond with ammonia to form ammonium ions \( \text{NH}_4^+ \). The nitrate ions \( \text{NO}_3^- \) from the nitric acid pair with the ammonium ions to create ammonium nitrate \( \text{NH}_4\text{NO}_3 \).
The balanced chemical equation for this reaction is simple, being \( \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \). Each side of the equation contains the same number of nitrogen, hydrogen, and oxygen atoms, maintaining the law of conservation of mass.
In the context of chemical reactions, nitric acid is a source of hydrogen ions \( \text{H}^+ \), which it can donate to bases like ammonia. When nitric acid reacts with ammonia, the hydrogen ions bond with ammonia to form ammonium ions \( \text{NH}_4^+ \). The nitrate ions \( \text{NO}_3^- \) from the nitric acid pair with the ammonium ions to create ammonium nitrate \( \text{NH}_4\text{NO}_3 \).
The balanced chemical equation for this reaction is simple, being \( \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \). Each side of the equation contains the same number of nitrogen, hydrogen, and oxygen atoms, maintaining the law of conservation of mass.
Sulfuric Acid
Sulfuric acid is another powerful acid, typically denoted by the chemical formula \( \text{H}_2\text{SO}_4 \). It is widely used in industrial procedures, such as refining crude oil and manufacturing chemicals, including fertilizers.
Known for its ability to donate more than one proton, sulfuric acid can dissociate to provide two hydrogen ions. This makes it particularly suited for reactions requiring multiple protons. When sulfuric acid reacts with ammonia, the two protons lead to the formation of two ammonium ions from two molecules of ammonia.
The sulfate ion \( \text{SO}_4^{2-} \), which is left after donating the protons, combines with the ammonium ions to form ammonium sulfate \( \text{(NH}_4)_2\text{SO}_4 \). The balanced equation \( 2\text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow \text{(NH}_4)_2\text{SO}_4 \) shows this pairing, ensuring each type of atom aligns perfectly on both sides of the equation.
Known for its ability to donate more than one proton, sulfuric acid can dissociate to provide two hydrogen ions. This makes it particularly suited for reactions requiring multiple protons. When sulfuric acid reacts with ammonia, the two protons lead to the formation of two ammonium ions from two molecules of ammonia.
The sulfate ion \( \text{SO}_4^{2-} \), which is left after donating the protons, combines with the ammonium ions to form ammonium sulfate \( \text{(NH}_4)_2\text{SO}_4 \). The balanced equation \( 2\text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow \text{(NH}_4)_2\text{SO}_4 \) shows this pairing, ensuring each type of atom aligns perfectly on both sides of the equation.
Balanced Chemical Equations
Balanced chemical equations are foundational in chemistry, representing the conservation of mass and charge in a reaction. A balanced equation means there is an equal number of each type of atom on both the reactant and product sides of the equation.
In our case, balancing involves ensuring the correct number of nitrogen, hydrogen, oxygen, and sulfur atoms on each side of the equations for reactions involving ammonia. For reaction with nitric acid, the balance is fairly straightforward as both reactant and product contain the same number of each atom type.
When dealing with sulfuric acid, things get a bit more complex. Because sulfuric acid can donate two protons, two ammonia molecules are needed to keep things even, leading to the larger ammonium sulfate product. Both the equations and their predictions reinforce the formative principle that matter is neither created nor destroyed, only transformed. Maintaining this balance is the essence of writing chemical equations correctly.
In our case, balancing involves ensuring the correct number of nitrogen, hydrogen, oxygen, and sulfur atoms on each side of the equations for reactions involving ammonia. For reaction with nitric acid, the balance is fairly straightforward as both reactant and product contain the same number of each atom type.
When dealing with sulfuric acid, things get a bit more complex. Because sulfuric acid can donate two protons, two ammonia molecules are needed to keep things even, leading to the larger ammonium sulfate product. Both the equations and their predictions reinforce the formative principle that matter is neither created nor destroyed, only transformed. Maintaining this balance is the essence of writing chemical equations correctly.
