What Precipitate, If Any, Forms When A Solution Of Ammonium Carbonate Is Mixed With A Solution Of Barium Chloride?A. $NH_4Cl$ B. $(NH_4)_2CO_3$ C. No Precipitate Forms. D. $BaCO_3$ E. $BaCl_2$
What Precipitate Forms When Ammonium Carbonate and Barium Chloride Solutions Are Mixed?
Understanding the Chemical Reaction
When a solution of ammonium carbonate (NH4)2CO3 is mixed with a solution of barium chloride BaCl2, a chemical reaction occurs. This reaction involves the exchange of ions between the two solutions, resulting in the formation of a precipitate. To determine which precipitate forms, we need to analyze the chemical equation and the solubility rules of the ions involved.
Chemical Equation
The chemical equation for the reaction between ammonium carbonate and barium chloride is:
(NH4)2CO3(aq) + BaCl2(aq) → BaCO3(s) + 2NH4Cl(aq)
In this equation, the ammonium carbonate (NH4)2CO3 reacts with barium chloride BaCl2 to form barium carbonate BaCO3 and ammonium chloride NH4Cl.
Solubility Rules
To determine which precipitate forms, we need to apply the solubility rules of the ions involved. The solubility rules state that:
- Most sodium, potassium, and ammonium salts are soluble.
- Most nitrates and acetates are soluble.
- Most chlorides, bromides, and iodides are soluble, except for those of silver, lead(II), and mercury(I).
- Most carbonates, phosphates, and silicates are insoluble, except for those of sodium, potassium, and ammonium.
Applying the Solubility Rules
Based on the solubility rules, we can determine that:
- Ammonium chloride NH4Cl is soluble, as it is a salt of ammonium.
- Barium carbonate BaCO3 is insoluble, as it is a carbonate salt.
- Ammonium carbonate (NH4)2CO3 is soluble, as it is a salt of ammonium.
Conclusion
Based on the chemical equation and the solubility rules, we can conclude that the precipitate that forms when a solution of ammonium carbonate is mixed with a solution of barium chloride is barium carbonate BaCO3.
Answer
The correct answer is D. BaCO3.
Additional Information
It's worth noting that the solubility of barium carbonate BaCO3 can be affected by factors such as temperature and pH. At high temperatures, barium carbonate BaCO3 can become less soluble, while at low pH, it can become more soluble. However, in the context of this reaction, barium carbonate BaCO3 is expected to be insoluble.
References
- Chemistry: An Atoms First Approach, by Steven S. Zumdahl
- General Chemistry: Principles and Modern Applications, by Linus Pauling
Key Takeaways
- The reaction between ammonium carbonate and barium chloride results in the formation of a precipitate.
- The precipitate that forms is barium carbonate BaCO3.
- The solubility of barium carbonate BaCO3 can be affected by factors such as temperature and pH.
Q&A: Ammonium Carbonate and Barium Chloride Reaction
Frequently Asked Questions
We've received many questions about the reaction between ammonium carbonate and barium chloride. Here are some of the most frequently asked questions and their answers:
Q: What is the chemical equation for the reaction between ammonium carbonate and barium chloride?
A: The chemical equation for the reaction between ammonium carbonate and barium chloride is:
(NH4)2CO3(aq) + BaCl2(aq) → BaCO3(s) + 2NH4Cl(aq)
Q: What is the precipitate that forms when a solution of ammonium carbonate is mixed with a solution of barium chloride?
A: The precipitate that forms is barium carbonate BaCO3.
Q: Why does barium carbonate form as a precipitate?
A: Barium carbonate forms as a precipitate because it is insoluble in water. According to the solubility rules, most carbonates are insoluble, except for those of sodium, potassium, and ammonium.
Q: Is ammonium chloride soluble or insoluble?
A: Ammonium chloride is soluble in water. According to the solubility rules, most sodium, potassium, and ammonium salts are soluble.
Q: Can the solubility of barium carbonate be affected by factors such as temperature and pH?
A: Yes, the solubility of barium carbonate can be affected by factors such as temperature and pH. At high temperatures, barium carbonate can become less soluble, while at low pH, it can become more soluble.
Q: What are some common applications of barium carbonate?
A: Barium carbonate has several common applications, including:
- As a pigment in paints and coatings
- As a filler in plastics and rubber
- As a component in the manufacture of glass and ceramics
- As a catalyst in the production of chemicals
Q: What are some common applications of ammonium chloride?
A: Ammonium chloride has several common applications, including:
- As a fertilizer in agriculture
- As a component in the manufacture of dyes and pigments
- As a catalyst in the production of chemicals
- As a component in the manufacture of pharmaceuticals
Q: Can the reaction between ammonium carbonate and barium chloride be used to produce other compounds?
A: Yes, the reaction between ammonium carbonate and barium chloride can be used to produce other compounds, including:
- Barium hydroxide: Ba(OH)2
- Ammonium hydroxide: NH4OH
- Carbon dioxide: CO2
Q: What are some safety precautions that should be taken when handling ammonium carbonate and barium chloride?
A: When handling ammonium carbonate and barium chloride, it is essential to take several safety precautions, including:
- Wearing protective gloves and eyewear
- Working in a well-ventilated area
- Avoiding contact with skin and eyes
- Following proper disposal procedures
References
- Chemistry: An Atoms First Approach, by Steven S. Zumdahl
- General Chemistry: Principles and Modern Applications, by Linus Pauling
Key Takeaways
- The reaction between ammonium carbonate and barium chloride results in the formation of a precipitate.
- The precipitate that forms is barium carbonate BaCO3.
- The solubility of barium carbonate can be affected by factors such as temperature and pH.
- Ammonium chloride is soluble in water.
- Barium carbonate has several common applications, including as a pigment in paints and coatings and as a component in the manufacture of glass and ceramics.