Consider The Reaction Below:${ NH_4^{+} + H_2O \rightarrow NH_3 + H_3O^{+} }$Which Is An Acid-conjugate Base Pair?A. { NH_4^{+} $}$ And { NH_3 $}$ B. { NH_4^{+} $}$ And { H_3O^{+} $}$ C. [$
Introduction
In chemistry, acids and bases play a crucial role in various chemical reactions. The Arrhenius definition of acids and bases states that acids are substances that increase the concentration of hydrogen ions (H+) in a solution, while bases are substances that increase the concentration of hydroxide ions (OH-) in a solution. However, the Bronsted-Lowry definition of acids and bases is more comprehensive and widely used. According to this definition, an acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton. In this article, we will discuss acid-conjugate base pairs and identify the acid-conjugate base pair in the given reaction.
What are Acid-Conjugate Base Pairs?
An acid-conjugate base pair is a pair of substances that are related to each other through the gain or loss of a proton (H+). When an acid donates a proton, it forms a conjugate base. Conversely, when a base accepts a proton, it forms a conjugate acid. The acid-conjugate base pair is a fundamental concept in chemistry, and it is essential to understand it to analyze various chemical reactions.
The Given Reaction
The given reaction is:
In this reaction, ammonium ion (NH4+) reacts with water (H2O) to form ammonia (NH3) and hydronium ion (H3O+).
Identifying the Acid-Conjugate Base Pair
To identify the acid-conjugate base pair in the given reaction, we need to analyze the reaction and determine which substance donates or accepts a proton.
- In the given reaction, ammonium ion (NH4+) donates a proton to form ammonia (NH3).
- Conversely, water (H2O) accepts a proton to form hydronium ion (H3O+).
Therefore, the acid-conjugate base pair in the given reaction is:
- Acid: NH4+ (ammonium ion)
- Conjugate base: NH3 (ammonia)
Conclusion
In conclusion, the acid-conjugate base pair in the given reaction is NH4+ and NH3. The ammonium ion (NH4+) donates a proton to form ammonia (NH3), while water (H2O) accepts a proton to form hydronium ion (H3O+). Understanding acid-conjugate base pairs is essential in chemistry, and it helps us analyze various chemical reactions.
Key Takeaways
- Acid-conjugate base pairs are related to each other through the gain or loss of a proton (H+).
- An acid donates a proton to form a conjugate base.
- A base accepts a proton to form a conjugate acid.
- The acid-conjugate base pair is a fundamental concept in chemistry.
Frequently Asked Questions
Q: What is an acid-conjugate base pair?
A: An acid-conjugate base pair is a pair of substances that are related to each other through the gain or loss of a proton (H+).
Q: What is the acid-conjugate base pair in the given reaction?
A: The acid-conjugate base pair in the given reaction is NH4+ and NH3.
Q: What is the difference between an acid and a base?
A: An acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton.
Q: What is the Bronsted-Lowry definition of acids and bases?
A: The Bronsted-Lowry definition of acids and bases states that an acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton.
References
- Arrhenius, S. (1887). On the Constitution of Bases. Journal of the Chemical Society, Transactions, 51, 244-253.
- Bronsted, J. N. (1923). The Kinetic Theory of Strong Electrolytes. Journal of the American Chemical Society, 45(10), 2473-2481.
- Lowry, T. M. (1923). The Kinetic Theory of Strong Electrolytes. Journal of the American Chemical Society, 45(10), 2481-2484.
Further Reading
- Chemistry: An Atoms First Approach. (2017). By Steven S. Zumdahl.
- General Chemistry: Principles and Modern Applications. (2017). By Linus Pauling.
Conclusion
Introduction
In our previous article, we discussed acid-conjugate base pairs and identified the acid-conjugate base pair in the given reaction. In this article, we will provide a comprehensive Q&A guide to help you understand acid-conjugate base pairs better.
Q&A Guide
Q: What is an acid-conjugate base pair?
A: An acid-conjugate base pair is a pair of substances that are related to each other through the gain or loss of a proton (H+).
Q: What is the difference between an acid and a base?
A: An acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton.
Q: What is the Bronsted-Lowry definition of acids and bases?
A: The Bronsted-Lowry definition of acids and bases states that an acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton.
Q: What is the Arrhenius definition of acids and bases?
A: The Arrhenius definition of acids and bases states that acids are substances that increase the concentration of hydrogen ions (H+) in a solution, while bases are substances that increase the concentration of hydroxide ions (OH-) in a solution.
Q: What is the acid-conjugate base pair in the given reaction?
A: The acid-conjugate base pair in the given reaction is NH4+ and NH3.
Q: What is the conjugate acid of a base?
A: The conjugate acid of a base is the substance that forms when the base accepts a proton.
Q: What is the conjugate base of an acid?
A: The conjugate base of an acid is the substance that forms when the acid donates a proton.
Q: What is the relationship between acid-conjugate base pairs and pH?
A: Acid-conjugate base pairs are related to pH, as the concentration of hydrogen ions (H+) in a solution affects the pH.
Q: What is the significance of acid-conjugate base pairs in chemistry?
A: Acid-conjugate base pairs are essential in chemistry, as they help us understand various chemical reactions and processes.
Q: Can you provide examples of acid-conjugate base pairs?
A: Yes, here are some examples of acid-conjugate base pairs:
- HCl (hydrochloric acid) and Cl- (chloride ion)
- H2SO4 (sulfuric acid) and HSO4- (hydrogen sulfate ion)
- NH4+ (ammonium ion) and NH3 (ammonia)
Q: How do acid-conjugate base pairs affect the pH of a solution?
A: Acid-conjugate base pairs can affect the pH of a solution by increasing or decreasing the concentration of hydrogen ions (H+).
Q: What is the relationship between acid-conjugate base pairs and buffers?
A: Acid-conjugate base pairs are related to buffers, as buffers are solutions that resist changes in pH by reacting with excess hydrogen or hydroxide ions.
Q: Can you provide examples of buffers?
A: Yes, here are some examples of buffers:
- HCl (hydrochloric acid) and NaOH (sodium hydroxide)
- H2SO4 (sulfuric acid) and Na2SO4 (sodium sulfate)
- NH4+ (ammonium ion) and NH3 (ammonia)
Conclusion
In conclusion, acid-conjugate base pairs are essential in chemistry, and understanding them is crucial to analyze various chemical reactions and processes. We hope this Q&A guide has helped you understand acid-conjugate base pairs better.
Key Takeaways
- Acid-conjugate base pairs are related to each other through the gain or loss of a proton (H+).
- An acid donates a proton to form a conjugate base.
- A base accepts a proton to form a conjugate acid.
- Acid-conjugate base pairs are essential in chemistry.
Frequently Asked Questions
Q: What is the difference between an acid and a base?
A: An acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton.
Q: What is the Bronsted-Lowry definition of acids and bases?
A: The Bronsted-Lowry definition of acids and bases states that an acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton.
Q: What is the Arrhenius definition of acids and bases?
A: The Arrhenius definition of acids and bases states that acids are substances that increase the concentration of hydrogen ions (H+) in a solution, while bases are substances that increase the concentration of hydroxide ions (OH-) in a solution.
References
- Arrhenius, S. (1887). On the Constitution of Bases. Journal of the Chemical Society, Transactions, 51, 244-253.
- Bronsted, J. N. (1923). The Kinetic Theory of Strong Electrolytes. Journal of the American Chemical Society, 45(10), 2473-2481.
- Lowry, T. M. (1923). The Kinetic Theory of Strong Electrolytes. Journal of the American Chemical Society, 45(10), 2481-2484.
Further Reading
- Chemistry: An Atoms First Approach. (2017). By Steven S. Zumdahl.
- General Chemistry: Principles and Modern Applications. (2017). By Linus Pauling.
Conclusion
In conclusion, acid-conjugate base pairs are essential in chemistry, and understanding them is crucial to analyze various chemical reactions and processes. We hope this Q&A guide has helped you understand acid-conjugate base pairs better.