Which Of The Following Is The Conjugate Acid Of $H_2PO_4^-$?A. $H_4PO_4^-$ B. \$HPO_4^{2-}$[/tex\] C. $H_3PO_4$ D. $PO_4^{3-}$
Conjugate acids play a crucial role in acid-base chemistry, and understanding their properties is essential for grasping various chemical reactions and processes. In this article, we will delve into the concept of conjugate acids and identify the conjugate acid of $H_2PO_4^-$.
What are Conjugate Acids?
A conjugate acid is a species that is formed when a base accepts a proton (H+ ion). In other words, it is the acid that is formed when a base donates a pair of electrons to a proton. Conjugate acids are essential in acid-base chemistry as they help to understand the behavior of acids and bases in various chemical reactions.
The Conjugate Acid-Base Pair
The conjugate acid-base pair is a fundamental concept in acid-base chemistry. It consists of a base and its corresponding conjugate acid. The conjugate acid is formed when the base accepts a proton, and the base is formed when the conjugate acid donates a proton. The conjugate acid-base pair is essential in understanding the pH of a solution and the behavior of acids and bases in various chemical reactions.
Identifying the Conjugate Acid of $H_2PO_4^-$
To identify the conjugate acid of $H_2PO_4^-$, we need to understand the structure of the phosphate ion. The phosphate ion has a charge of -3 and consists of four oxygen atoms and one phosphorus atom. When the phosphate ion accepts a proton, it forms a conjugate acid.
Option A: $H_4PO_4^-$
Option A is $H_4PO_4^-$, which is a species that has a charge of -1 and consists of four oxygen atoms, one phosphorus atom, and four hydrogen atoms. However, this species is not the conjugate acid of $H_2PO_4^-$, as it has an additional proton that is not present in the phosphate ion.
Option B: $HPO_4^{2-}$
Option B is $HPO_4^{2-}$, which is a species that has a charge of -2 and consists of four oxygen atoms, one phosphorus atom, and one hydrogen atom. However, this species is not the conjugate acid of $H_2PO_4^-$, as it has an additional oxygen atom that is not present in the phosphate ion.
Option C: $H_3PO_4$
Option C is $H_3PO_4$, which is a species that has a charge of 0 and consists of four oxygen atoms, one phosphorus atom, and three hydrogen atoms. This species is the conjugate acid of $H_2PO_4^-$, as it has one additional proton that is not present in the phosphate ion.
Option D: $PO_4^{3-}$
Option D is $PO_4^{3-}$, which is a species that has a charge of -3 and consists of four oxygen atoms and one phosphorus atom. However, this species is not the conjugate acid of $H_2PO_4^-$, as it has an additional oxygen atom that is not present in the phosphate ion.
Conclusion
In conclusion, the conjugate acid of $H_2PO_4^-$ is $H_3PO_4$. This species has one additional proton that is not present in the phosphate ion, making it the conjugate acid of $H_2PO_4^-$.
Understanding Conjugate Acids in Chemistry: Key Takeaways
- Conjugate acids are essential in acid-base chemistry and help to understand the behavior of acids and bases in various chemical reactions.
- The conjugate acid-base pair is a fundamental concept in acid-base chemistry and consists of a base and its corresponding conjugate acid.
- To identify the conjugate acid of a species, we need to understand the structure of the species and the number of protons it has.
- The conjugate acid of $H_2PO_4^-$ is $H_3PO_4$.
Frequently Asked Questions
- What is a conjugate acid? A conjugate acid is a species that is formed when a base accepts a proton (H+ ion).
- What is the conjugate acid-base pair? The conjugate acid-base pair is a fundamental concept in acid-base chemistry and consists of a base and its corresponding conjugate acid.
- How do we identify the conjugate acid of a species? We need to understand the structure of the species and the number of protons it has.
References
- Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
- Brown, T. E., LeMay, H. E., Bursten, B. E., & Murphy, C. (2012). Chemistry: The Central Science (12th ed.). Pearson Education.
- Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2011). General chemistry: Principles and modern applications (10th ed.). Pearson Education.
Conjugate Acids in Chemistry: Q&A =====================================
In our previous article, we discussed the concept of conjugate acids in chemistry and identified the conjugate acid of $H_2PO_4^-$ as $H_3PO_4$. In this article, we will answer some frequently asked questions about conjugate acids and provide additional information to help you understand this important concept in chemistry.
Q: What is a conjugate acid?
A: A conjugate acid is a species that is formed when a base accepts a proton (H+ ion). In other words, it is the acid that is formed when a base donates a pair of electrons to a proton.
Q: What is the conjugate acid-base pair?
A: The conjugate acid-base pair is a fundamental concept in acid-base chemistry and consists of a base and its corresponding conjugate acid. The conjugate acid is formed when the base accepts a proton, and the base is formed when the conjugate acid donates a proton.
Q: How do we identify the conjugate acid of a species?
A: To identify the conjugate acid of a species, we need to understand the structure of the species and the number of protons it has. We can do this by looking at the chemical formula of the species and determining how many protons it has.
Q: What is the difference between a conjugate acid and a strong acid?
A: A conjugate acid is a species that is formed when a base accepts a proton, while a strong acid is a species that completely dissociates in water to produce hydrogen ions (H+). In other words, a conjugate acid is a species that is formed when a base donates a pair of electrons to a proton, while a strong acid is a species that completely dissociates in water to produce hydrogen ions.
Q: Can a conjugate acid be a strong acid?
A: Yes, a conjugate acid can be a strong acid. For example, the conjugate acid of water (H2O) is hydronium ion (H3O+), which is a strong acid.
Q: What is the relationship between conjugate acids and pH?
A: Conjugate acids play a crucial role in determining the pH of a solution. The pH of a solution is a measure of the concentration of hydrogen ions (H+) in the solution. Conjugate acids can affect the pH of a solution by accepting or donating protons.
Q: Can conjugate acids be used to predict the pH of a solution?
A: Yes, conjugate acids can be used to predict the pH of a solution. By understanding the structure of the conjugate acid and the number of protons it has, we can determine how it will affect the pH of a solution.
Q: What are some common examples of conjugate acids?
A: Some common examples of conjugate acids include:
- The conjugate acid of water (H2O) is hydronium ion (H3O+)
- The conjugate acid of ammonia (NH3) is ammonium ion (NH4+)
- The conjugate acid of hydroxide ion (OH-) is water (H2O)
Conclusion
In conclusion, conjugate acids are an important concept in chemistry that play a crucial role in understanding acid-base chemistry. By understanding the structure of conjugate acids and the number of protons they have, we can determine how they will affect the pH of a solution. We hope this article has provided you with a better understanding of conjugate acids and their role in chemistry.
Frequently Asked Questions
- What is a conjugate acid? A conjugate acid is a species that is formed when a base accepts a proton (H+ ion).
- What is the conjugate acid-base pair? The conjugate acid-base pair is a fundamental concept in acid-base chemistry and consists of a base and its corresponding conjugate acid.
- How do we identify the conjugate acid of a species? We need to understand the structure of the species and the number of protons it has.
- Can a conjugate acid be a strong acid? Yes, a conjugate acid can be a strong acid.
References
- Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
- Brown, T. E., LeMay, H. E., Bursten, B. E., & Murphy, C. (2012). Chemistry: The Central Science (12th ed.). Pearson Education.
- Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2011). General chemistry: Principles and modern applications (10th ed.). Pearson Education.