Which Of The Following Is The Conjugate Base Of $HSO_3{ }^{-}$?A. $H_2SO_3$ B. \$HSO_3{ }^{+}$[/tex\] C. $SO_3{ }^{2-}$ D. $SO_2$

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Conjugate bases are a fundamental concept in chemistry, particularly in acid-base chemistry. They play a crucial role in understanding the behavior of acids and bases in various chemical reactions. In this article, we will explore the concept of conjugate bases and identify the conjugate base of $HSO_3{ }^{-}$.

What are Conjugate Bases?

A conjugate base is the species that results when an acid donates a proton (H+ ion). In other words, it is the base that is formed when an acid loses a proton. The conjugate base of an acid is always more basic than the original acid. This is because the conjugate base has one less proton than the original acid, making it more prone to accept a proton and form the original acid.

Identifying Conjugate Bases

To identify the conjugate base of a given acid, we need to remove a proton (H+ ion) from the acid. This can be done by simply removing the H+ ion from the acid formula. For example, the conjugate base of $HCl$ is $Cl^-$, which is formed by removing a proton from $HCl$.

Conjugate Base of $HSO_3{ }^{-}$

Now, let's apply this concept to the given acid, $HSO_3{ }^{-}$. To identify its conjugate base, we need to remove a proton from $HSO_3{ }^{-}$. This can be done by simply removing the H+ ion from the acid formula.

HSO3−→SO32−+H+HSO_3{ }^{-} \rightarrow SO_3{ }^{2-} + H^+

As we can see, the conjugate base of $HSO_3{ }^{-}$ is $SO_3{ }^{2-}$.

Conclusion

In conclusion, the conjugate base of $HSO_3{ }^{-}$ is $SO_3{ }^{2-}$. This is because the conjugate base is formed by removing a proton from the acid, resulting in a more basic species.

Answer

The correct answer is:

  • C. $SO_3{ }^{2-}$

Why is this the correct answer?

This is the correct answer because the conjugate base of $HSO_3{ }^{-}$ is formed by removing a proton from the acid, resulting in a more basic species. The other options, $H_2SO_3$, $HSO_3{ }^{+}$, and $SO_2$, are not the conjugate base of $HSO_3{ }^{-}$.

Understanding the Options

Let's take a closer look at the options:

  • A. $H_2SO_3$: This is the formula for sulfurous acid, which is not the conjugate base of $HSO_3{ }^{-}$.
  • B. $HSO_3{ }^{+}$: This is not a valid formula for a conjugate base.
  • C. $SO_3{ }^{2-}$: This is the correct answer, as explained earlier.
  • D. $SO_2$: This is the formula for sulfur dioxide, which is not the conjugate base of $HSO_3{ }^{-}$.

Conclusion

In this article, we will answer some frequently asked questions about conjugate bases in chemistry.

Q: What is the difference between an acid and its conjugate base?

A: An acid is a species that donates a proton (H+ ion), while its conjugate base is the species that results when the acid donates a proton. In other words, the conjugate base is the base that is formed when an acid loses a proton.

Q: How do I identify the conjugate base of a given acid?

A: To identify the conjugate base of a given acid, you need to remove a proton (H+ ion) from the acid. This can be done by simply removing the H+ ion from the acid formula.

Q: What is the relationship between an acid and its conjugate base?

A: The conjugate base of an acid is always more basic than the original acid. This is because the conjugate base has one less proton than the original acid, making it more prone to accept a proton and form the original acid.

Q: Can a conjugate base be an acid?

A: No, a conjugate base cannot be an acid. By definition, a conjugate base is the species that results when an acid donates a proton, and it is always more basic than the original acid.

Q: What is the difference between a conjugate base and a base?

A: A conjugate base is a specific type of base that is formed when an acid donates a proton. A base, on the other hand, is a species that accepts a proton (H+ ion). While all conjugate bases are bases, not all bases are conjugate bases.

Q: Can a conjugate base be a strong base?

A: Yes, a conjugate base can be a strong base. In fact, many strong bases are conjugate bases of weak acids.

Q: How do conjugate bases affect acid-base equilibria?

A: Conjugate bases can affect acid-base equilibria by accepting protons (H+ ions) and forming the original acid. This can shift the equilibrium towards the acid or the base, depending on the specific reaction.

Q: Can conjugate bases be used in chemical reactions?

A: Yes, conjugate bases can be used in chemical reactions. In fact, many chemical reactions involve the formation and reaction of conjugate bases.

Q: What are some common examples of conjugate bases?

A: Some common examples of conjugate bases include:

  • Cl^-$ (the conjugate base of $HCl$)

  • OH^-$ (the conjugate base of $H_2O$)

  • SO_3{ }^{2-}$ (the conjugate base of $HSO_3{ }^{-}$)

Conclusion

In conclusion, conjugate bases are an important concept in chemistry, particularly in acid-base chemistry. By understanding the relationship between acids and their conjugate bases, we can better understand acid-base equilibria and chemical reactions.

Frequently Asked Questions

  • What is the conjugate base of $HCl$?
  • What is the conjugate base of $H_2O$?
  • What is the conjugate base of $HSO_3{ }^{-}$?
  • Can a conjugate base be a strong base?
  • How do conjugate bases affect acid-base equilibria?

Answers

  • The conjugate base of $HCl$ is $Cl^-$.
  • The conjugate base of $H_2O$ is $OH^-$.
  • The conjugate base of $HSO_3{ }^{-}$ is $SO_3{ }^{2-}$.
  • Yes, a conjugate base can be a strong base.
  • Conjugate bases can affect acid-base equilibria by accepting protons (H+ ions) and forming the original acid.