What is the conjugate base of hso3−? express your answer as a chemical formula.
The Correct Answer and Explanation is:
The conjugate base of the bisulfite ion ((\text{HSO}_3^-)) is the sulfite ion, (\text{SO}_3^{2-}).
Explanation:
In acid-base chemistry, a conjugate base is the species that remains after an acid has donated a proton (H⁺). In this case, the bisulfite ion ((\text{HSO}_3^-)) can act as an acid, which means it has the potential to donate a proton to another molecule.
To understand this, consider the dissociation of bisulfite:
[
\text{HSO}_3^- \rightleftharpoons \text{H}^+ + \text{SO}_3^{2-}
]
Here’s the breakdown:
- Bisulfite Ion: The formula for bisulfite is (\text{HSO}_3^-). It contains one proton (H⁺) bound to the sulfite ion ((\text{SO}_3^{2-})).
- Conjugate Base: When (\text{HSO}_3^-) loses a proton (H⁺), the resulting species is the sulfite ion ((\text{SO}_3^{2-})). This is the conjugate base of bisulfite.
The key concept here is that the conjugate base is the particle that is left after an acid (such as (\text{HSO}_3^-)) donates a proton. Since (\text{HSO}_3^-) has a negative charge and contains a hydrogen atom, its conjugate base will have one less hydrogen, leading to the sulfite ion, which is also negatively charged, but has lost one proton.
Thus, the conjugate base of (\text{HSO}_3^-) is (\text{SO}_3^{2-}).
This principle is consistent with the Brønsted-Lowry theory of acids and bases, which defines acids as proton donors and bases as proton acceptors. In this case, (\text{HSO}_3^-) donates a proton to become (\text{SO}_3^{2-}).