Answer:
HSO₄⁻ is acting as a Brønsted-Lowry base because it is accepting a proton.
What is the Brønsted-Lowry Theory?
The Bronsted-Lowry theory states that acids act as proton donors, and bases act as proton acceptors; protons meaning hydrogen ions, since they only have 1 proton. This theory can be applied to practically any solvent.
HSO₄⁻(aq) + H₂O(l) ⇒ H₂SO₄(aq) + OH⁻(aq)
In the above equation:
- the HSO₄⁻ accepts a proton from H₂O to form H₂SO₄
- the H₂O donates a proton to the HSO₄⁻ to form OH⁻
Thus, the HSO₄⁻ is an base, and the H₂O is a acid.
Therefore, HSO₄⁻ is acting as a Brønsted-Lowry base because it is accepting a proton.