Question

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5. Which statement correctly describes HSO4- in the reaction represented by this equation?
HSO4- (aq) + H₂O(n) = H₂SO4(ng) + OH(aq)

* HSO4- is acting as a Brønsted-Lowry base because it is accepting a proton.

* HSO4- is acting as a Brønsted-Lowry acid because it is accepting a proton.

* HSO4- is acting as a Brønsted-Lowry acid because it is donating a proton.

* HSO4- is acting as a Brønsted-Lowry base because it is donating a proton.

Answer 1

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.