Problem 16.20

Designate the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of each equation, and also designate the conjugate acid and base on the right side:

(a) HBrO(aq) + H₂O(l) = H₃O⁺(aq) + BrO^-(aq)

Here, water accepts a proton from HBrO ; water is the Bronsted base, and HBrO the Bronsted acid on the left. Water accepts a proton to form hydronium ion (H₃O⁺, which is the Bronsted acid on the right, and hypobromous acid loses a proton to form hypobromite ion, which is the Bronsted base on the right.

(b)HSO₄^-(aq) + HCO₃^-(aq) = SO₄^-2(aq) + H₂CO₃(aq)

Notice that the hydrogen sulfate ion donates the proton to the bicarbonate ion on the left; hence, the acid is HSO₄^-(aq), and the base (the proton acceptor) is HCO₃^-(aq). The conjugate acid is carbonic (H₂CO₃(aq)) and the conjugate base is the sulfate ion.

(c)HSO₃^-(aq) + H₃O⁺(aq) = H₂SO₃(aq) + H₂O(l)

The proton donor (the acid) is the hydronium ion ( H₃O⁺(aq)), and the base (the proton acceptor) is HSO₃^-(aq). The conjugate acid is H₂SO₃(aq), and the conjugate base of hydronium ion is water. .