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. .
Doug Chapman email@example.com 8/11/08