Brønsted-Lowry acid Question?
The reaction that does not show the reaction of H2PO4− as a Brønsted-Lowry acid is
a. HPO42− (aq) + H3O+(aq) ↔ H2PO4− (aq) + H2O(l)
b. H2PO4−(aq) + OH− (aq) ↔ HPO42− (aq) + H2O(l)
c. HPO42− (aq) + HClO3(aq) ↔ H2PO4−(aq) + ClO3−(aq)
d. H2PO4−(aq) + HF (aq) ↔ H3PO4(aq) + F −(aq)
e. HPO42− (aq) + NH4+(aq) ↔ H2PO4−(aq) + NH3(aq)
I think B is the only one that shows it as a base... So is the question just incorrect? thanks!
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d. H2PO4−(aq) + HF (aq) ↔ H3PO4(aq) + F −(aq)
b shows it acting as an acid. By the bronsted-lowry definition an acid donates a proton(hydrogen ion) to a base. In b the H2PO4- donates an H+ to the OH- which forms water H2O. In d we have H2PO4- accepting a hydrogen ion from HF to become H3PO4 and by the bronsted-lowry theory a substance that accepts a hydrogen ion is acting as a base so in d the H2PO4- is acting as a base.