Which reaction best illustrates the behavior of the weak base H₂PO₄^- in aqueous solution? A)H₂PO₄^- (aq)+ H₂O (l) HPO₄^2- (aq)+ H₃O⁺ (aq) B)H₂PO₄^- (aq)+ H₂O (l) H₃PO₄(aq)+ OH^- (aq) C)H₂PO₄^- (aq) 2H⁺ (aq)+ PO₄^3- (aq) D)H₂PO₄^- (aq) H⁺ (aq)+ HPO₄^2- (aq) E)H₂PO₄^- (aq)+ H⁺ (aq) H₃PO₄(aq)

Question

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The weak base H₂PO₄^- can accept a proton (H+) to form its conjugate acid, H₃PO₄ (as shown in the reaction), indicating that it acts as a Bronsted-Lowry base in aqueous solution. Choices A, C, D, and E either do not involve any proton transfer or do not accurately represent the behavior of the weak base in aqueous solution.

Which Reaction Best Illustrates the Behavior of the Weak Base