H₂PO₄⁻ donates a proton (H⁺) to H₂O in the reaction H₂PO₄⁻ + H₂O ⇌ H₃O⁺ + HPO₄²⁻. This exemplifies H₂PO₄⁻'samphoteric nature, as it acts as an acid and transfers a proton to H₂O, resulting in H₃O⁺ and HPO₄²⁻ species.By examine thereactionwhere H₂PO₄⁻ acts as an acid and donates a proton (H⁺) to H₂O, which acts as a base:The balanced chemical equation is:H₂PO₄⁻ + H₂O ⇌ H₃O⁺ + HPO₄²⁻Here's a step-by-step breakdown of the reaction:1.Initial state:- H₂PO₄⁻: Dihydrogen phosphate ion (acting as an acid)- H₂O: Water (acting as a base)2.Dihydrogen Phosphate Ion(H₂PO₄⁻) as an Acid:Dihydrogen phosphate ion donates a proton (H⁺) to water, which acts as a base. This proton transfer leads to the formation of a hydronium ion and the hydrogen phosphate ion.H₂PO₄⁻ + H₂O ⇌ H₃O⁺ + HPO₄²⁻- H₂PO₄⁻ loses a proton (H⁺) to become HPO₄²⁻.- H₂O gains a proton (H⁺) to become H₃O⁺ (hydronium ion).3.Resulting Species:- HPO₄²⁻: Hydrogen phosphate ion (conjugate base of H₂PO₄⁻)- H₃O⁺: Hydronium ion (conjugate acid of H₂O)In this reaction, H₂PO₄⁻ donates a proton (acts as an acid) to H₂O, which accepts theproton(acts as a base). This behavior demonstrates the amphoteric nature of H₂PO₄⁻, as it can both donate and accept protons depending on the context.To know more aboutamphoteric naturerefer here :brainly.com/question/32552952##SPJ11Complete question :1. HC₆H₅O(aq) is an Arrhenius acid because it donates a proton (H⁺) to water. The chemical equation for this reaction is:2. Both H₂O and H₂PO₄⁻ are amphoteric, which means that they can act as both acids and bases.a) Write an equation to show how H₂PO₄⁻ can act as an acid with H₂O acting as a base....

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