Final answer:
The amphiprotic species among the given options are HCO₃⁻ (bicarbonate) and H₂O (water). They can both donate and accept protons, exemplifying their amphiprotic nature, unlike HNO₃ and HCl which are strong acids and not amphiprotic.
Step-by-step explanation:
Amphiprotic species are substances that can either donate a proton (H+) in a reaction and act as a Brønsted-Lowry acid, or accept a proton and act as a Brønsted-Lowry base. Amphiprotic behavior is an essential characteristic of substances that are involved in buffer solutions. Water (H₂O) and bicarbonate (HCO₃⁻) are two common examples of amphiprotic species.
Of the options provided (a) HCO₃⁻, (b) H₂O, (c) HNO₃, and (d) HCl, both (a) HCO₃⁻ and (b) H₂O are amphiprotic. Hydrochloric acid (HCl) and nitric acid (HNO₃) are not amphiprotic, they are strong acids that only donate protons.
HCO₃⁻ can act as an acid: HCO₃⁻(aq) + OH⁻(aq) → CO₃²⁻(aq) + H₂O(l), and as a base: HCO₃⁻(aq) + H⁺(aq) → H₂CO₃(aq) + Cl⁻(aq). Water is also amphiprotic; as an acid: H₂O(l) + NH₃(aq) → NH₄⁺(aq) + OH⁻(aq), and as a base: H₂O(l) + HCl(aq) → H₃O⁺(aq) + Cl⁻(aq).