Final answer:
The net ionic equations demonstrating the Brønsted-Lowry base character are:
b) H₂O + H⁺ ⟶ H₃O⁺
c) HCO₃⁻ + H₂O ⟶ CO₃²⁻ + H₃O⁺
Step-by-step explanation:
Brønsted-Lowry theory defines acids as proton (H⁺) donors and bases as proton acceptors. In the given net ionic equations, the species accepting protons showcase the Brønsted-Lowry base character.
Equation b) illustrates the self-ionization of water, where water (H₂O) accepts a proton (H⁺) to form the hydronium ion (H₃O⁺). This reaction signifies water acting as a base by accepting a proton.
Equation c) involves the bicarbonate ion (HCO₃⁻) accepting a proton from water to form the carbonate ion (CO₃²⁻) and hydronium ion (H₃O⁺). This equation also highlights the base behavior of HCO₃⁻ as it accepts a proton.
Conversely, equations a) and d) do not exhibit base behavior. Equation a) portrays the dissociation of nitric acid (HNO₃) into its ions but does not show a species accepting a proton. Equation d) involves the transfer of an electron (e⁻) in a redox reaction, not demonstrating a base character.
Therefore, equations b) and c) demonstrate the Brønsted-Lowry base behavior as they involve the acceptance of protons by water and bicarbonate ions, respectively. These reactions exemplify the fundamental principle of Brønsted-Lowry theory by showcasing proton acceptance, characterizing the behavior of bases in these chemical reactions.