Answer:
The compounds HCO₃⁻ and OH⁻ are acting like a Brønsted-Lowry base and the compounds H₂C0₃ H₂0 are acting like a Brønsted-Lowry acid.
Explanation:
According to the Brønsted-Lowry theory an acid is any species capable of donating a proton (H⁺) and a base is any species capable of accepting a proton (H⁺)
The conjugate base of a Brønsted-Lowry acid is the species that is formed after the acid donates its proton and the conjugate acid of Brønsted-Lowry base is the species that is formed after the base accepts a proton.
For example:
H₂SO₄ + OH⁻ ⇆ HSO₄⁻ + H₂O
In this equilibrium H₂SO₄ is acting like a Brønsted-Lowry acid and HSO₄⁻ is its conjugate base. Also OH⁻ is acting like a Brønsted-Lowry base and H₂O is its conjugate acid
So, HCO₃⁻ is acting like a Brønsted-Lowry base and H₂C0₃ is its conjugate acid. Also H₂O is acting like a Brønsted-Lowry acid and OH⁻ is its conjugate base.
