Taking into account the Brønsted-Lowry acid-base theory, the conjugate acid of HCO₂⁻ is H₂CO₂.
Brønsted-Lowry acid-base
The Brønsted-Lowry acid-base theory (or the Brønsted-Lowry theory) identifies acids and bases based on whether the species accepts or donates protons or H⁺.
According to this theory, acids are proton donors while bases are proton acceptors. That is, an acid is a species that donates an H⁺ proton while a base is a chemical species that accepts an H⁺ proton from the acid.
So, reactions between acids and bases are H⁺ proton transfer reactions.
Conjugate base and conjugate acid
Then, a conjugate base is an ion or molecule resulting from the acid that loses the proton, while a conjugate acid is an ion or molecule resulting from the base that gains the proton:
acid + base ⇄ conjugate base + conjugate acid
Conjugate acid of HCO₂⁻
Like a conjugate acid is an ion or molecule resulting from the base that gains the proton, the conjugate acid of HCO₂⁻ is H₂CO₂.
Learn more about the Brønsted-Lowry acid-base theory:
brainly.com/question/12916250?referrer=searchResults
brainly.com/question/1191429?referrer=searchResults
brainly.com/question/4000152?referrer=searchResults
brainly.com/question/12808135?referrer=searchResults
