Question

What is the conjugate base of $HCO_3^ -$ and ${H_2}O$ ?

Answer 1

In inorganic chemistry, bicarbonate is a type of carbonic acid that is deprotonated. It has the chemical formula $HCO_3^ -$ and is a polyatomic anion. The chemical formula for water is ${H_2}O$ .

Complete answer:
Conjugate acids and conjugate bases are included in the Bronsted-Lowry acid-base theory. The basic idea behind this theory is that when an acid and a base react, the acid forms its conjugate base, and the base forms its conjugate acid through proton exchange. The Arrhenius theory is a generalization of this theory.
In water, an acid loses a hydrogen ion when it dissociates into its ions. The conjugate base of acid is the species that is produced.
A conjugate acid and a conjugate base undergo the following chemical reaction:
$HX + {H_2}O \leftrightarrow {X^ - } + {H_3}{O^ + }$
Since the conjugate base is an anion, it can be identified in an acid-base reaction.
A more general definition is that the base member, ${X^ - }$ , of a pair of compounds that turn into each other by losing or gaining a proton is a conjugate base.
So, now we know that when an acid loses a hydrogen ion, the conjugate base is formed. As a result, the conjugate base of any compound is the compound after ${H^ + }$ has been removed from it.
${\left( {C{O_3}} \right)^{2 - }}$ is the conjugate base of the acid $HCO_3^ -$ .
The conjugate basis of ${H_2}O$ is $O{H^ - }$ .

Note:
The Bronsted-Lowry theory of acids and bases includes conjugate acids and bases. Remember that when an acid loses one of its hydrogen ions, a conjugate base is formed. An anion can be recognized as the conjugate base.