The species: $H_{2}O$,$HCO_{3}^{-}$,$HSO_{4}^{-}$,and $NH_{3}$ can act both as Bronsted acids and bases. For each case,give the corresponding conjugate acid and conjugate base.

$A$ Bronsted acid is a proton $(H^{+})$ donor,and a Bronsted base is a proton $(H^{+})$ acceptor. The conjugate acid is formed by adding a proton to the species,while the conjugate base is formed by removing a proton from the species. The results are summarized in the table below:

Species	Conjugate Acid	Conjugate Base
$H_{2}O$	$H_{3}O^{+}$	$OH^{-}$
$HCO_{3}^{-}$	$H_{2}CO_{3}$	$CO_{3}^{2-}$
$HSO_{4}^{-}$	$H_{2}SO_{4}$	$SO_{4}^{2-}$
$NH_{3}$	$NH_{4}^{+}$	$NH_{2}^{-}$