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 base.

(N/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 $(H^{+})$ to the species,while the conjugate base is formed by removing a proton $(H^{+})$ from the species.

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