Answer
Acid: $H_2{PO_4}^-$; Its conjugate base: $HP{O_4}^{2-}$
Acid: $H_2$; Its conjugate base: $H^-$
Acid: $HS{O_3}^-$; Its conjugate base: $S{O_3}^{2-}$
Acid: $HF$; Its conjugate base: $F^-$
Base: $P{O_4}^{3-}$; Its conjugate acid: $HP{O_4}^{2-}$
Base: $N{H_2}^-$; Its conjugate acid: $NH_3$
Base: $Cl{O_4}^-$; Its conjugate acid: $HClO_4$
Base: $Br^-$; Its conjugate acid: $HBr$
Work Step by Step
- These are conjugate acid-base pairs, so:
1. To go from acid to conjugate base (Or conjugate acid to base):
Remove one $(H^+)$;
- Remove one hydrogen, and subtract one from the charge:
Examples:
$H_2P{O_4}^- --\gt HP{O_4}^- -- \gt HP{O_4}^{2-}$
$HBr --\gt Br --\gt Br^-$
2. To go from base to conjugate acid (Or conjugate base to acid):
Add one $(H^+)$;
- Add one hydrogen, and sum one to the charge:
Examples:
$H^- --\gt {H_2}^- --\gt H_2$
$Cl{O_4}^- --\gt HCl{O_4}^- --\gt HClO_4$
