Answer
(a) Acid; $CNO^-$
(b) Base; $HOBr$
(c) Acid; $Cl{O_3}^-$
(d) Acid; $CH_3NH_2$
(e) Base; $ClN{H_3}^+$
(f) Base; $HON{H_3}^+$
Work Step by Step
1. Identifying if the compound is an acid or a base:
(a) Normally, when we have a "H" as the first element to be represented in a formula, this compound is an acid. (Unless there is another group that indicates basicity).
(b) This compound doesn't have a hydrogen, so it can't be an acid, but it has lone pairs in the hydrogen, which indicates basicity.
(c) Same as (a)
(d) The $-N{H_3}^+$ group is an acidity indicator.
(e) The $-N{H_2}$ group is a basicity indicator.
(f) Here, the rule in (a) doesn't apply, because we have $-NH_2$, which indicates basicity.
2. To get the conjugate base of an acid, remove one proton from its formula:
- Remove one hydrogen:
Ex: $HCNO -- \gt CNO$
- Subtract one from the charge:
Ex: $CNO -- \gt CNO^-$
3.To get the conjugate acid of a base, remove one proton from its formula:
- Add one hydrogen
Ex: $OBr^- --\gt HOBr^-$
- Add one to its charge:
Ex: $HOBr^- --\gt HOBr$
