Match the following, regarding nature of the oxides

List-I		List-II
(A)	H20	(I)	Basic
(B)	Na2O	(II)	Amphoteric
(C)	ZnO	(III)	Acidic
(D)	SO3	(IV)	Netural

We are given two lists. List‑I contains four oxides and List‑II describes four possible natures of oxides:

List‑I
(A) H₂O  (B) Na₂O  (C) ZnO  (D) SO₃

List‑II
(I) Basic  (II) Amphoteric  (III) Acidic  (IV) Neutral

To match each oxide with its correct nature we analyse them one by one.

1. Water (H₂O)
Water does not behave as a typical acid or base in its pure form. It undergoes self‑ionisation (2 H₂O ⇌ H₃O⁺ + OH⁻) but the concentrations of H⁺ and OH⁻ are equal, giving a neutral pH of 7. Hence H₂O is classified as a neutral oxide.
→ matches (IV).

2. Sodium oxide (Na₂O)
Na₂O reacts vigorously with water: Na₂O + H₂O → 2 NaOH. The product NaOH is a strong base, indicating that Na₂O is a basic oxide.
→ matches (I).

3. Zinc oxide (ZnO)
ZnO shows dual behaviour:
– With acids it forms salts, e.g., ZnO + 2 HCl → ZnCl₂ + H₂O.
– With strong bases it forms zincate ions, e.g., ZnO + 2 NaOH + H₂O → Na₂[Zn(OH)₄].
Because it reacts both as an acid and as a base, ZnO is classified as an amphoteric oxide.
→ matches (II).

4. Sulfur trioxide (SO₃)
SO₃ reacts with water to give a strong acid: SO₃ + H₂O → H₂SO₄. The resulting sulfuric acid is a strong mineral acid, so SO₃ is an acidic oxide.
→ matches (III).

Putting the matches together we obtain the final correspondence:

A → (IV)  B → (I)  C → (II)  D → (III)