A solution prepared by stirring Na2O(s) in water undergoes an acid-base reaction with a solution prepared from SO2(g) and water - VCE - SSCE Chemistry - Question 4 - 2007 - Paper 1

To determine which salt can be isolated from the acid-base reaction between Na2O and SO2, we first identify the products formed in the reaction.

When Na2O dissolves in water, it forms sodium hydroxide (NaOH), which is a strong base. On the other hand, SO2 in water typically leads to the formation of sulfurous acid (H2SO3), which partially dissociates into bisulfite (HSO3-) and sulfite ions (SO3^2-).

The reaction can be summarized as:

$2 ext{NaOH} + ext{H}_2 ext{SO}_3 \rightarrow ext{Na}_2 ext{SO}_3 + 2 ext{H}_2 ext{O}$

However, in the presence of excess oxygen or under different conditions, H2SO4 may also form, leading to:

$2 ext{NaOH} + ext{H}_2 ext{SO}_4 \rightarrow ext{Na}_2 ext{SO}_4 + 2 ext{H}_2 ext{O}$

Thus, the main salts that could potentially be produced are sodium sulfite (Na2SO3) and sodium sulfate (Na2SO4).

Given that Na2SO4 is listed in the options and is a typical product when strong base reacts with strong acids like H2SO4, the answer is:

D. Na2SO4.