Explain why, an aqueous solution of sodium sulphate is neutral while an aqueous solution of sodium carbonate is basic in nature.

An aqueous solution of sodium sulphate ($Na_2SO_4$) is neutral because it is a salt formed by the neutralization of a strong acid, sulphuric acid ($H_2SO_4$), and a strong base, sodium hydroxide ($NaOH$). Since both the parent acid and parent base are strong, the salt does not undergo hydrolysis and the solution remains neutral with a $\text{pH}$ of $7$.

An aqueous solution of sodium carbonate ($Na_2CO_3$) is basic because it is a salt formed by the reaction of a strong base ($NaOH$) and a weak acid, carbonic acid ($H_2CO_3$). In an aqueous solution, the carbonate ion undergoes hydrolysis to produce hydroxide ions ($OH^-$), which increases the concentration of $OH^-$ ions, making the solution basic ($\text{pH} > 7$):

$$Na_2CO_3(s) + 2H_2O(l) \rightarrow 2Na^+(aq) + 2OH^-(aq) + H_2CO_3(aq)$$