Answer
$ Na_2CO_3(s) + H_2SO_4(aq) \longrightarrow CO_2(g) + H_2O(l) + Na_2SO_4(aq)$
Work Step by Step
1. Identify the type of Acid-Base reaction:
Since $Na_2CO_3$ has the $CO_3^{2-}$ ion, and it is reacting with an acid ($H_2SO_4$), this is a reaction between an acid and a carbonate.
$Acid + Carbonate \longrightarrow CO_2(g) + H_2O(l) + Salt$
2. Find the identity of the salt.
The $H_2SO_4$ will donate its $H^+$ ions (since it is an acid). "$SO_4^-$" will remain in solution.
The carbonate ion ($CO_3^{2-})$ will react, leaving two sodium ions ($Na^+$) alone.
Therefore, the produced salt is: $Na_2SO_4$.
3. Follow the pattern:
$H_2SO_4(aq) + Na_2CO_3(s) \longrightarrow CO_2(g) + H_2O(l) + Na_2SO_4(aq)$
- The equation is balanced.
