Answer
$H_2SO_3(aq) + H_2O(l) \lt -- \gt HS{O_3}^-(aq) + H_3O^+(aq)$
$H{SO_3}^-(aq) + H_2O(l) \lt -- \gt S{O_3}^{2-}(aq) + H_3O^+(aq)$
Work Step by Step
1. Identify if the compound is a polyprotic acid or base:
- $H_2SO_3$ is an acid.
2. Write the ionization equation for the original acid.
- Write an equation where $H_2SO_3$ donates a proton to a water molecule.
3. Now, for polyprotic acids, the conjugate base is capable of donating one proton too, so write an equation where it does that.
- $HS{O_3}^-$ can act as an acid too, so write an equation where it donates a proton to a water molecule.
- Repeat "Step 3" for the next reaction, until the conjugate base is incapable of donating one proton.