Write down the molecular equation with the correct formulas and states of each substance. In this case, we already have it: Na₂CO₃(s) + H₂SO₃(aq) → Na₂SO₃(aq) + H₂O(l) + CO₂(g)
Balance the molecular equation by adding coefficients if needed to make sure that the number of atoms of each element is the same on both sides of the equation. In this case, the molecular equation is already balanced: Na₂CO₃(s) + H₂SO₃(aq) → Na₂SO₃(aq) + H₂O(l) + CO₂(g)
Write down the total ionic equation by breaking down all the soluble compounds into their ions and indicating their charges and states. Soluble compounds are those that dissolve in water and form aqueous solutions. You can use a solubility table or rules to determine which compounds are soluble or insoluble. In this case, we have two soluble compounds: H₂SO₃(aq) and Na₂SO₃(aq). We can break them down into their ions as follows: H₂SO₃(aq) → 2H⁺(aq) + SO₃²⁻(aq), Na₂SO₃(aq) → 2Na⁺(aq) + SO₃²⁻(aq). The other compounds are insoluble and remain as molecules: Na₂CO₃(s), H₂O(l), CO₂(g). The total ionic equation is: Na₂CO₃(s) + 2H⁺(aq) + SO₃²⁻(aq) → 2Na⁺(aq) + SO₃²⁻(aq) + H₂O(l) + CO₂(g)
Write down the net ionic equation by canceling out any spectator ions that appear on both sides of the equation. Spectator ions are those that do not change or participate in the reaction. In this case, we have two spectator ions: Na⁺(aq) and SO₃²⁻(aq). We can cancel them out from both sides of the equation. The net ionic equation is: Na₂CO₃(s) + 2H⁺(aq) → H₂O(l) + CO₂(g)