Answer:
1. H⁺ (aq) + NO₃⁻ (aq) + Na⁺ (aq) + OH⁻ (aq) → Na⁺ (aq) + NO₃⁻ (aq) + H₂O (l)
2. H⁺ (aq) + Cl⁻ (aq) + K⁺ (aq) + OH⁻ (aq) → K⁺ (aq) + Cl⁻ (aq) + H₂O (l)
3. 2H⁺ (aq) + SO₄²⁻ (aq) + Mg²⁺ (aq) + 2OH⁻ (aq) → Mg²⁺ (aq) + SO₄²⁻ (aq) + 2H₂O (l)
Explanation:
The ionic equation is an equation illustrating all the ions occurring in a reaction individually;
This is similar but can differ from the normal equation, because, typically, certain compounds consist of ions that dissociate in aqueous phase;
Net ionic equations can be found by eliminating all ions that remain the same, i.e. do not change state, which are known as spectator ions;
1. H⁺ (aq) + NO₃⁻ (aq) + Na⁺ (aq) + OH⁻ (aq) → Na⁺ (aq) + NO₃⁻ (aq) + H₂O (l)
Net: H⁺ (aq) + OH⁻ (aq) → H₂O (l)
NO₃⁻ ions are aqueous prior to the reaction and remain aqueous afterwards;
Similarly, the Na⁺ ions also remain aqueous;
The H⁺ and OH⁻, however, are aqueous (free ions in the solution) before the reaction;
After the reaction, these become the compound H₂O, a liquid so they do change state
2. H⁺ (aq) + Cl⁻ (aq) + K⁺ (aq) + OH⁻ (aq) → K⁺ (aq) + Cl⁻ (aq) + H₂O (l)
Net: H⁺ (aq) + OH⁻ (aq) → H₂O (l)
3. 2H⁺ (aq) + SO₄²⁻ (aq) + Mg²⁺ (aq) + 2OH⁻ (aq) → Mg²⁺ (aq) + SO₄²⁻ (aq) + 2H₂O (l)
Net: 2H⁺ (aq) + 2OH⁻ (aq) → 2H₂O (l)
