Write complete ionic and net ionic equations for each of the following reactions. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

(a) K2S (aq) + CoCl2 (aq) ? 2 KCl (aq) + CoS (s)

complete ionic equation?

complete net ionic equation?

(b) H2SO4 (aq) + CaCO3 (s) ? H2O (l) + CO2 (g) + CaSO4 (s)

complete ionic equation?

complete net ionic equation?

(c) 2 HClO (aq) + Ca (OH) 2 (aq) ? 2 H2O (l) + Ca (ClO) 2 (aq)

complete ionic equation?

complete net ionic equation?

a) Complete ionic equation:

2K⁺ (aq) + S⁻² (aq) + Co⁺² (aq) + 2Cl⁻ (aq) → 2K⁺ (aq) + 2Cl⁻ (aq) + CoS (s)

Complete net ionic equation:

S⁻² (aq) + Co⁺² (aq) → CoS (s)

b) Complete ionic equation:

H⁺ (aq) + SO₄⁻² (aq) + CaCO₃ (s) → H₂O (l) + CO₂ (g) + CaSO₄ (s)

Complete net ionic eqution:

H⁺ (aq) + SO₄⁻² (aq) + CaCO₃ (s) → H₂O (l) + CO₂ (g) + CaSO₄ (s)

c) Complete ionic equation:

2H⁺ (aq) + 2ClO⁻ (aq) + Ca⁺² (aq) + 2OH⁻ (aq) → 2H₂O (l) + Ca⁺² (aq) + 2ClO⁻ (aq)

Complete net ionic equation:

2H⁺ (aq) + 2OH⁻ (aq) → 2H₂O (l)

Explanation:

Ionic compounds are formed by two ions: a cation (with a positive charge), and an anion (negative charge). They're solid in ambient conditions and have high solubilities in water. When in aqueous solution, the ionic compound dissolves to its ions, this is the reason that the solution can conduct electricity.

The ionic equation represents the ions instead of the substances, and the net ionic equation represents only the ions that participate in the reaction. It means that if the same ion is present on both sides of the equation with the same amount, it is an intermediary and will be canceled. So, the ionic substance that is soluble will not be formed, only the ions will be present in the solution.

a) The ions are:

K2S = K⁺ (K is from group 1), S⁻² (S is from group 16)

CoCl₂ = Co⁺² (Co is from group 2), Cl⁻ (Cl is from group 17)

KCl = K⁺, Cl⁻

CoS = is solid, so it will not dissociate in ions.

Complete ionic equation:

2K⁺ (aq) + S⁻² (aq) + Co⁺² (aq) + 2Cl⁻ (aq) → 2K⁺ (aq) + 2Cl⁻ (aq) + CoS (s)

Complete net ionic equation:

S⁻² (aq) + Co⁺² (aq) → CoS (s)

b) The ions are:

H₂SO₄ = H⁺, SO₄⁻²

CaCO₃ = is solid, so doesn't form ions

H₂O = is the solvent, s doesn't dissociate

CO₂ = the gas will not dissociate either

CaSO₄ = is solid, so doesn't form ions

Complete ionic equation:

H⁺ (aq) + SO₄⁻² (aq) + CaCO₃ (s) → H₂O (l) + CO₂ (g) + CaSO₄ (s)

Complete net ionic eqution:

H⁺ (aq) + SO₄⁻² (aq) + CaCO₃ (s) → H₂O (l) + CO₂ (g) + CaSO₄ (s)

c) The ions are:

HClO = H⁺, ClO⁻

Ca (OH) ₂ = Ca⁺², OH⁻

H₂O = is the solvent and doesn't dissociate

Ca (ClO) ₂ = Ca⁺², ClO⁻

Complete ionic equation:

2H⁺ (aq) + 2ClO⁻ (aq) + Ca⁺² (aq) + 2OH⁻ (aq) → 2H₂O (l) + Ca⁺² (aq) + 2ClO⁻ (aq)

Complete net ionic equation:

2H⁺ (aq) + 2OH⁻ (aq) → 2H₂O (l)