Including all coefficients, charges, and phases, what is the correct net ionic equation for the following set of reactants? Assume that the contribution of protons from H2SO4 is near 100%. Ba (OH) 2 (aq) + H2SO4 (aq)

Express your answer as a chemical equation.

Answer: Ba²⁺ (aq) + 2OH⁻ (aq) + 2H⁺ (aq) + SO4²⁻ (aq) - - > BaSO₄ (s) + H₂O (l)

Explanation:

1) Start by writing the molecular chemical equation:

Ba (OH) ₂ (aq) + H₂SO4 (aq) - - > BaSO₄ + 2H₂O

2) Identify the kind of equation:

It is an acid base neutralization: double replacement reaction.

3) Identity the ions that dissociate from each reactant and its phases:

Ba (OH) ₂ (aq) - - - > Ba (²⁺ (aq) + 2OH⁻ (aq)

H₂SO₄ (aq) - - - > 2H⁺ (aq) + SO₄²⁻ (aq)

4) Ideintify the phases of the products:

BaSO₄ is a solid: BaSO₄ (s)

H₂O is liquid: H₂O (l)

5) Write the total ionic equation:

Ba²⁺ (aq) + 2OH⁻ (aq) + 2H⁺ (aq) + SO₄²⁻ (aq) - - > BaSO₄ (s) + H₂O (l)

6) Eliminate the spectator ions (those that are repeated in the reactant and product sides). Here there are not spectator ions, so the net ionic equation is the same total ionic equation.

Ba²⁺ (aq) + 2OH⁻ (aq) + 2H⁺ (aq) + SO4²⁻ (aq) - - > BaSO₄ (s) + H₂O (l)