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18 February, 23:21

What is the correct net ionic equation, including all coefficients, charges, and phases, 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.

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  1. 19 February, 02:12
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    Ba^2 + (aq) + 2OH - (aq) + 2H + (aq) + SO4^2 - (aq) → BaSO4 (s) + 2H2O (l)

    Explanation:

    Step 1: Data given

    the contribution of protons from H2SO4 is near 100 %.

    Step 2: The unbalanced equation

    . Ba (OH) 2 (aq) + H2SO4 (aq) → BaSO4 (s) + H2O (l)

    Step 3: Balancing the equation

    On the left side we have 4x H (2x in Ba (OH) 2 and 2x in H2SO4). On the right side, we have 2x H (in H2O).

    To balance the amount of H on both sides, we have to muliply H2O (on the right side) by 2.

    Ba (OH) 2 (aq) + H2SO4 (aq) → BaSO4 (s) + 2H2O (l)

    Step 4: The net ionic equation

    The net ionic equation, for which spectator ions are omitted - remember that spectator ions are those ions located on both sides of the equation - will.

    Ba^2 + (aq) + 2OH - (aq) + 2H + (aq) + SO4^2 - (aq) → BaSO4 (s) + 2H2O (l)

    After canceling those spectator ions in both side, look like this:

    Ba^2 + (aq) + 2OH - (aq) + 2H + (aq) + SO4^2 - (aq) → BaSO4 (s) + 2H2O (l)
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