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Barium hypochlorite and perchloric acid net ionic equation.

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This problem asks for the net ionic equation between barium hypochlorite and perchloric acid. The answer then turns out to be  [tex]ClO^-(aq)+H^+(aq)\rightleftharpoons HClO(aq)[/tex].

Net ionic equations

In chemistry, when a chemical reaction takes place, one can study three versions of the chemical equation representing it:

1. Complete molecular equation: shows all the substances, their phases of matter and every balanced atom. In this case, one can write:

[tex]Ba(ClO)_2(aq)+2HClO_4(aq)\rightarrow 2HClO(aq)+Ba(ClO_4)_2(aq)[/tex]

2. Complete ionic equation: shows all the aqueous salts and strong both acids and bases split into cation and anion; however, weak both acids and bases, such as the hypochlorous acid here, remain unionized as well as solid precipitates, liquids or gases:

[tex]Ba^{2+}(aq)+2(ClO)^-(aq)+2H^+(aq)+2(ClO_4)^-(aq)\rightarrow 2HClO(aq)+Ba^{2+}(aq)+2(ClO_4)^-(aq)[/tex]

3. Net ionic equation: cancels out the spectator ions (those equal on both reactants and products) and shows the relevant ions that undergo a reaction. In this case, both perchlorate and barium ions act as the spectator ones, consequently, we obtain:

[tex]2(ClO)^-(aq)+2H^+(aq)\rightarrow 2HClO(aq)\\\\(ClO)^-(aq)+H^+(aq)\rightarrow HClO(aq)[/tex]

That can also be written at equilibrium due to the concept of weak acid for the formation of hypochlorous acid:

[tex]ClO^-(aq)+H^+(aq)\rightleftharpoons HClO(aq)[/tex]

Learn more about spectator ions: https://brainly.com/question/15365313

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