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    Determining net ionic equation of a reaction

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    HINT: Aqueous ionic compounds exist as ions in solution. Start by writing the reactants as individual aqueous ions. Then use the solubility rules (https://sites.google.com/site/chempendix/solubility-chart) to identify any precipitates. Be sure to include phases and charges as necessary in your answer!

    Start by writing the reactants as individual aqueous ions.

    Ag^+ (aq)+NO^- 3(aq)+Ba^2+(aq)+OH^-(aq)
    ^ This three is a sub 3.

    It is acceptable to ignore coefficients for now, then balance at the very end. Next, check the solubilities (https://sites.google.com/site/chempendix/solubility-chart) of silver hydroxide and barium nitrate. Soluble products should be written as individual aqueous ions. Insoluble products should be written as solid compounds. Finally, cancel out species that appear on both sides of the equation.

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    Solution Preview

    Complete Molecular Equation:

    2AgNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2AgOH(s)

    (Note: Referring to the Solubility Rules, Ba(NO3)2 is soluble while AgOH is insoluble. Hence, the latter (AgOH) is the precipitate).

    Complete Ionic Equation:

    2Ag+(aq) + 2NO3-(aq) + Ba+2(aq) + 2OH-(aq) → Ba+2(aq) + 2NO3-(aq) + 2AgOH(s)

    To get the net ionic, cancel out common species ...

    Solution Summary

    The expert determines net ionic equations of a reaction.