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Chemical reactions that focus on the interactions of ions are referred to as the ionic equations. They are typically found in solutions and explain the precipitation of the compounds within the solutions. However, certain ions (specifically called spectator ions) aren’t involved during the process of precipitation. This is why it is important to explain these reactions by using net Ionic Equations.
The steps involved in writing an equation for the net Ionic can be listed in the following paragraphs:
I) Write and then balance the molecular equation that describes the reaction, incorporating the chemical components for each of them.
II) Dissociate the electrolytes that are strong (usually the aqueous compounds) into the ions that they are derived from. Except for those that are strong electrolytes, non-aqueous compounds cannot be dissociated into the ions.
II) Eliminate the spectator ions. They are the ones which are present on both directions of the equation.
IV) Add the remaining elements and ions in order to create the net Ionic Equation.
The net ionic equation shows the only chemical species that were involved in the reaction. According to the solubility rule strong electrolytes can dissolve completely in an aqueous solution. A balanced chemical equation is required to create the net ionic equation.
* Solubility – Solubility refers to the ability of a substance to dissolve in a solvent. Strong acids and bases are able to dissociate completely, forming ions. Aqueous substances only can be dissociated into ions.
* The balance chemical equation: Mass is not created nor destroyed according to the law on conservation of mass. This means that the product and reactant sides should have the same number of atoms.
* Spectator Ions: Spectatorions are ions that can be found on both sides of a reaction equation. This means that both the reactant and product sides have the same ions.
The following balanced chemical equation is
[katex]{\rm{2HBr}}\left( {{\rm{aq}}} \right){\rm{ + Ba}}{\left( {{\rm{OH}}} \right)_{\rm{2}}}\left( {{\rm{aq}}} \right)\longrightarrow{{}}{\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right){\rm{ + BaB}}{{\rm{r}}_{\rm{2}}}\left( {{\rm{aq}}} \right)[/katex]
It is evident from the balance equation that barium hydroxide reacts to hydro bromic acid to create barium bromide, and water.
The ionic equation of the balanced chemical equation is
[katex]{\rm{2}}{{\rm{H}}^{\rm{ + }}}\left( {{\rm{aq}}} \right){\rm{ + 2B}}{{\rm{r}}^{\rm{ – }}}\left( {{\rm{aq}}} \right){\rm{ + B}}{{\rm{a}}^{{\rm{2 + }}}}\left( {{\rm{aq}}} \right){\rm{ + 2O}}{{\rm{H}}^{\rm{ – }}}\left( {{\rm{aq}}} \right)\longrightarrow{{}}{\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right){\rm{ + B}}{{\rm{a}}^{{\rm{2 + }}}}\left( {{\rm{aq}}} \right){\rm{ + 2B}}{{\rm{r}}^{\rm{ – }}}\left( {{\rm{aq}}} \right)[/katex]
The following balanced chemical equation is
[katex]{\rm{2HBr}}\left( {{\rm{aq}}} \right){\rm{ + Ba}}{\left( {{\rm{OH}}} \right)_{\rm{2}}}\left( {{\rm{aq}}} \right)\longrightarrow{{}}{\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right){\rm{ + BaB}}{{\rm{r}}_{\rm{2}}}\left( {{\rm{aq}}} \right)[/katex]
This reaction requires an ionic equation.
[katex]{\rm{2}}{{\rm{H}}^{\rm{ + }}}\left( {{\rm{aq}}} \right){\rm{ + 2B}}{{\rm{r}}^{\rm{ – }}}\left( {{\rm{aq}}} \right){\rm{ + B}}{{\rm{a}}^{{\rm{2 + }}}}\left( {{\rm{aq}}} \right){\rm{ + 2O}}{{\rm{H}}^{\rm{ – }}}\left( {{\rm{aq}}} \right)\longrightarrow{{}}{\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right){\rm{ + B}}{{\rm{a}}^{{\rm{2 + }}}}\left( {{\rm{aq}}} \right){\rm{ + 2B}}{{\rm{r}}^{\rm{ – }}}\left( {{\rm{aq}}} \right)[/katex]
The net ionic formula for the given balanced chemical equation is obtained by removing the spectator ions.
The net ionic equation can be summarized as follows:
[katex]\begin{array}{l}\\{\rm{2}}{{\rm{H}}^{\rm{ + }}}\left( {{\rm{aq}}} \right){\rm{ + 2O}}{{\rm{H}}^{\rm{ – }}}\left( {{\rm{aq}}} \right)\longrightarrow{{}}{\rm{2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right)\\\\\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\left( {{\rm{or}}} \right)\\\\{{\rm{H}}^{\rm{ + }}}\left( {{\rm{aq}}} \right){\rm{ + O}}{{\rm{H}}^{\rm{ – }}}\left( {{\rm{aq}}} \right)\longrightarrow{{}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right)\\\end{array}[/katex]
Answer:
The net ionic equation can be summarized as follows:
[katex]{{\rm{H}}^{\rm{ + }}}\left( {{\rm{aq}}} \right){\rm{ + O}}{{\rm{H}}^{\rm{ – }}}\left( {{\rm{aq}}} \right)\longrightarrow{{}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right)[/katex]