Respuesta :
Explanation:
An equation is said to be balanced when the number of atoms on both reactant and product side are equal in number.
Whereas an equation where electrolytes in an aqueous solution are represented as dissociated ions is known as an ionic equation.
For example, [tex]HCl(aq) + LiOH(aq) \rightarrow H_{2}O(l) + LiCl(aq)[/tex] can be represented in ionic form as follows.
[tex]H^{+} + Cl^{-} + Li^{+} + OH^{-} \rightarrow H_{2}O(l) + Li^{+} + Cl^{-}[/tex]
Now, cancelling the common ions present on both sides of the equation. The resulting, ionic equation will be as follows.
[tex]H^{+} + OH^{-} \rightarrow H_{2}O(l)[/tex]
The balanced complete ionic equation is
[tex]{{\text{H}}^ + }\left({aq}\right)+{\text{C}}{{\text{l}}^ - }\left( {aq}\right)+{\text{L}}{{\text{i}}^ + }\left({aq}\right)+{\text{O}}{{\text{H}}^ - }\left({aq} \right)\to{{\text{H}}_2}{\text{O}}\left( l \right)+{\text{L}}{{\text{i}}^ + }\left({aq}\right)+{\text{C}}{{\text{l}}^ - }\left({aq}\right)[/tex]
Further Explanation:
The three types of equations that are used to represent the chemical reaction are as follows:
1. Molecular equation
2. Total ionic equation
3. Net ionic equation
The reactants and products remain in undissociated form in the molecular equation. In the case of total ionic equation, all the ions that are dissociated and present in the reaction mixture are represented while in the case of net or overall ionic equation only the useful ions that participate in the reaction are represented.
The steps to write the complete or total ionic reaction are as follows:
Step 1: Write the molecular equation for the reaction with the phases in the bracket.
In the reaction, HCl reacts with LiOH to form LiCl and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] . The balanced molecular equation of the reaction is as follows:
[tex]{\text{HCl}}\left({aq}\right)+{\text{LiOH}}\left({aq}\right)\to{{\text{H}}_{\text{2}}}{\text{O}}\left( l \right)+{\text{LiCl}}\left( {aq}\right)[/tex]
Step 2: Dissociate all the compounds with the aqueous phase to write the total ionic equation. The compounds with solid and liquid phases remain same. The total ionic equation is as follows:
[tex]{{\text{H}}^ + }\left({aq}\right)+{\text{C}}{{\text{l}}^ - }\left({aq}\right)+{\text{L}}{{\text{i}}^ + }\left({aq}\right)+{\text{O}}{{\text{H}}^ - }\left({aq}\right)\to{{\text{H}}_2}{\text{O}}\left( l \right)+{\text{L}}{{\text{i}}^ + }\left({aq}\right)+{\text{C}}{{\text{l}}^ - }\left({aq}\right)[/tex]
Therefore, the complete ionic equation obtained is as follows:
[tex]{{\text{H}}^ + }\left({aq}\right)+{\text{C}}{{\text{l}}^ - }\left({aq}\right)+{\text{L}}{{\text{i}}^ + }\left({aq}\right)+{\text{O}}{{\text{H}}^ - }\left({aq}\right)\to{{\text{H}}_2}{\text{O}}\left( l \right)+{\text{L}}{{\text{i}}^ + }\left({aq}\right)+{\text{C}}{{\text{l}}^ - }\left({aq}\right)[/tex]
Learn more:
1. Balanced chemical equation: https://brainly.com/question/1405182
2. Oxidation and reduction reaction: https://brainly.com/question/2973661
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Chemical reaction and equation
Keywords: net ionic equation, complete ionic equation, Li+, OH-, Cl-, LiCl, HCl, H2O, LiOH, solid phase, liquid phase, aqueous phase.
