Chemistry, 30.07.2019 02:00 janiyahlanae66

Write a balanced complete ionic equation for: hi(aq)+rboh(aq)→

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Answer from: jasmine3051

The complete ionic equation for the reaction is as follows:

$\boxed{{{\mathbf{H}}^ + }\left( q \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right) + {\mathbf{O}}{{\mathbf{H}}^ - }\left( {aq} \right) \to {{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}\left( l \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right)}$

Further Explanation:

Double displacement reaction is defined as the reaction in which ions of two compound interchange with each other to form the product. For example, the general double displacement reaction between two compounds AX and BY is as follows:

${\text{AX}} + {\text{BY}} \to {\text{AY}} + {\text{BX}}$

The three types of equations that are used to represent the chemical reaction are as follows:

1. Molecular equation

2. Complete ionic equation

3. Net ionic equation

The reactants and products remain in undissociated form in molecular equation. In the case of complete ionic equation, all the ions that are dissociated and present in the reaction mixture are represented while in the case of net ionic equation only the useful ions that participate in the reaction are represented.

The steps to write the complete ionic reaction are as follows:

Step 1: Write the molecular equation for the reaction with the phases in the bracket.

In the reaction, HI reacts with RbOH to form RbI and ${{\text{H}}_{\text{2}}}{\text{O}}$ . The balanced molecular equation of the reaction is as follows:

${\text{HI}}\left( {aq} \right) + {\text{RbOH}}\left( {aq} \right) \to {\text{RbI}}\left( {aq} \right){\text{ + }}{{\text{H}}_{\text{2}}}{\text{O}}\left( l \right)$

Step 2: Dissociate all the compounds with the aqueous phase to write the complete ionic equation. The compounds with solid and liquid phase remain same. The complete ionic equation is as follows:

${{\mathbf{H}}^ + }\left( q \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right) + {\mathbf{O}}{{\mathbf{H}}^ - }\left( {aq} \right) \to {{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}\left( l \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right)$

Learn more:

1. Balanced chemical equation link

2. Oxidation and reduction reaction link

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: Double displacement reaction, types of equation, molecular equation, complete ionic equation, net ionic equation, RbI, RbOH, H2O, HI, chemical reaction.

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