Question

A beaker of nitric acid is neutralized with dilute aqueous solution of calcium hydroxide.Write a net ionic equation for this reaction.

Answer 1

The net ionic equation is $\boxed{2{{\text{H}}^ + }\left( {aq} \right) + 2{\text{O}}{{\text{H}}^ - }\left( {aq} \right) \to 2{{\text{H}}_{\text{2}}}{\text{O}}\left( l \right)}$.

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 the total ionic equation, all the ions that are dissociated and present in the reaction mixture are represented while in the case of overall or net ionic equation only the useful ions that participate in the reaction are represented.

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

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

In the reaction, ${\text{HN}}{{\text{O}}_3}$ reacts with ${\text{Ca}}{\left( {{\text{OH}}} \right)_2}$ to form ${\text{Ca}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}$ and ${{\text{H}}_{\text{2}}}{\text{O}}$. The balanced molecular equation of the reaction is as follows:

$2{\text{HN}}{{\text{O}}_3}\left( {aq} \right) + {\text{Ca}}{\left( {{\text{OH}}} \right)_2}\left( {aq} \right) \to {\text{Ca}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_2}\left( {aq} \right) + 2{{\text{H}}_{\text{2}}}{\text{O}}\left( l \right)$

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

$2{{\text{H}}^+}\left({aq}\right)+2{\text{NO}}_3^-\left({aq}\right)+{\text{C}}{{\text{a}}^{2+}}\left({aq}\right)+2{\text{O}}{{\text{H}}^-}\left({aq}\right)\to{\text{C}}{{\text{a}}^{2+}}\left({aq}\right)+2{\text{NO}}_3^-\left({aq}\right)+2{{\text{H}}_{\text{2}}}{\text{O}}\left(l\right)$

Step 3: The common ions on both sides of the reaction get cancelled out to get the net ionic equation.

$2{{\text{H}}^+}\left({aq}\right)+\boxed{2{\text{NO}}_3^-\left( {aq} \right)}+\boxed{{\text{C}}{{\text{a}}^{2+}}\left({aq}\right)}+2{\text{O}}{{\text{H}}^-}\left({aq}\right)\to\boxed{{\text{C}}{{\text{a}}^{2+}}\left({aq}\right)}+\boxed{2{\text{NO}}_3^-\left({aq}\right)}+2{{\text{H}}_{\text{2}}}{\text{O}}\left(l\right)$

Therefore, the net ionic equation is as follows:

$2{{\text{H}}^+}\left({aq}\right)+2{\text{O}}{{\text{H}}^-}\left({aq}\right)\to 2{{\text{H}}_{\text{2}}}{\text{O}}\left(l\right)$

Learn more:

1. Balanced chemical equation: brainly.com/question/1405182

2. Oxidation and reduction reaction: brainly.com/question/2973661

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: net ionic equation, H2O, HNO3, Ca2+, NO3-, OH-, Ca(NO3)2, Ca(OH)2, 2OH-, 2H+, 2NO3-, molecular equation, total ionic equation, liquid, solid, aqueous.

Answer 2

Complete balanced equation: 2HNO₃  +  Ca(OH)₂  →  Ca(NO₃)₂  +  2H₂O

Ionized equation (with spectator ions): 
   2H⁺  +  2NO₃⁻  +  Ca²⁺  +  2OH⁻   →  Ca²⁺  +  2NO₃⁻  +  2H₂O

By eliminating the ions that are the same of both sides of the equation (spectator ions):
    
2H⁺  +   2OH⁻   →    2H₂O    [Net Ionic Equation]