Question

Another metal phosphate is iron phosphate. It will behave similar to calcium phosphate in an acid solution. What is the net ionic equation including phases for FePO4(s) dissolving in H3O+(aq)?

Answer 1

The net ionic equation is $\boxed{{\text{FeP}}{{\text{O}}_4}\left(s\right)+{{\text{H}}_3}{{\text{O}}^+}\left({aq}\right)\to{\text{F}}{{\text{e}}^{3+}}\left({aq}\right)+{\text{HPO}}_4^{2-}\left({aq}\right)+{{\text{H}}_2}{\text{O}}\left(l\right)}$

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 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 net ionic reaction are as follows:

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

In the reaction, ${\text{FeP}}{{\text{O}}_4}$ ionizes in aqueous medium to form ${\text{F}}{{\text{e}}^{3+}}$ and ${{\text{H}}_{\text{2}}}{\text{O}}$. The balanced molecular equation of the reaction is as follows:

${\text{FeP}}{{\text{O}}_4}\left(s\right)+{{\text{H}}_3}{{\text{O}}^+}\left({aq}\right)\to{\text{F}}{{\text{e}}_2}{\left({{\text{HP}}{{\text{O}}_4}}\right)_3}\left({aq}\right)+{{\text{H}}_2}{\text{O}}\left(l\right)$

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

${\text{FeP}}{{\text{O}}_4}\left(s\right)+{{\text{H}}_3}{{\text{O}}^+}\left({aq}\right)\to{\text{F}}{{\text{e}}^{3+}}\left({aq}\right)+{\text{HPO}}_4^{2-}\left({aq}\right)+{{\text{H}}_2}{\text{O}}\left(l\right)$

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

${\text{FeP}}{{\text{O}}_4}\left(s\right)+{{\text{H}}_3}{{\text{O}}^+}\left({aq}\right)\to{\text{F}}{{\text{e}}^{3+}}\left({aq}\right)+{\text{HPO}}_4^{2-}\left({aq}\right)+{{\text{H}}_2}{\text{O}}\left(l\right)$

Therefore, the net ionic equation obtained is as follows:

${\text{FeP}}{{\text{O}}_4}\left(s\right)+{{\text{H}}_3}{{\text{O}}^+}\left({aq}\right)\to{\text{F}}{{\text{e}}^{3+}}\left({aq}\right)+{\text{HPO}}_4^{2-}\left({aq}\right)+{{\text{H}}_2}{\text{O}}\left(l\right)$

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, FePO4, H3O+, Fe3+, HPO42-, H2O, aqueous phase, dissociate, molecular equation, water.

Answer 2

Iron phosphate when in an acid solution ionizes or dissociates into ions. The ions are the Iron (III) and the HPO4^2-. The net ionic equation should be as follows:

FePO4(s)+H3O +(aq)⇌Fe^3+(aq)+HPO4^2−(aq)+H2O(l)