To determine the net ionic equation for the given reaction, we need to follow these steps:
1. Identify the Total Ionic Equation:
The total ionic equation is given as:
[tex]\[
6 \, \text{Na}^+ + 2 \, \text{PO}_4^{3-} + 3 \, \text{Ca}^{2+} + 6 \, \text{Cl}^- \longrightarrow 6 \, \text{Na}^+ + 6 \, \text{Cl}^- + \text{Ca}_3(\text{PO}_4)_2
\][/tex]
2. Identify Spectator Ions:
Spectator ions are ions that appear in the same form on both sides of the equation. Here, Na[tex]\(^+\)[/tex] and Cl[tex]\(^-\)[/tex] are spectator ions, as they do not change during the reaction.
3. Remove Spectator Ions:
After removing Na[tex]\(^+\)[/tex] and Cl[tex]\(^-\)[/tex], we are left with:
[tex]\[
2 \, \text{PO}_4^{3-} + 3 \, \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2
\][/tex]
So, the net ionic equation for the given reaction is:
[tex]\[
2 \, \text{PO}_4^{3-} + 3 \, \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2
\][/tex]
