To determine the net ionic equation from the provided total ionic equation, 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 on both sides of the equation unchanged. From the total ionic equation, we can see that [tex]\(\text{Na}^{+}\)[/tex] and [tex]\(\text{Cl}^{-}\)[/tex] are present on both the reactant and product sides.
3. Remove Spectator Ions:
By removing the spectator ions ([tex]\(\text{Na}^{+}\)[/tex] and [tex]\(\text{Cl}^{-}\)[/tex]), we simplify the equation to focus on the species that actually undergo change. After removing these ions, we are left with:
[tex]\[
2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2
\][/tex]
4. Write the Net Ionic Equation:
The net ionic equation only includes the ions and molecules directly involved in the reaction. Hence, the net ionic equation for the given total ionic equation is:
[tex]\[
2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2
\][/tex]
In conclusion, the net ionic equation for the reaction is:
[tex]\[
2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2
\][/tex]
