Answer :
To find the net ionic equation for the given reaction, we need to follow these steps:
1. Write down the total ionic equation:
The given equation is:
[tex]\[ \text{Na}^+ + 2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} + 6 \text{Cl}^- \longrightarrow 6 \text{Na}^+ + 6 \text{Cl}^- + \text{Ca}_3(\text{PO}_4)_2 \][/tex]
2. Identify and cancel spectator ions:
Spectator ions are ions that do not participate in the actual reaction and appear unchanged on both sides of the equation. In this case, Na^+ and Cl^- are spectator ions because they appear on both sides of the equation.
3. Remove spectator ions to obtain the net ionic equation:
After removing the spectator ions (Na^+ and Cl^-), we are left with:
[tex]\[ 2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2 \][/tex]
Thus, 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]
1. Write down the total ionic equation:
The given equation is:
[tex]\[ \text{Na}^+ + 2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} + 6 \text{Cl}^- \longrightarrow 6 \text{Na}^+ + 6 \text{Cl}^- + \text{Ca}_3(\text{PO}_4)_2 \][/tex]
2. Identify and cancel spectator ions:
Spectator ions are ions that do not participate in the actual reaction and appear unchanged on both sides of the equation. In this case, Na^+ and Cl^- are spectator ions because they appear on both sides of the equation.
3. Remove spectator ions to obtain the net ionic equation:
After removing the spectator ions (Na^+ and Cl^-), we are left with:
[tex]\[ 2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2 \][/tex]
Thus, 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]
