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What is the net ionic equation for the reaction represented by the following total ionic equation?

[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]

A. [tex]\[ 2 \text{Na}_3\text{PO}_4 + 3 \text{CaCl}_2 \longrightarrow 6 \text{NaCl} + \text{Ca}_3(\text{PO}_4)_2 \][/tex]

B. [tex]\[ 2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2 \][/tex]

C. [tex]\[ 2 \text{PO}_4^{3-} + 3 \text{Ca}^{2+} + 6 \text{Cl}^{-} \longrightarrow 6 \text{Na}^{+} + \text{Ca}_3(\text{PO}_4)_2 \][/tex]

D. [tex]\[ 2 \text{P}^{5+} + 8 \text{O}^{2-} + 3 \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2 \][/tex]

Sagot :

GinnyAnswer
To find the net ionic equation for the reaction represented by the given total ionic equation:

[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]

we need to follow these steps:

1. Identify the spectator ions: Spectator ions are those ions that appear unchanged on both sides of the equation. In this case, the spectator ions are [tex]\( \text{Na}^+ \)[/tex] and [tex]\( \text{Cl}^- \)[/tex] because they appear on both the reactant and product sides of the equation in identical forms.

2. Remove the spectator ions from the total ionic equation:

[tex]\[ 6 \, \text{Na}^+ \text{(spectator ion)} + 2 \, \text{PO}_4^{3-} + 3 \, \text{Ca}^{2+} + 6 \, \text{Cl}^- \text{(spectator ion)} \longrightarrow 6 \, \text{Na}^+ \text{(spectator ion)} + 6 \, \text{Cl}^- \text{(spectator ion)} + \text{Ca}_3(\text{PO}_4)_2 \][/tex]

3. Simplify the equation by removing the spectator ions:

[tex]\[ 2 \, \text{PO}_4^{3-} + 3 \, \text{Ca}^{2+} \longrightarrow \text{Ca}_3(\text{PO}_4)_2 \][/tex]

Therefore, 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]

This equation shows the formation of calcium phosphate from phosphate ions ([tex]\( \text{PO}_4^{3-} \)[/tex]) and calcium ions ([tex]\( \text{Ca}^{2+} \)[/tex]).
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