Frosty0110idn
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What is the net ionic equation for the reaction that is 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 :

GinnyAnsweridn
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]
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