To determine the net ionic equation for the reaction between [tex]\( \text{Na}_2\text{SO}_4 \)[/tex] and [tex]\( \text{CaCl}_2 \)[/tex], we need to follow these steps:
1. Write the balanced molecular equation:
[tex]\[
\text{Na}_2\text{SO}_4(aq) + \text{CaCl}_2(aq) \rightarrow \text{CaSO}_4(s) + 2 \text{NaCl}(aq)
\][/tex]
2. Write the complete ionic equation:
Since [tex]\( \text{Na}_2\text{SO}_4 \)[/tex] and [tex]\( \text{CaCl}_2 \)[/tex] are soluble in water, they dissociate into their respective ions:
[tex]\[
2 \text{Na}^+(aq) + \text{SO}_4^{2-}(aq) + \text{Ca}^{2+}(aq) + 2 \text{Cl}^-(aq) \rightarrow \text{CaSO}_4(s) + 2 \text{Na}^+(aq) + 2 \text{Cl}^-(aq)
\][/tex]
3. Identify and remove the spectator ions:
Spectator ions are ions that appear on both sides of the ionic equation without undergoing any change. In this case, [tex]\( \text{Na}^+ \)[/tex] and [tex]\( \text{Cl}^- \)[/tex] are the spectator ions.
4. Write the net ionic equation:
After removing the spectator ions, we are left with the ions that participate in forming the precipitate:
[tex]\[
\text{SO}_4^{2-}(aq) + \text{Ca}^{2+}(aq) \rightarrow \text{CaSO}_4(s)
\][/tex]
The net ionic equation for the reaction between [tex]\( \text{Na}_2\text{SO}_4 \)[/tex] and [tex]\( \text{CaCl}_2 \)[/tex] is:
[tex]\[
\text{SO}_4^{2-}(aq) + \text{Ca}^{2+}(aq) \rightarrow \text{CaSO}_4(s)
\][/tex]
So, the correct answer is:
A. [tex]\( \text{SO}_4^{2-}(aq) + \text{Ca}^{2+}(aq) \rightarrow \text{CaSO}_4(s) \)[/tex]
