To determine the correct net ionic equation for the reaction between calcium hydroxide, [tex]\( Ca(OH)_2 \)[/tex], and sulfuric acid, [tex]\( H_2SO_4 \)[/tex], we need to break down the reaction into its ionic components.
1. Write the balanced molecular equation:
[tex]\[ Ca(OH)_2 \, + \, H_2SO_4 \, \rightarrow \, CaSO_4 \, + \, 2H_2O \][/tex]
2. Dissociate the strong electrolytes into their ions:
[tex]\[ Ca(OH)_2 \rightarrow Ca^{2+} + 2OH^- \][/tex]
[tex]\[ H_2SO_4 \rightarrow 2H^+ + SO_4^{2-} \][/tex]
3. Combine the ions to form the products:
[tex]\[ Ca^{2+} + 2OH^- + 2H^+ + SO_4^{2-} \rightarrow CaSO_4 + 2H_2O \][/tex]
4. Identify and remove the spectator ions, which do not participate in the reaction. In this case, there are no spectator ions in the simplified form. However, the net ionic reaction focuses on the ions that are actively involved in forming the neutral water molecule:
[tex]\[ 2H^+ + 2OH^- \rightarrow 2H_2O \][/tex]
Since the correct equation above forms water and calcium sulfate, we then simplify the net ionic reaction to encompass only the essential ions involved:
The final correct net ionic equation is:
[tex]\[ 2H^+ + 2OH^- \rightarrow 2H_2O \][/tex]
Simplifying:
[tex]\[ H^+ + OH^- \rightarrow H_2O \][/tex]
So, the correct net ionic equation for the reaction between [tex]\( Ca(OH)_2 \)[/tex] and [tex]\( H_2SO_4 \)[/tex] is:
[tex]\[ H^+ + OH^- \longrightarrow H_2O \][/tex]
Thus, the answer to the given question is:
[tex]\[ H^+ + OH^- \longrightarrow H_2O \][/tex]
