Questions: 4. What would be net ionic equation for the reaction of a sodium hydroxide and sulfuric acid? 5. What are the spectator ions in the above reaction?

4. What would be net ionic equation for the reaction of a sodium hydroxide and sulfuric acid? 5. What are the spectator ions in the above reaction?
Transcript text: 4. What would be net ionic equation for the reaction of a sodium hydroxide and sulfuric acid? 5. What are the spectator ions in the above reaction?
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Solution

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Solution Steps

Step 1: Write the balanced molecular equation

The balanced molecular equation for the reaction between sodium hydroxide (NaOH) and sulfuric acid (H\(_2\)SO\(_4\)) is: \[ \text{2 NaOH} + \text{H}_2\text{SO}_4 \rightarrow \text{Na}_2\text{SO}_4 + 2 \text{H}_2\text{O} \]

Step 2: Write the complete ionic equation

Next, we write the complete ionic equation by dissociating all strong electrolytes into their ions: \[ 2 \text{Na}^+ + 2 \text{OH}^- + 2 \text{H}^+ + \text{SO}_4^{2-} \rightarrow 2 \text{Na}^+ + \text{SO}_4^{2-} + 2 \text{H}_2\text{O} \]

Step 3: Identify and remove spectator ions

Spectator ions are ions that appear on both sides of the complete ionic equation and do not participate in the actual reaction. In this case, the spectator ions are \(\text{Na}^+\) and \(\text{SO}_4^{2-}\).

Step 4: Write the net ionic equation

After removing the spectator ions, the net ionic equation is: \[ 2 \text{OH}^- + 2 \text{H}^+ \rightarrow 2 \text{H}_2\text{O} \] This can be simplified to: \[ \text{OH}^- + \text{H}^+ \rightarrow \text{H}_2\text{O} \]

Final Answer

The net ionic equation for the reaction of sodium hydroxide and sulfuric acid is: \[ \boxed{\text{OH}^- + \text{H}^+ \rightarrow \text{H}_2\text{O}} \]

The spectator ions in the above reaction are: \[ \boxed{\text{Na}^+ \text{ and } \text{SO}_4^{2-}} \]

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