What is the net ionic equation for this reaction?

[tex]\[ 2 \text{KOH (aq)} + \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow 2 \text{H}_2\text{O (l)} + \text{K}_2\text{SO}_4 \text{(aq)} \][/tex]

A. [tex]\( 2 \text{K}^+ + \text{OH}^- + 2 \text{H}^+ + \text{SO}_4^{2-} \rightarrow 2 \text{H}_2\text{O (l)} + 2 \text{K}^+ + \text{SO}_4^{2-} \)[/tex]

B. [tex]\( 2 \text{KOH} + \text{H}_2\text{SO}_4 \rightarrow 2 \text{H}_2\text{O} + \text{K}_2\text{SO}_4 \)[/tex]

C. [tex]\( 2 \text{KOH} + 2 \text{H}^+ + \text{SO}_4^{2-} \rightarrow 2 \text{H}_2\text{O (l)} + 2 \text{K}^+ + \text{SO}_4^{2-} \)[/tex]

D. [tex]\( \text{OH}^- + 2 \text{H}^+ \rightarrow 2 \text{H}_2\text{O (l)} \)[/tex]



Answer :

Okay, let's carefully determine the net ionic equation for the given reaction:

[tex]\[ 2 \text{KOH} (aq) + \text{H}_2\text{SO}_4(aq) \rightarrow 2 \text{H}_2\text{O} (\ell) + \text{K}_2\text{SO}_4(aq) \][/tex]

### Step-by-step solution:

1. Dissociate all strong electrolytes into their ions:

The reactants:
[tex]\[ 2 \text{KOH} (aq) \rightarrow 2 \text{K}^+ (aq) + 2 \text{OH}^- (aq) \][/tex]
[tex]\[ \text{H}_2\text{SO}_4(aq) \rightarrow 2 \text{H}^+ (aq) + \text{SO}_4^{2-} (aq) \][/tex]

The products:
[tex]\[ \text{K}_2\text{SO}_4(aq) \rightarrow 2 \text{K}^+ (aq) + \text{SO}_4^{2-} (aq) \][/tex]
[tex]\[ 2 \text{H}_2\text{O} (\ell) \text{ (is a liquid and does not dissociate into ions)} \][/tex]

2. Write the complete ionic equation including all ions:

[tex]\[ 2 \text{K}^+ (aq) + 2 \text{OH}^- (aq) + 2 \text{H}^+ (aq) + \text{SO}_4^{2-} (aq) \rightarrow 2 \text{H}_2\text{O} (\ell) + 2 \text{K}^+ (aq) + \text{SO}_4^{2-} (aq) \][/tex]

3. Identify the spectator ions:

Spectator ions are ions that appear on both sides of the equation and do not participate in the actual reaction. Here, the spectator ions are:
[tex]\[ 2 \text{K}^+ (aq) \text{ and } \text{SO}_4^{2-} (aq) \][/tex]

4. Remove the spectator ions to find the net ionic equation:

When we remove the spectator ions, we get:
[tex]\[ 2 \text{OH}^- (aq) + 2 \text{H}^+ (aq) \rightarrow 2 \text{H}_2\text{O} (\ell) \][/tex]
Simplify the coefficients:
[tex]\[ \text{OH}^- (aq) + \text{H}^+ (aq) \rightarrow \text{H}_2\text{O} (\ell) \][/tex]

Thus, the correct net ionic equation for the reaction is:

Choice D: [tex]\( \text{OH}^- (aq) + \text{H}^+ (aq) \rightarrow \text{H}_2\text{O} (\ell) \)[/tex]