When sulfuric acid ([tex]$\text{H}_2\text{SO}_4$[/tex]) reacts with sodium hydroxide ([tex]$\text{NaOH}$[/tex]), the reaction that takes place is a neutralization reaction. In a neutralization reaction, an acid reacts with a base to produce a salt and water. Let's look at the balanced chemical equation for the reaction between sulfuric acid and sodium hydroxide:
[tex]$\text{H}_2\text{SO}_4 + 2 \text{NaOH} \rightarrow \text{Na}_2\text{SO}_4 + 2\text{H}_2\text{O}$[/tex]
This equation shows that sulfuric acid reacts with sodium hydroxide in a 1:2 molar ratio to produce water and a salt. The salt produced in this reaction is sodium sulfate ([tex]$\text{Na}_2\text{SO}_4$[/tex]).
To verify which salt is produced from the given options:
- [tex]$K_2SO_3$[/tex]: This is potassium sulfite, not produced in this reaction.
- [tex]$Na_2SO_4$[/tex]: This is sodium sulfate, and it matches our balanced chemical equation.
- [tex]$Na_2SO_3$[/tex]: This is sodium sulfite, not produced in this reaction.
- [tex]$K_2SO_4$[/tex]: This is potassium sulfate, not produced in this reaction.
Therefore, the correct answer is:
[tex]$\text{Na}_2\text{SO}_4$[/tex]
