To determine which compound is acting as an acid in the chemical reaction, we need to understand the Bronsted-Lowry theory of acids and bases. According to this theory, an acid is a substance that donates a proton (H+ ion), while a base is a substance that accepts a proton.
Let's analyze the given chemical reaction:
[tex]\[ 2 \text{LiOH} + \text{H}_2\text{SO}_4 \rightarrow 2 \text{H}_2\text{O} + \text{Li}_2\text{SO}_4 \][/tex]
1. Identify the compounds involved in the reaction:
- [tex]\( \text{LiOH} \)[/tex] : lithium hydroxide
- [tex]\( \text{H}_2\text{SO}_4 \)[/tex] : sulfuric acid
- [tex]\( \text{H}_2\text{O} \)[/tex] : water
- [tex]\( \text{Li}_2\text{SO}_4 \)[/tex] : lithium sulfate
2. Determine the role of each compound:
- Sulfuric acid ([tex]\(\text{H}_2\text{SO}_4\)[/tex]) is a commonly known strong acid.
- Lithium hydroxide ([tex]\(\text{LiOH}\)[/tex]) is a base because it can accept protons (H+ ions).
- Water ([tex]\(\text{H}_2\text{O}\)[/tex]) is typically the product of an acid-base reaction and is neutral.
- Lithium sulfate ([tex]\(\text{Li}_2\text{SO}_4\)[/tex]) is a salt formed from the neutralization reaction.
3. Identify the proton donor (acid):
- In this reaction, sulfuric acid ([tex]\(\text{H}_2\text{SO}_4\)[/tex]) donates protons (H+ ions) to lithium hydroxide ([tex]\(\text{LiOH}\)[/tex]), which accepts the protons.
Therefore, the compound acting as an acid in the reaction is [tex]\( \text{H}_2\text{SO}_4 \)[/tex].
So, the correct answer is:
[tex]\[ \boxed{H_2SO_4} \][/tex]
