To determine how many moles of NaOH would be needed to neutralize 1 mole of H₂SO₄ (sulfuric acid), we need to examine the chemical reaction involved in the neutralization process.
The balanced chemical equation for the neutralization of H₂SO₄ with NaOH is:
[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 indicates that one molecule of sulfuric acid (H₂SO₄) reacts with two molecules of sodium hydroxide (NaOH) to produce one molecule of sodium sulfate (Na₂SO₄) and two molecules of water (H₂O).
From the stoichiometry of the reaction, we see that:
- 1 mole of H₂SO₄ requires 2 moles of NaOH to be completely neutralized.
Therefore, if we have 1 mole of H₂SO₄, it would require 2 moles of NaOH for complete neutralization.
In conclusion, 2 moles of NaOH are needed to neutralize 1 mole of H₂SO₄.
