A 25.0 mL sample of H₂SO₄ requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid?
H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O

Question

A 25.0 mL sample of H₂SO₄ requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid? H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O

Quizplus · Accepted Answer

According to the balanced chemical equation, it takes 1 mole of H₂SO₄ to react with 2 moles of KOH. 
In the given problem, 20.0 mL of 2.00 M KOH is used to neutralize 25.0 mL of H₂SO₄.

To find the molarity of the acid, we can use the formula:
Molarity of acid = (Molarity of KOH) x (Volume of KOH) / (Volume of acid)

Molarity of acid = (2.00 M) x (20.0 mL) / (25.0 mL) = 1.60 M 
Therefore, the molarity of the acid is 1.60 M.

The correct answer is option D.

A 250 ML Sample of H₂SO₄ Requires 20