Exactly 17.0 mL of a H₂SO₄ solution was required to neutralize 45.0 mL of 0.235 M NaOH.What was the concentration of the H₂SO₄ solution?
Given: H₂SO₄ (aq) + 2NaOH (aq) → 2H₂O (l) + Na₂SO₄ (aq)

Question

Quizplus · Accepted Answer

The concentration of the H₂SO₄ solution can be calculated using the stoichiometry of the reaction and the volumes and concentration of NaOH. Given the 1:2 stoichiometry between the acid and NaOH, the moles of NaOH are first calculated (45.0 mL * 0.235 M = 10.575 mmol), which are twice the moles of the acid. Therefore, the moles of the acid are 5.2875 mmol. The concentration of the acid is then the moles of acid divided by its volume in liters (5.2875 mmol / 17.0 mL = 0.311 M).