A 50.0 mL sample of an aqueous H₂SO₄ solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄ is ________ M. A)0.234 B)0.469 C)0.150 D)0.300 E)0.938

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is:H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂OFrom the stoichiometry of the reaction, we can see that 1 mole of H₂SO₄ reacts with 2 moles of NaOH. Therefore, the number of moles of H₂SO₄ in the 50.0 mL sample is:(0.0625 L NaOH) × (0.375 M NaOH) × (1 mol H₂SO₄ / 2 mol NaOH) = 0.0117 mol H₂SO₄The concentration of H₂SO₄ in the solution is therefore:(0.0117 mol H₂SO₄) / (0.0500 L solution) = 0.234 MTherefore, the correct answer is A) 0.234 M.

A 500 ML Sample of an Aqueous H2SO4 Solution Is Titrated

A 500 ML Sample of an Aqueous H₂SO₄ Solution Is Titrated