45.00 mL of an aqueous H₂SO₄ solution required 32.0 mL of 0.200 M KOH(aq)to neutralize it completely. The molarity of the H₂SO₄ solution is therefore Hint: Write out the balanced neutralization reaction before beginning the problem.

Question

Quizplus · Accepted Answer

The balanced neutralization reaction is:H₂SO₄(aq) + 2KOH(aq) → K₂SO₄(aq) + 2H₂O(l)From the stoichiometry of the balanced equation, we see that 1 mol of H₂SO₄ reacts with 2 mol of KOH. Therefore, the number of moles of H₂SO₄ in the 45.00 mL sample is:(32.0 mL KOH)(0.200 mol KOH/L KOH)(1 mol H₂SO₄/2 mol KOH) = 0.00320 mol H₂SO₄The molarity of the H₂SO₄ solution is therefore:(0.00320 mol H₂SO₄)/(45.00 mL H₂SO₄ solution)(1 L/1000 mL) = 0.0711 M

4500 ML of an Aqueous H2SO4 Solution Required 32

4500 ML of an Aqueous H₂SO₄ Solution Required 32