Chemical Reaction

Question

Given a balanced chemical equation between H₂SO₄(aq) and KOH(aq)

   H2SO4(aq) + 2 KOH(aq) → K2SO4(aq) + 2 H2O(l)

What volume (in mL) of 0.69 M H₂SO₄(aq) solution is necessary to completely react with 127 mL of 0.47 M KOH(aq)?

Note: (1) The unit of volume of H₂SO₄(aq) is in mL



       (2) Insert only the numerical value (integer) of your answer (do not include the units or chemical in your answer).

Answer 1

moles KOH present = 0.127 L x 0.47 mol/L = 0.05969 mol

moles H2SO4 needed = 0.05969 mol KOH x 1 mol H2SO4 / 2 mol KOH = 0.02985 mol

volume H2SO4 needed: 0.69 mol/L * x L = 0.02985 mol and x = 0.0435 L = 43.5 ml