Troubling question

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 0.5 M H₂SO₄(aq) solution is necessary to completely react with 132 mL of 0.44 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

If you have 132 mL of 0.44 M KOH, you can figure out the number of moles of it that you have. 0.44 M = 0.44 moles/liter. You have 132 mL which is 0.132 liters. So 0.44 moles/liter x 0.132 liters = 0.05808 moles of KOH

Your balanced chemical reaction equation says for every 2 moles of KOH, you need only 1 mole of H₂SO₄ so if you have 0.05808 moles of KOH, you only need half that amount of H₂SO₄ or 0.02904 moles.

The concentration of H₂SO₄ is 0.5 M or 0.5 moles/liter. To calculate the volume, take the 0.02904 moles divided by 0.5 moles/liter to get 0.05808 liters and then multiply by 1000 to get 58 mL