Please help me asap

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 0.59 M H₂SO₄(aq) solution is necessary to completely react with 146 mL of 0.24 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

Well 146 ml (0.146 l) of 0.24 M KOH contains 0.146 x 0.24 moles

From the equation for each mole of KOH you need 0.5 moles of H2SO4 to react

So moles of H2SO4 needed = 0.146 x 0.24 x 0.5

1 l of the H2SO4 solution contains 0.59 moles

So you need (0.146 x 0.24 x 0.5 / 0.59) l of H2SO4 solution = (0.146 x 0.24 x 0.5 / 0.59) x 1000 ml

You can do the calculation