Question

NaOH +H2SO --> Na2SO4 + H2O

1. balance equation

2. How many ml of 0.45 M NaOH is needed to completely neutralize 55ml of 0.25m H2SO4

Answer 1

Balanced equation is

2NaOH + H₂SO₄ -----> Na₂SO₄ + 2H₂O

Number of moles of H2SO4 = molarity * volume of solution in L

Number of moles of H2SO4 = 0.25 * 0.055 = 0.014 mole

From the balanced equation we can say that

1 mole of H2SO4 requires 2 mole of NaOH so

0.014 mole of H2SO4 will require

= 0.014 mole of H2SO4 *(2 mole of NaOH / 1 mole of H2SO4)

= 0.028 mole of NaOH

Molarity of NaOH = number of moles of NaOH / volume of solution in L

0.45 = 0.028 / volume of solution in L

volume of solution in L = 0.028 / 0.45 = 0.062 L

1L = 1000 mL

0.062 L = 62 mL

Therefore, the volume of NaOH required would be 62 mL