What volume of 1.5 M sodium hydroxide solution is required to completely neutralize 250 mL of 4.0 M sulfuric acid?

Answer 1

mol H₂SO₄ = .25 L x .4 mol/L = .1 mol

mol NaOH required = .1 mol

volume NaOH solution = .1 mol x 1L/1.5 mol = .067 L or 67mL NaOH solution

Answer 2

2NaOH + H₂SO₄ ==> Na₂SO₄ + 2H₂O ... balanced equation

moles H₂SO₄ present = 250 ml x 1 L/1000 ml x 4.0 moles/L = 1.00 moles

moles NaOH needed = 1.00 moles H₂SO₄ x 2 moles NaOH/mole H₂SO₄ = 2.00 moles NaOH needed

Volume of NaOH needed:

(x L)(1.5 mol/L) = 2.00 moles

x = 1.33 L of NaOH needed