What volume of 0.250 M H2SO4 is needed to react with 50.0 mL of 0.100 M NaOH?

mol(NaOH) = 0.1 M x 50mL / 1000 = 0.005 moles
From the Balanced reaction equation
mol(NaOH) = 0.005 moles is equivalent to '2'
Hence
mol(H2SO4) = 0.005/2 = 0.0025 moles is equivalent to '1'
Hence
mol(H2SO4) 0.0025 = 0.25 M x volmL / 1000
Algebraically rearrange
vol/mL = 0.0025 x 1000 / 0.25 = 10 mL ( The answer) !!!!

H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l)
OR: Mole ratio H₂SO₄ : NaOH = 1 : 2

No. of milli-moles of NaOH reacted = (1.00 mmol/mL) × (50.0 mL) = 50.0 mmol
No. of milli-moles of H₂SO₄ needed = (50 mmol) × (1/2) = 25 mmol
Volume of H₂SO₄ needed = (25 mmol) / (0.25 mmol/mL) = 100 mL