Volume to titrate to the equivalence point- I'm stumped please help

What volume of 0.375M NaOH is required to titrate 30.0 mL of 0.125M H2SO4 to the equivalence point?
(a) 10.0 mL (b) 20.0 mL (c) 30.0 mL (d) 40.0 mL

answer is (b) 20.0 ml from answer key but I cant find it - I'm stumped
please help

i give you one of multiple methods

H2SO4 + 2NaOH--> Na2SO4 + 2 H2O

so you see , you need 2 molecules of NaOH for 1 molecule of H2SO4

30mL=0.03L of 0.125M H2SO4 contains 0.125*0.03=0.00375 moles of H2SO4
to titrate by NaOH you need 2*0.00375=0.0075moles of NaOH
The solution of 0.375 M contains 0.375 moles by liter
so you need 0.0075/0.375=0.02L of your solution

answer b is correct since 0.02L=20mL