What volume (in mL) of 0.0914 M NaOH solution is needed to neutralize 60.7 mL of 0.701 M H2SO4 solution

The answer has to be in 3 significant figures. however, just the work would suffice cuz thats what i really need. Desperate to learn this.

write a balanced equation

2NaOH(aq) + H2SO4(aq) ---> Na2SO4(aq) + 2H2O(l)

This shows you that you need 2 moles of NaOH to neutralise 1 mole H2SO4

moles HS2O4 = molarity x litres
= 0.701 M x 0.0607 L
= 0.0425507 mol H2SO4

So moles NaOH needed = 2 x moles H2SO4
= 0.0851014 moles

Now workout what volume of 0.0914 M NaOH has this many moles

Molarity = moles / Litres
Therefore litres = moles / Molarity
= 0.0851014 mol / 0.0914 M
= 0.931 L
= 931 ml (3 sig figs)