Stoichiometry (Help please)

1. Sulfuric acid and sodium hydroxide react to form sodium sulfate and water.
H2SO4 + 2 NaOH ---> Na2SO4 + 2 H20

a. Given: 250g Na2SO4
Unknown: mol NaOH

Could someone show me how to solve this problem? I'm confused. :/

Ok, based on the assumption that all of your reactant was used up to make the product, your overall scheme to solve this should be: mass Na2SO4 --> moles Na2SO4 --> moles NaOH
250 g Na2SO4 * 1 mol / 142.04 g * 2 mol NaOH / mol Na2SO4

So you have to determine how much NaOH was used to make 250 g of sodium sulfate (Na2SO4)
First thing you do is convert 250g of Na2SO4 to moles of Na2SO4 and you do that by dividing Na2SO4 molecular weight. Once you have the moles of Na2SO4, your balanced chemical equation says that there is 2 moles of NaOH for every one Na2SO4, so you just multiply the moles of Na2SO4 you found by 2 and viola your answer!

Does that make sense?