Okay.. I think I found the rite answer for this question.. but just making sure I did it rite

What is the molar concentration of silver nitrate in solution with sodium sulfate?

And the mass of silver sulfate produced is 5.47g, and the volume of silver nitrate that is reacting is 100ml

... I got .351mol/L... does that sound rite?

I'm too lazy to do the math right now, but check your setup:

take the 5.47g Ag2(SO4) and convert to moles Ag2(SO4)

then recog. That one mole Ag2(SO4) yields two Ag+ ions so multiply x 2

this gives moles Ag ions which is the same as moles AgNO3 since 1 Ag "used"

then divide by 0.100 L

if this is what you did then great... most common problem here is probably people forgetting to multiply by 2 to convert moles Ag2(SO4) to moles Ag