[V3RA]

You add 500 mL of 0.1 M AgNO3 solution to a solution containing an excess of NaSO4.  What mass of precipitate will be formed?

I am completely lost on how to begin this problem... can anyone assist?

[Arkcon]

Well, to start with, its useful to write a balanced chemical reaction.  That way, you have an image in your mind of what is happening.  Can you do that for us?

[V3RA]

AgNO3 + NaSO4 -> Ag(SO4) + NaNO3

And then I think I would do the ionic equations, correct?

Ag⁺ + SO4^- -> Ag(SO4)
Na⁺ + NO3^- -> NaNO3

But if I refer to my solubility table, neither of those products form a precipiate... so I must have done something wrong.

[Borek]

No such thing as NaSO₄.

[V3RA]

NaSO4 does exist, the more common form is Na2SO4. Anyway, after looking over what I posted I realized my answer was complete. This particular question did not produce a precipitate.

[Stovn0611]

The question doesn't produce a precipitate? I thought that Ag2SO4 would precipitate considering it's solubility in water is only 0.31 g/100 mL water

[Arkcon]

NaSO4 does exist, the more common form is Na2SO4.

Really?  Do you have a citation for that?  Or at least an explanation for how the charges are balanced?  Assuming there's a precipitate -- and since the problem specifies one, we might as well play along, there's no points on the exam for "doesn't occur", you will need to know how much of each reagent is consumed to solve this problem, and we need to use compounds that exist.

[CKabes]

I don't think NaSO4 exists. Going from Na⁺ to Na⁺² requires a little more than 4.5 million joules, which is enough energy to power a 60 watt lightbulb for more than 21 hours (1 joule/watt/second). I think you mean Na₂SO₄.

[Borek]

But if I refer to my solubility table, neither of those products form a precipiate...

The simplest answer: NaSO₄ is not the only substance that you listed that doesn't exist. But once you will understand what is the problem with NaSO₄, you should see where is the other problem.