We mix 10 grams of BaCl2 (does not has a ksp) with 5 grams of Ag2SO4 (has a ksp), we get a precipitate.

1) What does that precipitate contain?

2) What ions does the solution contain?

Given Ksp of BaSO4=1.08*10^-10 } Ksp of AgCl=1.5*10^-10 } ksp of Ag2SO4=2.8*10^-5

My confusion:

since BaCl2 dissociate completely -> BaCl2(s) -> Ba+2(aq) + 2Cl-(aq)

Finding the moles of Ba+2=0.048moles

Finding the moles of Cl-=0.096moles

Ag2SO4 is more soluble than BaSO4 and AgCl, but it has been said by lab professor than we can say that it dissolves completely and then test ourselves (Why?, what if it doesn't?)

So if we suppose it dissolves completely, i can treat it like BaCl2.

Finding the moles of Ag+=0.032moles

Finding the moles of SO4-2=0.016moles

Precipitate:

BaSO4 -> 0.016 moles 3.73 grams

AgCl-> 0.032 moles 4.58 grams

Ions remaining:

SO4-2=5.6*10-9 Ba+2=0.032 Cl-=0.064 Ag+=2.34*10^-9

How can we test now that our theory that Ag2SO4 dissolve completely? all of our calculations are based on that it did, what if it dissolved 50% or 80%, then we will have less Ag+ and SO4-2 and all our calculations will be wrong, is there a way to verify it? and when we can we use that theory that a salt dissolves completely since a ksp was given (it's not that small but still).

Appreciate the help

Thanks