In class, we've been working on predicting equations given particular chemicals, and later, actually testing some of them. I've been doing just fine, but I'm stuck on one of them-- 1. The problem statement, all variables and given/known data + attempted solutions I was given: AgNO3 + Na2SO4, and was told to predict what the products would be. Here is what my equation looks like--I know it's a double replacement reaction, and I matched up the ions, balanced them, and determined their solubility(using my rules): 2AgNO3(aq) + Na2SO4(aq) yields 2NaNO3 (aq) + Ag2SO4 (precipitate) However, when I did the lab, the 2 solutions, when mixed together, did not form a precipitate/did not form a solid. Thus, this means that the products of this reaction should all be aqueous, so that Ag2SO4 (precipate) should actually be aqueous. This does not seem to make sense to me though, as in my rules, it states that "sulfate salts are soluble/aqueous, but there are exceptions with Ag, Hg, Pb, Ca, Ba, and Sr" I repeated the lab 3 more times, getting the same results. Is there some sort of extra exception in this solubility rule? Why didn't I get a precipitate when my equation states that I should?