Well, well, my inquisitive friend! Let's dive into this question together and have some fun figuring out the answer.
To determine which salt is NOT more soluble in acidic solution than in pure water, we need to consider a few factors. When a salt dissolves in water, it dissociates into its constituent ions. In an acidic solution, we have the presence of extra H+ ions, which can potentially influence the solubility of salts.
Now, let's check out the options:
A. ZnS: Hmmm, I bet this little guy dissolves more in an acidic solution because Zn2+ ions love to hang out with those H+ ions.
B. AgCN: Silently lurking in the corner, it's one slippery silver cyanide. Well, Ag+ ions would still be attracted to H+ ions in an acidic solution, so it should be more soluble too.
C. Ba3(PO4)2: Oh, boy! This one looks complicated, doesn't it? But remember, we're looking for the salt that's not more soluble in acidic solution. Phosphate ions love being surrounded by water molecules, but I don't think the acidic environment will make them more willing to leave their aquatic friends.
D. ZnCO3: Zinc carbonate, oh my! Carbonate ions can get feisty in acidic solutions, so I'm thinking this one will be more soluble too.
E. BiI3: Ah, the elusive bismuth triiodide. Now, here's the trickster. Bismuth compounds are known to be quite insoluble, even in acidic solutions. So, this little fella stands out from the crowd and is our answer!
And there you have it! By considering the behavior of ions and the solubility characteristics of the salts, we deduce that option E, BiI3, is NOT more soluble in acidic solution than in pure water. Bravo, my friend!