Final answer:
Fe(OH)3, BaSO4, and MgCO3 are exceptions to the solubility rules as they are considered insoluble due to their specific chemical properties. Conversely, LiF, AgNO3, and Na2S are soluble, following the general solubility rules.
Step-by-step explanation:
The student is asking about the solubility rules for ionic compounds in water. According to the solubility rules provided, there are several exceptions to the general trends that can be applied to the list of compounds given (Fe(OH)3, BaSO4, LiF, AgNO3, Na2S, MgCO3). Here are the exceptions:
Fe(OH)3 is insoluble because hydroxide salts of transition metals are generally insoluble.
BaSO4 is insoluble as it is one of the specific exceptions stated among most sulfate salts.
MgCO3 is generally insoluble because Group II carbonates are insoluble.
On the other hand, LiF is soluble because salts of alkali metals have no exceptions to their solubility. Similarly, AgNO3 is soluble due to nitrates always being soluble, irrespective of the cation paired with them. Lastly, Na2S is soluble because it contains a sodium (Na+) cation, which is an alkali metal cation with solubility, as noted by the first rule.