Final answer:
To predict the solubility of ionic compounds in water, solubility rules that consider the combination of cations and anions are used. These rules classify compounds such as Zn(NO3)2 as soluble and compounds such as Sr3(PO4)2 as insoluble.
Step-by-step explanation:
To predict whether an ionic compound is soluble in water, we refer to a set of general guidelines known as solubility rules. These rules help us to categorize compounds as soluble or insoluble by considering the ions they contain. For the given set of compounds, we would use the solubility trends and specific rules mentioned in Table 9.5.1 and Table 4.3.1.
- Zn(NO3)2 is soluble because all nitrates (NO3) are soluble.
- PbBr2 is generally insoluble, except when combined with a strong ion like a nitrate.
- Sr3(PO4)2 is insoluble because most phosphates are not soluble.
- Mg(OH)2 is insoluble because hydroxides are typically insoluble except for those of alkali metals and Ba^2+.
- KBr is soluble because all compounds of alkali metal ions like K+ are soluble.
- Pb(NO3)2 is soluble due to the presence of the nitrate ion.
- BaSO4 is insoluble because sulfates of Ba^2+, Sr^2+, and Pb^2+ are typically insoluble.
- AgCl is insoluble due to the presence of Ag+ which forms insoluble chlorides, except when paired with the ion of an alkali metal or NH4+.
- Ba(NO3)2 is soluble given that all nitrates are soluble.
- Pbl2, although lead halides are generally insoluble, iodides are often the exception and are soluble.
- Mg(NO3)2 is soluble as it contains a nitrate ion.
- FeCl3 is soluble because chlorides are generally soluble, with some exceptions like Ag+, Pb^2+, and Hg2^2+.
- Pb(CH3COO)2 is soluble as most acetates are soluble.