On the basis of the general solubility rules given in Table...

On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion. a. PbS b. $\mathrm{Mg}(\mathrm{OH})_{2}$ c. $\mathrm{Na}_{2} \mathrm{SO}_{4}$ d. $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}$ e. $\mathrm{BaCO}_{3}$ f. $\mathrm{AlPO}_{4}$ g. $\mathrm{PbCl}_{2}$ h. $\mathrm{CaSO}_{4}$

On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion.
a. PbS
b. $\mathrm{Mg}(\mathrm{OH})_{2}$
c. $\mathrm{Na}_{2} \mathrm{SO}_{4}$
d. $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}$
e. $\mathrm{BaCO}_{3}$
f. $\mathrm{AlPO}_{4}$
g. $\mathrm{PbCl}_{2}$
h. $\mathrm{CaSO}_{4}$

Key Concepts

General Solubility Rules

These are a set of guidelines used to predict whether an ionic compound is likely soluble in water. They include rules such as most compounds containing alkali metal ions (and ammonium) being soluble, while many compounds with non-alkali metal cations forming insoluble salts with anions like sulfides, hydroxides, carbonates, and phosphates.

Solubility of Sulfides

Sulfides are generally insoluble in water except when they are paired with alkali metal cations or ammonium ions. This low solubility is due to the strong ionic lattice that is not sufficiently overcome by the solvation energy provided by water.

Solubility of Hydroxides

Most hydroxides are insoluble in water, except for those of the alkali metals and ammonium. This is because the lattice energies of most metal hydroxides are too high compared to the hydration energy provided by water molecules, preventing dissolution.

Solubility of Sulfates

While many sulfate compounds are soluble in water, there are notable exceptions such as those of barium, lead, and calcium in some cases. The solubility of these compounds depends on the balance between the lattice energy of the salt and the hydration energy released when the salt dissolves.

Solubility of Carbonates

Carbonate salts are generally insoluble in water due to their relatively high lattice energies, except when paired with alkali metal ions or ammonium ions. This low solubility reflects the tendency of carbonate to form precipitates with many cations.

Solubility of Phosphates

Phosphates typically have very low solubility in water, as the lattice energy of these compounds is not sufficiently overcome by the hydration energy. Salts with alkali metal ions or ammonium are exceptions to this general rule.

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