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

On the basis of the general solubility rules given in Table 7.1 , for each of the following compounds, explain why the compound would $n o t$ be expected to be appreciably soluble in water. Indicate which of the solubility rules covers each substance's particular situation. a. iron(III) hydroxide b. calcium carbonate c. cobalt(III) phosphate d. silver chloride e. barium sulfate

On the basis of the general solubility rules given in Table 7.1 , for each of the following compounds, explain why the compound would $n o t$ be expected to be appreciably soluble in water. Indicate which of the solubility rules covers each substance's particular situation.
a. iron(III) hydroxide
b. calcium carbonate
c. cobalt(III) phosphate
d. silver chloride
e. barium sulfate

Key Concepts

General Solubility Rules

These rules are empirical guidelines that indicate which ionic compounds tend to dissolve in water and which do not. They help predict solubility by noting trends, such as the high solubility of alkali metal and nitrate salts and the general insolubility of many hydroxides, carbonates, phosphates, and certain sulfates.

Precipitation Reactions

Precipitation reactions occur when mixing aqueous solutions leads to the formation of an insoluble solid, called a precipitate. The solubility rules allow one to predict if an insoluble compound will form, based on whether the product’s ion combinations are known to be insoluble in water.

Metal Hydroxide Solubility

Most metal hydroxides, especially those that are not paired with alkali metals, are generally insoluble in water. This is due to the strong lattice energies present in these compounds that are not sufficiently counteracted by hydration energy, resulting in little dissociation in aqueous solutions.

Halide Solubility Exceptions

Although halide salts are usually soluble, there are important exceptions. Certain metal halides, particularly those involving silver, lead, or mercury, form compounds that have appreciable covalent character and strong lattice energies, making them less soluble than other halides.

Sulfate Solubility Exceptions

Sulfate salts are commonly soluble, yet some, such as those of heavy or certain alkaline earth metals, have low solubility. The precipitation of these compounds occurs because the lattice energy in these specific sulfates is relatively high compared to the energy provided by hydration, thereby limiting their solubility in water.

Carbonate and Phosphate Solubility

Carbonates and phosphates are typically insoluble in water except when associated with alkali metals or ammonium ions. The insolubility arises because the lattice energies of these compounds generally exceed the hydration energy provided by water, inhibiting significant dissolution.

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