Which compound or compounds in each of the following groups...

Which compound or compounds in each of the following groups is (are) soluble in water?
(a) $\mathrm{CuO}, \mathrm{CuCl}_{2}, \mathrm{FeCO}_{3}$
(b) $\mathrm{AgI}, \mathrm{Ag}_{3} \mathrm{PO}_{4}, \mathrm{AgNO}_{3}$
(c) $\mathrm{K}_{2} \mathrm{CO}_{3}, \mathrm{KI}, \mathrm{KMnO}_{4}$

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Key Concepts

Solubility Rules for Ionic Compounds

This concept involves a set of empirical guidelines that predict whether an ionic compound will dissolve in water. For instance, compounds containing alkali metal ions and ammonium ions, as well as most nitrate, acetate, and chloride salts, are commonly soluble. Exceptions exist, however, such as certain phosphates and carbonates that are insoluble except when paired with highly soluble cations.

Ionic Dissolution Process

The dissolution of ionic compounds in water is driven by the interactions between the polar water molecules and the ions in the lattice. When water molecules surround individual ions, the process, known as hydration, helps to overcome the lattice energy that holds the ionic solid together, leading to the formation of a homogeneous solution.

Role of Lattice Energy and Hydration Energy

The solubility of an ionic compound depends on a balance between lattice energy and hydration energy. Lattice energy is the energy required to separate the ions in the ionic lattice, while hydration energy is the energy released when water molecules interact with and stabilize the free ions. A compound is soluble if the hydration energy compensates for the lattice energy.

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