Indicate whether each of the following ionic compounds is...

Indicate whether each of the following ionic compounds is soluble or insoluble in water: (9.3)
a. $\mathrm{KNO}_{3}$
b. $\mathrm{PbCl}_{2}$
c. $\mathrm{Mg}(\mathrm{OH})_{2}$
d. $\mathrm{NaBr}$
e. $\mathrm{Hg}_{2} \mathrm{Cl}_{2}$

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Key Concepts

Exceptions to General Solubility Rules

While solubility rules are useful for predicting behavior of ionic compounds in water, there are notable exceptions. Specific interactions between ions, structural factors, and other stabilizing forces can cause some compounds to behave differently than the general rules would suggest, underscoring the importance of experimental verification in certain cases.

Hydration Energy and Lattice Energy

This concept involves comparing the energy released when ions become surrounded by water molecules (hydration energy) with the energy required to break apart the ionic lattice (lattice energy). A compound is more likely to be soluble if the hydration energy outweighs the lattice energy, enabling the ions to dissociate in water.

Solubility Rules for Ionic Compounds

These rules provide guidelines to predict whether an ionic compound will dissolve in water. They generally indicate that salts containing alkali metal ions or nitrate ions are soluble, while compounds with certain metal cations or those containing hydroxide ions may be insoluble. Understanding these rules allows one to quickly assess the solubility of many ionic compounds.

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