Solubility Table

Solubility rules are guidelines that predict whether ionic compounds will dissolve in water. They're essential in chemistry for predicting precipitation reactions, understanding chemical interactions in solutions, and determining which compounds will form precipitates in laboratory experiments.

Select the cation and anion of your compound from the dropdown menus. The table will show whether the resulting ionic compound is soluble, insoluble, or slightly soluble based on established solubility rules, along with the specific rule that applies.

Slightly soluble means the compound dissolves in water but only to a limited extent. These compounds typically have low solubility values and may form precipitates when their solubility limit is exceeded in solution.

For most ionic compounds, solubility increases with temperature. The solubility table shows values at different temperatures to help you understand how much of a compound can dissolve at specific conditions, which is important for laboratory work and industrial processes.

Yes, there are several important exceptions to solubility rules. For example, while most sulfates are soluble, barium sulfate and lead sulfate are insoluble. The table includes these exceptions to provide accurate predictions for compound solubility.

A saturated solution contains the maximum amount of solute that can dissolve at a given temperature and pressure. A dilute solution contains less solute than the maximum and can still dissolve more of the compound.

Precipitate formation depends on the solubility of the compound. When the concentration of ions exceeds the compound's solubility limit, or when two solutions are mixed and form an insoluble compound, a precipitate will form as a solid.