What are the solubility trends in ionic compounds?

Ionic compounds' solubility generally increases with temperature and decreases with increasing ionic size or charge.

In more detail, the solubility of ionic compounds is influenced by several factors. One of the most significant is temperature. As a general rule, the solubility of most ionic compounds increases as the temperature rises. This is because the increased kinetic energy of the water molecules makes it easier for them to break apart the ionic lattice and dissolve the ions.

Another important factor is the size and charge of the ions. Larger ions tend to be less soluble because they have a lower charge density, meaning the charge is spread out over a larger area. This makes it harder for the water molecules to surround and dissolve the ions. Similarly, ions with a lower charge are also less soluble for the same reason.

The nature of the solvent also plays a role. Polar solvents, like water, are good at dissolving ionic compounds because they can surround and separate the positive and negative ions. Non-polar solvents, on the other hand, are not good at dissolving ionic compounds because they cannot separate the ions as effectively.

Lastly, the 'like dissolves like' rule applies. This means that polar compounds will dissolve in polar solvents and non-polar compounds will dissolve in non-polar solvents. Since ionic compounds are polar, they are more likely to dissolve in polar solvents like water.

Remember, these are general trends and there can be exceptions. For example, some ionic compounds become less soluble with increasing temperature. Always refer to solubility charts or experimental data for specific compounds.