What does the term deprotonated imply about a compound's solubility?

The term "deprotonated" refers to the removal of a proton (H⁺ ion) from a compound, typically resulting in the formation of a negatively charged species or an anion. The solubility of a compound in water can be significantly affected by its protonation state. Generally, when a compound is deprotonated, it becomes more polar due to the presence of negatively charged groups.

However, the solubility also depends on the nature of the substance itself. Some deprotonated compounds can become less soluble depending on their structure and the interactions they form with water molecules. This reduced solubility can stem from factors like hydrophobic characteristics or the formation of insoluble salt in solution.

For instance, while certain deprotonated organic acids may have increased solubility in water, others may not, particularly if they lead to species that are less favorable for solvation. Therefore, it is common to associate the deprotonation of a compound with being not very soluble, as deprotonation may lead to the formation of larger, more complex ions or compounds that do not easily interact with water compared to their protonated counterparts.