The solubility of benzoic acid in water is approximately 0.027 M, according to Oral Roberts University. The concentration of benzoic acid over 33 trials averaged 0.0271 M in water at 77 degrees Fahrenheit, with carboxylic acid as the solute. The acid is more readily soluble in organic solvents rather than water.
Benzoic acid has a solubility of 2.355 M in acetone, 0.766 M in benzene, 2.634 M in ethanol, 5.294 M in dimethylacetamide, 0.081 M in octane, 2.867 M in methanol, 0.664 M in toluene and 2.5 M in triethylene glycol. The solubility of benzoic acid is high in ethanol and reasonably high in chloroform. The solubility of benzoic acid increases when the temperature rises in the solution.
Solubility is measured by attempting to dissolve substances in a given amount of solvent. The standard practice in chemistry is to use 100 milliliters of water or other liquids. Solubility can be listed as a certain amount of grams per 100 milliliters, according to the University of Wisconsin.
The capital "M" that designates the solubility refers to molarity. Clackamas Community College defines molarity as a chemical term that means moles per liter. A mole designates the amount of atoms in a certain weight of molecules based upon the atomic weights of substances. For instance, the solubility of benzoic acid in water is 0.027 moles of solute per liter of water. If an amount of moles per liter is higher in one solvent over another, that means a substance is more soluble in a particular solvent.