Hydrotrope
A hydrotrope is a compound that solubilises hydrophobic compounds in aqueous solutions. Typically, hydrotropes consist of a hydrophilic part and a hydrophobic part (like surfactants) but the hydrophobic part is generally too small to cause spontaneous self-aggregation.
Hydrotropes do not have a critical concentration above which self-aggregation 'suddenly' starts to occur (as found for micelle- and vesicle-forming surfactants, which have a critical micelle concentration or cmc and a critical vesicle concentration or cvc, respectively). Instead, some hydrotropes aggregate in a step-wise self-aggregation process, gradually increasing aggregation size. However, many hydrotropes do not seem to self-aggregate at all, unless a solubilisate has been added. Hydrotropes are in use industrially. Hydrotropes are used in detergent formulations to allow more concentrated formulations of surfactants. Examples of hydrotropes include sodium p-toluenesulfonate and sodium xylene sulfonate.
The term hydrotropy was originally put forward by Carl Neuberg[1] to describe the increase in the solubility of a solute by the addition of fairly high concentrations of alkali metal salts of various organic acids. However, the term has been used in the literature to designate non-micelle-forming substances, either liquids or solids, organic or inorganic, capable of solubilizing insoluble compounds.
The chemical structure of the conventional Neuberg’s hydrotropic salts (proto-type, sodium benzoate) consists generally of two essential parts, an anionic group and a hydrophobic aromatic ring or ring system. The anionic group is obviously involved in bringing about high aqueous solubility, which is a prerequisite for a hydrotropic substance. The type of anion or metal ion appeared to have a minor effect on the phenomenon[1]. On the other hand, planarity of the hydrophobic part has been emphasized as an important factor in the mechanism of hydrotropic solubilization[2][3]
Additives may either increase or decrease the solubility of a solute in a given solvent. These salts that increase solubility are said to ‘salt in’ the solute and those salts that decrease the solubility ‘salt out’ the solute. The effect of an additive depends very much on the influence, it has on the structure of water or its ability to compete with the solvent water molecules.[4] A convenient quantitation of the effect of a solute additive on the solubility of another solute may be obtained by the Setschetow equation:[5]
- ; where
- S0 = solubility in the absence of the additive
- S = solubility in the presence of the additive
- Ca = concentration of the additive
- K = salting coefficient, which is a measure of the sensitivity of the activity coefficient of the solute towards the salt.
References
- ^ a b Neuberg, C., Biochem. Z., 1916, 76, 107.
- ^ Evstigneev, M.P., Evstigneev V.P., Hernandez Santiago A.A., Davies, David B. 2006. Effect of a mixture of caffeine and nicotinamide on the solubility of vitamin (B2) in aqueous solution. European Journal of Pharmaceutical Sciences 28 (1-2) 59-66.
- ^ Suzuki,H., Sunada, H., 1998. Mechanistic studies on hydrotropic solubilization of nifedipine in nicotinamide solution, Chem & Pharm Bulletin.46 (1) 125-130.
- ^ Da Silva, R.C., Spitzer, M., Da Silva, L.H.M., Loh, W., 1999. Investigations on the mechanism of aqueous solubility increase caused by some hydrotropes, Thermochimica Acta., 328, 161-167.
- ^ Singhai, A., 1992. Studies on solubilization, formulation and evaluation of some drugs, Dept. of Pharm. Sci. Dr. H. S. Gaur vishwavidhyalaya., Sagar, 10.
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