|This scientific article needs additional citations to secondary or tertiary sources (December 2009)|
|This article relies largely or entirely upon a single source. (June 2015)|
||This article needs attention from an expert in Chemistry. The specific problem is: complete lack of expert content derived from secondary sources, and chosen with a broad scholarly view of the modern discipline. (June 2015)|
||This article requires immediate attention for repeated appearance of dubious, naive, and non-scholarly statements on the title subject. (June 2015)|
The dissolution of gases, liquids, or solids into a liquid or other solvent is a process by which these original states become solutes (dissolved components), forming a solution of the gas, liquid, or solid in the original solvent. Solid solutions are the result of dissolution of one solid into another, and occur, e.g., in metal alloys, where their formation is governed and described by the relevant phase diagram.[not verified in body] In the case of a crystalline solid dissolving in a liquid, crystalline structure must disintegrated such that the separate atoms, ions, or molecules are released. For liquids and gases, the molecules must be be able to form non-covalent intermolecular interactions with those of the solvent for a solution to form.
The free energy of the overall, isolated process of dissolution must be negative for it to occur, where the component free energies contributing include those describing the disintegration of the associations holding the original solute components together, the original associations of the bulk solvent, and the old and new associations between the undissolved and dissolved materials.[not verified in body]
Dissolution is of fundamental importance in all chemical processes, natural and unnatural, from the decomposition of a dying organism and return of its chemical constituents into the biosphere, to the laboratory testing of new, man-made soluble drugs, catalysts, etc. Dissolution testing is widely used in industry, including in the pharmaceutical industry to prepare and formulate chemical agents of consistent quality that will dissolve, optimally, in their target millieus as they were designed.
Dissolution by class of compound
|This section does not cite any references or sources. (June 2015)|
Gaseous elements and compounds may also dissolve in another liquid depending on the compatibility of the chemical and physical bonds in the substance with those of the solvent.[dubious ] Hydrogen bonds play an important role in aqueous dissolution.
- NaCl(s) → Na+(aq) + Cl−(aq)
In a colloidal dispersed system, small dispersed particles of the ionic lattice exist in equilibrium with the saturated solution of the ions, i.e.
- NaCl(aq) Na+(aq) + Cl−(aq)
The solubility of ionic salts in water is generally determined by the degree of solvation of the ions by water molecules. Such coordination complexes occur by water donating spare electrons on the oxygen atom to the ion. The behavior of this system is characterised by the activity coefficients of the components and the solubility product, defined as:
The ability of an ion to preferentially dissolve (as a result of unequal activities) is classified as the Potential Determining Ion. This in turn results in the remaining particle possessing either a net positive/negative surface charge.
The solubility of polymers depends on the chemical bonds present in the backbone chain and their compatibility with those of the solvent.[dubious ] The Hildebrand solubility parameter is commonly used to evaluate polymer solubility. The closer the value of the parameters, the more likely dissolution will occur.[vague]
Rate of dissolution
|This section may have been copied and pasted from http://www.sciencedirect.com/science/article/pii/S0378517306005813/ ( · ), possibly in violation of Wikipedia's copyright policy. Please remedy this by editing this article to remove any non-free copyrighted content and attributing free content correctly, or flagging the content for deletion. Please be sure that the source of the copyright violation is not itself a Wikipedia mirror. (June 2015)|
||This section may require cleanup to meet Wikipedia's quality standards. The specific problem is: that the sophistication of the content of this section, esp. the prose following the equation, relative to the rest of the article, makes it suspect with regard to its use of this single paywalled source. (June 2015)|
The rate of dissolution quantifies the speed of the dissolution process. It depends on the chemical natures of the solvent and solute,[vague] the temperature (and possibly to a small degree, the pressure), the degree of undersaturation,[vague] the presence of a means of mixing during the dissolution, the interfacial surface area,[vague] and the presence of "inhibitors" (e.g., substances adsorbed on the surface).[vague]
- m, mass of dissolved material
- t, time
- A, surface area of the interface between the dissolving substance and the solvent
- D, diffusion coefficient
- d, thickness of the boundary layer of the solvent at the surface of the dissolving substance
- Cs, mass concentration of the substance on the surface
- Cb, mass concentration of the substance in the bulk of the solvent
For dissolution limited by diffusion, Cs is equal to the solubility of the substance. When the dissolution rate of a pure substance is normalized to the surface area of the solid (which usually changes with time during the dissolution process), then it is expressed in kg/m2s and referred to as "intrinsic dissolution rate". The intrinsic dissolution rate is defined by the United States Pharmacopeia.
Dissolution rates vary by orders of magnitude between different systems. Typically, very low dissolution rates parallel low solubilities, and substances with high solubilities exhibit high dissolution rates, as suggested by the Noyes-Whitney equation. However, this is not a rule.[according to whom?]
- Aristides Dokoumetzidis, Panos Macheras, 2006, "A century of dissolution research: From Noyes and Whitney to the Biopharmaceutics Classification System", Int. J. Pharm. 321(1-2), pp. 1–11, DOI 10.1016/j.ijpharm.2006.07.011, see , accessed 19 June 2015.[Subscription required]