Colloidal dispersions

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When two different substances are mixed together so that they mingle intimately, a two–component system is produced. When one component is distributed uniformly throughout the second, the first component is called the dispersed phase and the second, the dispersion medium or continuous phase. Either phase may be solid, liquid, or gas.

Frequently in pharmacy a solid substance is dispersed in a liquid, usually water, and the resulting substance may have the characteristics of either a molecular dispersion (true solution), a colloidal solution, or a coarse dispersion depending on the particle size of the dispersed solid. In true solutions, the dispersed particles are ions or small molecules having particle size less than one nanometer (nm) In colloidal dispersions, the particles are either single, large molecules of high molecular weight (macromolecules) or aggregates of smaller molecules with diameters between 1 nm and 500 nm in size (0.001 – 0.5). In coarse dispersion the particles are greater than 500 nm in diameter. Note that the particle size ranges given are not rigid and overlap does occur between each dispersion class.

The dispersed phase of a colloidal dispersion may be classified as being either lyophilic (solvent–loving) or lyophobic (solvent–hating). If the solvent is water, these classifications are termed as hydrophylic and hydrophobic respectively.

Since a uniform dispersion of particles is important for the diagnostic and therapeutic effectiveness as well as the safety of administration of pharmaceutical colloids, stability against settling or coprecipitation is an important consideration. The addition of a hydrophilic colloid to a hydrophobic one causes the hydrophilic colloid to adsorb onto and completely surround the hydrophobic particles which then take on some of the properties of the hydrophilic colloid. The hydrophilic colloid shields the hydrophobic system from the destabilizing effects of electrolytes; thus the hydrophilic substance is called a«protective colloid». Stability of such a system is enhanced, because in order to precipitate the hydrophobic colloid, both the protective solvent sheath surrounding it and the electric charge must be removed. Gelatin and methylcellulose derivatives are commonly used as protective colloids.

Sometimes in pharmaceutical formulations buffer salts are added to maintain a pH required for product stability. Occasionally such buffers may contribute to potential instability by forming insoluble salts with metallic ions. This problem may occur especially with phosphate buffers since most heavy metal phosphates are insoluble. If an insoluble phosphate salt precipitates from a colloidal dispersion, it may co–precipitate the colloidal particles along with it. To prevent this phenomenon from occurring, chelatingagents may be used that will preferentially complex the metal ions, and thus prevent them from reacting with the phosphate. Alternatively, nonphosphate buffers may be substituted for phosphate buffers, when feasible, to prevent the instability.

II.10. Составьте схему–классификацию типов дисперсионных коллоидных растворов на основании содержания текста.

II.11. Назовите меры, предохраняющие фармацевтические коллоидные растворы от порчи.

II.13. Прочтите текст С и составьте перечень инструкций по приготовлению эмульсий.