Colloidal Dispersions
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CHAPTER 21 Colloidal Dispersions
Bill J Bowman, PhD Clyde M Ofner III, PhD Hans Schott, PhD
The British chemist Thomas Graham applied the term “colloid” An appreciable fraction of atoms, ions, or molecules of col- (derived from the Greek word for glue) ca 1850 to polypeptides loidal particles are located in the boundary layer between the such as albumin and gelatin; polysaccharides such as acacia, particle and the dispersion medium. The boundary layer be- starch, and dextrin; and inorganic compounds such as gelati- tween a particle and air is commonly referred to as a surface; nous metal hydroxides and Prussian blue (ferric ferrocyanide). whereas, the boundary layer between a particle and a liquid or Contemporary colloid and surface chemistry deals with an un- solid is commonly referred to as an interface. The ions/molecules usually wide variety of industrial and biological systems. A few within the particle and within the medium are surrounded on all examples include catalysts, lubricants, adhesives, latexes for side by similar ions/molecules and have balanced force fields; paints, rubbers and plastics, soaps and detergents, clays, ink, however, the ions/molecules at surfaces or interfaces are sub- packaging films, cigarette smoke, liquid crystals, drug delivery jected to unbalanced forces of attraction. Consequently, a surface systems, cell membranes, blood, mucous secretions, and aque- free energy component is added to the total free energy of col- ous humors.1–3 loidal particles and becomes important as the particles become smaller and a greater fraction of their atoms, ions, or molecules are located in the surface or interfacial region. As a result, the solubility of very fine solid particles and the vapor pressure of DEFINITIONS AND CLASSIFICATIONS very small liquid droplets are greater than the corresponding values for coarse particles and drops of the same materials. Colloidal Systems and Interfaces SPECIFIC SURFACE AREA—Decreasing particle size in- Except for high molecular weight polymers, most soluble sub- creases the surface-to-volume ratio, expressed as the specific surface area (Asp ). Specific surface area may expressed as the stances can be prepared as either low molecular weight solu- 2 3 tions, colloidal dispersions, or coarse suspensions depending area (A, cm ) per unit volume (V, cm ) or per unit mass (M, 2 3 upon the choice of dispersion medium and dispersion tech- gram). For a sphere, A 4 r and V 4/3 r , then Asp is: 4 nique. Colloidal dispersions consist of at least two phases—one 2 2 A 4 r 3 cm 3 or more dispersed or internal phases, and a continuous or ex- A cm 1 sp 3 3 ternal phase called the dispersion medium or vehicle. Colloidal V 4/3 r r cm r dispersions are distinguished from solutions and coarse disper- For density (d) of the material expressed as g/cm3, the specific sions by the particle size of the dispersed phase, not its compo- surface area is: sition. Colloidal dispersions contain one or more substances that have at least one dimension in the range of 1–10 nm at the A A 4 r2 3 cm2 lower end, and a few m at the upper end (covering about three Asp M Vd 4/3 r3d rd g orders of magnitude). Thus blood, cell membranes, thinner nerve fibers, milk, rubber latex, fog, and beer foam are colloidal Table 21-1 illustrates the effect of comminution on the specific systems. Some materials, such as emulsions and suspensions of surface area of a material initially consisting of one sphere hav- most organic drugs, are coarser than true colloidal systems but ing a 1-cm radius. The specific surface area increases as the ma- exhibit similar behavior. Even though serum albumin, acacia, terial is broken into a larger number of smaller and smaller and povidone form true or molecular solutions in water, the size spheres. Activated charcoal and kaolin are solid adsorbents of the individual solute molecules places such solutions in the having specific surface areas of about 6 106 cm2/g and 104 1–3,5–10 colloidal range (particle size 1 nm). cm2/g, respectively. One gram of activated charcoal has a sur- Several features distinguish colloidal dispersions from face area equal to 1/6 acre because of its extensive porosity and coarse suspensions and emulsions. Colloidal particles are usu- internal voids. ally too small for visibility in a light microscope because at least one of their dimensions measures 1 m or less. They are, how- ever, often visible in an ultramicroscope and almost always in Physical States of Dispersed an electron microscope. Conversely, coarse suspended particles and Continuous Phases are usually visible to the naked eye and always in a light mi- croscope. In addition, colloidal particles, as opposed to coarse A useful classification of colloidal systems is based upon the particles, pass through ordinary filter paper but are retained by state of matter of the dispersed phase and the dispersion dialysis or ultrafiltration membranes. Also, unlike coarse par- medium (ie, whether they are solid, liquid, or gaseous).2,7,8 ticles, colloidal particles diffuse very slowly and undergo little Common examples and various combinations are shown in or no sedimentation or creaming. Brownian motion maintains Table 21-2. The terms sols and gels are often applied to colloidal the dispersion of the colloidal internal phases. dispersions of a solid in a liquid or gaseous medium. Sols tend
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Table 21-1. Effect of Comminution on the Specific highly hydrated ions (eg, carboxylate, sulfonate, and alkylam- Surface Area of a Volume of 4 /3 cm3, Divided into monium ions) and/or organic functional groups that bind wa- Uniform Spheres of Radius Ra ter through hydrogen bonding (eg, hydroxyl, carbonyl, amino, and imino groups). NUMBER OF SPHERES R A (cm2/cm3) sp Hydrophilic colloidal dispersions can be further subdivided 1 1 cm 3 as: 103 0.1 cm 1 mm 3 10 106 0.1 mm 3 102 True solutions: water-soluble polymers (eg, acacia and povidone). 109 0.01 mm 3 103 Gelled solutions, gels, or jellies: polymers present at sufficiently high 1012 1 m3 104 concentrations and/or at temperatures where their water solubility 1015 0.1 m3 105 is low. Examples include relatively concentrated solutions of gelatin 1018 0.01 m3 106 and starch (which set to gels upon cooling) and methylcellulose (which gels upon heating). 1021 1 nm 3 107 23 8 Particulate dispersions: solids that do not form molecular solutions but 10 0.1 nm 3 10 remain as discrete though minute particles. Bentonite and micro- a Shaded region corresponds to colloidal particle-size range. crystalline cellulose are examples of these hydrosols. Lipophilic or oleophilic substances have a strong affinity for oils. Oils are nonpolar liquids consisting mainly of hydro- carbons having few polar groups and low dielectric constants. to have a lower viscosity and are fluid. If the solid particles form Examples include mineral oil, benzene, carbon tetrachloride, bridged structures possessing some mechanical strength, the vegetable oils (eg, cottonseed or peanut oil), and essential oils system is then called a gel. Prefixes typically designate the dis- (eg, lemon or peppermint oil). Oleophilic colloidal dispersions persion medium. For example, hydrosol (or hydrogel), alcosol include polymers such as polystyrene and unvulcanized or (or alcogel), and aerosol (or aerogel), designate water, alcohol, gum rubber dissolved in benzene, magnesium, or aluminum and air, respectively. stearate dissolved or dispersed in cottonseed oil, and activated charcoal which forms sols or particulate dispersions in all oils.
Interaction Between Dispersed Phases LYOPHOBIC DISPERSIONS and Dispersion Mediums The dispersion is said to be lyophobic (solvent-hating) when Ostwald originated another useful classification of colloidal there is little attraction between the dispersed phase and the dispersions based on the affinity or interaction between the dispersion medium. Hydrophobic dispersions consist of parti- dispersed phase and the dispersion medium.2,3,8 This classi- cles that are only hydrated slightly or not at all because water fication refers mostly to solid-in-liquid dispersions. Colloidal molecules prefer to interact with one another instead of solvat- dispersions are divided into the two broad categories, lyophilic ing the particles. Therefore, such particles do not disperse or dis- and lyophobic. Some soluble, low molecular weight substances solve spontaneously in water. Examples of materials that form have molecules with both tendencies and associate in solution, hydrophobic dispersions include organic compounds consisting forming a third category called association colloids. largely of hydrocarbon portions with few, if any, hydrophilic functional groups (eg, cholesterol and other steroids); some non- ionized inorganic substances (eg, sulfur); and oleophilic materi- LYOPHILIC DISPERSIONS als such as polystyrene or gum rubber, organic lipophilic drugs, paraffin wax, magnesium stearate, and cottonseed or soybean The system is said to be lyophilic (solvent-loving) if there is oils. Materials such as sulfur, silver chloride, and gold form hy- considerable attraction between the dispersed phase and the drophobic dispersions without being lipophilic. There is no liquid vehicle (ie, extensive solvation). The system is said to be sharp dividing line between hydrophilic and hydrophobic dis- hydrophilic if the dispersion medium is water. Due to the persions. For example, gelatinous hydroxides of polyvalent met- presence of high concentrations of hydrophilic groups, solids als (eg, aluminum and magnesium hydroxide) and clays such as bentonite, starch, gelatin, acacia, and povidone swell, (eg, bentonite and kaolin) possess some characteristics of disperse, or dissolve spontaneously in water to the greatest both.2,3,6,8 Common lipophobic dispersions include water-in- degree possible without breaking covalent bonds. Hydrophilic oil emulsions, which are essentially lyophobic dispersions in colloids often contain ionized groups that dissociate into lipophilic vehicles.
Table 21-2. Classification of Colloidal Dispersions According to State of Matter
DISPERSION MEDIUM (VEHICLE) DISPERSE PHASE SOLID LIQUID GAS SOLID Zinc Oxide Paste USP, toothpaste Sols: Bentonite Magma NF, Solid aerosols: (dicalcium phosphate or calcium Trisulfapyrimidines Oral Suspension Epinephrine Bitartrate Inhalation carbonate with aqueous sodium USP, Alumina and Magnesia Oral Aerosol USP, Isoproterenol carboxymethylcellulose binder), Suspension USP, Tetracycline Oral Sulfate Inhalation Aerosol USP, and pigmented plastics (titanium Suspension USP, Betamethasone smoke, and dust. dioxide in polyethylene). Valerate Lotion USP, and Prednisolone Acetate Ophthalmic Suspension USP. LIQUID Absorption bases (aqueous Emulsions: Mineral Oil Emulsion Liquid aerosols: medium in Hydrophilic USP, Benzyl Benzoate Lotion Metaproterenol Sulfate Petrolatum USP), emulsion bases USP, and soybean oil in water Inhalation Aerosol USP, (oil in Hydrophilic Ointment for parenteral nutrition, milk, Povidone-Iodine Topical USP, Lanolin USP), and butter and mayonnaise. Aerosol USP, mist, and fog. GAS Solid foams (foamed plastics Foams, carbonated beverages, and No colloidal dispersions. and rubbers) and pumice effervescent salts in water. 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 295
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ASSOCIATION COLLOIDS Organic compounds that contain large hydrophobic moieties on the same molecule with strongly hydrophilic groups are said to be amphiphilic. The individual molecules are generally too small to be in the colloidal size range, but they tend to associ- ate into larger aggregates when dissolved in water or oil. These compounds are designated association colloids because their aggregates are large enough to qualify as colloidal particles. Examples include surfactant molecules that associate into mi- celles above their critical micelle concentration (CMC) and phospholipids that associate into cellular membranes and lipo- somes, which have been used for drug delivery.
PROPERTIES OF COLLOIDAL DISPERSIONS Particle Shape Particle shape depends upon the chemical and physical nature of the dispersed phase and the method employed to prepare the dispersion (preparation methods are described in later sections). Primary particles exist in a wide variety of shapes, and their aggregation produces an even wider variety of shapes and structures. Preparation methods such as mechanical comminu- Figure 21-1. Transmission electron micrograph of a well-crystallized, tion and precipitation generally produce randomly shaped par- fine-particle kaolin. Note hexagonal shape of the clay platelets (courtesy, ticles unless the precipitating solids possess pronounced crys- John L. Brown, Engineering Experiment Station, Georgia Institute of tallization habits or the solids being ground possess strongly Technology). developed cleavage planes. For example, micronized particles of sulfonamides and other organic powders and precipitated aluminum hydroxide gels typically have irregular random shapes. An exception is bismuth subnitrate; hydrolyzing bis- have a larger specific surface area. For example, the grade muth nitrate solutions with sodium carbonate precipitates with the smallest average diameter, 5 nm, has a specific sur- lath-shaped particles. In addition, precipitated silver chloride face area of 380 m2/g. The finer-grade particles tend to sinter particles show their cubic nature under the electron micro- or grow together into chain-like aggregates resembling pearl scope. Lamellar or plate-like solids often preserve their lamel- necklaces during the manufacturing process (Fig 21-4). La- lar shape during mechanical comminution because milling and texes of polymers, such as latex-based paints, are aqueous dis- micronization break up the stacks of thin plates, in addition to persions prepared by emulsion polymerization. Their particles fragmenting plates in the lateral dimensions. In these materi- als, the molecular cohesion between layers is much weaker than the cohesion within layers. Examples of such materials in- clude graphite, mica, and kaolin (Fig 21-1). In a like manner, macroscopic asbestos and cellulose fibers consist of bundles of microscopic and submicroscopic fibrils that have very small di- ameters. Mechanical comminution splits these bundles into their component fibrils as well as cutting them shorter. Figure 21-2 shows the individual, needle- or rod-shaped cellulose crys- tallites formed after breaking up the aggregated bundles of mi- crocrystalline cellulose. These crystallites average 0.3 m in length and 0.02 m in width, which places them in the colloidal size range. Microcrystalline cellulose is a fibrous thickening agent and tablet additive made by the controlled hydrolysis of cellulose. Its manufacture is described in the 16–18th editions of this text, which also contain an electron micrograph of the porous, spongy, and compressible fibril bundle aggregates used in tableting. Except in the special cases of clay and cellulose just men- tioned, regular shaped particles are typically produced by con- densation rather than disintegration methods. For example, colloidal silicon dioxide is a white powder consisting of sub- microscopic spherical particles of rather uniform size (ie, nar- row particle size distribution). It is manufactured by high- temperature, vapor-phase hydrolysis of silicon tetrachloride in an oxy-hydrogen flame (ie, a flame produced by burning hydrogen in a stream of oxygen). It is commonly referred to as fumed or pyrogenic silica because of this manufacturing process. Different grades are produced by different reaction conditions. Figure 21-3 shows the relatively large, single Figure 21-2. Transmission electron micrograph of Avicel RC-591 thick- spherical particles of colloidal silicon dioxide. Their average ening grade microcystalline cellulose. The needles are individual cellulose diameter of 50 nm corresponds to the comparatively small crystallites; some are aggregated into bundles (courtesy, FMC Corpora- specific surface area of 50 m2/g. Smaller spherical particles tion; Avicel is a registered trademark of FMC Corporation). 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 296
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Figure 21-3. Transmission electron micrograph of Aerosil OX 50, ground Figure 21-4. Transmission electron micrograph of Aerosil 130, ground and dusted on. The spheres are translucent to the electron beam, causing and dusted on. The spheres are fused together into chain-like aggregates overlapping portions to be darker owing to an increased thickness (cour- (courtesy, Degussa AG of Hanau, Germany; Aerosil is a registered trade- tesy, Degussa AG of Hanau, Germany; Aerosil is a registered trademark of mark of Degussa). The suffix 130 indicates the specific surface area in Degussa). The suffix 50 indicates the specific surface area in m2/g. m2/g.
are spherical because polymerization of the solubilized liquid uid or gaseous suspending medium and represents a three-di- monomers takes place inside spherical surfactant micelles. mensional random walk. Some clays grow as plate-like particles possessing straight Suspended colloidal particles and solute molecules undergo edges and hexagonal angles (eg, bentonite and kaolin) (Fig 21- both rotational and translational Brownian movements. For 1). Other clays have lath-shaped (nontronite) or rod-shaped translational motion, Einstein derived the equation: particles (attapulgite).11 – Emulsification produces spherical droplets to minimize the x 2Dt oil-water interfacial area. Cooling an emulsion below the melt- where –x is the mean displacement in the x-direction in time, t, ing point of the dispersed phase freezes the dispersed particles and D is the diffusion coefficient. Einstein also showed that for in a spherical shape. For instance, paraffin may be emulsified spherical particles of radius, r, under conditions valid for in 80°C water and then cooled to room temperature to produce Stokes’ law and Einstein’s law of viscosity: a hydrosol containing spherical particles. Sols of viruses and globular proteins, which are hydrophilic, contain compact par- RT D ticles possessing definite geometric shapes. For example, the 6 rN poliomyelitis virus is spherical, the tobacco mosaic virus is where R is the gas constant, T is the absolute temperature, N rod-shaped, and the serum albumins and globulins are prolate ellipsoids of revolution (football-shaped). is Avogadro’s number, and is the viscosity of the suspending medium. A common measure of the mobility of a dissolved molecule or Diffusion and Sedimentation suspended particle in a liquid medium is the diffusion coeffi- cient. At room temperature, using units of cm2/sec, the value of The molecules of a gas or liquid are engaged in a perpetual and sucrose in water is 4.7 10 6 and the value of serum albumin random thermal motion causing collisions with one another in water is 6.1 10 7. Diffusion is a slow process on a macro- and with the container wall billions of times per second. Each scopic scale. Using the value of 1 10 7 cm2/sec, Brownian mo- collision changes the direction and the velocity of these tion causes a particle to move in one direction an average molecules. The continuous motion of molecules of a dispersion distance of 1 cm in 58 days, 1 mm in 14 hours, or 1 m in 0.05 medium randomly buffets any dissolved molecules and sus- seconds. As seen in the above equation, smaller molecules dif- pended colloidal particles. The random bombardment imparts fuse faster in a given medium. The radius of a sucrose molecule an erratic movement called Brownian motion to solutes and is smaller than that of a serum albumin molecule; the calcu- particles. This phenomenon is named after the botanist Robert lated values are 0.44 nm and 3.5 nm, respectively (assuming a Brown who first observed it under the microscope in an aque- spherical shape). Steroids have only slightly higher molecular ous pollen suspension. The Brownian motion of colloidal parti- weights than sucrose; however, their diffusion coefficients in cles magnifies the random movements of molecules in the liq- petrolatum-based absorption bases are in the 10 10 to 10 8 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 297
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cm2/sec range. These much smaller diffusion coefficients are The concentration of inorganic and organic colloidal disper- caused by the much higher vehicle viscosity. Passive diffusion sions and of bacterial suspensions can be measured by their (driven by a concentration gradient and carried out through Tyndall effect or turbidity. Turbidity, , is defined by an equa- Brownian motion) is important in the release of drugs from top- tion analogous to Beer’s law for the absorption of light,2,5–8 ical preparations and in the gastrointestinal absorption of namely: drugs. 1 I0 Brownian motion and convection currents maintain dis- ln l I solved molecules and small colloidal particles in suspension t indefinitely. This is true for all intrinsically stable systems where I0 and It are the intensities of the incident and transmit- when dissolution or dispersion occurs spontaneously and the ted light beams, and l is the length of the dispersion through corresponding free energy change is negative (see below). In which the light passes. The concentration of dispersed particles metastable or diuturna dispersions, Brownian motion pre- may be measured in two ways using turbidity. In turbidimetry, vents sedimentation and may extend their life for years. a spectrophotometer or photoelectric colorimeter is used to As particle size or r increases, Brownian motion decreases as measure the intensity of the light transmitted in the incident seen by the –x proportionality to r 1/2. Larger particles have a direction. The theoretical and practical aspects of determining greater tendency than smaller particles of the same material to the particle size of suspensions by turbidimetry and the feasi- settle to the bottom of the dispersion, provided the densities of bility of estimating their particle-size distribution are dis- 13 the dispersed phase, dP, and the liquid vehicle, dL, are suffi- cussed in two chapters by Kourti et al. If the dispersion is less ciently different (sedimentation, when dP dL). On the other turbid, the intensity of light scattered at 90° to the incident hand, larger particles will rise to the top of the dispersion when beam is measured with a nephelometer. Both methods require dP dL. This is known as creaming. The Stokes equation re- careful standardization, using suspensions that contain known flects the rate of sedimentation/creaming; it is expressed as: amounts of particles similar to those being studied. The turbid- ity of hydrophilic colloidal systems such as aqueous solutions of 2(d d )r2gt h P L gums, proteins, and other polymers is far weaker than that of 9 lyophobic dispersions. These solutions appear clear to the naked eye; however, their turbidity can be measured with a where h is the height (or distance) that a spherical particle photoelectric cell/photomultiplier tube and used to determine moves in time, t, and g is the acceleration of gravity. The equa- the molecular weight of the solute. tion illustrates that this rate is proportional to r2. Conse- The theory of light scattering was developed in detail by quently, as Brownian motion diminishes with increasing parti- Lord Rayleigh. For white, nonabsorbing nonconductors or di- cle size, the tendency of particles to sediment or cream is electrics like sulfur and insoluble organic compounds, the equa- increased. At a critical radius, the distance, h, that a particle tion obtained for spherical particles whose radius is small com- settles/creams equals the mean displacement, –x, due to Brown- pared to the wavelength of light ( ) is:2,5–8 ian motion over the same time interval, t, and therefore, the two are equal.12 Intravenous vegetable oil emulsions have little ten- 4 2n 2(n n )2 I I 0 1 0 (1 cos2 ) dency to cream because their mean droplet size, 0.2 m, is s 0 4d2c smaller than the critical radius. In most pharmaceutical sus- pensions, sedimentation prevails. I0 is the intensity of the unpolarized incident light; Is is the in- tensity of light scattered in a direction making an angle, , with the incident beam and measured at a distance, d. The scattered light is largely polarized. The concentration, c, is expressed as Light Scattering the number of particles per unit volume. The refractive indices, The optical properties of a medium are determined by its re- n1 and n0, refer to the dispersion and the dispersion medium, fractive index. Light will pass through the medium undeflected respectively. Since the intensity of scattered light is inversely when the refractive index is uniform throughout. However, proportional to the fourth power of the wavelength, blue light when there are discrete variations in the refractive index from ( 450 nm) is scattered much more strongly than red light the presence of particles or caused by small-scale density fluc- ( 650 nm). Colloidal dispersions of colorless particles appear tuations, part of the passing light will be scattered in all direc- blue when the incident white light is viewed in scattered light tions. When a narrow beam of sunlight is admitted through a (ie, in lateral directions such as 90° to the incident beam). Loss small hole into a darkened room, bright flashing points reveal of the blue rays due to preferential scattering leaves the trans- the presence of the minute dust particles suspended in the air. mitted light yellow or red. Preferential scattering of blue radia- A beam of light striking a particle polarizes the atoms and tion sideways accounts for the blue color of the sky, sea, molecules of that particle and induces dipoles, which act as sec- cigarette smoke, and diluted milk and for the yellow-red color ondary sources and reemit weak light of the same wavelength of the rising and setting sun viewed head-on. as the incident light. This phenomenon is called light scatter- The particles in pharmaceutical suspensions, emulsions, ing. The scattered radiation propagates in all directions away and lotions are generally larger than the wavelength of light, . from the particle. In a bright room, the light scattered by the When the particle size exceeds /20, destructive interference dust particles is too weak to be noticeable. between the light scattered by different portions of the same Colloidal particles suspended in a liquid also scatter light. particle lowers the intensity of the scattered light and changes When an intense, narrowly defined beam of light is passed its angular dependence. Rayleigh’s theory was extended to through a suspension, its path becomes visible because of the large and strongly absorbing and conducting particles by Mie light scattered by the particles in the beam. This Tyndall Beam and to nonspherical particles by Gans.1,2,5–8 It is possible to de- is characteristic of colloidal systems and becomes most visible termine the average particle size and even the particle size dis- when viewed against a dark background in a direction perpen- tribution of colloidal dispersions and coarser suspensions by dicular to the incident beam. The magnitude of the turbidity or means of turbidity measurements using appropriate precau- opalescence depends upon the nature, size, and concentration tions in experimental techniques and interpretations. of the dispersed particles. For example, when clear mineral oil DYNAMIC LIGHT SCATTERING—Light scattered by a is dispersed in an equal volume of a clear, aqueous surfactant moving particle undergoes a Doppler shift; its frequency in- solution, the resultant emulsion is milky white and opaque due creases slightly when the particle moves towards the photode- to light scattering. However, microemulsions containing emul- tector and decreases slightly when it moves away. This shift is sified droplets that are only about 40 nm in diameter (ie, much so small that it can only be detected by very intense, strictly smaller than the wavelength of visible light) are transparent monochromatic laser light. 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with a broadened frequency. Smaller particles diffuse faster their points of contact or entanglement, thus bringing about than larger ones and therefore produce greater Doppler broad- phase separation or precipitation. Hydrophobic bonding is an ening. If the particles are spherical, monodisperse, and their important contribution to the interchain attraction between concentration is so dilute that they neither attract nor repel one polypeptide chains even in solution. another, the frequency broadening can be used to estimate the Most water-soluble polymers have a higher solubility in hot particle diffusion coefficient, D. As noted above, the diffusion water than in cold water and tend to precipitate upon cooling coefficient is inversely proportional to the particle radius. The because the sheaths of hydration surrounding adjacent chains measured radius is actually the hydrodynamic radius (rH), become too sparse to prevent interchain attraction. Cooling di- which comprises the particle plus its attached water of hydra- lute solutions tends to separate them into a solvent phase and tion. The technique is called dynamic or quasi-elastic light scat- a viscous liquid phase that contains practically the entire tering. The technique is also called photon correlation spec- amount of polymer but still a large excess of solvent. This pro- troscopy (PCS) because it counts and correlates the number of cess is called simple coacervation and the polymer-rich liquid scattered photons over very short time intervals. For polydis- phase is referred to as a coacervate.1,15 If the polymer solution perse spherical colloidal particles, it estimates the particle size is concentrated enough and/or the temperature is low enough, distribution.2,5,8,9 Particles that are asymmetric rather than cooling causes the formation of a continuous network of precip- spherical and/or extensively hydrated have a larger rH and itating chains attached to one another through weak cross- hence smaller D value than unsolvated spherical particles with links that consist of interchain hydrogen bonds and van der the same dry volume. It is not possible to separate the effect of Waals forces at the points of mutual contact. Segments of regu- hydration upon rH, and D from the effect of asymmetry by PCS larly sequenced polymer chains will associate laterally into alone; either hydration or particle shape must be determined by crystalline bundles or crystallites. However, irregular chain other means.2,5,7–9 structures, such as those found in random copolymers, ran- In a related technique that uses a fiber-optic Doppler anemo- domly substituted cellulose ethers and esters, and highly meter (FODA), a laser beam is carried into the interior of a branched polymers like acacia, will prevent crystallization colloidal dispersion via a fiber-optic cable. Particles in the small during precipitation from solution. In these cases, chain entan- volume of dispersion around the immersed tip scatter light with glements provide the sole temporary crosslinks. A network of the Doppler frequency shift back into the same fiber to the associated polymer chains immobilizes the solvent, which may detector. This method is suitable for concentrated dispersions result in the separation of gelatinous precipitates or highly that are opaque to the laser beam and would have to be diluted swollen flocs, and in the case of more concentrated polymer extensively for conventional dynamic light scattering measure- solutions, may even cause the solution to set to a gel. 14 ments (see also the chapter by JC Thomas in reference 13). The most important factors causing phase separation, pre- cipitation, and gelation of polymer solutions are the chemical nature of the polymer and the solvent, temperature, polymer Viscosity concentration, and polymer molecular weight. Lower tempera- tures, higher concentrations, and higher molecular weights Most lyophobic dispersions have viscosities only slightly promote gelation and produce stronger gels. For a typical greater than that of the liquid vehicle. This holds true even at gelatin, 10% solutions acquire yield values and begin to gel at comparatively high volume fractions of the disperse phase un- about 25° C, 20% solutions gel at about 30° C, and 30% solu- less the particles form continuous network aggregates through- tions gel at about 32° C. The gelation is reversible, and the gels out the vehicle, in which case yield stresses are observed. By liquefy when heated above these temperatures. Regardless of contrast, the apparent viscosities of lyophilic dispersions, espe- concentration, gelation is rarely observed above 34° C, and cially of polymer solutions, are several orders of magnitude therefore, gelatin solutions do not gel at body temperature (ie, greater than the viscosity of the solvent or vehicle even at con- 37° C). Agar and pectic acid solutions set to gels at only a few centrations of only a few percent solids. Lyophilic dispersions percent of solids. Unlike most water-soluble polymers, methyl- are also generally much more pseudoplastic or shear-thinning cellulose, hydroxypropyl cellulose, and polyethylene oxide are than lyophobic dispersions. more soluble in cold water than in hot water. Therefore, their solutions tend to gel upon heating (ie, thermal gelation) instead of cooling. Gel Formation When dissolving powdered polymers in water, temporary gel formation often slows dissolution considerably. As water The flexible chains of dissolved polymers interpenetrate and diffuses into loose clumps of the powder, their exterior fre- entangle because of the constant Brownian motion of their quently turns to a cohesive gel of solvated particles encasing segments. The chains constantly writhe and change their con- the remaining dry powder. Such globs of gel dissolve very formations. Each chain is encased in a sheath of solvent slowly because of their high viscosity and the low diffusion molecules that solvate its functional groups. For example, coefficients of the polymers. For large-scale dissolution, it is water molecules are hydrogen-bonded to the hydroxyl groups helpful to disperse the polymer powder in water at tempera- of polyvinyl alcohol, hydroxyl groups, and ether linkages tures where the solubility of the polymer is lowest before it of polysaccharides, ether linkages of polyethylene oxide or can agglomerate into lumps of gel. Most polymer powders, polyethylene glycol, amide groups of polypeptides and povi- such as sodium carboxymethylcellulose, are dispersed with done, and carboxylate groups of anionic polyelectrolytes. This high shear in cold water before the particles can hydrate and envelope of water of hydration prevents chain segments that swell into sticky gel grains that agglomerate into lumps. Once are in close proximity from touching and attracting one another the powder is well dispersed, the mixture is heated with mod- through interchain hydrogen bonds and van der Waals forces erate shear to about 60°C for the quickest dissolution. Be- as they do in the solid state. The free solvent between the cause methylcellulose hydrates more slowly in hot water, the chains’ solvation sheaths acts as a lubricant allowing the sol- powder is dispersed with high shear in 1/5 to 1/3 of the re- vated chains to slip past one another when the solution flows. quired amount of water heated to 80–90° C. Once the powder However, any factor that lowers the hydration of dissolved is finely dispersed, the remaining amount of water is added macromolecules will reduce or thin out the sheath of hydration cold, or even as ice, and moderate stirring causes prompt dis- separating adjacent chains. When hydration is low, contiguous solution. For maximum clarity, fullest hydration, and highest chains tend to attract one another through secondary valence viscosity, the solution should be cooled to 0–10° C for about an forces such as hydrogen bonds and van der Waals forces, which hour. Alternatively, the polymer powder may be prewetted establish weak and reversible cross-links between the chains at with a water-miscible organic solvent (eg, ethyl alcohol or 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 299
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propylene glycol) that does not swell the polymer. The solvent hydrophilic colloids disperse or dissolve spontaneously in water should be added in a proportion of 3–5 parts of solvent to one and their sols are intrinsically stable. Therefore, the polymer part of polymer. If other nonpolymeric, powdered adjuvants may be redissolved by removing the coagulating salt through are to be incorporated into the solution, they are dry-blended dialysis or by adding more water. Whenever hydrophilic colloidal with the polymer powder and should comprise only 1/4 or less dispersions undergo irreversible precipitation or gelation, chem- of the blend for the best results. ical reactions are involved. Neither dilution with water, heating, Large increases in the concentration of polymer solutions nor attempts to remove the gelling or precipitating agent by may lead to precipitation and gelation. One way of effectively washing or dialysis will liquefy these gels. increasing the concentration of aqueous polymer solutions is to Most of the hydrophilic and water-soluble polymers men- add inorganic salts. The salts will bind part of the water in the tioned previously are only slightly soluble or insoluble in alco- solution in order to become hydrated. Competition for water of hol. Addition of alcohol to their aqueous solutions may cause hydration dehydrates the polymer molecules and precipitates precipitation or gelation because it lowers the dielectric con- them. This phenomenon is called salting out and may cause the stant of the medium and tends to dehydrate the hydrophilic so- polymer to separate as a concentrated, viscous liquid solution, lute. Alcohol also lowers the concentrations at which elec- a simple coacervate, or a solid gel. Because of its high solubility trolytes salt out hydrophilic colloids. Therefore, alcohol is often in water, ammonium sulfate is often used to precipitate and referred to as a nonsolvent or precipitant. However, the addi- separate proteins from dilute solutions. However, salting out is tion of alcohol to an aqueous polymer solution may cause coac- reversible and subsequent addition of water redissolves the ervation (ie, the separation of a concentrated viscous liquid precipitated polymers and liquefies their gels. phase) rather than precipitation or gel formation. Sucrose also HOFMEISTER OR LYOTROPIC SERIES—The effec- competes for water of hydration with hydrophilic colloids and tiveness of electrolytes to cause salting out depends upon their may cause phase separation. However, most hydrophilic sols extent of hydration. The Hofmeister or lyotropic series arranges tolerate substantially higher concentrations of sucrose than of ions in order of increasing hydration and increasing effective- electrolytes or alcohol. Lower viscosity grades of a given poly- ness in salting out hydrophilic colloids. The series for monova- mer are usually more resistant to the effects of electrolytes, al- lent and divalent cations are cohol, and sucrose than grades having higher viscosities and molecular weights. Cs Rb NH4 K Na Li The gelation temperature or gel point of gelatin is highest at its isoelectric point, where the attachment of adjacent chains and through ionic bonds between carboxylate ions and alkylammo- nium, guanidinium, or imidazolium groups is most extensive. Ba2 Sr2 Ca2 Mg2 Since carboxyl groups are not ionized in strongly acidic media The Hofmeister series governs many colloidal phenomena, in- such as gastric juices, interchain ionic bonds are practically cluding the effect of salts upon the temperature of gelation, the nonexistent in this environment and interchain attraction is swelling of aqueous gels, and the viscosity of hydrosols, and the limited to hydrogen bonds and van der Waals forces. Therefore, permeability of membranes towards salts. The series is ob- the combination of an acidic pH that is considerably below the served in many phenomena involving small atoms or ions and isoelectric point and a temperature of 37° C completely pre- true solutions, including the ionization potential and elec- vents the gelation of gelatin solutions. Conversely, if a polymer tronegativity of metals; the heats of hydration of cations; the size owes its solubility to the ionization of these weakly acid groups, of hydrated cations; the viscosity, surface tension, and infrared reducing the pH of its solution below 3 may lead to precipitation spectra of salt solutions; and the solubility of gases in salt solu- or gelation. This is observed with carboxylated polymers such tions. This series also arranges cations in order of increasing as many gums, sodium carboxymethylcellulose, and carbomer. ease in displacement from cation-exchange resins based on the Adjusting the media to higher pH values returns the carboxyl smaller hydrated specie size (eg, K displaces Na and Li ). Ad- groups to their ionized state and reverses the gelation or pre- sorption in the Stern layer of particles (see below) also illus- cipitation. However, gelation temperatures typically depend 16,17 trates the series. The lithium ion is more extensively hydrated, more upon temperature and concentration than pH. and therefore, Li (aq), including the hydration shell, is larger Hydrogen carboxymethylcellulose swells and disperses but than Cs (aq). Due to its smaller size, the hydrated cesium ion does not dissolve in water. Only the sodium, potassium, ammo- can approach a negative particle’s surface more closely than the nium, and triethanolammonium salts of carboxylated polymers hydrated lithium ion. Moreover, because of its greater electron are well soluble in water. In the case of carboxymethylcellulose, cloud, the Cs ion is more polarizable than the Li ion. There- salts with heavy metal cations (eg, silver, copper, mercury, fore, the Cs ion is more strongly adsorbed in the Stern layer. lead) and trivalent cations (eg, aluminum, chromic, ferric) are For anions, in order of decreasing effectiveness in salting practically insoluble. Salts with divalent cations, especially of out, the lyotropic series is the alkaline earth metals, have borderline solubilities. Gener- ally, higher degrees of substitution tend to increase the toler- 3 2 2 2 F citrate HPO4 tartrate SO4 acetate ance of carboxymethylcellulose toward salts. When inorganic salts of heavy or trivalent cations are mixed Cl NO3 ClO3 Br ClO4 I CNS with alkali metal salts of carboxylated polymers in solution, Iodides and thiocyanates, and to a lesser extent bromides and precipitation or gelation occurs due to metathesis. For instance, nitrates, actually tend to increase the solubility of polymers in if a soluble copper salt is added to a solution of sodium car- water (ie, salt them in).1,2,5–8 These large polarizable anions re- boxymethlycellulose, the double decomposition can be schemat- duce the extent of hydrogen bonding among water molecules, ically written as: and thereby, make more of the hydrogen-bonding capacity of R1COO Na R2COO Na CuSO4 → water available to the solute. Most salts, except for nitrates, bromides, perchlorates, iodides, and thiocyanates, raise the O O
temperature of precipitation or gelation of most hydrophilic col- ∧ loidal solutions. Exceptions among hydrophilic colloids are R1CCuCR2 Na3SO4 J ∧ methylcellulose, hydroxypropyl cellulose, and polyethylene OO oxide, whose gelation temperatures or gel melting points are lowered by salting out. R1 and R2 represent two carboxymethylcellulose chains, which Most hydrophilic sols require electrolyte concentrations of are cross-linked by a chelated copper ion. Dissociation of the 1 M or higher to induce precipitation or gelation. In addition, cupric carboxylate complex is negligible. 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 300
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Electric Properties the surface of an aluminum hydroxide particle that has one such negative group neutralized by a Na counterion: ORIGIN OF ELECTRIC CHARGES—Particles can ac- quire charges from several sources. In proteins, one end group of HO the polypeptide chain and any aspartic and glutamic acid units J contribute carboxylic acid groups, which are ionized into nega- AlMOH tively charged carboxylate ions in neutral to alkaline media. The HO other chain end group and any lysine units contribute amino HO OH groups, while arginine units contribute guanidine groups, and J histidine units contribute imidazole groups. The nitrogen atoms Al J of these groups become protonated in neutral to acid media. These covalently attached anions and cations confer a negative HO O HNa and positive charge to the molecule, respectively. Therefore, pro- HO J teins may be referred to as polyelectrolytes (polymeric elec- M trolytes or salts). However, they are not the only organic poly- Al OH mers that contain ionic groups, and thus, many substances may HO be considered to be polyelectolytes. For example, natural polysaccharides of vegetable origin such as acacia, tragacanth, At a pH of 8.5 to 9.1, there are neither Al(OH) nor Al(OH) alginic acid, and pectin contain carboxylic acid groups, which 2 4 ions on the particle surface but only neutral Al(OH)3 are ionized in neutral to alkaline media. Agar and carrageenan, molecules.18,19 Therefore, the particles have no charge and do as well as the animal polysaccharides heparin and chondroitin not need counterions for charge neutralization. This pH is con- sulfate, contain sulfate groups, which are strongly acidic and sidered to be the isoelectric point. In the case of inorganic par- ionize even in acid media. Cellulosic polyelectrolytes include ticulate compounds such as aluminum hydroxide, it also is sodium carboxymethylcellulose, while synthetic carboxylated called the zero point of charge. polymers include carbomer, a copolymer of acrylic acid. Bentonite clay is a lamellar aluminum silicate. Each lattice Counterions are required for electroneutrality of the ioniz- layer consists of a sheet of hydrated alumina sandwiched be- ing groups on polyelectrolytes. Counter-ions dissociate from tween two silica sheets. Isomorphous replacement of Al3 by ionogenic functional groups and can be replaced by other ions of Mg2 or of Si4 by Al3 confers net negative charges to the thin like charge. For example, in neutral and alkaline media, Na , 2 2 clay lamellas in the form of cation-exchange sites resembling K , Ca , and Mg are among the counterions neutralizing silicate ions built into the lattice. The counterions producing the negative charges of the carboxylate groups, and if hy- electroneutrality are usually Na (sodium bentonite) or Ca2 drochloric acid was used to make the medium acidic and to sup- (calcium bentonite). ply the protons, Cl is present to neutralize any of the cationic Silver iodide sols can be prepared by the reaction: groups mentioned previously. These counterions are not an in- tegral part of the protein particle but are located in its immedi- AgNO3 NaI → AgI(s) NaNO3 ate vicinity. Alternatively, at a specific intermediate pH value In the bulk of the silver iodide particles, there is a 1:1 stoichio- (4.5–7 for most proteins), the carboxylate anions and the alky- lammonium, guanidinium, and imidazolium cations on the metric ratio of Ag :I ions. If the above reaction is carried out with an excess of silver nitrate, there will be more Ag ions same molecule neutralize each other exactly. There is no need for counterions because the ionized functional groups are in ex- than I ions in the surface layer of the particles. The particles will then be positively charged and the counterions surround- act balance. At this pH value, called the isoelectric point, the protein particle or molecule is neutral; its electrical charge is ing them will be NO3 . If the reaction is carried out using an ex- neither negative nor positive, but zero.2,6,8 act stoichiometric 1:1 ratio of silver nitrate to sodium iodide or Most inorganic particulate compounds are also charged. with an excess sodium iodide, the surface of the particles will contain more I ions than Ag ions.6–8 The particles will then Aluminum hydroxide, Al(OH)3, may be dissolved by acids and 3 be negatively charged and the counterions surrounding them alkalis to form aluminum ions, Al , and aluminate ions, Al(OH) , respectively. In neutral or weakly acid media (ie, will be Na . 4 An additional mechanism through which particles acquire acid concentrations too low to cause dissolution), an aluminum 5,7,8,10 hydroxide particle has some positive charges attributed to Al3 electric charges is by the adsorption of ions, including ionic valences that have not been completely neutralized. The surfactants. This is discussed in more detail in a later section. schematic below represents a portion of the surface of an alu- ELECTRIC DOUBLE LAYERS—As described previously, the surface layer of a silver iodide particle prepared using an minum hydroxide particle that has one such positive charge neutralized by a Cl counterion: excess of sodium iodide contains more I ions than Ag ions; whereas, the bulk of the particle contains the two ions in an HO equimolar proportion. The aqueous solution in which such par- J ticles are suspended contains relatively high concentrations of M Al OH Na and NO3 , a lower concentration of I , and traces of H , HO OH , and Ag . The negatively charged particle surface attracts positive ions from the solution and repels negative ions. There- HO J fore, the solution immediately surrounding the particle surface contains a much higher concentration of Na (counterions) and Al Cl a much lower concentration of NO3 ions than in the bulk solu- HO tion. A number of Na ions equal to the number of excess I HO ions in the surface (ie, the number of I ions in the surface layer J M minus the number of Ag ions in the surface layer) and equiv- Al OH alent to the net negative surface charge of a particle are pulled HO towards its surface. These counterions tend to approach the particle surface as closely as their hydration spheres permit In weakly alkaline media (ie, base concentrations too low to (Helmholtz double layer); however, thermal agitation of the wa- transform the aluminum hydroxide particles completely into ter molecules tends to disperse them throughout the solution. aluminate and dissolve them), the aluminum hydroxide parti- Consequently, the layer of counterions surrounding the particle cles bear some negative charges due to the presence of a few is spread out. The Na ion concentration is highest in the im- aluminate groups. The schematic below represents a portion of mediate vicinity of the negative surface, where the ions form a 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 301
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compact layer called the Stern layer. The Na ion concentra- bilizes the dispersion against interparticle attachments or co- tion decreases with distance from the surface, throughout a dif- agulation. The electrostatic repulsive energy has a range in the fuse layer called the Gouy-Chapman layer. Therefore, the order of . sharply defined, negatively charged particle surface is sur- A quantitative theory of the interaction between lyophobic rounded by a cloud of Na counterions required for electroneu- disperse particles was worked out independently by Derjaguin trality. The combination of the two layers of oppositely charged ions constitutes an electric double layer, which is illustrated in the top part of Figure 21-5. The electric potential of a plane is equal to the work re- quired to bring a unit electric charge from infinity (in this case, from the bulk of the solution) to that plane against electrostatic forces. If the plane is the surface of a particle, the potential is called surface or 0 potential, which measures the total poten- tial of the double layer (Fig 21-5). This is the thermodynamic potential that operates in galvanic cells. Upon moving away from the particle surface towards the bulk solution in the di- rection of the horizontal axis, the potential drops rapidly across the Stern layer because the Na ions in the immediate vicinity of the particle surface screen Na ions that are farther removed in the diffuse part of the double layer from the effect of the neg- ative surface charge. The decrease in potential across the Gouy- Chapman layer is more gradual. As the composition of the dif- fuse double layer gradually approaches that of the bulk liquid, where the anion concentration equals the cation concentration, the potential asymptotically approaches zero. In view of this in- definite end point, the thickness of the diffuse double layer ( ) is arbitrarily defined as the distance over which it takes the po- tential at the boundary between the Stern and Gouy-Chapman layers to drop to 0.37 (equal to 1/e) of its value (Fig 21- 5).1,2,4,6–10 The thickness of double layers usually ranges from 1 to 100 nm and decreases as the concentration of electrolytes in solution increases. This occurs more rapidly for higher valence counterions. The value of is approximately equal to the recip- rocal of the Debye-Hückel theory parameter ( ). The electrokinetic or (zeta) potential has practical impor- tance because it can be measured experimentally. In aqueous dispersions, organic particles containing polar functional groups, and even relatively hydrophobic inorganic particles, are surrounded by a layer of water of hydration, which is asso- ciated with the particles through ion-dipole and dipole-dipole interactions. When a particle moves, this shell of water, and all of the ions located inside it, moves along with the particle. Con- versely, if water or an aqueous solution flows through a fixed bed of these solid particles, the hydration layer surrounding each particle remains attached to it. The electric potential at the plane of shear or slip separating the bound water from the free water is the potential. It does not include the Stern layer and includes only the part of the Gouy-Chapman layer that lies outside the hydration shell (Fig 21-5). STABILIZATION BY ELECTROSTATIC REPULSION— When two uncharged hydrophobic particles are in close prox- imity, they attract each other by van der Waals secondary va- lences, mainly London dispersion forces. For individual atoms and molecules, these forces decrease with the seventh power of the distance between them. In the case of two particles, every atom of one particle attracts every atom of the other particle. Because the attractive forces are nearly additive, they decay much less rapidly with interparticle distance, approximately with the second or third power of the distance between them. Therefore, whenever two particles approach each other closely, the attractive forces take over and cause them to adhere. Co- agulation occurs as the primary particles aggregate into in- creasingly larger secondary particles or flocs. If the dispersion consists of two kinds of particles, one having positive and the other negative charges, the electrostatic attraction between such oppositely charged particles is superimposed on the at- traction by van der Waals forces and coagulation is accelerated. If the dispersion contains only one kind of particle with the same surface charge and charge density (the most common Figure 21-5. Electric double layer at the surface of a silver iodide particle case) then electrostatic repulsion tends to prevent the particles (upper part) and the corresponding potentials (lower part). The distance from approaching closely enough to come within the effective from the particle surface, plotted on the horizontal axis, refers to both the range of each other’s van der Waals attractive forces. This sta- upper and lower portions of the figure. 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 302
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and Landau in the USSR and by Verwey and Overbeek in the the absolute value of the potential is small, the resultant Netherlands in the early 1940s.1–3,5,7–9 Detailed calculations potential energy is negative and van der Waals forces of at- may be found in Chapter 21 of RPS-17. The so-called DLVO the- traction predominate over electrostatic repulsion at all inter- ory predicts and explains many, but not all, experimental data; particle distances. Such sols coagulate rapidly. its refinement to account for discrepancies is ongoing. The The two identical particles, whose interaction is depicted in DLVO theory is summarized in Figure 21-6, where curve WA Figure 21-6, have a large (positive or negative) potential, re- represents the van der Waals attractive energy, which de- sulting in an appreciable positive or repulsive potential energy creases approximately by the second power of the interparticle at intermediate distances. However, Brownian motion, convec- distance, and curve ER represents the electrostatic repulsive tion currents, sedimentation, or stirring of the dispersion will energy, which decreases exponentially with interparticle dis- eventually put them on a collision course. As the two particles tance. Because of the combination of these two opposing effects, approach each other, the two counterion atmospheres begin attraction predominates at small and large distances; whereas to interpenetrate or overlap at point A, corresponding to the repulsion may predominate at intermediate distances. Nega- distance, dA. This produces a net repulsive (positive) energy be- tive energy values indicate attraction and positive values indi- cause of the work involved in distorting the diffuse double lay- cate repulsion. The resultant curve DPBAS, obtained by alge- ers and pushing water molecules and counterions aside. If the braic addition of curves WA and ER, gives the total, net energy particles continue to approach each other, the repulsion be- of interaction between two particles. tween their surface charges increases the net potential energy Interparticle attraction depends mainly upon the chemical of interaction to its maximum positive value at B, where most of nature and particle size of the dispersed material. Once these the intervening water and counterions have been displaced. If have been selected, the attractive energy between particles is the height of the potential energy barrier B exceeds the kinetic fixed and cannot be readily altered. Electrostatic repulsion de- energy of the approaching particles, they will not come any pends upon the 0 potential, or the density of the surface closer to each other than the distance dB and will then move charge, and upon the thickness of the double layer, both of away from each other. A net positive potential energy of about which govern the magnitude of the potential. Thus, dispersion 25 kT units usually suffices to keep them apart and renders the stability correlates to some extent with this potential.6 The dispersion stable (k is the Boltzmann constant and T is absolute potential can be widely adjusted using additives, especially temperature). At T 298°K, the required potential energy for ionic surfactants, water-miscible solvents, and electrolytes. If stabilization corresponds to 1 10 12 erg or 1 10 5 J. The kinetic energy of a particle is of the order of kT. On the other hand, if the kinetic energy of the approaching particles exceeds the potential energy barrier B, the particles will continue to approach each other past dB, where the van der Waals forces of attraction become increasingly more important compared to the electrostatic repulsion. Therefore, the net po- tential energy of particle interaction decreases to zero and then becomes negative. This now pulls the particles closer together. When the particles touch, at a distance, dP, the net energy has acquired a large negative value of P. This deep minimum in po- tential energy corresponds to a very stable situation in which the particles adhere. Since it is unlikely that enough kinetic en- ergy can be supplied to the particles or that their potential can be increased sufficiently to cause them to climb out of the po- tential energy well P, they are permanently attached to each other. When most or all of the primary particles agglomerate into secondary particles by this process, the sol coagulates. Any closer approach of the two particles than the touching distance dP will cause a very rapid rise in potential energy along PD be- cause the solid particles would interpenetrate each other and cause atomic orbitals to overlap (Born repulsion). COAGULATION OF HYDROPHOBIC DISPERSIONS— The height of the potential energy barrier and the range over which the electrostatic repulsion is effective (or the thickness of the double layer) determine the stability of hydrophobic disper- sions. Both factors are reduced by the addition of electrolytes. The transition between a coagulating and a stable sol is gradual and depends upon the time of observation. Therefore, standard- ized conditions must be used to classify a sol as either coagulated or coagulating, or stable (ie, fully dispersed). To determine the coagulating concentration of a given elec- trolyte for a given sol, a series of test tubes is filled with equal portions of the sol. Identical volumes of electrolyte solutions having increasing concentrations are added to the test tubes with vigorous stirring. After a certain rest period (eg, 2 hours), the mixtures are agitated again. After an additional, shorter rest period (eg, 1/2 hour), they are inspected for signs of coagu- lation. The tubes are then classified into two group; one show- ing no signs of coagulation and the other showing at least some signs such as visible flocs. Alternatively, they can be classified into one group showing complete coagulation and another Figure 21-6. Curves representing the van der Waals energy of attraction showing none or incomplete coagulation, such as some defloc- (WA), the energy of electrostatic repulsion (ER), and the net energy of in- culated colloid left in the supernatant. In either case, the sepa- teraction (DPBAS) between two identical charged particles, as a function ration between the two classes is quite sharp. The intermediate of the interparticle distance. agitation breaks the weakest interparticle bonds and brings 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 303
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smaller particles into contact with larger ones, thus sharpening the surface potential. When silver nitrate is added to the nega- the distinction between coagulation and stability. After repeat- tively charged silver iodide dispersion, some of its silver ions are ing the experiment with a narrower range of electrolyte con- incorporated into the negatively charged surface of the particles. centrations, the coagulation value (c ) of the electrolyte (ie, the This lowers the magnitude of the particle’s surface charge by re- cv ducing the excess of I ions in the surface. Therefore, silver salts lowest concentration at which the electrolyte coagulates the sol) are exceptionally effective coagulating agents because they reduce is established with good reproducibility.2,6–8 the magnitude of both the 0 potential and the potential. Indif- Typical ccv values for a silver iodide sol prepared with an ex- ferent salts, which only reduce the potential, require much cess of iodide are listed in Table 21-3. The following conclusions higher salt concentrations for comparable reductions in this po- can be drawn from the left half of Table 21-3: tential. The other potential-determining ion of silver iodide is the I ion. Alkali iodides have ccv values higher than 141 mmol/L be- 1. The ccv does not depend upon the valence of the anion. For exam- cause they supply iodide ions that enter the surface layer of the sil- ple, nitrate and sulfate salts of the same metal have nearly iden- ver iodide particles and increase its excess of I ions over Ag ions, tical c values. cv thereby making the 0 potential more negative. Bromide and 2. The differences between the ccv’s of cations having the same va- chloride ions act similarly but less effectively. The principal po- lence are relatively minor. However, there is a slight but signifi- tential-determining ion for proteins is H (and hence OH ); those cant trend of decreasing ccv with increasing atomic number in both for aluminum hydroxide are OH (and hence H ) and, Al3 as well the alkali and the alkaline earth metal groups. Arranging these as Fe3 and Cr3 , which form mixed hydroxides with Al3 . cations in order of decreasing ccv produces the Hofmeister or ly- 5. The cationic surfactant and the alkaloidal salts (which also be- otropic series in decreasing size of hydrated specie. For monova- have as cationic surfactants) on the right side of Table 21-3 con- lent cations, the lyotropic series is described above. The atomic stitute the second exception to the Schulze-Hardy rule. Surface- weight of cesium is 19x greater than that of lithium, but the Cs active compounds contain both hydrophilic and hydrophobic ion in aqueous solution is less hydrated and therefore smaller than moieties within the same molecule. The dual nature of these com- the hydrated Li ion. It is also more polarizable. Therefore, the pounds causes them to accumulate at interfaces. Dodecylammo- Cs ion can approach the surface of a negatively charged particle nium and alkaloidal cations are able to displace inorganic mono- suspended in water more closely and is more extensively ad- valent cations from the Stern layer of a negatively charged silver sorbed. This reduces its ccv making cesium salts more effective co- iodide particle. This occurs because they are not only attracted to agulants than lithium salts for negatively charged hydrosols. the particle by electrostatic forces but also by van der Waals 3. The coagulation values depend primarily upon the valence of the forces between their hydrocarbon moieties (ie, dodecyl chains in counterions, decreasing by one to two orders of magnitude for the case of the dodecylammonium ions) and the solid particle. each unit increase in the valence of the counterions (Schulze- Since they are strongly adsorbed from solution onto the particle Hardy rule). According to the DLVO theory, the coagulation val- surface and do not tend to dissociate from it, surface-active ues vary inversely with the sixth power of the valence of the coun- cations are very effective in reducing the negative potential of terions. For mono-, di-, and trivalent counterions, they should be silver iodide particles. Therefore, they have lower ccv values than in the ratio: purely inorganic cations with the same valence. 6. Anionic surfactants, like those containing lauryl sulfate ions, also 1 1 1 6 : 6 : 6 or 100 : 1.6 : 0.14 have a tendency to adsorb at solid-liquid interfaces. However, elec- 1 2 3 trostatic repulsion between the negatively charged surface of the
The mean ccv values for the mono-, di-, and trivalent counteri- silver iodide particles, whose surface layer contains an excess of ons in Table 21-3 are 141, 2.45, and 0.068 mmol/L, respec- iodide ions, and the surface-active anions usually prevents adsorp- tively. This results in a ratio of 100:1.7:0.05, which is in satis- tion from occurring below the critical micelle concentration. If ad- sorption does occur, it increases the density of the negative charges factory agreement with the DLVO theory. in the particle surface, and therefore, raises the ccv value of the an- The following conclusions can be drawn from the right half ionic surfactant above the value corresponding to its valence. of Table 21-3: 4. The cations on the right side of Table 21-3 constitute obvious The addition of water-miscible solvents such as alcohol, glyc- exceptions to the preceding conclusions. Ag is a potential- erin, propylene glycol, or polyethylene glycols to aqueous dis- determining counterion, those whose concentration determines persions lowers the dielectric constant of the medium. This re- duces the thickness of the double layer and, therefore, reduces the range over which electrostatic repulsion is effective, and lowers the size of the potential energy barrier. As a result, the Table 21-3. Coagulation Values for Negative Silver addition of sufficient amounts of such solvents tends to coagu- a Iodide Sol late aqueous dispersions. At lower concentrations, these sol-
ELECTROLYTE ccv (mmol/L) ELECTROLYTE ccv (mmol/L) vents do not induce coagulation themselves, but make the dis- persions more sensitive to coagulation by added electrolytes (ie, LiNO 165 AgNO 0.01 3 3 they lower the c value). NaNO 140 1/2(C H NH ) SO 0.07 cv 3 12 25 3 2 4 Progressive addition of salts having counterions of high va- 1/2(Na2SO4) 141 Strychnine nitrate 1.7 KNO 136 1/2(Morphine sulfate) 2.5 lence gradually reduces the potential of colloidal particles to 3 zero. Eventually, the sign of the potential may be inverted, 1/2(K2SO4) 138 and its magnitude may then increase in the opposite direction. RbNO3 126 The and potentials of aqueous sulfamerazine suspensions Mean 141 0 are negative above their isoelectric points, and those of bismuth 3 Mg(NO3)2 2.60 Quinine sulfate 0.7 subnitrate are positive. However, the addition of Al to the for- 3 MgSO4 2.57 mer and of PO4 to the latter in large enough amounts inverts Ca(NO3)2 2.40 the sign of their potentials, while their 0 potentials remain Sr(NO3)2 2.38 unchanged. Surface-active ions of opposite charge may also pro- Ba(NO3)2 2.26 duce such charge inversions. Zn(NO3)2 2.50 The superposition of the van der Waals attractive energy, Pb(NO3)2 2.43 with its long-range effectiveness, and the electrostatic repulsive Mean 2.45 energy, with its intermediate-range effectiveness, frequently produces a shallow minimum (designated S in Fig 21-6) in the Al(NO3)3 0.067 La(NO ) 0.069 resultant energy-distance curve at interparticle distances dS 3 3 that are several times greater than . If this minimum in poten- Ce(NO3)3 0.069 tial energy is small compared to kT, Brownian motion prevents Mean 0.068 aggregation. For large particles, such as those of many pharma- a Data from Kruyt HR. Colloid Science, vols I and II. Houston: Elsevier, 1949 ceutical suspensions, and for particles that are large in one or and 1952 and unpublished data. two dimensions (eg, rods and plates), this secondary minimum 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 304
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may be deep enough to trap them at distances dS from each When the particles cannot be individually observed using a micro- other. This requires a depth of several kT units. Such fairly long- scope, other electrophoresis methods are employed.6,8,21,23,24 In moving range and weak energies of attraction produce loose aggregates boundary electrophoresis, the movement of the boundary formed be- or flocs that can be redispersed by agitation or by reducing the tween a sol or solution and the pure dispersion medium in an electric 1,2,5,7,8,10,20 field is studied. If the dispersed phase is colorless, the boundary is lo- concentration of flocculating electrolytes. This re- cated by the refractive index gradient (Tiselius apparatus, frequently versible aggregation process involving the secondary minimum used with protein solutions). If several species of particles or solutes is called flocculation. By contrast, aggregation in the deep pri- with different mobilities are present, each will form a boundary moving mary minimum P is called coagulation and is irreversible. with a characteristic velocity. Unlike microelectrophoresis, this method ELECTROKINETIC PHENOMENA—When a dc electric permits the identification of different colloidal components in a mixture, field is applied to a dispersion, the particles move towards the the measurement of the electrophoretic mobility of each, and an esti- electrode having a charge opposite to that on their surface. The mation of the relative amounts present. 25,26 counterions located inside their hydration shell are dragged Capillary Electrophoresis—Capillary electrophoresis (CE) along while the counterions in the diffuse double layer outside is a widely used separation technique best suited for charged, water- soluble molecules having molecular weights ranging from those of the plane of slip, in the free or mobile solvent, move toward the amino acids and peptides to nucleic acids. CE has the following advan- other electrode. This phenomenon is called electrophoresis. If tages: it provides fast and efficient separations, requires only minute the charged surface is immobile, as is the case with a packed amounts of sample, is applicable to a wide range of analytes, and (in con- bed of particles or a tube filled with water, application of an trast to HPLC) employs aqueous media rather than organic solvents. electric field causes the counterions in the free water to move Electrophoresis is carried out in horizontal capillaries of fused silica towards the opposite electrode, dragging solvent with them. (which is transparent to ultraviolet) of 20 to 100 m bore and 20 to 100 This flow of liquid is called electroosmosis, and the pressure cm length. Both capillary ends are bent downward. Each end is im- produced by it is called electroosmotic pressure. Conversely, if mersed in a vial filled with a buffer solution that contains an electrode assembly. The electrodes are connected to an adjustable high-voltage dc the liquid is made to flow past charged surfaces by applying hy- power supply. As the dissolved analytes migrate past a detection win- drostatic pressure, displacement of the counterions in the free dow in the capillary, their concentrations are measured by ultraviolet water produces a potential difference between the two ends of absorption or by (often laser-induced) fluorescence. The silica capillar- the tube or bed called streaming potential. These three phe- ies are often coated externally with a very thin layer of polyimide to re- nomena depend upon the relative motion of the charged surface duce their fragility. This plastic coating is burned off in the window and the diffuse double layer outside the plane of slip surround- area. ing the surface. Actually, most of the diffuse double layer lies The capillary is filled with buffer solution, the sample is injected at within the free solvent and, therefore, can move along the sur- one end, and a constant high potential difference E is applied, which face.5–8, 21 All three electrokinetic phenomena measure the produces a potential gradient or field strength in the range of 300 to 400 V/cm. If E 20,000 V and the total capillary length d 57 cm, then same potential, which is the potential at the plane of slip. r E/dr 350 V/cm. The velocity of migration, v, is the capillary length to Microelectrophoresis—The particles of pharmaceutical suspen- the detector, d , divided by the migration time, t, of the analyte from the sions and emulsions, bacteria, erythrocytes and other isolated cells, la- L capillary injection end to the detection window. If dL 50 cm and t 10 tex particles, and many contaminant particles in pharmaceutical solu- min 600 sec, then v 50/600 0.083 cm/sec. The electrophoretic mo- tions are visible in a microscope. Therefore, their potentials are bility (v/(E/d)) is (0.083 cm/sec)/(350 V/cm) 2.4 10 4 cm2/Vsec. conveniently measured by microelectrophoresis. A potential difference, In addition to electrophoresis, electro-osmosis may play an important E, applied between two electrodes that are dipped into a dispersion and role in CE. The isoelectric point of hydrated silica is approximately 1.8. separated by a distance, d, produces the potential gradient or field The weakly acidic silanol groups become increasingly ionized with in- strength, E/d, expressed as V/cm. The average velocity, v, of the parti- creasing pH. Conditioning the capillary with a NaOH solution and then cles in response to the applied potential difference is determined using with the buffer ensures that its wall is charged uniformly with partially the eyepiece micrometer of a microscope and a stopwatch, and used to ionized silanol groups. These negatively charged sites attract cationic calculate the potential by the Smoluchowski equation: counterions from the buffer to form an electric double layer. When an electric potential is applied, the cations in the diffuse part of the double 4 4 v layer beyond the plane of shear (Fig 21-5) migrate toward the negative D E/d D electrode, entraining water of hydration. Because of the small bore of the capillaries compared to the diffuse double layer thickness, the electro-os- The electrophoretic mobility, , is equal to v/(E/d) and is the velocity motic flow (EOF) can be substantial. The EOF moves in a plug profile caused by a potential gradient of 1 V/cm. According to the Smoluchowski rather in the customary parabolic profile of laminar flow. At high pH, the equation, particle size and shape do not affect the potential. However, if EOF is strong because the silanol groups are extensively ionized. Am- the particle radius is smaller than or comparable to (in which case the photeric peptides are negatively charged and try to migrate toward the particles cannot be detected in a microscope), a factor of 6 replaces the 4. positive electrode or anode. This motion is often overwhelmed by a strong The viscosity, , and the dielectric constant, D, refer to the aqueous and opposite EOF, which drags them toward the negative electrode or medium within the double layer and cannot be measured directly.22 By cathode. These analytes move from the injection point in the anode com- using the values for water at 25°C, expressing the velocity in m/sec and partment toward the cathode. The order of arrival at the detection win- the electrophoretic mobility in ( m/sec)/(volts/cm), and converting into dow is: cationic analytes (whose electrophoretic migration toward the the appropriate units, the Smoluchowski equation is reduced to 12.9 cathode is superimposed and accelerated by the EOF), nonionic analytes with given as millivolts (mV). Zeta potentials as high as 180 mV (which migrate exclusively by EOF), and anionic analytes (whose net mi- have been reported.1,6,21 If the particle surface has appreciable conduc- gration velocity is that of the EOF minus their electrophoretic migration tance, the absolute value of the potential calculated by this equation velocity toward the anode). may be too small.2,7,21,22 Dispersions of hydrophobic particles having po- At low pH, the EOF is small and the peptides are positively charged. tentials below 20–30 mV are frequently unstable and tend to coagulate. Their migration toward the cathode is then superimposed and acceler- The chief experimental precautions in microelectrophoresis mea- ated by the EOF in the same direction. The direction of the EOF can be surements are: reversed by adding a cationic surfactant, such as cetyltrimethylammo- 1. Electroosmosis causes liquid to flow along the walls of the cell con- nium bromide, to the buffer. It will react and neutralize the silanol taining the dispersion. This in turn produces a return flow into the groups, and excess surfactant adsorbed on the silica will confer a posi- center of the cell. Therefore, the microscope must be focused on the tive charge to it. The Br counterions cause an EOF toward the anode. stationary boundary between the two liquid layers that are flowing The EOF can be suppressed by coating the silica capillaries with a poly- in opposite directions in order to measure the true velocity of the mer or by using Teflon capillaries. particles. Unless the heat generated by the electric resistance of the buffer so- 2. Following the motion of single particles in a microscopic field and lution (Joule heating) is dissipated, it causes the temperature to in- measuring their velocity is only possible using very dilute disper- crease with time and promotes temperature gradients across the capil- sions. Therefore, many dispersions must be diluted before making lary. This interferes with reproducibility and sharpness of the CE such determinations. Since the potential depends largely upon the separations. The amount of heat generated is directly proportional to nature, ionic strength, and pH of the suspending medium, disper- the square of the field strength (which is large) and to the conductivity sions should not be diluted with water but with solutions having of the buffer solution. While decreasing the voltage, using longer or compositions identical to their continuous phase (eg, with their own smaller-bore capillaries and/or more dilute buffer solution would reduce serum that has been separated by ultrafiltration or centrifugation). the rate of heat generation; it would also increase the separation times. 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 305
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Short separation times reduce the band broadening due to analyte dif- chain commonly exceeds 10 nm. Particulate or corpuscular hy- fusion, improving the resolution. Therefore, the capillary is cooled with drophilic colloidal dispersions are formed by solids that swell a thermostatted liquid. and are peptized in water but whose primary particles do not A variation of CE is micellar electrokinetic (capillary) chromatogra- dissolve or break down into individual molecules or ions. phy (MEKC).25, 26 The analytes are solubilized in micelles of an ionic surfactant, such as sodium dodecyl sulfate, which is added to the buffer solution at a concentration well above its critical micelle concentration Water-Soluble Polymers of 8 10 3M. MEKC is suited particularly to separate neutral analytes of limited water solubility, which are extensively partitioned into the Most of the hydrophilic colloidal systems used to prepare phar- micelles, but is also applicable to ionic analytes. Anionic analytes, being maceutical dosage forms are molecular solutions of water-solu- well soluble in water, either do not partition into the micelles or form ble, high molecular weight polymers. These polymers are either mixed micelles with the anionic surfactant. Cationic analytes often form linear or slightly branched but not cross-linked. Water-soluble precipitates with anionic surfactants. Therefore, their separation by MEKC is best carried out with cationic surfactants. polymers may be divided into three classes according to their The combination of a nonionic and an ionic surfactant produces origin: mixed micelles. These have lower surface charge densities and larger • Natural polymers include polysaccharides (acacia, agar, heparin sizes than the micelles of ionic surfactants, and hence they have lower sodium, pectin, sodium alginate, tragacanth, xanthan gum) and electrophoretic mobilities. Thus, addition of a nonionic to an ionic sur- polypeptides (casein, gelatin, protamine sulfate). Of these, agar factant narrows the migration time window, which is the difference be- and gelatin are only soluble in hot water. tween the migration times of the bulk solution in EOF and of the mi- • Cellulose derivatives are produced by chemically modifying cel- celles, and often shortens the analysis time. lulose obtained from wood pulp or cotton to produce soluble poly- Analytes with molecular weights of 5000 or higher are not solubi- mers. Cellulose is an insoluble, linear polymer of glucose units in lized by micelles. Therefore, while they can be analyzed by CE, they can- the ring or pyranose form joined by -1,4 glucosidic linkages. not be analyzed by MEKC. Although anionic micelles tend to migrate Each glucose unit (except for the two at the terminal chain ends) toward the anode, a strong EOF in neutral or alkaline media will drag contains a primary hydroxyl group on the No. 6 carbon and two them toward the cathode, but with a velocity retarded by their own mi- secondary hydroxyls on the No. 2- and 3-carbons. Chemical mod- gration velocity. If a neutral analyte is partly solubilized in micelles and ification of cellulose involves substitutions at these hydroxyl partly dissolved molecularly in the buffer solution, the latter portion groups with the primary hydroxyl group being the most reactive. has a shorter migration time because its velocity is that of the EOF. 25,26 The extent of such reactions is expressed as degree of substitu- Capillary gel electrophoresis employs capillaries filled with a gel tion (DS), the number of substituted hydroxyl groups per glucose of cross-linked polyacrylamide, which suppresses EOF. Isotachophore- 26 residue. The highest value for DS is 3. Fractional values are sis and isoelectric focusing, described in previous editions of this text, most common because the DS is averaged over a multitude of are other modalities of CE. glucose residues. A DS value of 0.6 indicates that some glucose repeat units are not substituted while others substituted once or even twice. LYOPHILIC DISPERSIONS Some soluble cellulose derivatives are listed below. Their DS values correspond to their respective pharmaceutical grades; the Lyophilic dispersions consist either of polymers dissolved in a groups shown replace the hydrogen atoms of the cellulosic hydrox- good solvent or of insoluble but extensively solvated particles yls. Official derivatives include methylcellulose (DS 1.65–1.93); (MOMCH3) and sodium carboxymethylcellulose (DS 0.60–1.00); dispersed in a liquid medium that has a high affinity or attrac- M M M M tion for them. The free energy of dissolution or dispersion is ( O CH2COO Na ). Hydroxyethylcellulose (DS 1.0); ( O (CH2CH2O)nH) and hydroxypropylcellulose (DS 2.5); Gs Hs T Ss, where Hs and Ss are the heat or enthalpy change, and the entropy change of dissolution or dispersion, re- MOM(MCHMCH2MOM)nH spectively. For dissolution of polymers and dispersion of partic- ulate solids to occur spontaneously, G must be negative. Since s CH3 both of these processes are exothermic (ie, occur with the evolu- tion of heat), their Hs is negative. Since the number of avail- are manufactured by adding ethylene oxide and propylene oxide, able conformations of the polymer chains increases considerably respectively, to alkali-treated cellulose. The value of n is about 2.0 upon dissolution, and the number of positions and orientations for hydroxyethylcellulose and not much greater than 1.0 for hy- droxypropylcellulose. Hydroxypropylmethylcellulose is prepared of the solid particles increases considerably upon their disper- by reacting alkali-treated cellulose first with methyl chloride to sion in the liquid, their Ss is positive (ie, there is an increase in introduce methoxy groups (DS 1.1–1.8) and then with propy- randomness). The negative enthalpy change and the positive en- lene oxide to introduce propylene glycol ether groups (DS tropy change of dissolution/dispersion both contribute to mak- 0.1–0.3). In general, the introduction of hydroxypropyl groups into ing Gs negative. Therefore, both types of colloidal systems are cellulose slightly reduces its water solubility while promoting its formed spontaneously when powders of solid polymers and par- solubility in polar organic solvents such as short-chain alcohols, ticulate solids are brought into contact with the liquid disper- glycols, and some ethers. sion medium. They are thermodynamically stable and re- The molecular weight of native cellulose is so high that soluble versible (ie, they are easily reconstituted after the dispersion derivatives of approximately the same degree of polymerization would dissolve too slowly and their solutions would be excessively medium has been removed). The van der Waals energies of at- viscous even at concentrations of 1%. To overcome these diffi- traction between dissolved macromolecules or between dis- culties, controlled degradation is used to break the cellulose persed lyophilic solid particles are smaller than Gs and are chains into shorter segments. Commercial grades cellulose therefore insufficient to cause flocculation or coagulation of the derivatives, such as sodium carboxymethylcellulose, come in var- dispersed phase. Furthermore, the solvation layers surrounding ious molecular weights or viscosity grades as well as with various dissolved macromolecules and dispersed lyophilic particles form degrees of substitution. a physical barrier preventing their close approach. Official cellulose derivatives that are insoluble in water but Most liquid dispersed systems of pharmaceutical interest are soluble in some organic solvents include ethylcellulose (DS 2.2–2.7); (MOC2H5); cellulose acetate phthalate (DS 1.70 for aqueous. Therefore, most of the lyophilic colloidal systems dis- acetyl and 0.77 for phthalyl); hydroxypropylmethylcellulose ph- cussed below consist of hydrophilic solids dissolved or dispersed thalate; and polyvinyl acetate phthalate. Collodion, a 4.0% (w/v) in water. Most of the products mentioned below are official in the solution of pyroxylin (cellulose dinitrate) in a mixture of 75% (v/v) USP or NF, where more detailed descriptions may be found; ether and 25% (v/v) ethyl alcohol, is also a cellulose based, they are also discussed in detail elsewhere in this text. Hy- lyophilic colloidal system. drophilic colloids can be divided into two classes (ie, soluble and •Water-soluble synthetic polymers consist mostly of high mole- particulate materials). Solutions of water-soluble polymers cular weight polyethylene glycols, or polyethylene oxides, and molecularly dissolved in water may be classified as colloidal dis- vinyl derivatives such as polyvinyl alcohol, povidone or persions because the individual molecules are in the colloidal polyvinylpyrrolidone, and carbomer (Carbopol), a copolymer of particle size range: the diameter of a randomly coiled polymer acrylic acid. 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 306
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A second classification of hydrophilic polymers is based upon because of a positive (endothermic) Hs term, which makes the their charge. Nonionic or uncharged polymers include methyl- reverse process (agglomeration) the spontaneous one. Aqueous cellulose, hydroxyethyl and hydroxypropyl cellulose, ethylcellu- dispersions of hydrophobic solids or liquids can be prepared by lose, pyroxylin, polyethylene oxide, polyvinyl alcohol, and povi- physical means that supply an appropriate amount of energy to done. Anionic or negatively charged polyelectrolytes include the system. However, they are unstable. The van der Waals at- carboxylated polymers (eg, acacia, alginic acid, pectin, traga- tractive forces between the particles are stronger than the sol- canth, xanthan gum, and carbomer) at pH values that result vation forces that promote particle dispersal, and therefore, the in the ionization of their carboxyl groups. Sodium alginate, particles tend to aggregate. Most of the discussion of lyophobic sodium carboxymethylcellulose, and polypeptides (eg, sodium dispersions deals with hydrosols consisting of hydrophobic caseinate) at pH values above their isoelectric points are also solids or liquids dispersed in an aqueous media because water anionic. Sulfuric acid is a stronger acidic group that exists as a is the most widely used vehicle. Such hydrosols consist of aque- monoester in agar and heparin and as a monoamide in heparin. ous dispersions of insoluble organic and inorganic compounds, Cationic or positively charged polyelectrolytes are rare. Exam- which usually have low degrees of hydration. Organic com- ples include chitin, a polysaccharide found in the shells of bee- pounds that are preponderantly hydrocarbon in nature and tles and crustaceans, and polypeptides at pH values below their possess few hydrophilic or polar groups are hydrophobic, and isoelectric points. Protamines such as protamine sulfate are therefore, insoluble in water. strongly basic due to their high arginine content and have iso- Like all lyophobic dispersions, hydrophobic dispersions are electric points around pH 12. intrinsically unstable. In their most thermodynamically stable state, the dispersed phase has coalesced into large crystals or drops, so that the specific surface area and surface free energy Particulate Hydrophilic Dispersions are minimized. Therefore, mechanical, chemical, or electrical The dispersed phase of these sols consists of solids that swell in energy must be supplied to break up the dispersed phase into water and spontaneously break up into particles having colloidal smaller particles and overcome the resulting increase in sur- dimensions. The dispersed particles have high specific surface face free energy that occurs from the parallel increase in spe- areas and are extensively hydrated. Bentonite NF is a hydrated cific surface area. aluminum silicate that crystallizes in a layer structure with in- Hydrophobic dispersions can be prepared by either disper- dividual lamellas 0.94 nm thick. Their top and bottom surfaces sion methods (the reduction of coarse particles to colloidal consist of sheets of oxygen ions from silica and an occasional dimensions through comminution or peptization) or condensa- sodium ion neutralizing a silicate ion-exchange site. The clay tion methods (the aggregation of small molecules or ions particles contain stacks of these lamellas. Water penetrates be- into particles having colloidal dimensions). Dispersion methods tween these lamellas to hydrate the oxygen ions and causes ex- tend to produce sols that have wide particle size distributions. tensive swelling. The bentonite particles in bentonite magma Conversely, condensation methods may produce essentially consist of single lamellas or packets of a few lamellas with inter- monodisperse sols provided specialized techniques are em- calated water. Their specific surface area amounts to several ployed. Methods of purification to remove low molecular-weight, hundred square meters per gram. Kaolin USP is also a hydrated water-soluble impurities from hydrosols have been reviewed in aluminum silicate having a layer structure. In kaolin, hydrated the corresponding chapter of the previous Remington edition. alumina lattice layers alternate with silica layers. Therefore, one of the two external surfaces of a kaolin plate consists of a sheet of oxygen ions from silica whereas the other is a sheet of hydrox- ide ions from hydrated alumina. Both surfaces are well hydrated Preparation by Dispersion Methods but water cannot penetrate into the individual lattice layers. The first method, mechanical disintegration of solids and liq- Therefore, the particles do not swell in water or exfoliate into uids into smaller particles before or during dispersion within a thin plates. As a result, kaolin plates dispersed in water are fluid vehicle, is frequently carried out by the input of mechani- much thicker than those of bentonite, about 0.04 to 0.2 m. Mag- cal energy via shear or attrition. Equipment such as colloid and nesium Aluminum Silicate NF, also known as Veegum®, is a clay ball mills, micronizers and, for emulsions, homogenizers is de- similar to bentonite but contains magnesium; it is white whereas scribed elsewhere in this text and in Reference 27. Dry grind- bentonite is gray. Colloidal Activated Attapulgite USP also con- ing with inert, water-soluble diluting agents also produces col- sists of magnesium aluminum silicate. However, rather than loidal dispersions. For example, sulfur hydrosols may be having a lamellar habit like the other three clays, it crystallizes prepared by triturating the powder with urea or lactose fol- in the form of long needles approximately 20 nm in width.27 lowed by shaking with water. Ultrasonic generators provide ex- The following additional hydrophilic particles can also pro- ceptionally high concentrations of energy. However, the suc- duce colloidal dispersions in water. Titanium dioxide is a white cessful dispersion of solids by means of ultrasonic waves can pigment with excellent covering power. Colloidal silicon dioxide only be achieved with comparatively soft materials such as consists of roughly spherical particles that are covered with many organic compounds, sulfur, talcum, and graphite. In siloxane and silanol groups. Microcrystalline cellulose is hy- cases where fine emulsions are mandatory, such as soybean oil- drophilic because of the hydroxyl and ether groups on the surface in-water emulsions for intravenous feeding, emulsification by of the cellulose crystals. Gelatinous precipitates of hydrophilic ultrasound waves is the method of choice.27 The formation of compounds such as aluminum hydroxide gel, aluminum phos- aerosols is described elsewhere in this text. phate gel, and magnesium hydroxide consist of coarse flocs pro- Peptization is a second dispersion method used to prepare duced by agglomeration of the colloidal particles formed in the colloidal dispersions. The term is defined as the breaking up initial stages of precipitation. of aggregates (or secondary particles) into smaller aggregates (or primary particles) that are within the colloidal size range. Primary particles are those particles that are not formed from LYOPHOBIC DISPERSIONS smaller ones. Peptization is synonymous with deflocculation. It can be brought about by the removal of flocculating agents, Lyophobic dispersions are intrinsically unstable and irre- usually electrolytes, or by the addition of deflocculating or versible because of the lack of attraction between the dispersed peptizing agents, usually surfactants, water-soluble polymers, and continuous phases. Unlike lyophilic dispersions, their large or ions that adsorb onto the particle surface.6,8 When pow- surface free energy is not lowered by solvation, their dispersion dered activated charcoal is added to water with stirring, the process does not take place spontaneously, and they are not aggregated grains cannot be completely broken up and the re- easily reconstituted. For lyophobic dispersions, Gs is positive sulting suspension is gray and translucent. The addition of 0356 ch 021(293-318).ps 3/7/05 8:14 AM Page 307
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