For medical or health purposes, the FDA now allows both the grind and electrical manufacturing techniques to be used. Of these two methods, however, the electro-colloidal process is generally considered to be far superior.
The chemical method, described below, is restricted to industrial or commercial applications. With the grind method, the inorganic or organic particles are usually no finer than four one-hundred-thousandths of an inch, or about one micron, which is outside the upper end of the ideal size range by a factor of Such particles may or may not be electrically charged.
Even if a charge is present, the size of the particles may be great enough that the repelling forces are unable to overcome the pull of gravity. Thus, particles will tend to settle to the bottom of the solution, and much of the effectiveness of the colloidal system will be lost. While some sols owe their stability to particle size, charge and high dispersion, others employ a mechanical stabilizer added to the medium.
The downside to this is that stabilizers tend to block the effects of the colloids, and the particles will still eventually settle if the solution is allowed to stand long enough. If the inorganic or organic particles are within the size range of 1 to nm and are uniformly charged, no stabilizer is required to maintain suspension indefinitely in deionised water, as long as no disruptive influence intrudes.
Thus, the integrity and power of a colloidal system is a factor of the interplay among size, charge, concentration, and interaction between particle and medium. It should be mentioned that shape is also a factor.
In recent years, the chemical process has been widely employed to replace the inferior grind method, because it provides a convenient shortcut to the more difficult electro- colloidal process. But it also has drawbacks, one of which is the difficulty in getting the chemicals acids back out of the colloidal solution.
After studying the health benefits of various forms of colloidal silver, Dr. Leonard Keene Hirschberg, A. A simple illustration will suggest the immense power potential of a colloidal system. The total surface of a one-inch cube of iron is six square inches.
By colloidal chemistry, the cube can be divided into particles having a total surface area in the range of ,, square inches, all expressing electrical energy. The total surface area of the particles in a quarter teaspoon is greater than that of a football field.
This is the only method that will create a true colloidal system by manufacture. Products that are simple mixtures of metal and liquid cannot possess nearly the potential of electro colloids, and are therefore of questionable value.
The proper electrical process allows inorganic or organic particles that are well within the colloidal size range to be drawn off an ingot. Animated by Brownian movement, they are able to remain in suspension in a liquid medium almost indefinitely. Because many nutrients are best transported through the body in water, the best medium to use for ingested nutritional products is pure, de-ionized water.
All other things being equal, the number of particles varies inversely according to the cube of the size change, so if size is reduced 50 percent, overall number is multiplied by eight. This is a mathematical proof, and is determined by actual count using an electron microscope and by atomic absorption.
Obviously, ideal size is element dependent. Size is controlled by frequency, amperage and micro-meshes, among other things. The ultimate colloidal sol contains ultra-fine and ultra-light particles in the range of 0. There is no visible accumulation of inorganic or organic particles either in the solution or settled on the bottom. Products that show visible particles in the solution or at the bottom of the container indicate that the particles are either too large or have not received the proper electrical charge.
The metallic particles in a sol may vary in concentration, but more is not necessarily better, unless we have correspondingly smaller particles. In fact, the reverse is usually true- less is better, and in essence, less is more, functionally speaking, because as noted earlier, the higher the concentration in a solution, the more likely the attraction force will overcome the repelling charge.
But even before this happens, effectiveness is reduced. The highest quality colloid will have a certain maximum number of particles. This will prevent further aggregation at that size.
A quick way to see if a solution contains colloids is by observing the Tyndall effect. A clear colloidal dispersion will appear turbid when a sharp and intense beam of light is passed through. The scattered light also takes on a cone shape within the solution.
A simple way to observe this is to shine a very bright flashlight through a test tube of the dispersion in a dark room Figure 2. The ideal form of colloidal silver, for example, will have a golden yellow color. As the size of each particle increases, the color of the suspension proceeds from yellow to brown to red to gray to black.
Additionally, color varies with concentration, use of a stabilizer, and the presence or absence of other trace elements. To confirm that a product is a true colloidal, examine the ingredients. If it contains an ingredient other than the designated colloidal particles, the product may not be suitable. If no additional ingredient is listed, but the product requires refrigeration, it means there is an ingredient in it that might spoil at room temperature. Properly prepared using the electro-colloidal method, a colloidal system requires no such ingredient.
Needless to say, a product with instructions to shake before using is also quite suspect. Humeral medicine died in as a result of the influence of the Virchow school. Cellular pathology tells only part of the story of disease. The colloidal integrity of the intercellular fluids, or humeral milieu, is the sine qua non of life itself. The state of health is present when there is unhindered flow of life- force through every part of the humeral system. The real function of body cells is to maintain the milieu in a state of functional efficiency -OC Gruner.
At the present time, colloidal chemistry plays a major role in over 7, industries, and, as noted earlier, most study in colloids has been applied to industrial processes.
In the last few decades of the 19th century, and even well into the 20th, there was considerable awareness of the importance of colloids to human health. But with the rise and sway of monomorphic, allopathic, cell-oriented medicine, this area of study fell by the wayside. Therefore, there is currently comparatively little awareness of, or focus on, colloids in the living system.
It is now realized that-disregarding the fact that bacteria are alive-they may, owing to their colloidal character and that of the toxins and some other substances they produce-be destroyed by substances which bear an electrical charge opposite to that of the bacteria or their colloidal products. Colloidal silver, for example, has no recorded side effects. Yet they are completely safe and natural. Moreover, the antibiotic cannot really alter the condition which supported the evolution of the target form, and may not even kill it but only instigate an evasive pleomorphosis and potentiate a worse scenario later.
This is not to mention the negative effect on the health and vitality of the intestinal villi. Metal solids have the further therapeutic advantage of acting most rapidly in faintly alkaline solutions, so that when properly prepared they are not affected adversely by normal blood.
Before a therapeutic substance can exert its full effect it must be converted into the ionized or into the colloidal state. The drugs employed to combat disease should be in the colloidal state, i. Only so can they be expected to exert their full potency.
The task of thus bringing their remedial virtue to its highest point is not an easy one, for colloidal substances, unless prepared with consummate skill and meticulous care, lack stability, and are prone to precipitation when brought into contact with the electrolytes normally present in the body tissues and fluids.
Though Searle was speaking in terms of pharmaceuticals, the information also applies to food supplements. Since surfaces present, and interact through, electrical and magnetic energies, the electrical characteristics of colloids take on fundamental importance. For example, sick, dead and broken-down cells are attracted to colloids by electromagnetic force, as iron filings are attracted to a magnet. The resulting complexes are carried into the lymph, which recycles what it can, while the rest are carried to the bloodstream to be eliminated.
The surface energies of colloids have powerful effects on physical and chemical activity. Unhomogenized milk is not a solution, it's asuspension because the fat aka cream will separate from the restof the milk and rise to the top, since fat is less densethan water. Is water a colloid? Sand in water is an example of a suspension. Asolution is a homogenous mixture of two or more substances whereone substance has dissolved the other.
An example of a solution issaltwater. Colloids are homogenous mixtures where theparticles are small enough that they stay suspended. Is Vinegar a colloid? This clear liquid is a solution sincelight easily passes through and it never separates.
Theseparticles, although sounding small, are still much bigger than theparticles in a solution. A common example of a colloid ismilk. How is butter a colloid? Cream is a colloid as it's made up of tinyparticles of fat dispersed in water. If you put cream in a jar andshake for a about 10 minutes the fat molecules stick together,making butter and a liquid called buttermilk.
Butteris also a colloid as there are water molecules trapped inbetween the fat. Is ketchup a colloid? Ketchup is a colloid, i. Ketchup is in fact a sol, which is solidparticles suspended in liquid.
How do you identify a colloid? To identify a colloid mixture from a solution,you can use the Tyndall effect. Chem1 Virtual Textbook.
Learning Objectives Summarize the principal distinguishing properties of solutions, colloidal dispersions, and suspensions. For the various dispersion types emulsion, gel, sol, foam, etc. Describe the origins of Brownian motion and how it can observed. Describe the electric double layer that surrounds many colloidal particles. Explain the mechanisms responsible for the stability of lyophilic and lyophobic colloidal dispersions.
Define: surfactant, detergent, emulsifier, micelle. Give some examples of how colloidal dispersions can be made. Explain why freezing or addition of an electrolyte can result in the coagulation of an emulsion.
Describe some of the colloid-related principles involved in food chemistry, such as the stabilization of milk and mayonaisse, the preparation of butter, and the various ways of cooking eggs.
Describe the role of colloids in wastewater treatment. Introducing Colloids Colloids occupy an intermediate place between [particulate] suspensions and solutions, both in terms of their observable properties and particle size. Solutions are homogeneous mixtures whose component particles are individual molecules whose smallest dimension is generally less than 1 nm. Within this size range, thermal motions maintain homogeneity by overcoming the effects of gravitational attraction.
Colloidal dispersions appear to be homogeneous, and the colloidal particles they contain are small enough generally between nm to exhibit Brownian motion, cannot be separated by filtration, and do not readily settle out.
But these dispersions are inherently unstable and under certain circumstances, most colloidal dispersions can be "broken" and will "flocculate" or settle out. The particles that form suspensions are sometimes classified into various size ranges. The nature of colloidal particles To begin, you need to recall two important definitions: a phase is defined as a region of matter in which the composition and physical properties are uniform.
Thus ice and liquid water, although two forms of the single substance H 2 O, constitute two separate phases within a heterogeneous mixture. A solution is a homogeneous mixture of two or more substances consisting of a single phase. Think of sugar dissolved in water. Smaller is bigger What makes colloidal particles so special is not so much their sizes as it is the manner in which their surface areas increase as their sizes decrease.
What will be the surface area of this cube? Now let us cut this cube into smaller cubes by making 10 slices in each direction. How many smaller cubes wil this make, and what will be the total surface area? Each new cube has a face length of 0. But there are 10 3 of these smaller cubes, so the total surface area is now 60 cm 2 -- quite a bit larger than it was originally! Colloidal Dispersions Colloidal matter commonly exists in the form of colloidal-sized phases of solids, liquids, or gases that are uniformly dispersed in a separate medium sometimes called the dispersions phase which may itself be a solid, liquid, or gas.
The sudden release of pressure as the lava is ejected from the volcano allows dissolved gases to expand, producing tiny bubbles that get frozen into the matrix. Pumice is distinguished from other rocks by its very low density.
Aerogels are manufactured rigid solids made by removing the liquid from gels, leaving a solid, porous matrix that can have remarkable and useful physical properties. Aerogels based on silica, carbon, alumina and other substances are available. Milk is basically an emulsion of butterfat droplets dispersed in an aqueous solution of carbohydrates.
Opal consists of droplets of liquid water dispersed in a silica SiO 2 matrix. Large molecules can behave as colloids Very large polymeric molecules such as proteins, starches and other biological polymers, as well as many natural polymers, exhibit colloidal behavior. Macroscopic or microscopic? The most important feature that distinguishes them from other particulate matter is that: Colloids dispersed in liquids or gases are sufficiently small that they do not settle out under the influence of gravity.
Optical properties of colloidal dispersions Colloidal dispersions are distinguished from true solutions by their light-scattering properties.
The Ultramicroscope Colloidal particles are, like molecules, too small to be visible though an ordinary optical microscope. Brownian motion If you observe a single colloidal particle through the ultramicroscope, you will notice that it is continually jumping around in an irregular manner. Electrical Properties of Colloids In general, differences in electric potential exist between all phase boundaries.
Stability of colloidal dispersions What keeps the colloidal particles suspended in the dispersion medium? These are very important practical matters: Colloidal products such as paints and many foods e. The only practical way of disposing them is to separate the colloidal material from the much greater volume of the dispersion medium most commonly water. Simple evaporation of the water is usually not a practical option; it is generally too slow, or too expensive if forced by heating.
Electrical forces help keep colloids dispersed When particles of colloidal dimension suspended in a liquid collide with each other, they do so with much smaller kinetic energies than is the case for gases, so in the absence of any compensating repulsion forces, we might expect van der Waals or dispersion attractions to win out.
Interactions with the solvent Colloids can be divided into two general classes according to how the particles interact with the dispersions medium often referred to as the "solvent".
Lyophilic colloids In one class of colloids, called lyophilic "solvent loving" colloids, the particles contain chemical groups that interact strongly with the solvent, creating a sheath of solvent molecules that physically prevent the particles from coming together. Lyophobic colloids Most of the colloids in manufactured products exhibit very little attraction to water: think of oil emulsions or glacially-produced rock dust in river water.
Stabilization by cloaking "Stabilization by stealth" has unwittingly been employed since ancient times through the use of natural gums to stabilize pigment particles in inks, paints, and pottery glazes. Steric stabilization Alternatively, attaching a lyophobic material to a colloid of any type can surround the particles with a protective shield that physically prevents the particles from approaching close enough to join together. Surfactants and micelle formation Surfactants and detergents are basically the same thing.
Amphiphiles possess the very important property of being able to span an oil-water interface. By doing so, they can stabilize emulsions of both the water-in-oil and oil-in-water types. Such molecules are essential components of the lipid bilayers that surround the cells and cellular organelles of living organisms. How detergents remove "dirt" The "dirt" we are trying to remove consists of oily or greasy materials whose hydrophobic nature makes them resistant to the action of pure water. Bile: your body's own detergent Oils and fats are important components of our diets, but being insoluble in water, they are unable to mix intimately with the aqueous fluid in the digestive tract in which the digestive enzymes are dissolved.
Microemulsions Ordinary emulsions are inherently unstable; they do not form spontaneously, and once formed, the drop sizes are sufficiently large to scatter light, producing a milky appearance. Build up molecular-sized particles atoms, ions, or small molecules into aggregates within the colloidal size range. Condensation Dispersion processes all require an input of energy as new surfaces are created.
Condensation Numerous methods exist for building colloidal particles from sub-colloidal entities. For example, a sample of paraffin wax is dissolved in ethanol, and the resulting solution is carefully added to a container of boiling water. Formation of precipitates under controlled conditions The trick here is to prevent the initial colloidal particles of the newly-formed compound from coalescing into an ordinary precipitate, as will ordinarily occur when solutions of two dissolved salts are combined directly.
An alternative that is sometimes useful is to form the sol by a chemical process that procedes more slowly than direct precipitation: Sulfur sols are readily formed by oxidation of thiosulfate ions in acidic solution: Sols of oxides or hydrous oxides of transition metals can often be formed by boiling a soluble salt in water under slightly acidic conditions to prevent formation of insoluble hydroxides: Addition of a dispersant usually a surfactant can sometimes prevent colloidal particles from precipitating.
Thus barium sulfate sols can be prepared from barium thiocyanate and NH 4 2 SO 4 in the presence of potassium citrate. Ionic solids can often selectively adsorb cations or anions from solutions containing the same kinds of ions that are present in the crystal lattice, thus coating the particles with protective electric charges. How Dispersions are Broken That oil-in-vinegar salad dressing you served at dinner the other day has now mostly separated into two layers, with unsightly globs of one phase floating in the other.
The consequent breakup of the emulsion can proceed through various stages: Coalescence - smaller drops join together to form larger ones; Flocculation - the small drops stick together without fully coalescing; Creamin g - Most oils have lower densities than water, so the drops float to the surface, but may not completely coalesce; Breaking - the ultimate thermodynamic fate and end result of the preceding steps.
Coagulation and flocculation The processes described above that allow colloids to remain suspended sometimes fail when conditions change, or equally troublesome, they work entirely too well and make it impossible to separate the colloidal particles from the medium; this is an especially serious problem in wastewater settling basins associated with sewage treatment and operations such as mining and the pulp-and-paper industries.
Addition of an electrolyte Coagulation of water-suspended dispersions can be brought about by raising the ionic concentration of the medium. Gelatine is a protein-like material made by breaking down the connective tissues of animal skins, organs, and bones. The many polar groups on the resulting protein fragments bind them together, along with water molecules, to form a gel. A number of so-called super-absorbant polymers derived from cellulose, polyvinyl alcohol and other materials can absorb huge quantities of water, and have found uses for products such as disposable diapers, environmental spill control, water retention media for plants, surgical pads and wound dressings, and protective inner coatings and water-blockers in fiber optics and electrical cables.
Gels can be fragile! Our bodies are mostly gels The interior the cytoplasm of each cell in the soft tissues of our bodies consists of a variety of inclusions organelles suspended in a gel-like liquid phase called the cytosol. Food colloids Most of the foods we eat are largely colloidal in nature. Dairy products Milk is basically an emulsion of lipid oils "butterfat" dispersed in water and stabilized by phospholipids and proteins. Homogenizer The stabilizers present in fresh milk will maintain its uniformity for hours, but after this time the butterfat globules begin to coalesce and float to the top "creaming".
Eggs: colloids for breakfast, lunch, and dessert A detailed study of eggs and their many roles in cooking can amount to a mini-course in colloid chemistry in itself. Whipped cream and meringues The other colloidal personalities eggs can display are liquid and solid foams.
Paints and inks Paints have been used since ancient times for both protective and decorative purposes. Inks The most critical properties of inks relate to their drying and surface properties; they must be able to flow properly and attach to the surface without penetrating it — the latter is especially critical when printing on a porous material such as paper. Please visit the James Hutton Institute website.
Colloids are microscopic particles with sizes in the range 1 to 0. Because of their small size they tend not to settle out of suspensions, being influenced by Brownian motion and minor currents in the bulk of the solution. Colloids play an important role in the transfer of nutrients and pollutants in the environment over short and long distances.
For example, colloids can transport nutrients such as phosphate through channels in soil to deeper horizons, as well as over much longer distances in surface waters.
For chemical species strongly bound to soil, colloids can be the main vehicle for their transport.
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