Clouds are what type of colloid

In many emulsions, however, the dispersed phase tends to coalesce, form large drops, and separate. Therefore, emulsions are usually stabilized by an emulsifying agent , a substance that inhibits the coalescence of the dispersed liquid.

For example, a little soap will stabilize an emulsion of kerosene in water. Milk is an emulsion of butterfat in water, with the protein casein as the emulsifying agent. Mayonnaise is an emulsion of oil in vinegar, with egg yolk components as the emulsifying agents.

Condensation methods form colloidal particles by aggregation of molecules or ions. If the particles grow beyond the colloidal size range, drops or precipitates form, and no colloidal system results. Clouds form when water molecules aggregate and form colloid-sized particles. If these water particles coalesce to form adequately large water drops of liquid water or crystals of solid water, they settle from the sky as rain, sleet, or snow.

Many condensation methods involve chemical reactions. We can prepare a red colloidal suspension of iron III hydroxide by mixing a concentrated solution of iron III chloride with hot water:. A colloidal gold sol results from the reduction of a very dilute solution of gold III chloride by a reducing agent such as formaldehyde, tin II chloride, or iron II sulfate:.

Some gold sols prepared in are still intact the particles have not coalesced and settled , illustrating the long-term stability of many colloids. Pioneers made soap by boiling fats with a strongly basic solution made by leaching potassium carbonate, K 2 CO 3 , from wood ashes with hot water.

Animal fats contain polyesters of fatty acids long-chain carboxylic acids. When animal fats are treated with a base like potassium carbonate or sodium hydroxide, glycerol and salts of fatty acids such as palmitic, oleic, and stearic acid are formed. The salts of fatty acids are called soaps. Figure 3. Soaps contain a nonpolar hydrocarbon end blue and an ionic end red. The ionic end is a carboxylate group. The length of the hydrocarbon end can vary from soap to soap.

Soaps form insoluble calcium and magnesium compounds in hard water; detergents form water-soluble products—a definite advantage for detergents. Figure 4. Detergents contain a nonpolar hydrocarbon end blue and an ionic end red.

The ionic end can be either a sulfate or a sulfonate. The length of the hydrocarbon end can vary from detergent to detergent. The cleaning action of soaps and detergents can be explained in terms of the structures of the molecules involved. The hydrocarbon nonpolar end of a soap or detergent molecule dissolves in, or is attracted to, nonpolar substances such as oil, grease, or dirt particles.

The ionic end is attracted by water polar , illustrated in Figure 5. As a result, the soap or detergent molecules become oriented at the interface between the dirt particles and the water so they act as a kind of bridge between two different kinds of matter, nonpolar and polar. Home Question Answer Fog and cloud are both colloidal in nature. How do they differ? Fog and cloud are both colloidal in nature.

Best Answer In both fog and cloud, the dispersed phase is liquid and the dispersion medium is air gas. Related questions Both soap and detergent are some type of salts. What is the difference between them. A colloid is a heterogeneous mixture. The size of the solutes in this mixture is so small that they cannot be seen individually with naked eyes, and seems to be distributed uniformly throughout the mixture.

Milk is a colloid, with tiny globs of butterfat suspended throughout the liquid. Whipped cream is a colloid too. If you think about the humidity on a hot day, you know that moisture is held in the air. At higher altitudes, that water condenses and sometimes freezes into wispy clouds. It is evenly distributed… See full answer below. The clouds consist of charged particles of water dispersed in air.

Was this answer helpful? Question is : Cloud is a colloidal dispersion of , Options is : 1. Because the dispersed particles of a colloid are not as large as those of a suspension, they do not settle out upon standing. The Table below summarizes the properties and distinctions between solutions, colloids, and suspensions. Particle size: 0. Particle size: nm, dispersed; large molecules or aggregates.

Particle size: over nm, suspended; large particles or aggregates. May either scatter light or be opaque. Colloids are unlike solutions because their dispersed particles are much larger than those of a solution.

The dispersed particles of a colloid cannot be separated by filtration, but they scatter light, a phenomenon called the Tyndall effect. When light is passed through a true solution, the dissolved particles are too small to deflect the light. However, the dispersed particles of a colloid, being larger, do deflect light. The Tyndall effect is the scattering of visible light by colloidal particles.

All three are examples of colloids. Suspensions may scatter light, but if the number of suspended particles is sufficiently large, the suspension may simply be opaque and the light scattering will not occur. Figure 2. Figure The table below lists examples of colloidal systems, most of which are very familiar.