Αποτελέσματα Αναζήτησης
26 Αυγ 2023 · In this chapter, we will consider the nature of solutions, and examine factors that determine whether a solution will form and what properties it may have. In addition, we will discuss colloids—systems that resemble solutions but consist of dispersions of particles somewhat larger than ordinary molecules or ions.
- 11.0: Introduction
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- 11.3: Solubility
Solution. According to Henry’s law, for an ideal solution...
- Colligative Properties
Determine the number of moles of ions present in the...
- The Dissolution Process
Figure \(\PageIndex{2}\): Samples of helium and argon...
- 11.0: Introduction
Colloid is a term that has come to encompass solid particles suspended in a liquid (a colloidal dispersion), microscopic droplets in a liquid (an emulsion), or either solid or liquid phases suspended in a gas (an aerosol).
Colloid systems (or simply colloids) are a specific form of disperse systems. They include systems with a comparatively high degree of dispersion, in which the particle size range from 0.10 to 1000 nm (1 nm = 1∙10-9 m). The particles of colloid systems cannot be seen through an ordinary microscope.
What is a colloid? Finely-divided dispersion of one phase in another. Size of dispersed (“solute-like”) entity >> ordinary molecules. Example: blood cell in water. Solution. homogeneous particles are molecules. Colloid. size 1–1000 nm. particles remain suspended. Suspension. heterogeneous particles settle out. Examples.
A. Solutions are homogeneous mixtures of two or more substances in which the components are present as individual atoms, molecules or ions. 1. The individual components are uniformly distributed and are fare too small to be seen by eye. a. Liquid and gas solutions do not scatter much light and therefore are transparent (clear).
Choose suspension, colloid, or solution to answer the following statements: Large particles settle out on standing. Medium size particles settle out on standing, scatters light. Very small particles do not settle out on standing. Chocolate milk. Fog . Smoke. Muddy water. Orange juice. Whipped cream. Sugar water. 3% hydrogen peroxide. Salt water.
The answer lies in the intermolecular forces discussed in Chapter 10. There are three interactions we must consider. The ions or molecules in a lattice are collectively attracted to one another. Likewise, the molecules in a sample of pure solvent are attracted to one another.
