1	Chapter 8 Solutions
2	Water that makes the most common solutions CO 8.1 Ocean water is a solution in which many different substances are dissolved.
3	Solutions keep properties of both: Solvent and the solute Fig. 8.1 The colored crystals are the solute, and the clear liquid is the solvent. Stirring produces the solution.
4	Solutions could be sold solutions Fig. 8.2 Jewelry often involves solid solutions in which one metal has been dissolved in another metal.
5	Solubility is different Table 8.1
6	Saturated solutions Fig. 8.3 In a saturated solution, the dissolved solute is in dynamic equilibrium with the undissolved solute.
7	Gas in liquids: solutions C.C. 8.1 Carbon dioxide escaping from an opened bottle of a carbonated beverage.
8	Concentrated vs. dilute olutions Fig. 8.4 Both solutions contain the same amount of solute. A concentrated solution (left) contains a relatively large amount that could dissolve. A dilute solution contains a relatively small amount of solute compared with the amount that could dissolve.
9	Ionic solids breaks into ions in solutions Fig. 8.5 When an ionic solid, such as sodium chloride, dissolves in water, the water molecules hydrate the ions.
10	Immiscible liquids can be separated Fig. 8.6 Oil spills can be contained to some extent by using trawlers and a boom apparatus because oil and water, having different polarities, are relatively insoluble in each other.
11	Solubility rules for ionic solids Table 8.2
12	Solubility of vitamins CC 8.2 Solubility of Vitamins .
13	Total volume don’t add up Fig. 8.7 When volumes of two different liquids are combined, the volumes are not additive.
14	Measuring volume of solutions Fig. 8.8 Identical volumetric flasks are filled to the 50.0-mL mark with ethanol and with water. When the two liquids are poured into a 100mL volumetric flask, the volume is seen to be less.
15	Orange juice is it a homogenous solutions? Fig. 8.9 Frozen orange juice concentrate is diluted with water prior to drinking.
16	Concentration of drugs in solution
17	Different types of solutions
18	Does the light pass through solutions Fig. 8.10 A beam of light travels through a true solution without being scattered. This is not the case for a colloidal dispersion.
19	Solute lowers the vapor pressure Fig. 8.11 Close-ups of the surface of a liquid solvent before and after solute has been added.
20	Solute lowers the freezing point Fig. 8.12 A water-antifreeze mixture has a higher boiling point and lower freezing point than pure water.
21	Solute increase the osmotic pressure Fig. 8.13 (a) Osmosis can be observed with this apparatus. (b) The liquid level in the tube rises until equilibrium is reached.
22	Semi permeable memebreane only allows the solvent molecules to pass Fig. 8.14 Enlarged views of a semi-permeable membrane separating (a) pure water and a salt-water solution, and (b) a dilute salt-water solution.
23	Osmotic pressure Fig. 8.15 Osmotic pressure is the amount of pressure needed to prevent the solution in the tube from rising as a result of the process of osmosis.
24	Water can move up through capillary action Fig. 8.16 The dissolved substances in tree sap create a more concentrated solution than the surrounding ground water.
25	Would the blood cell survive? (a) Hyptonic solution
26	Three types of solutions Table 8.3
27	Colligative properties of solutions
28	How does dialysis work? Fig. 8.18 In dialysis, there is a net movement of ions from a region of higher concentration to a region of lower concentration.
29	Removing impurities through dialysis Fig. 8.19 Impurities can be removed from a colloidal dispersion by using a dialysis procedure.
30	Dialysis machine a life saver CC 8.4