2. COS 2.0, 2.1, 2.2, 2.3 IDENTIFY SOLUTIONS IN TERMS OF COMPONENTS, SOLUBILITY, CONCENTRATION, AND CONDUCTIVITY. COMPARE SATURATED, UNSATURATED AND SUPERSATURATD SOLUTIONS. COMPARE CHARACTERISTICS OF ELECTROLYTES AND NONELECTROLYTES. DESCRIBE FACTORS THAT AFFECT SOLUBILITY AND RATE OF SOLUTION, INCLUDING NATURE OF SOLUTE AND SOLVENT, TEMPERATURE, AGITATION, SURFACE AREA AND PRESSURE ON GASES.

3. WHAT YOU’LL LEARN Compare the properties of suspensions, colloids, & solutions. Explain the meaning of solubility & compare the solubilities of various substances. Examine the factors that affect the rates at which solids and gases dissolve in liquids. Explain how solvents work. Compare & contrast saturated, unsaturated, & supersaturated solutions.

4. SOLUTIONS & MIXTURES

5. SOLUTIONS  homogeneous mixture of two or more substances uniformly dispersed in a single phase

6. MIXTURE any combination or blend of different elements

7. HETEROGENOUS MIXTURES

8. Suspension mixture in which the solute particles are large enough to be seen Particles may settle over time or filtered out Example: natural orange juice, which contains particles of pulp.

9. Suspension

10. Colloids mixture whose particles never settle Particles are smaller than suspensions Examples: milk, paint Tyndall effect Scattering of light

11. EMULSION Any mixture of two or more immiscible liquids in which one liquid is dispersed in another. Examples Mayonnaise Egg yolk creams

12. HOMOGENOUS MIXTURES

13. HOMOGENOUS MIXTURE substances are evenly distributed “well mixed” Look/have the same composition throughout Particles are small and not easily recognized can be separated by physical means (dissolution, centrifuge, gravimetric filtering, etc.) Examples: Salt water Sugar water Milk Yogurt

14. Miscible two or more liquids that can dissolve into each other in various proportions example: gasoline (100 liquids)

15. Immiscible two or more liquids that do not mix with each other example: oil & water

16. PARTS OF A SOLUTION SOLUTE part of a solution that is being dissolved (lesser amount/%) SOLVENT part of a solution that dissolves the solute (greater amount/%) Solute + Solvent = Solution EXAMPLES air: 78% nitrogen, 21% oxygen sterling silver: 92.5% silver, 7.5% copper

17. ALLOY mixture of a metal with one or more elements that retains original properties of metal NAMECOMP.USE bronzeCopper, tinJewelry marine hardware BrassCopper, zincHardware musical instruments Sterling silver Silver, copper Tableware, jewelry COMMON ALLOYS

18. HOW SUBSTANCES DISSOLVE

19. RULE FOR DISSOLVING SOLUTES IN A SOLVENT Like solutes dissolve in like solvents

20. HOW SUBSTANCES DISSOLVE water molecules are constantly moving causing negative-positive ions to attract “breaking” bonds Universal solvent

21. POLAR has oppositely charged ends (+ and -) water molecules Compound Molecule that has an uneven distribution of electrons

22. NONPOLAR have same charges on its ends (+ & +) or (- & -) Petroleum products Compound Electrons are equally distributed among atoms

23. DISSOLVING PROCESS

24. SURFACE AREA (CRYSTAL SIZE) dissolving takes place at surface area smaller crystals dissolve faster increases surface area more surface area faster dissolving less surface area slower dissolving Example: piece of candy

25. SURFACE AREA (CRYSTAL SIZE)

26. TEMPERATURE increasing temperature speeds up molecule movement increase in speed causes more solvent particles to “bump” into solute breaking them down lower temperature slows down process Example: sugar in hot water

27. AGITATION AKA: mixing or stirringAKA: mixing or stirring increase in stirring causes more solvent particles to “bump” into soluteincrease in stirring causes more solvent particles to “bump” into solute causing more solute to dissolvecausing more solute to dissolveExample: sugar in watersugar in water

28. SOLUBILITY AND CONCENTRATION

29. Solvation combination of solvent molecules with molecules or ions of the solute

30. Solubility max amount of a solute that will dissolve in a given quantity of solvent at a given temperature and pressure.

31. Soluble easily dissolves in water limit to how much of a substance will dissolve. different substances have different solubilities.

32. Insoluble never dissolves, such as oil

33. Concentration amount of a particular substance in a given volume of solution

34. Concentrated solution whose ratio of solute to solvent is relatively high

35. Dilute solution whose ratio of solute to solvent is relatively low

36. TYPES OF SOLUTIONS

37. UNSATURATED  contains less than max amount of solute that can dissolve at a particular temperature UNSATURATED SOLUTION more solute dissolves

38. SATURATED contains max quantity of solute that dissolves at that temperature. SATURATED SOLUTION no more solute dissolves

39. SUPERSATURATED contain more solute than is possible to be dissolved are unstable. is only temporary, accomplished in two ways: Warm solvent so that it will dissolve more, then cool solution Evaporate some of solvent carefully so that solute does not solidify and come out of solution. SUPERSATURATED SOLUTION becomes unstable, crystals form

40. PRESSURE affects solubility of gases in liquids Gases are more soluble at... low temperatures. high pressures Example: Soda goes flat quickly at room temperature carbon dioxide gas escapes

41. ELECTROLYTES & NONELECTROLYTES

42. AQUEOUS SOLUTIONS SSSSolution in which solvent is water (most common)

43. Electrolytes  substance that dissolves in water to give a solution ability to conduct an electric current. Examples:  sodium chloride  silver nitrate  gatorade - + salt

44. Nonelectrolytes substances that dissolve in water that does not conduct electricity Examples Sugar water Alcohol benzene - + sugar