Solutions!

1. Solutions!

2. Recall Classification of Matter Also called solutions Also called suspensions

3. Heterogeneous Mixtures • See visibly different regions • Granite • Dirt • Cereals • Oil & Vinegar • See a boundary • Ice cube in water Memory Jogger

4. Homogeneous Mixtures • Particles are very small – on the atomic scale • Can’t see the particles • Can’t sort the particles • Can’t get trapped by filter • Can’t scatter light • Particles are evenly distributed • Particles do not separate • Liquid & gas phase solutions look translucent Memory Jogger

5. CuSO4(aq) source source Which is a solution & how do you know?

6. Solution • A homogeneous mixture of 2 or more substances in a single physical state (phase). • Exist in all 3 phases.

7. Parts of a Solution • Solute= dissolved substance. • Solvent= dispersing medium.

8. Identify the solute and solvent in each picture.

9. Solute = ? Solvent = ?

10. Hints to identify solute & solvent • Solute– changes phase, substance you have less of • Solvent– substance you have the most of, maintains phase

11. Aqueous Solutions • Wateris the solvent. • Transition metalsform brightly colored solutions.

12. Solutions occur in all 3 phases!

13. Gas dissolved in a solid

14. CO2 in and out of water Mixture Solution When you see bubbles, it’s a mixture not a solution!

15. Alloys Alloys

16. Sublimation

17. Soluble • Soluble– capable of being dissolved. • Asubstance that dissolves in another substance issolublein that substance.

18. Insoluble • A substance that does not dissolve in another substance.

19. Amounts that can dissolve • Solubility = maximum amount of 1 substance that will dissolve in a given amount of another substance. • LIMITSto the amounts of most liquid or solid solutes that will dissolve in a given solvent. • Temperatureand pressurecan affect solubility.

20. Factors that affect the rate of dissolving • Rate of dissolving is different from the amount that will dissolve! • Rate is how fast. Several factors influence rate of dissolving. • Temperature • Stirring or Agitation • Surface Area of Solute • Amount of solute already dissolved.

21. Dissolving • Dissolving is a physical change. • All physical & chemical changes are accompanied by changes in energy.

22. Equations for Dissolving C6H12O6(s)  C6H12O6(aq) NaCl(s)  Na+(aq) + Cl-(aq)

23. source Covalent substances dissolve to produce molecules in solution.

24. Ionic substances dissolve to produce ions in solution. Movie: Dissolution of NaCl

25. Solvation • Interaction between the solvent molecules and the solute particles. Solute particles are surrounded by solvent particles in the dissolving process. • Solute particles may be ions, polar molecules, or nonpolar molecules. • Solvent molecules may be polar or nonpolar.

26. Hydration • Specific name for the solvent-solute interaction when the solvent is water.

27. Hydration of chloride ion. Also called a molecule-ion interaction.

28. Molecule-ion interaction The solute-solvent interaction must be greater than the interaction between solute particles for dissolving to occur.

29. What about when covalent substances dissolve? • Covalent substances can be polar or nonpolar. • General rule: Like Dissolves Like. • H2O is a very polar solvent, so it tends to dissolve polar solutes. Oil is nonpolar: oil does not dissolve well in water. • Ionic substances will dissolve in polar solvents.

30. Vocabulary Interlude • Miscible: two liquids that will mix in any amounts. • Water and ethanol are miscible in all proportions. • Immiscible: Liquids that cannot mix • Oil and water are immiscible.

31. Solvation in different systems.

32. Solubility • Amount of solute that will dissolve in a specific solvent at a givenTEMPERATURE and PRESSURE. • Determined experimentally. • Units: grams solute per 100 grams solvent

33. Solubility Curves of Selected Solids Solubility traces for most but not all solids have +’ve slopes. The hotter the solvent, the more solute dissolves.

34. Solubility Curves

35. Why do we heat the water up when making rock candy?

36. Solubility Curves of Selected Gases Solubility traces for all gases have –’ve slopes. Why do fish like cold water?

37. Why do you see bubbles form on the side of the beaker as the water warms up? (It’s not hot enough to boil.)

38. Oil & H2O are immiscible.

39. Types of Solutions

40. Electricity • What do you need to conduct electricity? Mobile charged particles!!!!

41. Vocabulary Interlude • Electrolyte: A substance that dissolves in water to form a solution that conducts electricity. (There are ions in the solution.) • Nonelectrolyte: A substance that dissolves in water to form a solution that does not conduct electricity. (There are neutral molecules in solution.)

42. Electrolyte vs. Nonelectrolyte Which solution conducts a current?

43. Dilute vs. Concentrated • Tell you relative amount of solute in solvent. • Concentrated – relatively large amounts of solute. • Dilute – relatively small amounts of solute.

44. Which solution is the most dilute? The most concentrated? How do you know? The stronger the color, the more concentrated the solution.

46. Which solution is more concentrated?More dilute? What can you say about thenumber of solute particlesin pictures b and c? It’s the same!

47. Unsaturated Solution • Has lesssolute than the maximum amount that will dissolve at that temperature and pressure.

48. Saturated Solution • No more solute will dissolve in it at that temperature & pressure. • Solubility = amount of solute required to form a saturated solution.

49. The solution is saturated when the solute stops dissolving.

50. Dynamic Equilibrium = Saturated Solution Microscopic level: Rate of dissolving = Rate of recrystallization. Macroscopic level: No apparent change.