1. Notes Chapter 9
Book chapter 7

2. 9-1 Nature of Solutions
Video #17(solutions: CC)
*Solution: p229
homo mixture in which one subst is dissolved in another subst
”Well mixed”

3. -Properties of Solution
-2 parts make up a solution
*Solute:
subst that is
dissolved
*Solvent:
the subst that does
the dissolving

4. -the solvent is usually a liquid
ex: water(aqueous solution)
*Tincture:
when alcohol is the solvent in the solution

5. -more properties of solutions
Partic are indiv atoms, ions, or molecules
Liquid solution appears clear

6. 3. Cannot be easily separated by simple means such a filtering
4. Solute molecules are evenly spread among solvent molecules(all parts are ident)

7. -Conductivity of Solutions
-good conductor if it contains ions
-nonconductor if it does not contain ions
*Dissociation:
separation of ions from a cmpnd during solution

8. *Electrolytes:
aqueous solution that conducts electricity
-usually ionic cmpnds
*Nonelectrolytes:
not conduct ele
-usually covalent cmpds

9. *Ionization:
formation of ions from solute molecules by the action of a solvent

10. -Model of the solution process
Solute part are separated from the surface of the solid solute(Dissolving)
-endothermic(takes up nrg)

11. 2. Solvent molecules are moved apart to allow solute molecules to enter the liquid surrounding the solid solute
-endothermic

12. 3. Solute molecules are attracted to solvent molecules
-exothermic

13. 9-2 Making Solutions

14. -Types of Solutions *miscible: 2 liquids that dissolve in each other
ex: water and alcohol
-alloy:
solutions of solids in solids

15. -Rate of Solution
-Ways to increase the rate of dissolving the solute – pp236
1. Heat it
2. Stir it
3. Crush it

16. -Solubility
-Measure of how much of a solute can be dissolved in a given amnt of solvent under certain conditions
pp239

17. -Solubility
-solubility depends on the nature of the solute and solvent

18. -Solubility
-it is the mass of solute that can be dissolved in a definite amnt of solvent at a spcfc temp
-factors that effect solubility
1.Temp
2. Pressure

19. -temp
~solubility is increased in solids when temp is raised
~solubility is decreased in gases when temp is raised

21. How much Sodium Chloride can be dissolved at 80 degrees Celsius?
40 grams
If I want to dissolve 100 grams of Potassium Nitrate, how hot will the solvent need to be?
57 degrees Celsius

22. ex: graph demo
-pressure
~solid and liquid practically no effect
~gases dissolved in liquids, higher pressure higher solubility; and vise versa

23. *Effervescence:
escape of gas from a liquid solution

24. -Concentration of Solutions pp240
*amnt of solute dissolved in a certain amnt of solvent
*Concentrated:
much solute
*Dilute:
little solute
-also can be described as saturated, unsaturated, supersat

25. 1. Saturated Solutions
*contains all the solute it can possibly hold at a given temp
-temp must always be given

26. 2. Unsaturated Solution
*contains less solute than it can possibly hold at a given temp

27. 3. Supersaturated Solution
*holds more solute than is normal for that temp.
-supersat solu:
is unstable

28. 9-3 Water-The Universal Solvent
-most common subst on earth
-65% of body mass
*Insoluble:
will not dissolve

29. -Structure of a Water Molecule
-unequal sharing produces an uneven charge
*Polarity:
oppositely charged ends

30. -Polar and Nonpolar Molecules
-Like dissolves Like
EX: Water Molecule Structure on board
ex: p683

31. -Water Quality
-the taste, odor, and appearance of water determines its quality
*Hard water:
contains large amnts of dissolved metal ions
*Soft water:
no metal ions

32. -Special Properties of Solutions
-when a solute is dissolved in a liquid solvent, the freezing pnt is lowered/boiling pnt raises
*Freezing pnt depression:
*Boiling pnt elevation:

33. 9-4 Suspensions and Colloids
Video #18(solution, suspen, coll)
-physical prop determine whether a mixture is a suspension or a colloid

34. -solute part are larger than atoms, ions, or molecules
Suspension: p456
hetero mixture
-solute part are larger than atoms, ions, or molecules
-part. large enough to be seen without a microscope
-will settle out over time

35. *Colloids: p455
homo mixture
-not true solution
-part. to small to be seen
-does not separate
-does scatter light

36. *Brownian Motion:
constant movement of colloid particles

37. 9-5 Acids
-properties
1.pH below 7
2.taste sour

38. 3.turns blue litmus paper red
4.reacts with metals to produce H gas
5.ionizes in water to produce H+
6.proton donor

39. *Indicators:
show definite color change when mixed with an acid
ex: litmus, phenolphtalein
*Hydronium ion H3O+: H+&water molecule

40. -Common Acids
-Strong acids
HCl
H2SO4
HNO3

41. -Common Acids
-Weak acids
H2CO3
H3BO3
HC2H3O2

42. 9-6 Bases
-properties
1.taste bitter
2.slippery to touch

43. 9-6 Bases
3.turn litmus from red to blue
4.turn phenolphthalein pink
5.dissolve fats and oils
6.contain hydroxide ions(OH-)

44. 9-7 Acids and Bases in Sol.: Salts
*pH:
measure of the hydronium ion (H3O)
-indicates how acidic the solution is

45. 9-7 Acids and Bases in Sol.: Salts
- 0<7 =
acid
- 7>14 =
base
- 7 =
neutral

46. -Determining Solution pH
-by using an indicator
ex: pH, litmus, phen, methyl orange, bromthyol blue

47. -Formation of Salts acid + base -> salt + water *neutralization:
*precipitate:
a solid
*precipitation:
process of forming a solid
Is a 2Bl replacement rxn