1. Physical Properties of Solutions
Chapter 12
Solution Stoichiometry
end of Chapter 4

2. A ____________is a _______ mixture of 2 or more substances
The _______is(are) the substance(s) present in the _______ amount(s)
The _______is the substance present in the ______ amount
12.1

3. An _______ is a substance that, when dissolved in water, results in a solution that ____ conduct _____.
A _______is a substance that, when dissolved, results in a solution that _____ conduct ______.
____electrolyte
______ electrolyte
_____ electrolyte
4.1

4. A _______ contains the ______ amount of a _____ that will dissolve in a given solvent at a specific ______.
An _______ contains _____ solute than the _____ has the ______ to dissolve at a specific _______.
A __________contains more _____ than is present in a _______ solution at a specific temperature.
Sodium acetate crystals rapidly form when a seed crystal is
added to a supersaturated solution of sodium acetate.
12.1

5. Three types of interactions in the solution process:
DHsoln = DH1 + DH2 + DH3
12.2

6. “like dissolves like”
Two substances with similar _________forces are likely to be soluble in each other.
________ molecules are soluble in ______ solvents
CCl4 in C6H6
_______ molecules are soluble in _____solvents
C2H5OH in H2O
______compounds are more soluble in _____solvents
NaCl in H2O or NH3 (l)
12.2

7. Concentration Units
The ________ of a solution is the amount of _____ present in a given quantity of ______ or solution.
Percent by Mass
x 100%
% by mass =
Mole Fraction (X)
12.3

8. Concentration Units Continued
Molarity (M)
M =
Molality (m)
m =
12.3

9. What is the molality of a 5
What is the molality of a 5.86 M ethanol (C2H5OH) solution whose density is g/mL?
m = = =
12.3

10. Convert % mass to Molarity
What is the Molarity of a 95% acetic acid solution? (density = g/mL)

11. Temperature and Solubility
Solid solubility and temperature
12.4

12. Fractional crystallization is the separation of a mixture of substances into pure components on the basis of their differing solubilities.
Suppose you have 90 g KNO3 contaminated with 10 g NaCl.
12.4

13. Temperature and Solubility
Gas solubility and temperature
12.4

14. Pressure and Solubility of Gases
The solubility of a gas in a liquid is proportional to the pressure of the gas over the solution (______).
c = kP
low P
high P
low c
high c
12.5

15. Solution Stoichiometry (Chapter 4)
The _________of a solution is the amount of solute present in a given quantity of solvent or solution.
M = molarity =
What mass of KI is required to make 500. mL of
a 2.80 M KI solution? x x x =
4.5

16. 4.5

17. _________is the procedure for preparing a less __________solution from a more __________solution.
Dilution
Add Solvent = =
4.5

18. How would you prepare 60.0 mL of 0.2 M
HNO3 from a stock solution of 4.00 M HNO3? =
4.5

19. Gravimetric Analysis Dissolve unknown substance in water
React unknown with known substance to form a ________
Filter and dry precipitate
Weigh _________
Use chemical formula and mass of precipitate to determine amount of unknown ion
4.6

20. __________________– the point at which the reaction is complete
Titrations
In a titration a solution of accurately ________is added gradually added to another solution of _______concentration until the chemical reaction between the two solutions is complete.
__________________– the point at which the reaction is complete
_________– substance that changes ______ at (or near) the
equivalence point
Slowly add _____
to unknown ____
UNTIL
the indicator
changes color
4.7

21. What volume of a 1.420 M NaOH solution is
Required to titrate mL of a 4.50 M H2SO4
solution? M
acid rx
coef. M
base x 1 x 1 x =
4.7

22. Colligative Properties of Nonelectrolyte Solutions
Colligative properties are properties that depend only on the _____________________and not on the __________particles.
Vapor-Pressure Lowering
P1 = X1 P 1
P 1
= vapor pressure of pure solvent
X1 = mole fraction of the solvent
Raoult’s law
If the solution contains only one solute:
X1 = 1 – X2
P 1
- P1 = DP = X2
X2 = mole fraction of the solute
12.6

23. Fractional Distillation Apparatus
12.6

24. Boiling-Point Elevation
DTb = Kb m
12.6

25. Freezing-Point Depression
DTf = Kf m
12.6

26. 12.6

27. What is the freezing point of a solution containing 478 g of ethylene glycol (antifreeze) in 3202 g of water? The molar mass of ethylene glycol is g.
m =
12.6

28. Colligative Properties of Nonelectrolyte Solutions
Vapor-Pressure Lowering
Boiling-Point Elevation
Freezing-Point Depression
Osmotic Pressure (p)
12.6

29. Colligative Properties of Electrolyte Solutions
_______NaCl solution
____ ions in solution
i should be
nonelectrolytes __
NaCl __
CaCl2 __
12.7

30. Change in Freezing Point
Which would you use for the streets of Bloomington to lower the freezing point of ice and why? Would the temperature make any difference in your decision?
sand, SiO2
Rock salt, NaCl
Ice Melt, CaCl2

31. Colligative Properties of Electrolyte Solutions
Boiling-Point Elevation
DTb = i Kb m
Freezing-Point Depression
DTf = i Kf m
12.7

32. Change in Freezing Point
Common Applications of Freezing Point Depression
Ethylene glycol – deadly to small animals
Propylene glycol

33. Change in Boiling Point
Common Applications of Boiling Point Elevation

34. Freezing Point Depression
At what temperature will a 5.4 molal solution of NaCl freeze?

35. Osmotic Pressure (p)
Osmosis is the selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated one.
A semipermeable membrane allows the passage of solvent molecules but blocks the passage of solute molecules.
Osmotic pressure (p) is the pressure required to stop osmosis.
more
concentrated
dilute
12.6

36. Osmotic Pressure (p) p = MRT High P Low P
M is the molarity of the solution
R is the gas constant
T is the temperature (in K)
12.6

37. A cell in an: isotonic hypotonic hypertonic
solution
hypotonic
solution
hypertonic
solution
12.6

38. Colloid versus solution
A colloid is a _______of particles of one substance throughout a dispersing medium of another substance.
Colloid versus solution
collodial particles are much _____than solute molecules
collodial suspension is not as ________as a solution
12.8

39. Colloids
Brownian motion
Tyndall Effect

40. Suspensions These are mixed, but not dissolved in each other
Will settle over time
Particles are bigger than 1 micrometer (larger than colloid)
Examples: dust in air, muddy water