Solution and Water Notes
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1. __________________________ a solid solution that is a mixture of 2 pure elements. Higher strength
greater resistance to corrosion than pure metals
1. In a __________________________ the particles settle from the solvent because they are large,
unless they are mixed constantly. Size is over 1000 nm.
2. __________________________ mixture in which the particles do not settle
a. Examples: ____________________________________________________
3. __________________________ colloids scatter light when it is shined upon them
a. Why do we use low beams on cars when driving in fog?
b. Colloids appear __________________________ because particles can’t be seen
c. The particles are large enough to scatter light
Solution
Colloid
Suspension
0.01 – 1.0 nm
1.0 – 1000 nm
over 1000 nm
can be filtered out
Doesn’t separate on standing
May scatter light but not
transparent
4. __________________________ The molecules spread out throughout the liquid
5. __________________________ - a tendency to stick to other polar substances.
a. Example: Glass may carry a partial charge along its surface. That’s why rain droplets stick to
windows.
6. __________________________ is the tendency of water molecules to stick together.
a. Example: As long as you don’t break the surface, the paper clip will remain on top of the water.
7. __________________________ are between like molecules
8. forces at the surface constitute __________________________
9. When the attractive forces are between unlike molecules, they are said to be ______________________
a. __________________________- the attraction of the surface of a liquid to the surface of a solid.
10. __________________________- is the resistance of a liquid to flow.
a. Example: Water is less viscous than honey, because water flows more easily
11. __________________________- is a measure of a substance’s mass per unit of volume
Solution and Water Notes
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12. When the __________________________pushing up on the object is greater than the force of gravity
pulling down on the object, the object rises to the surface. If the __________________________is less
than the force of gravity, the object sinks to the bottom
13. __________________________ force of attraction between molecules, ions, or molecules and ions
a. Dipole-dipole
i. 2 polar molecules
ii. Hydrogen bonding
b. Dipole-induced dipole-polar & nonpolar
c. Induced dipole-induced dipole: ___________________________
14. Decide what type of IMF is in each case and place them in order of increasing strength.
a. Methane-methane
b. Water-water
c. methane-water
15. Effects of Inter Molecular Forces (IMF)
a. IMF’s __________________________with molecular mass
b. As IMF __________________________, boiling point, melting point, and surface tension
__________________________.
c. As IMF __________________________, solubility __________________________.
d. Effects boiling/freezing points, solubility, and surface tension associated with liquids
16. __________________________is a force that tends to pull adjacent parts of a liquid’s surface together,
there by decreasing surface area to the smallest possible size.
a. _____Force of attraction = ______surface tension
b. H2O has a _____ surface tension because of __________________________
c. __________________________ are the attractive force between the atoms making up a
molecule
d. __________________________the attractive force between two molecules
17. Properties of Water
a. Water is __________________________
b. Water forms __________________________
c. When water freezes it expands to form a __________________________
18. __________________________is the weak intermolecular force between the H end of one molecule
and the O, N, or F end of another molecule
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19. __________________________Capable of being dissolved
20. __________________________The amount of a substance that dissolves in a given quantity of solvent
at a certain temperature and pressure
a. Common units are __________________________
21. __________________________ - A homogeneous mixture of 2 or more substances in a single phase
a. __________________________ – substance dissolving
b. __________________________ – does the dissolving
22. Concentrations
a. __________________________ To have the maximum amount of solute dissolved
b. __________________________ Does not have maximum amount of solute dissolved
c. __________________________ More solute in solution; usually by means of heating solutions.
23. Factors Affecting Solubility
a. Polar liquids tend to dissolve in polar solvents. __________________________
b. __________________________ liquids: mix in any proportions. ex. _______________________
c. __________________________ liquids: do not mix. ex: __________________________
d. Polar __________________________
e. Nonpolar __________________________
f.
Polar water molecules interacting with positive and negative ions of a salt.
g. Hydrogen Bonding –__________________________
24. __________________________– The separation of ions when an ionic compound dissolves
25. __________________________– Physical state in which the opposing process of dissolution and
crystallization of a solute occurs at equal rates
a. The solute dissolves and then reform the ionic solid at the __________________________
26. Electrolytes
a. __________________________completely dissociate into ions; solutions strongly conduct
electricity. Typical compounds: ____________________________________________________
b. __________________________incompletely dissociate into ions; solutions weakly conduct
electricity. Typical compounds: ____________________________________________________
c. __________________________no dissociation; solutions don't conduct electricity. Typical
compounds: ____________________________________________________
27. Solubility Rules:
a. All common compounds of Group I and ammonium ions are soluble.
b. All nitrates, acetates, and chlorates are soluble.
Solution and Water Notes
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c. All binary compounds of the halogens (other than F) with metals are soluble, except those of Ag,
Hg(I), and Pb. Pb halides are soluble in hot water.)
d. All sulfates are soluble, except those of barium, strontium, calcium, lead, and mercury (I). The
latter three are slightly soluble.
e. Except for rule 1, carbonates, hydroxides, oxides, silicates, and phosphates are insoluble.
f.
Sulfides are insoluble except for calcium, barium, strontium, magnesium, sodium, potassium,
and ammonium.
28. __________________________are insoluble products of a chemical reaction between solutions
29. Factors Affecting Solubility
a. __________________________will affect solubility.
b. If the solution process absorbs energy then the solubility will be ________________________as
the temperature is __________________________.
c. If the solution process releases energy then the solubility will _________________________with
__________________________temperature.
d. As temperature increases, solubility of solids generally _________________________
e. Gases get less soluble as temperature __________________________
f.
The higher the pressure, the greater the chance of a gas molecule striking the surface and
entering the solution, the __________________________
30. Factors affecting the rate of dissolving
a. Increasing the __________________________of the solute
b. __________________________the solution
c. __________________________the solvent
31. Colligative Properties
a. Properties that depend on the __________________________of solute particles but not on
their __________________________.
b. Effects properties of solutions
c. Depends on # of solutes in a solution
d. Two types of colligative properties are:
i. __________________________– The boiling point temperature is raised
ii. __________________________- The freezing point temperature is lowered.
32. Formulas
a. __________________________
b. __________________________
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
kb = molal boiling point elevation constant (for water = 0.51oC / m)

kf = molal freezing point depression constant

i = van’t Hoff factor (number of dissolved particles)

m = concentration in molality

T = change in temperature
(for water = 1.86oC/m)
33. What is the boiling point of a solution in which 10.144 g of NaCl is dissolved in 100.0 g of water?
34. What is the boiling point of a solution in which 45.8 g of CaCl2 is dissolved in 250.0 g of water?
35. Some beautiful blue crystal azulene (0.640 g) were dissolved in 100.0 g of benzene. The boiling point of
the solution was 80.23oC. Calculate the molar mass of azulene.
36. How many grams of ethylene glycol (C2H4(OH)2) must be added to 5.50 kg of water to lower the freezing
point of the water from 0.0oC to –10.0oC?
37. Assuming that NaCl dissociates completely into its ions when dissolved in water, how much sodium
chloride must be dissolved in 5.50 kg of water to lower the freezing point from 0oC to –10.0oC?
38. Camphor is a solid at room temperature (melting point=179.75oC). When melted it is a good solvent for
many nonionic compounds, and it has a very large kf value (-40.0 oC/molality). If you dissolve 0.640 g of
azulene in 100.0 g of camphor, the freezing point is 177.75oC. Calculate the molar mass.
Solution and Water Notes
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39. __________________________which are liquids that evaporate readily, (have relatively weak forces of
attraction between particles).
40. __________________________which evaporate slowly, have relatively strong attractive forces between
particles.
41. __________________________is the conversion of a liquid to a vapor within the liquid as well as at its
surface. It occurs when the equilibrium vapor pressure of the liquid equals the atmospheric pressure.
42. __________________________Is graph of temperature vs. pressure that indicates the conditions under
which gaseous, liquid, and solid phases of particular substances exist
43. __________________________of a substance indicates the temperature and pressure conditions at
which the solid, liquid, and vapor of the substance can coexist at equilibrium.
44. __________________________of a substance indicates the critical temperature and critical pressure,
above which the substance cannot exist in the liquid state
45. Critical temperature (tc)
46. Critical pressure