1. Solutions I
Test Review

2. 1. Identify solution/solvent
Mixture
Solute
Solvent
Gatorade
Gatorade powder
Water
club soda
Carbon dioxide
air
oxygen
nitrogen
gold
Other metals
Gold
vinegar (5% acetic acid)
Acetic acid
water

3. 2. Solutions, suspensions, and colloids
sand mixed with water
brass
c. cloud
d. air
e. milk
f. a mixture that quickly settles into a watery liquid and an oily liquid
g. a mixture that is transparent, does not scatter light
h. mayonnaise
suspension
Solution (solid solution/alloy)
colloid
Solution (gas solution)
colloid
suspension
colloid
colloid

4. 3. Describe the dissolving of calcium iodide on a molecular level
3. Describe the dissolving of calcium iodide on a molecular level. (Explain the orientation of the water molecules around the calcium ions and the iodide ions.) I-
Ca+ O H H

5. 4. The grams of solute that will dissolve in 100 grams of water expresses ________
solubility

6. 5. List 3 actions to increase the rate a solute will dissolve in a solvent.
1. stir
2. crush
3. increase/decrease temperature (exothermic/endothermic)

7. 6. Place the following in order of increasing rate of dissolving:
a. granulated sugar, cold tea, stirred
b. sugar cube, hot tea, unstirred
c. sugar cube, cold tea, unstirred
d. granulated sugar, hot tea, stirred 2 3 4 1

8. 7. Alcohol dissolves in water; the two liquids are ______________
miscible (or polar)

9. Non-polar dissolves non-polar
Like dissolves Like
Polar dissolves Polar
Non-polar dissolves non-polar

10. 8. Which of the following will dissolve in water? KNO3 CCl4 MgCl2
gasoline (C8H18)
Ionic Compound
Non-Polar
Ionic Compound
Non-Polar

11. 9. Which of the following will dissolve in cyclohexane, C6H12?
NaCl
Br2
all brinclhof elements are non-polar
H2O
KNO3
benzene (C6H6)
all hydrocarbons are non-polar

12. 10. Determine whether the following is describing a saturated solution, an unsaturated solution, or a supersaturated solution.
clear solution on top of test tube, solid on bottom
more solute will dissolve
crystals immediately form when disturbed
saturated
unsaturated
Super-saturated

13. 11. Name 2 things I can do to get more gas to dissolve.
Decrease the temperature or
increase the pressure

14. 12 a)I have a saturated solution of potassium chlorate dissolved in 100 mL of water at 50C. What mass of potassium chlorate is in there? If I raise the temperature to 90C, how much more potassium chlorate can I add and still have a saturated solution?
50g -
20g
= 30g KClO3

15. Above the line = supersaturated
On the line = saturated
Below the line = unsaturated

16. For solubility curve problems
g solute =
g solute
g water
100g water
grams water = mL water

17. 12 b) I have a solution with 170 g of sodium nitrate dissolved in 250 mL of water at 10C. Is this solution saturated, unsaturated, or supersaturated? 68
170 g solute
g solute =
250mL water
100g water
unsaturated

18. 12 c) I have a saturated solution of potassium nitrate at 50C
12 c) I have a saturated solution of potassium nitrate at 50C. I slowly cool the solution to 20C with no potassium nitrate precipitating out. What type of solution do I now have at 20C?
supersaturated

19. 13)A substance that can conduct enough electricity (when dissolved in water) to make a light bulb glow brightly is a strong electrolyte. An example of this type of substance would be sodium chloride in water. A substance that can conduct enough electricity (when dissolved in water) to make a light bulb glow dimly is a weak electrolyte; an example of this type of substance is HF, acetic acid, etc. A substance that will not conduct electricity (when dissolved in water) is called a non-electrolyte and an example would be sugar in water.

20. Remember, A substance must be DISSOLVED in water to be an electrolyte
Ex. NaCl by itself is not an electrolyte, NaCl in water is a strong electrolyte

21. 14. Which of the following solutions will conduct electricity
14. Which of the following solutions will conduct electricity? Provide reasons.
Both a. and c. have positive and negative charges in their solutions

22. Sulfuric acid = bright (creates more ions)
15. Sulfuric acid ionizes a great deal in water; HCN is an acid that does not ionize much at all in water. Describe their effects on a light bulb when dissolved in water.
Sulfuric acid = bright (creates more ions)
HCN = no light

23. 16. Which of the following solutions will have the greatest effect on the freezing point of 1 liter of water? (Assume equal solubilities in water.)
1 mol sodium fluoride NaF  2 ions
1 mol magnesium bromide MgBr2  3 ions
2 mol potassium chloride 2KCl  4 ions
1 mol aluminum chloride AlCl3  4 ions
2 mol aluminum chloride 2AlCl3  8 ions