Unit 10 Solutions Review
Name: ________________
Period: ______
1. The substance that is being dissolved is called the__SOLUTE____.
2. An electrolyte is a chemical that (does or doesn’t) conduct electricity in a solution?
DOES
3. Put the following symbols on the correct location of the water molecule: δ- , δ+ , δδ-
δ+
δ+
4. When a substance has a negative and positive side, we would describe that molecule
as__POLAR_______.
5. A solution that contains as much solute as possible is described as:
SATURATED
6. A solution that contains more solute than possible at that temperature is described as:
SUPERSATURATED
7. A solution that contains less solute than possible is described as:
UNSATURATED
8. What could you do to the pressure and temperature of a solution to increase the
solubility of a gas?
INCREASE PRESSURE & DECREASE TEMPERATURE
9. What are the three factors that affect the rate of dissolution of a solid?
SURFACE AREA, AGITATION, TEMPERATURE
10. What could you do to each of these factors that would increase the rate of dissolution
of a solid?
INCREASE
11. A mixture is considered a suspension if: ___PARTICLES SETTLE __
12. A mixture is considered a colloid if:__ PARTICLES DON’T SETTLE, BUT TYNDALL EFFECT
OCCURS ____________________
13. A mixture is considered a solution if: __PARTICLES DON’T SETTLE, NO TYNDALL EFFECT
________________________
14. What is the Tyndall Effect? WHEN LIGHT IS SCATTERED DUE TO VERY SMALL PARTICLES
IN ITS PATH. TYNDALL EFFECT IS DISPLAYED IN COLLOIDS
15. The solubility rules show that most salts containing which ion is insoluble?
a. K+
b. Pb+2
c. Na+
d. Li+
Unit 10 Solutions Review
Name: ________________
Period: ______
16. What does “likes dissolve likes” mean?
POLAR SUBSTANCES DISSOLVE POLAR SUBSTANCES AND NONPOLAR DISSOLVES NONPOLAR
17. What can you do to a supersaturated solution that would make the solute precipitate
out?
ADD A CRYSTAL
18. What is the molarity of a solution that contains 4.05mol of NaCl and has a volume of
0.190 L?
M = mol solute / liters solution
= 4.05 mol / 0.19 L
= 21.3 Molar
19. What is the volume of an 8.5 M NaCl solution that contains 9.09 mol of NaCl?
M = mol solute / liters solution
8.5 M = 9.09 mol / L solution
L solution = 9.09 mol / 8.5 M
= 1.1 L
20. Describe the equilibrium when a substance is dissolving.
EQUILIBRIUM EXISTS WHEN THE RATE OF DISSOLUTION EQUALS THE RATE OF
CRYSTALLIZATION
21. How many liters of solution can be produced from 2.5 moles of solute if a 2.0 M
solution is needed?
2.0 M = 2.5 mol / L solution
L solution = 2.5 mol / 2.0 M
= 1.3 L solution
22. How many grams of potassium nitrate are required to prepare 0.250 L of a
0.700 M solution?
M = mol / L
0.700 M = mol / 0.250 L
0.700 M X 0.250 L = mol
0.175 mol KNO3 | 101.11 g KNO3 = 17.7 g KNO3
| 1 mol KNO3
Unit 10 Solutions Review
Name: ________________
Period: ______
23. How many moles of sucrose are dissolved in 250 mL of solution if the solution
concentration is 0.150 M?
M = mol / L
0.150 M = mol sucrose / 0.250 L solution
0.150 M X 0.250 L = mol sucrose
0.0375 mol sucrose
24. A commercial ammonia solution is labeled 7.4M. How many liters of this solution are
needed to prepare 2.5 liters of 3.0 M NH3 for the laboratory?
M1 X V1 = M2 X V2
7.4 M X V1 = 3.0 M X 2.5 L
V1 = 3.0 M X 2.5 L / 7.4 M
= 1.0 L
25. A teacher starts with 0.250L of a 0.050M NaOH solution and dilutes it to 1.5L. What is
the concentration of NaOH in the new solution?
M1 X V1 = M2 X V2
0.050 M X 0.250 L = M2 X 1.5 L
0.050 M X 0.250 L / 1.5 L = M2
0.0083 M
Unit 10 Solutions Review
Name: ________________
Period: ______
Fill in the following table using the solubility curve:
Solution
Saturated or Unsaturated?
a solution that contains 70g of
NaNO3 at 30°C (in 100 mL
H2O)
Unsaturated
a solution that contains 50g of
NH4Cl at 50°C (in 100 mL H2O)
Saturated
a solution that contains 20g of
KClO3 at 50°C (in 100 mL H2O)
Saturated
a solution that contains 70g of
KI at 0°C (in 100 mL H2O)
Unsaturated
If unsaturated: How much
more solute can dissolve in
the solution?
About 25 g
About 60 g