Honors Chemistry
Name _________________________________
Chapter 12: Solutions Worksheet I
Date _____/_____/_____
Period _____
Matching: Match the following terms with the phrase that best describes its meaning.
__d___ 1. mixture
a. medium sized solute particles that can only be seen
using a laser and the particles will NOT settle out of
the mixture
__g___ 2. heterogeneous
__c___ 3. suspension
b. a mixture that has the same consistency throughout
__h___ 4. solvent
c. the solute is visible with the naked eye and will fall
out of the mixture upon standing
__b___ 5. homogeneous
d. two or more things physically combined
__i___ 6. alloy
__a___ 7. colloid
e. the part of a solution that is being dissolved and is in
the smallest proportion
__j___ 8. solution
f. a dissolvable substance
__e___ 9. solute
g. a mixture that does NOT have the same consistency
throughout
__l___ 10. insoluble
__f___ 11. soluble
h. the part of a solution that does the dissolving and is
in the largest proportion
__n___ 12. pure substance
i. a solid – solid solution such as brass or steel
__k___ 13. water (H2O)
j. the smallest sized solute particles that cannot be
seen even when using a laser and the particles will
NOT settle out of the mixture
__m___ 14. Molarity (M)
k. the universal solvent
l. a substance that will not dissolve
m. moles of solute per 1 liter of solution
n. an element or compound
Completion: Use the following word bank to fill in the correct responses to the given questions.
solution
suspension
solute
solvent
dissolve
suspension
insoluble
solubility
precipitate
soluble
concentrated
saturated
unsaturated
alloy
colloid
dilute
water
1. What term is used to describe a substance dissolving?
soluble
2. What is a solid – solid solution of two or more metals called?
alloy
3. A mixture in which the particles are so small that they will not reflect the “light” from a
laser is called
solution
.
4. A solution that contains a large amount of solute per amount of solvent is called a
concentrated
solution and is said to be strong.
5. What is the term that is used to describe a solid being formed when two or more liquids
are mixed together?
precipitate
6. When a solution is made, what is the smaller portion of the solution called? In other
words, what is the part that is being dissolved called?
solute
7. A solution that contains as much solute as it can hold at a given temperature is called
saturated
.
8. When a solution is made, what is the larger portion of the solution called? In other
words, what is the part that is doing the dissolving called?
9. A mixture in which the particles settle out upon stand is called
solvent
suspension
The particles in the mixture can be seen with the naked eye.
10. If a substance will NOT dissolve it is said to be
insoluble
.
11. A solution that will hold more solute is said to be
unsaturated
.
12. A solution that contains a small amount of solute per amount of solvent is called a
dilute
solution and is said to be weak.
.
13. A mixture in which the particles can only be seen with a laser and do NOT settle out upon
standing is called a
colloid
.
14. The amount of solute that can be dissolved in a solvent at a given temperature is
described as the solutes
solubility
.
15. Due to the fact that so many substances dissolve in
water
, it is called
the universal solvent.
Completion: Explain how each of the following would affect the equilibrium.
H2O
AgNO3(s)
+
22 kJ/mole

AgNO3(aq)
a. Heating the solution – adding heat affects the side that absorbs energy and
causes the reaction to shift away. The reaction shifts to the right.
b. Removing solid silver nitrate – removing the solid causes the reaction to
shift to the side that the solid is being removed from. It causes the
reaction to shift to the left.
c. Cooling the solution – cooling the solution indicates that energy is being
removed from the side that energy is involved. It causes the reaction to
shift to the left
d. Adding solid silver nitrate – adding solid affects the side that solid is listed
and causes the reaction to shift away from that side. It causes the
reaction to shift to the right.
Calculations: Show all work for the following calculations.
1. Calculate the molarity, molality, and mass percent of acetic acid, C2H3O2H, in a solution
composed of 14.1 g of acetic acid and 250 g of water with a final solution volume of 260
mL.
14.1 g C2H3O2H
1 mole C2H3O2H = 0.235 mole C2H3O2H
60.06 g C2H3O2H
0.235 mole C2H3O2H = 0.90 M
0.26 L
0.235 mole C2H3O2H = 0.94 m
0.25 Kg
14.1 g C2H3O2H x 100 = 5.4 %
260 g
2. How many grams of C2H5OH are required to prepare 25 mL of a 0.400 M solution?
0.025 L C2H5OH
0.400 moles C2H5OH
1 L C2H5OH
46.08 g C2H5OH
moles C2H5OH
= 0.46 g C2H5OH
3. The level of vitamin C (C6H8O6) in blood is about 0.2 mg per 100 mL. What is the
concentration of vitamin C in blood?
0.2 mg C6H8O6
1 g C6H8O6
1000 mg C6H8O6
1 mole C6H8O6
176.14 g C6H8O6
= 1 x 10-6 mole C6H8O6
1 x 10-6 mole C6H8O6 = 1 x 10-5 M C6H8O6
0.1 L C6H8O6
4. What is the normality of a solution in which 45.32 grams of Ca(OH)2 is dissolve in 90 mL
of water? (Assume the density of the water and the density of the solution are both
1.000 g/mL)
45.32 g Ca(OH)2
1 mole Ca(OH)2
74.10 g Ca(OH)2
= 0.6116 mole Ca(OH)2
90 mL H2O
1.000 g H2O
1 mL
= 90 g + 45.32 g = 140 g solution
140 g solution
1 mL solution
1 L solution
1.000 g
1000 mL
solution
= 0.14 L
solution
0.6116 mole Ca(OH)2 = 4.4 M Ca(OH)2
0.14 L Ca(OH)2
2 eq x 4.4 M Ca(OH)2 = 8.8 N Ca(OH)2
5. Calculate the number of moles of Ca(OH)2 in 150.0 mL of a 0.500 M solution.
0.1500 L Ca(OH)2
0.500 moles Ca(OH)2
1 L Ca(OH)2
0.0750 moles Ca(OH)2