Chapter 15
Practice Problems
Vocabulary
Define the following terms:
1.) Solution
2.) Solvent
3.) Solute
4.) Aqueous solutions
5.) Saturated
6.) Unsaturated
7.) Supersaturated
8.) Concentrated
9.) Dilute
10.)
Mass percent
11.)
Molarity
12.)
Standard solution
13.)
Dilution
14.)
Neutralization reaction
15.)
Normality
16.)
Colligative property
17.)
Equivalent weight
18.)
Equivalent of an acid
19.)
Equivalent of a base
Answer the following using vocabulary terms:
1.) What does the solubility of a solute depend on?
Problems
1.) What happens to the solubility of a gas when the temperature increases?
2.) The label “aqueous H2SO4” means that there is a relatively _____ amount of
H2SO4 in the solution.
3.) If 59.5 g of NaCl is added to 250 g of water, calculate the mass percent of NaCl
in the solution.
4.) If 625 g of NaOH is dissolved into a final total volume of 25.0 L, what is the
molarity of the solution?
5.) Calculate the new molarity that results from the addition of 30 mL of water
to 150mL of 0.251 M HCl.
6.) What is the volume (in L) of 0.25 M Na2SO4 solution is needed to precipitate
all the barium, as BaSO4 from 12.5 mL of 0.15 M Ba(NO3)2 solution?
7.) What volume of 0.700 M NaOH solution is needed to neutralize 43 mL of
0.45 M HCl solution?
8.) Calculate the normality of .134 M HNO3.
9.) If 36.2 mL of 0.158 M CaCl2 solution is added to 37.5 mL of 0.149 M Na2CO3,
what mass of NaCl will be precipitated? The balanced reatction is: CaCl2 +
Na2CO3  CaCO3 + 2 NaCl
10.)
If 10.0 mL of 0.1926 M HNO3 solution is needed to neutralize 0.035 M
Ca(OH)2 solution of unknown volume, what is the volume of the calcium
hydroxide?
11.)
Solve problem number 10 using ionic and net ionic equations.
12.)
Find the limiting reactant of Ba(NO3)2 + KCrO4  BaCrO4 + KNO3
13.)
Using the same problem at question 12, find the mass of the product
containing chromium (II) oxide.
14.)
If 250mL of 0.125 M AgNO3 is added to 150 mL of 0.0125 M NaCl, find
the mass of the aqueous product.
15.)
Find the molarity of the two products resulting from 100mL of .1 M
NaOH and 100 mL of .10 M HCl.
Chapter 15
Answers
Vocabulary
Define:
1.)
2.)
3.)
4.)
5.)
6.)
A homogeeous mixture
The dissolving medium in a solution
A substance dissolved in a solvent to form a solution
A solution in which water is the dissolving medium, or solvent
A solution that contains as much solute as can be dissolved in that solution
A solution that has not reached the limit of solute that will dissolve in that
solution
7.) A solution that contains more dissolved solid than a saturated solution will
hold at that temperature.
8.) When a relatively large amount of solute is dissolved
9.) When a relatively small amount of solute is dissolved.
10.)
Expresses the mass of solute present in a given mass of a solution
11.)
The number of moles of solute per volume of solution in liters
12.)
A solution whose concentration is accurately known
13.)
The process of adding more solvent to a solution
14.)
An acid-base reaction
15.)
The number of equivalents of solute per liter of solution
16.)
A solution property that depends on the number of solute particles
present
17.)
The mass in grams of 1 equivalent (equiv) of that acid or base
18.)
The amount of that acid that can furnish 1 mol of H+ ions.
19.)
The amount of base that can furnish 1 mol of OH- ions.
Answer:
1.) It depends on the interactions between the solvent and solute particles.
Problems
1.)
2.)
3.)
4.)
5.)
6.)
7.)
8.)
9.)
It decreases
Low
19.2%
0.5 M
0.206 M
0.075 L
27.6 mL
.134 mol/L or .134 normal solution
138.3 g
10.)
11.)
12.)
13.)
14.)
15.)
27.5mL
Ionic: Ca2+(aq) + 2OH-(aq) +2H-(aq) + 2NO3-  Ca2+ + 2NO3- +2H2O(l)
a. Net ionic: 2OH-(aq) + 2H+ (aq) 2H2O(l)
Ba(NO3)2
.88g
.1598g
.01 M NaCl and .01 M H2O