Name _____________________
Chemistry 110
Practice Final Exam
(solubility rules are given below!)
Problem Solving
Answer the following questions in the spaces provided. You must show ALL of your work to receive
credit for an answer. Place your final answer, with attention to significant figures and units, in the
boxes provided.
Ion(s)
Group IA and
ammonium
Acetate and nitrates
Rule
Group IA and ammonium salts are
all soluble.
Acetates and nitrates are soluble.
Chlorides, bromides,
and iodides
Most halides (Group VII A) are
soluble.
sulfate
Most sulfates are soluble.
carbonate
Most carbonates are insoluble.
phosphate
Most phosphates are insoluble.
sulfide
Most sulfides are insoluble.
hydroxide
Most hydroxides are insoluble.
Practice Final Exam
Sp 2010
Exceptions
None: all species containing these
ions will be assumed soluble
None: all species containing these
ions will be assumed soluble
Silver, mercury, and lead (II):
halides containing these cations
are NOT soluble
Calcium sulfate, strontium sulfate,
barium sulfate, silver sulfate, lead
(II) sulfate are NOT soluble
Group IA and ammonium
carbonates: these compounds ARE
soluble
Group IA and ammonium
phosphates: these compounds
ARE soluble
Group IA and ammonium sulfides:
these ARE soluble
Group IA and ammonium
hydroxides, calcium hydroxide,
strontium hydroxide, and barium
hydroxide: these ARE soluble
Page 1 of 8
Chemistry 110
Clark College
1. Nomenclature. For each set below:
a. Determine if the following are ionic (I) or covalent (C).
compound based on the name given.
Ionic (I) or
Compound
Covalent (C)
Then write the formula for the
Formula
potassium phosphide
hydrobromic acid
N/A
Dioxygen pentachloride
sodium phosphate
nickel (II) phosphate
Lead (II) hydroxide
Carbon tetrachloride
b. Determine if the following are ionic (I) or covalent (C). Then write the name of the compound
based on the name given.
Ionic (I) or
Name
Formula
Covalent (C)
TiN2
Mn(NO3)3
Al2(CO3)3
N/A
H2SO4 (aq)
Si3Cl4
NaCl
N2O4
2. A reaction requires 1235.0 g of K2SO4. How many moles of K2SO4 is that?
Practice Final Exam
Sp 2010
Page 2 of 8
Chemistry 110
Clark College
3. Classify the following reactions as single displacement or double displacement
TiCl4(l) + 2 Ca(s) → 2 CaCl2(s) + Ti(s)
This reaction is a (circle one):
Double Displacement
Single displacement
3Sr(OH)2(aq) + 2H3PO4(aq) → Sr3(PO4)2 (s) + 6H2O(l)
This reaction is a (circle one):
Double Displacement
Single displacement
4. Use the solubility rules to determine if the following compounds are soluble (aq) or insoluble (s).
Ca(OH)2
K2CO3
PbCl2
Ca3(PO4)2
5. From the reactants given, provide the molecular, ionic, and net ionic equations. You must write
molecular and ionic for all reactions, If no reaction occurs, indicate that in the net-ionic by writing
NR
_____K3PO4(aq) + _____Ca(NO3)2(aq) → _______________________________________________________
Ionic: _____________________________________________________________________________________
Net-ionic: _________________________________________________________________________________
_____KOH(aq) + _____HCl (aq) → ____________________________________________________________
Ionic: _____________________________________________________________________________________
Net-ionic: _________________________________________________________________________________
Practice Final Exam
Sp 2010
Page 3 of 8
Chemistry 110
Clark College
5. From the starting materials given, predict the products of the reactions and provide a balanced
complete molecular equation. Do not forget your phases!
_____ Na (s) + _____ Pb(NO3)2(aq) → ________________________________________________
_____Ca(s) + _____HNO3(aq) → ___________________________________________________
_____K(s) + _____H2O(l) → _______________________________________________________
6. You are given two aqueous solutions. One contains 82.55 grams of sodium carbonate and the
other contains an excess amount of cobalt (III) nitrate. Using the balanced chemical reaction for
reaction of these two solutions, answer the questions below
Molecular Equation:
3 Na2CO3
a.
(aq)
+
2Co(NO3)3
(aq)

6NaNO3
(aq)
+ Co2(CO3)3
(s)
Please calculate the molar masses for all reactants and products – show all work and pay attention to
significant figures
Question continues on next page . . .
Practice Final Exam
Sp 2010
Page 4 of 8
Chemistry 110
b.
Clark College
Determine the theoretical yield the “easiest” product to isolate in this reaction. show all work and
pay attention to significant figures
Theoretical Yield = _______________________________________
c. If you obtained an 85.2% yield of product, how much product, in grams, did you actually obtain?
show all work and pay attention to significant figures
7. Benzoic Acid has the following elemental analysis: C 68.836%, H 4.9619%, O 26.202%.
Determine its empirical formula show all work
8. The molecular weight of benzoic acid is 122.13 g/mol. Determine its molecular formula. show
all work
Practice Final Exam
Sp 2010
Page 5 of 8
Chemistry 110
Clark College
9. Fill in the table below:
56Fe
40Ca____
115In
26 protons
______ protons
49 protons
______ electrons
18 electrons
49 electrons
______ neutrons
______ neutrons
_____ neutrons
15N-3
64Cu+2
127I
______ protons
______ protons
53 protons
_____ electrons
_____ electrons
______ electrons
______ neutrons
______ neutrons
______ neutrons
10. Write balanced nuclear reactions for the following
a.
48
22 Ti undergoing
positron emission
b. The formation of Tungsten-184 through electron capture (Tungsten is element W)
c. Lead-208 undergoing α decay (lead is element Pb)
d. Formation of 210Po through positron emission
e. Astatine-210 undergoing beta decay (Astatine is element At)
Practice Final Exam
Sp 2010
Page 6 of 8
Chemistry 110
Clark College
Multiple Choice: Circle the correct answer
1. The number of grams in a 15.22 mole sample of nitrogen gas is:
A. 213.7 grams
B. 426.5 grams
C. 0.5432 grams
D. 1.086 grams
2. The mass number for an atom is equal to:
A. The number of protons.
B. The number of protons + electrons.
C. The number of protons + neutrons.
D. The number of electrons + neutrons.
3. The radius of a proton is approximately 1.0 x 10-13 mm. What is the radius in meters?
A. 1.0 x 10-16 m
B. 1.0 x 10-10 m
C. 1.0 x 10-12 m
D. 1.0 x 1015 m
4. 292.15 K is equivalent to: (note: K = oC + 273.15)
A. 19°C
B. 19.00°C
C. 19.000°C
D. 565.30°C
Practice Final Exam
Sp 2010
Page 7 of 8
Chemistry 110
Clark College
5. The density of acetone is 0.7857 g/mL. What is the volume of 92.4 g of acetone?
A. 117.602 mL
B. 118 mL
C. 0.00850 mL
D. 72.6 mL
6. Which of the following compounds is a metalloid?
A. P
B. K
C. As
D. He
7. Which of the following compounds is a noble gas?
A. Na
B. N
C. Ni
D. Ne
8. When solution of sulfuric acid and barium nitrate are mixed, a solid is formed. The spectator ions
(the species that do not react to form the product) in the reaction is/are:
A. only SO42-.
B. only H+.
C. only NO3-1.
D. both H+ and NO3 -.
Practice Final Exam
Sp 2010
Page 8 of 8