Download Final Exam Review Packet

Honors Chemistry
Final Exam Review
2011-12
Name ____________________________________________
Test Date: ____________ Time: ______________________
Room #: ______________ Proctor: ____________________
Unit 1: Measurement
1. A block of sodium with measurements 4.00 cm x 3.00 cm x 6.25 cm has a measured mass of 76.1 g. The
accepted density for sodium if 0.971 g/cm3. Calculate the percent error.
_____ 2. A 49.5 gram sample of tin at 95.0°C is placed into 145 grams of water. The water and tin reach thermal
equilibrium at a temperature of 26.1°C. What was the initial temperature of the water?
a. 22.4 °C
b. 24.9 °C
c. 27.3 °C
d. 29.8 °C
3. If 145 J of heat are added to an unknown metal of mass 121 g, the temperature of the metal goes from 22.2°C to
24.3°C. Calculate the specific heat of the metal.
Unit 2: Matter & Energy
_____ 4. Benzene, C6H6, boils at 80.1˚C and has a density of 0.877 g/cm3. Determine the quantity of heat that is required
to vaporize a 45.6 mL sample of benzene at 35.0˚C.
a. 3140 J
b. 4370 J
c. 15800 J
d. 18900 J
_____ 5. If a gas’s temperature increases, what happens to the pressure and volume?
a. Pressure increases and volume increases
b. Pressure decreases and volume decreases
c. Pressure decreases and volume increases
d. Pressure increases and volume decreases
_____ 6. A gas is collected over water in a eudiometer tube until the pressure is equilibrated with the atmospheric
pressure. The volume of gas in the eudiometer is 28.5 mL. The temperature of the water is 36.0°C and the
barometric pressure is 758 mm Hg. What is the volume of this gas at STP?
a. 23.6 mL
b. 25.1 mL
c. 30.3 mL
d. 32.2 mL
7. A balloon is filled to a volume of 745 mL with 158 grams of steam at 112°C. After a brief period of cooling, the
balloon’s volume is measured to be 735 mL. How much heat energy did the steam lose?
_____ 8. Which of the following occurs during a phase change?
a. Temperature increases
b. Kinetic energy increases
c. Heat energy increases
d. All of the above
_____ 9. Which lettered region represents the phase with the highest intermolecular forces?
A
B
C
D
E
Increasing Temperature
a.
b.
c.
d.
e.
D
E
C
B
A
Time
Unit 3: Atomic Theory & Nuclear
10. Write the isotopic symbols for atoms with the following:
a. 9 p+ and 10 no ________________
b. 25 p+ and 30 no________________
_____ 11. A chlorine atom has atomic number 17 and mass number 35. It has
i. 17 protons, 17 electrons, and 18 neutrons
ii. 35 protons, 35 electrons, and 17 neutrons
iii. 17 protons, 17 electrons, and 52 neutrons
iv. 18 protons, 18 electrons, and 17 neutrons
12. Complete the following chart:
Isotopic
Symbol
a
b
Isotope Name
Atomic
Number
Mass
Number
# protons
# electrons
# neutrons
16
8O
manganese-56
2
13. Determine the average atomic mass of the following mixtures of isotopes.
126
128
a. 80.% 127
53 I , 17% 53 I , 3% 53 I
_____ 14. If samples of two different elements each represent one mole, then
a. they are equal in mass.
b. they contain the same number of atoms
c. their molar masses are equal
d. they have the same atomic mass
15. Calculate the number of atoms in 10.0 g of aluminum.
16. Determine the mass in grams of 5.00 x 1023 mol of oxygen atoms.
17. Write balanced nuclear equations for the following:
a. The alpha decay of neptunium-237
b. The beta decay of bismuth-210
c. Alpha-particle bombardment of plutonium-239 produces a neutron and another isotope.
d. With what particle would you bombard sulfur-32 with to produce hydrogen-1 and phosphorus-32?
18. How much time will be required for a sample of radioactive tritium (t1/2 = 12.5 years) to lose 75 % of its
radioactivity?
_____ 19. A 900. mg sample of platinum-197 is found to have a mass of 56.3 mg after exactly 3 days. What is the halflife of platinum-197 in hours?
a. 24 hrs
b. 18 hrs
c. 0.75 hrs
d. 16 hrs
3
Unit 4: Chemical Compounds
20. Write the name if given the formula or the formula if given the name.
a. HBr(aq)
n. molybdous acid
___________________________________
b. Cu2C2O4
___________________________________
o. calcium phosphate
___________________________________
c. Cl2O7
___________________________________
p. arsenic triiodide
___________________________________
___________________________________
d. Al(ClO4)3
q. magnesium sulfate heptahydrate
___________________________________
___________________________________
e. Fe(NO3)3 • 9H2O
r.
___________________________________
___________________________________
f.
SO3
___________________________________
g. HNO2 (aq)
___________________________________
h. Pb(Cr2O7)2
___________________________________
i.
N2O5
___________________________________
j.
H3BO2 (aq)
___________________________________
k. SnBr4
___________________________________
l.
Ti(IO)3
____________________________________
m. Ga2(WO3)3
iron(III) carbonate
s. sodium acetate
___________________________________
t.
manganese(IV) telluride
___________________________________
u. scandium arsenite
___________________________________
v. tetraphosphorous decoxide
___________________________________
w. phosphorous acid
___________________________________
x. hydroselenic acid
___________________________________
y. acetic acid
___________________________________
z. platinum(II) perbromate
___________________________________
____________________________________
4
21. Determine the molar mass of chromium(II) phosphite.
22. Determine the percent composition of manganese(VII) arsenate.
23. How many electrons are present in a 20.54 gram sample of calcium ions?
24. What mass of aluminum hypochlorite contain 1.574 x 1023 hypochlorite ions?
25. An unknown gas has an effusion rate that is 0.845 times that of dinitrogen pentoxide. What is the
molar mass of the unknown gas?
26. Determine the relative effusion rate of carbon monoxide and carbon dioxide. Interpret your answer.
5
27. Organic – provide names or structures where applicable.
a.
f.
CH3 Br
CH3
CH3 CH2 CH CH C
CH3
CH3
F
CH CH2 CH3
CH3 C
CH3
CH2
CH CH2 CH C
CH3
CH3 Cl
b.
g.
CH3
CH3 CH2 CH2 C
CH3
CH2 CH CH3
CH3
c.
h.
Br
CH3
CH3
CH2
CH3
CH3 CH CH CH CH CH CH3
Br
CH3 CH2 C
CH
CH CH CH3
Br
CH3
Cl
d. 4-ethyl-2-methyl-1-heptene
i. 3-ethyl-2,6-dimethylheptane
e. 3-ethyl-2-methyl-1-octene
j. 4,4-dimethyl-2-pentyne
6
Unit 5: Mole
28. The following pertains to the compound, potassium hypomolybdite.
a. Calculate the mass of oxygen in potassium hypomolybdite if there are 3.91x1024 formula units.
b. Calculate the total number of ions in 154.3 g of potassium hypomolybdite.
c. Calculate the mass of potassium hypomolybdite needed to make 250. mL of a 0.500 M solution.
29. An unknown gas was collected over water. Determine the molar mass of the unknown gas if a 0.167 g
sample occupies a volume of 69.8 mL at 60.0°C. The barometric pressure is 752.8 torr.
30. An unknown gas is determined to have an empirical formula of CH2. If a 0.176 g sample of this gas
occupies a volume of 35.0 mL at 134 kPa and 175°C, determine its molecular formula.
31. 123g of sucrose is dissolved in 568g of water. The solution has a density of 1.34g/ mL. Determine the
molarity and molality of the solution.
32. A compound is found to be 47.1% carbon, 6.54%H, and 46.4% chlorine. The rate of effusion of this
compound in the gaseous state was measured relative to oxygen gas. Nitrogen was found to effuse at
rate that was 2.34 times faster than this compound. Determine the molecular formula of the compound.
7
Unit 6: Chemical Equations
33. Calculate for the reaction 2Al (s) + 3Cl2 (g) 2AlCl3 (s) from the data.
2Al (s) + 6 HCl (aq) 2 AlCl3 (aq) + 3 H2 (g)
H = -1049.0 kJ
HCl (aq) HCl (g)
H = +74.8 kJ
2 H2 (g) + 2 Cl2 (g)  4 HCl (g)
H = -3690.0 kJ
AlCl3 (s) AlCl3 (aq)





H = -323.0 kJ
34. Using bond energies, calculate the enthalpy change for the following reactions:
35. Using bond energies, calculate molar heat of combustion for 1 mole of methane:
36. Based on the diagram to the right, determine:
a. Endo or Exo? _______________________
b. ΔHforward =
_______________________
c. Eaforward =
_______________________
d. ΔHreverse =
_______________________
e. Eareverse =
_______________________
8
37. Sketch a potential energy curve that is represented by the following values of ΔH and Ea.
 ΔHreverse = -10 kJ
 Eaforward = +40 kJ
 Activated Complex = 50 kJ
 Is this an endothermic or exothermic reaction?
38. Write complete balanced chemical equations. Indicate precipitate for double replacement reactions.
a. Zinc carbonate decomposes.
b. Strontium is mixed with chlorine gas.
c. Combustion of octane.
d. Iron is added to acetic acid.
e. Potassium oxide is mixed with water.
f. Lithium chlorate decomposes.
g. Potassium hydroxide is added to sulfuric acid.
h. Sulfur trioxide is bubbled through water.
i. Zinc is dropped into hydrochloric acid.
j. Decomposition of calcium oxide.
k. Gold metal dropped into sulfurous acid.
l. Silver nitrate is added to ammonium phosphate.
m. Fluorine is added to sodium bromide.
n. Carbonic acid is heated.
9
Unit 7: Stoichiometry
____ 39. Given the reaction of propane burning in air, how many grams of oxygen gas are required to burn 3.01  1023
propane molecules?
a.
b.
c.
d.
e.
80.0 g
40.0 g
160 g
16.0 g
64.0 g
____ 40. A mixture of calcium oxide and calcium carbonate that had a mass of 3.454 g was heated until all
the calcium carbonate was decomposed. After heating, the sample had a mass of 3.102 g. Calculate the mass
of calcium carbonate present in the original sample.
a.
b.
c.
d.
e.
0.400 g
0.800 g
1.00 g
1.60 g
0.200 g
____ 41. The following statements apply to the interpretation of chemical equations. Not all of the statements are true.
Which response includes all of the true statements, and no others?
I.
II.
III.
IV.
V.
a.
b.
c.
d.
e.
The sum of the number of moles of the reactants must equal the sum of the number
of moles of products in a balanced equation.
The sum of the number of grams of the reactants that react must equal the sum of
the number of grams of the products produced by the reaction.
The following equation for the reaction involving hypothetical substances, A, B, C,
and D, implies that the products C and D are always produced in a three to one
mole ratio. A + 2B  3C + D
The equation shown in III implies that in any reaction involving A and B as
reactants, A must be the limiting reactant.
The total number of atoms in the reactants that react must always equal the total
number of atoms in the products produced by the reaction.
I and V
I, II, and III
II, IV, and V
II, III, and V
III, IV, and V
____ 42. The thermite reaction is performed using 8.6 g iron(III) oxide and 1.8 g powdered aluminum metal. Which
reactant is in excess and by how much?
a.
b.
c.
d.
e.
Al, 0.3 g
Fe2O3, 2.0 g
Al, 2.1 g
Al, 1.1 g
Fe2O3, 3.3 g
10
____ 43. The reaction of 5.0 g of fluorine gas with excess chlorine gas produced 5.6 g of chlorine trifluoride. What is the
percent yield of the reaction?
a.
b.
c.
d.
e.
58%
69%
76%
86%
92%
____ 44. Suppose 600. g of phosphorus reacts with 1300. g of sulfur in a synthesis reaction. How many grams of
tetraphosphorus decasulfide can be produced, assuming an 80.0% yield for the reaction
a.
b.
c.
d.
e.
4.62  102 g
1.44  103 g
2.16  103 g
4.92  103 g
6.50  102 g
____ 45. Sulfuric acid is probably the most important industrial chemical because it is used in so many industrial
processes to produce or purify other chemicals. It can be produced by a three step process. First, sulfur is
burned in air to give sulfur dioxide. Second, the sulfur dioxide is converted to sulfur trioxide by passing the
sulfur dioxide over a catalyst in the presence of oxygen at a high temperature. Third, the sulfur trioxide is
reacted with water to form sulfuric acid. What mass of sulfuric acid would be formed from 1.00 x 103 kg of
sulfur, if the three steps gave yields as listed below?
S + O2  SO2
2SO2 + O2  2SO3
SO3 + H2O  H2SO4
92.5%
72.6%
98.2%
a.
b.
c.
d.
e.
____ 46.
a.
b.
c.
d.
e.
____ 47.
4.03  103 kg
2.02  103 kg
3.06  103 kg
2.84  103 kg
2.22  103 kg
What mass of a 25.0% barium nitrate solution contains 40.0 grams of barium nitrate?
117 g
160 g
321 g
10.0 g
62.5 g
If 45.0 mL of 0.250 M lead(IV) chloride solution reacts with 20.0 mL of ammonium sulfate, what is the
molarity of the ammonium sulfate solution?
a.
b.
c.
d.
e.
____ 48.
0.502 M
1.25 M
2.25 M
1.13 M
0.563 M
What mass of calcium carbonate is required to react with 100. mL of a 2.00 M hydrochloric acid solution?
a. 5.00 g
b. 10.0 g
c. 15.0 g
11
d. 20.0 g
e. 23.0 g
____ 49. What volume of 0.150 M silver nitrate solution is required to react with 80.0 mL of 0.0660 M calcium chloride
solution according to the following reaction?
a.
b.
c.
d.
e.
____ 50.
a.
b.
c.
d.
e.
____ 51.
a.
b.
c.
d.
e.
____ 52.
a.
b.
c.
d.
e.
____ 53.
a.
b.
c.
d.
e.
____ 54.
a.
b.
c.
d.
e.
70.4 mL
140 mL
26.8 mL
35.2 mL
60.2 mL
How many grams of calcium hydroxide are contained in 1500. mL of a 0.0250 M calcium hydroxide solution?
3.17 g
2.78 g
1.85 g
2.34 g
3.47 g
What volume of 0.0750 M barium hydroxide will completely react with 125 mL of 0.0350 M hydrochloric
acid?
29.2 mL
42.0 mL
230. mL
536 mL
53.6 mL
What is the molarity of a sulfurous acid solution if 23.7 mL of this solution requires 16.8 mL of 0.296
M sodium hydroxide for titration to its endpoint?
0.210 M
0.358 M
0.105 M
0.421 M
0.0525 M
How much heat is released when 75 g of octane is burned completely?
7200 kJ
8360 kJ
4.1  105 kJ
3600 kJ
5500 kJ
How much heat is evolved in the formation of 35.0 grams of iron(III) oxide from its elements at 25C and 1.00
atm pressure?
90.4 kJ
180.7 kJ
151 kJ
360.1 kJ
243. 9 kJ
Unit 8: Electrons
55. Calculate and determine the type of EMR:
15
a. the energy of a photon with a frequency of 8.77x10 s−1
12
b. the frequency of a photon with an energy of 1.88x10−25 J.
56. Write the shortened configuration and orbital notation for:
a. Silver
57. What is the total number of electrons that will be in p orbitals in 8.31 moles of ground state zinc atoms?
58. In the hydrogen atom, the energy associated with the fifth energy level is −8.72x10−20 J while the energy of the
first energy level is −2.18x10−18 J.
a. Calculate the energy change from n=5 to n=1?
b. Calculate the wavelength of the emitted photon?
_____ 59. Which of the following colors has the highest frequency?
a. blue
b. red
c. violet
d. yellow
_____ 60. Which of the following has the longest wavelength?
a. U.V.
b. I.R.
c. X-ray
d. gamma
Unit 9: Bonding
61. Draw the Lewis dot structure for strontium nitride.
62. By use of electronegativity, identify each of the following bonds as: nonpolar, polar covalent, or ionic.
CH4
H2O
RbI
O2
13
63. How many coordinate covalent bonds are present in 6.93 x 1024 molecules of perchloric acid?
64. Show all possible resonance structures for the carbonate ion.
65. What is the electron geometry, molecular geometry and bond angle for the carbonate ion?
66. Complete the following table using your knowledge of Lewis Structures and VSEPR theory.
Lewis Structure
Structural Formula
(indicate polarity)
electron
geometry
bond
angle
molecular
geometry
CH2Cl2
H2S
14
BF3
NF3
Unit 10: Solutions
____ 67. Consider the three statements below. Which numbered response contains all the statements that are true and no
false statements?
I.
II.
III.
a.
b.
c.
d.
e.
____ 68.
a.
b.
c.
d.
e.
____ 69.
a.
b.
c.
d.
e.
____ 70.
Hydration is a special case of solvation in which the solvent is water.
The oxygen end of water molecules is attracted toward Ca2+ ions.
The hydrogen end of water molecules is attracted toward Cl- ions.
I
II
III
I and II
I, II, and III
Which of the following solutions would not be expected to exist?
NaCl in CCl4 (carbon tetrachloride, a nonpolar solvent)
NaCl in water
Pentane, C5H12, in CCl4
Methyl alcohol, CH3OH, in water
Vegetable oil in mineral oil
The molality of a solution is
the mass of solute divided by the kilograms of solvent.
The moles of solute divided by the liters of solvent.
the moles of solute divided by the kilograms of solvent.
the mass of solute divided by the liters of solution.
the moles of solute divided by the liters of solution.
Calculate the molality of a solution that contains 25 g of H2SO4 dissolved in 80. g of H2O.
15
a. 1.6 m
b. 2.2 m
c. 3.2 m
d. 6.3 m
e. 7.0 m
____ 71 Calculate the molality of a 10.0% phosphoric acid solution in water.
a. 0.380 m
b. 0.760 m
c. 1.13 m
d. 1.51 m
e. 1.89 m
____ 72. What mass of water must be used to dissolve 20.0 grams of ethanol, C2H5OH, to prepare a 0.0500 molal
solution of ethanol?
a. 3.76 kg
b. 4.00 kg
c. 8.70 kg
d. 6.35 kg
e. 7.18 kg
____ 73. Which aqueous solution would have the lowest vapor pressure at 25 C?
a. 1 M NaCl
b. 1 M Na3PO4
c. 1M sucrose, C12H10O11
d. 1 M MgCl2
e. 1 M glucose, C6H12O6
____ 74.
a.
b.
c.
d.
e.
____ 75.
a.
b.
c.
d.
e.
____ 76.
a.
b.
c.
d.
e.
____ 77.
a.
b.
c.
Which of these aqueous solutions would be expected to have the highest boiling point?
0.100 m calcium chloride
0.200 m sodium hydroxide
0.050 m potassium sulfate
0.050 m aluminum sulfate
0.200 m glucose
If 4.27 grams of sucrose, C12H22O11, are dissolved in 15.2 grams of water, what will be the boiling point of the
resulting solution?
101.64C
100.42C
99.626C
100.73C
101.42C
Calculate the boiling point of a solution prepared by dissolving 70.0 g of naphthalene, C10H8 (a nonvolatile
nonelectrolyte), in 220.0 g of benzene, C6H6. The Kb for benzene = 2.53C/m. The boiling point of pure
benzene is 80.1C.
87.8C
73.8C
83.2C
86.4C
106.3C
Calculate the freezing point of a solution that contains 68.4 g of sucrose in 300. g of water.
- 0.186C
- 0.372C
- 0.558C
16
d.
e.
____ 78.
a.
b.
c.
d.
e.
____ 79.
a.
b.
c.
d.
e.
____ 80.
____
____
____
____
____
a.
b.
c.
d.
e.
81.
a.
b.
c.
d.
e.
82.
a.
b.
c.
d.
e.
83.
a.
b.
c.
d.
e.
84.
a.
b.
c.
d.
e.
85.
a.
b.
c.
d.
- 0.744C
-1.24C
Which of the following statements regarding a 1 M sucrose solution is not correct?
The boiling point is greater than 100C.
The freezing point is less than that of a 1 M NaCl solution.
The freezing point is less than 0.0C.
The boiling point is less than that of a 1 M NaCl solution.
The vapor pressure at 100C is less than 760 torr.
A 4.305-gram sample of a nonelectrolyte is dissolved in 105 grams of water. The solution freezes at -1.23C.
Calculate the molecular weight of the solute.
39.7 g/mol
58.4 g/mol
46.2 g/mol
62.0 g/mol
74.2 g/mol
When 35.0 g of an unknown nonelectrolyte is dissolved in 220.0 g of benzene, the solution boils at 83.2C.
Calculate the molecular weight of the unknown nonelectrolyte. The Kb for benzene = 2.53C/m. The boiling
point of pure benzene is 80.1C.
130 g/mol
20.3 g/mol
183 g/mol
156 g/mol
194 g/mol
The following describe properties of substances. Which one is not a property of acids?
They have a sour taste.
They react with metal oxides to form salts and water.
They react with other acids to form salts and water.
Their aqueous solutions conduct an electric current.
They react with active metals to liberate H2.
Which of the following is not a common property of aqueous solutions of most bases?
They have a bitter taste.
They have a slippery feeling.
They change the colors of many indicators.
They react with protonic acids to form salts and stronger bases.
Their aqueous solutions conduct an electric current.
According to the Arrhenius theory, which of the following is an acid?
NH3
CH4
HCl
H2
NaOH
According to the Brønsted-Lowry theory, a base is defined as __________.
an electron pair acceptor
a proton acceptor
an electron pair donor
a proton donor
any species that can produce hydroxide ions in aqueous solution
A Brønsted-Lowry acid is defined as a __________.
species that donates a proton
species that accepts a proton
species that accepts a share in an electron pair
species that makes available a share in an electron pair
17
e.
____ 86.
a.
b.
c.
d.
e.
____ 87.
a.
b.
c.
d.
e.
____ 88.
species that produces hydroxide ions in aqueous solution
Which of the following can be a Brønsted-Lowry acid?
AlCl3
CH4
NaOH
H2O
H2
Which one of the following species could not react as a Brønsted-Lowry acid?
HCl
H2O
CaO
NH3
CH3COOH
In the equation
HF + H2O
a.
b.
c.
d.
e.
____ 89.
a.
b.
c.
d.
e.
H3O+ + F-
H2O is a base, and HF is its conjugate acid.
H2O is an acid, and HF is the conjugate base.
HF is an acid, and F- is its conjugate base.
HF is a base, and H3O+ is its conjugate acid.
HF is a base, and F- is its conjugate acid.
Which of the following does not represent a conjugate acid-base pair?
H2O/OHH3O+/OHHCl/ClHNO3/NO3NH4+/NH3
____ 90. Write the net ionic equation for the complete neutralization of HBr by Ca(OH)2. Use H+ rather than H3O+.
What is the sum of the coefficients?
a. 6
b. 8
c. 3
d. 4
e. 5
____ 91. Which of the following reactions is the net ionic equation for the acid-base reaction between H2CO3 and
Sr(OH)2?
a. H2CO3 + Sr2+ + 2 OH-  SrCO3 + 2 H2O
b. H3O+ + OH-  2 H2O
c. 2 H3O+ + Sr2+ + 2 OH-  Sr2++ 4 H2O
d. H2CO3 + 2 OH-  2 H2O+ CO32e. H2CO3 + Sr(OH)2 2H2O+ Sr2+ + CO32____ 92. The molar concentration of the Ca2+ ion is __________ and the molar concentration of OH- ion is __________
in 0.015 M calcium hydroxide.
a. 0.015 M; 0.015 M
b. 0.015 M; 0.030 M
c. 0.030 M; 0.015 M
d. 0.030 M; 0.030 M
e. not enough information to calculate
18
____ 93. A solution having a pH of 1.4 would be described as __________.
a. distinctly basic
b. slightly basic
c. neutral
d. slightly acidic
e. distinctly acidic
____ 94. Calculate the pH of a solution that has the H3O+ concentration of 0.50 M.
a. - 0.30
b. 13.70
c. 0.30
d. 7.30
e. 0.50
____ 95. Calculate the pH of a solution in which [OH-] = 2.50  10-4 M.
a. 0.40
b. 3.60
c. -3.60
d. 10.40
e. 13.60
____ 96. What is the concentration of H3O+ ions in a solution in which pH = 4.32?
a. 4.8  10-5 M
b. 6.2  10-4 M
c. 5.1  10-4 M
d. 8.6  10-5 M
e. 3.5  10-4 M
____ 97. What is the pH of a 0.400 M nitric acid solution?
a. 0.40
b. 2.05
c. 0.60
d. 4.12
e. 1.67
____ 98.
a.
b.
c.
d.
e.
____ 99.
What is the pH of 500. mL of solution containing 0.0124 gram of calcium hydroxide?
2.96
3.17
9.68
10.83
11.04
Concentrated hydrochloric acid is about 12.1 M. What volume of concentrated HCl is required to produce
5500 mL of 0.250 M?
a. 980 mL
b. 0.114 L
c. 98 mL
d. 0.211 L
e. 1114 mL
____ 100. A laboratory stock solution is 1.50 M sodium hydroxide. Calculate the volume of this stock solution that
would be needed to prepare 300. mL of 0.200 M sodium hydroxide.
a. 2.25 mL
b. 10.0 mL
c. 40.0 mL
d. 1.00 mL
e. 0.100 mL
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____ 101. When a solution is diluted, what is the relationship of the number of moles of solute in the more concentrated
initial volume of solution to the number of moles of solute in the less concentrated final volume of solution?
a. The ratio of the numbers is directly proportional to the two volumes.
b. The ratio of the numbers is inversely proportional to the two volumes.
c. The number of moles of solute in the more concentrated initial volume is always greater.
d. The number of moles of solute in the less concentrated final volume is always greater.
e. The number of moles of solute in both solutions is the same.
____ 102. Calculate the molarity of the resulting solution if 25.0 mL of 2.40 M sulfuric acid solution is
diluted to 300. mL.
a. 0.200 M
b. 29.0 M
c. 2.00 M
d. 0.400 M
e. 0.0400 M
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