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WorksheetsPeriod 9 Chem Final Review
Total questions: 164
Worksheet time: 15hrs 14mins
Name
Class
Date
1.
All matter is composed of atoms
a)
True
b)
False
2.
Pure substances consist of:
a)
Elements
b)
Compounds
c)
Elements and Compounds
d)
Mixtures
3.
Elements can be composed of two or more types of atoms
a)
True
b)
False
4.
Compounds are 2 or more elements held together by:
a)
Chemical Bonds
b)
Physical Bonds
c)
Nuclear Fusion
d)
Nuclear Fission
5.
A mixture can be:
a)
Heterogeneous
b)
Homogeneous
c)
Both
d)
Neither
6.
Mass is the measure of Earth's gravitational pull on an object
a)
True
b)
False
7.
Salt dissolving in water is an example of a:
a)
Matter Change
b)
Chemical Change
c)
Dissolvation Change
d)
Physical Change
8.
What is not a sign of a chemical change?
a)
Burning
b)
Production of Sound
c)
State of Matter Change
d)
Formation of a Gas
9.
When salt dissolves in water, water is the solvent
a)
True
b)
False
10.
What is not an example of how to separate a mixture?
a)
Chromatography
b)
Centrifugation
c)
Diluting
d)
Distillation
11.
Kinetic energy is energy of...?
a)
Stored energy
b)
Motion
c)
gas
d)
atoms
12.
Chemicals and mechanical energy are forms of potential energy.
a)
True
b)
False
13.
What is accuracy?
a)
A measurement
b)
How close a value is to the actual value
c)
How close a set of values are to one another
14.
Precision is how close a set of values are to one another.
a)
True
b)
False
15.
The mass of an object if 1.345 grams. What is the limitation?
a)
+/- .01
b)
+/- .1
c)
none of the above
d)
+/- .001
16.
Non-zero digits are...?
a)
Significant
b)
non-significant
17.
Captive zeros between sig figs are...?
a)
Non-significant
b)
Significant
18.
Trailing zeros to the right of a sig fig and a decimal place?
a)
Non-significant
b)
Significant
19.
All leading zeros are...?
a)
Non-significant
b)
Significant
20.
Zeros to the right of a number before the decimals are...?
a)
Significant
b)
Non-significant
21.
22.05 + 16.1 =
a)
39
b)
38.15
c)
38.2
d)
46
22.
6.1 x 10 4 x 4.45 x 107 =
a)
3 x 1011
b)
2.7 x 10 14
c)
2.7 x 10 12
d)
2.714 x 1012
23.
128.6 - 2.3468 =
a)
126.2532
b)
126.3
c)
127
d)
130.0
24.
404 / 32.0
a)
12.6
b)
13.0
c)
14.5
d)
12.6250
25.
Which Scientist discovered the Electron and what did they use?
a)
Thomson & Cathode Ray Tube
b)
Rutherford & Gold Foil
c)
Bohr & Emission Spectrum of Hydrogen
d)
Thomson & Plum Pludding
26.
Atoms can be subdivided
a)
True
b)
False
27.
What did the Plum Pudding Model propose?
a)
Model of the atom
b)
Model of a Nucleus
c)
Fired tiny positively charged alpha particles
d)
Electrons orbit nucleus
28.
What did Rutherford conclude about the Gold Foil Experiment?
a)
Atoms can be negatively or positively charged
b)
Atoms have a Nucleus
c)
Atom is made with smaller particles
d)
Atoms are electrically neutral
29.
Who proposed the Invisible unit of an element is an atom?
a)
Thomson
b)
Bohr
c)
Rutherford
d)
Dalton
30.
What is the electron configuration for Sulfur?
a)
1s2 2s1 3s1 3p6
b)
1s2 2s2 2p6 3s1 3p6
c)
1s2 2s2 2p6 3s1
d)
1s2 2s2 2p6 3s2 3p4
31.
What is wavelength?
a)
distance between the crests of a wave
b)
Form of energy
c)
Distance between the atoms
d)
Number of waves that pass a point during a certain time period
32.
What is the lowest energy state of an e-?
a)
Light State
b)
Ground State
c)
Excited State
d)
Unstable State
33.
What is Electromagnetic Radiation?
a)
Form of energy that is produced by oscillating electric and magnetic disturbance
b)
Energy given off
c)
Arrange of electrons in a atom
d)
Form of energy that is produced through atoms
34.
Where is the proton located?
a)
Electron
b)
Electron Cloud
c)
Nucleus
d)
Neutron
35.
What is the nucleus made of?
a)
Protons and Neutrons
b)
Nothing
c)
Protons and Electrons
d)
Neutrons and Electrons
36.
What is the first group of the periodic table?
a)
Alkali metals
b)
alkaline earth metals
c)
transition metals
d)
halogens
37.
What is the second group on the periodic table?
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
halogens
38.
Groups 3-12 of the periodic table are the ...?
a)
Alkali metals
b)
Alkaline earth metals
c)
transition metals
d)
halogens
39.
Elements #57-70 are classified as the...?
a)
Lanthanide metals
b)
actinide metals
c)
transition metals
40.
Elements #89-102 are classified as the?
a)
lanthanide series
b)
actinide series
c)
transition metals
41.
The metals group of the periodic table include what?
a)
alkali metals, alkaline earth metals, transition metals, and the lanthanide and actinide series
b)
alkali metals, alkaline earth metals, and transition metals
c)
lanthanide series and actinide series
d)
transition metals
42.
What are located on the step-line of the periodic table?
a)
metalloids
b)
halogens
c)
noble gasses
43.
what are the nonmetals?
a)
halogens
b)
noble gasses
c)
halogens and noble gasses
44.
what is group 17 on the periodic table?
a)
metalloids
b)
halogens
c)
noble gasses
45.
what is group 18 on the periodic table?
a)
halogens
b)
metalloids
c)
noble gasses
46.
what are the horizontal rows on the periodic table called? (#1-7)
a)
periods
b)
groups
c)
slots
47.
what are the vertical columns of the periodic table called? (#1-18)
a)
periods
b)
groups
c)
slots
48.
the main group elements are in the?
a)
s and p blocks
b)
D block
c)
F block
49.
the transition metals are in the...?
a)
s and p blocks
b)
D blocks
c)
F block
50.
The lanthanide/actinide series are in the...?
a)
s and p block
b)
D block
c)
F block
51.
what element is considered its own group?
a)
hydrogen
b)
helium
52.
What did John Newlands do?
a)
Nothing
b)
Made the periodic table
c)
Arranged elements in order of atomic mass (Not in table form yet..) Properties repeated every 8th element
d)
Rearranged elements by increasing atomic number
53.
What did Dimitri Mendeleev do?
a)
Arranged elements by increasing atomic mass and grouped elements with similar properties together.
b)
Discovered the neutron
c)
made the periodic law
d)
Created atomic number
54.
What is the periodic law?
a)
Explained natural and synthetic elements
b)
Nuclear chemistry
c)
Chemical & physical properties of elements are functions of their atomic number
d)
Not sure
55.
What causes nuclear fusion?
a)
energy
b)
The fusion of two nuclei lighter than iron or nickel generally releases energy while the fusion of nuclei heavier than iron or nickel absorbs energy
c)
nuclei being absorbed
56.
What happens in the process of nuclear fusion?
a)
3 hydrogen nuclei combine to form 2 helium atoms
b)
3 helium atoms combine to make 7 hydrogen nuclei
c)
4 hydrogen nuclei combine to form 1 helium atom
57.
What is the fusion reaction
a)
Nuclear fusion is a process where 2 or more nuclei combine to form an element wit a higher atomic number
b)
The number of protons = the same number of electrons
c)
Nuclear fusion is a process where 2 or more nuclei combine to form an element with a higher atomic
58.
What did Henry Moseley do?
a)
Rearranged elements by increasing atomic number
b)
Rearranged elements by increasing atomic weight
59.
What is fission?
a)
The act of dividing or splitting something into two or more parts
b)
making something come together/fuse together
c)
both orange and red
d)
not sure
60.
What is fusion?
a)
Do not remember
b)
atoms coming together to make one
c)
neutrons combining
d)
The process of joining two or more things together to form a single entity
61.
Who is "the father of the periodic table"?
a)
John Newlands
b)
Neil Bohr
c)
Dmitri Mendeleev
d)
Henry Moseley
62.
What are the four major periodic trends?
a)
Electronegativity, Ionization Energy, Atomic Radius, Electron Affinity
b)
s block, d block, p block, f block
c)
gases, liquids, solids, aqueous solutions
d)
alkali metals, halogens, transition metals, noble gases
63.
What is Atomic Radius? How is it measured?
a)
a measure of the size of an atom- measured by using a ruler
b)
a measure of the size of its atoms- measured from center of atom out to boundary of electron cloud.
64.
What does electronegativity mean?
a)
the energy required to remove an electron from a gaseous atom or ion.
b)
The amount of pull an atom has on other atoms
c)
A measure of the tendency of an atom to attract a bonding pair of electrons.
d)
How much energy it takes to attract other electrons
65.
What is ionization Energy?
a)
the energy required to remove an electron from a gaseous atom or ion.
b)
A measure of the tendency of an atom to attract a bonding pair of electrons.
66.
Does electron affinity increase or decrease from left to right on the periodic table? Top to bottom?
a)
increases- decreases
b)
decreases- increases
67.
Ionization energy increases when moving left to right on the periodic table and decreases when going from top to bottom.
a)
true
b)
false
68.
What is electron affinity?
a)
The energy required to remove an electron from a gaseous atom or ion.
b)
The amount of energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion.
69.
Does electronegativity increases as moving left to right on the periodic table? Top to bottom?
a)
increases- decreases
b)
decreases- decreases
70.
Does Atomic radius increase or decrease as moving left to right on the periodic table? Top to bottom?
a)
decreases- increases
b)
increases- decreases
c)
increases- decreases
d)
none of the above
71.
How is an ion the same as its parent ion?
a)
nothing is the same
b)
atom and ion have same # of protons and neutrons
c)
nucleus changes
d)
same #of electrons
72.
What is the charge on a Hydrogen ion?
a)
+1
b)
1
c)
2
73.
What is the formula of calcium oxide?
a)
CaO2
b)
CaO
c)
Ca2O
d)
CO
74.
which types of elements become cations?
a)
nonmetals
b)
all metals
c)
only transition metals
d)
some metals and some metalloids
75.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
76.
What is the formula for aluminum sulfide?
a)
Al2S3
b)
Al3S2
c)
Al2SO4
d)
AlS
77.
What is the formula for lithium cyanide?
a)
Li2CN
b)
LiCN2
c)
LiC2N
d)
LiCN
78.
What is the formula for chromium III bromide?
a)
Cr3Br
b)
CrBr3
c)
CrBr
d)
Cr3Br3
79.
LiBr is called
a)
lithium bromine
b)
lithium (I) bromine
c)
lithium bromide
d)
lithuim (I) bromide
80.
How is an ion different from its parent atom
a)
nothing is different
b)
different # of protons
c)
different # of electrons
81.
What is an attractive force between molecules?
a)
Intermolecular force
b)
ion-ion force
c)
dipole-dipole force
d)
Dispersion force
82.
If the ED range is greater than 2.1 what kind of bond is it?
a)
polar covalent bond
b)
ionic bond
c)
nonpolar covalent bond
d)
hydrogen bond
83.
Ionic bonding involves the transfer of electrons
a)
True
b)
False
84.
what is an intermolecular force?
a)
attractive forces between atoms
b)
attractive forces between bonds
c)
attractive forces between compounds
d)
attractive forces between molecules
85.
what happens during nonpolar covalent bonding?
a)
Electrons are shared unequally between atoms
b)
Involves the transfer of electrons
c)
molecules form compounds
d)
Electrons are shared equally between atoms
86.
what is the ED range for a polar covalent bond?
a)
ED > 2.1
b)
ED = 0.51-2.1
c)
ED = 0-0.5
d)
ED < 0
87.
What type of covalent bond is formed when one of the atoms provides both of the electrons in a shared pair
a)
Coordinate Covalent Bond
b)
Nonpolar Covalent Bonding
c)
Polar Covalent Bonding
d)
All of them
88.
A repeating pattern of ions is?
a)
Electronegativity
b)
Ion-Ion Forces
c)
Crystal Lattice
d)
Dipole-Dipole Forces
89.
A molecule that has a partial positive charge and a partial negative charge is a dipole molecule
a)
True
b)
False
90.
Hydrogen bonding occurs when electrons are shared unequally between atoms
a)
True
b)
False
91.
What kind of chemical reaction is this:
2H₂O --> 2H₂ + O₂
2H₂O --> 2H₂ + O₂
a)
synthesis reaction
b)
decomposition reaction
c)
combustion reaction
d)
single displacement reaction
92.
What kind of chemical reaction is this:
8Fe + S₈ --> 8FeS
8Fe + S₈ --> 8FeS
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
combustion reaction
d)
single displacement reaction
93.
What kind of chemical reaction is this:
AgNO₃ + NaCl → AgCl + NaNO₃
AgNO₃ + NaCl → AgCl + NaNO₃
a)
synthesis reaction
b)
combustion reaction
c)
double displacement reaction
d)
single displacement reaction
94.
What kind of chemical reaction is this:
Zn + H₂SO₄ → ZnSO₄ + H₂
Zn + H₂SO₄ → ZnSO₄ + H₂
a)
Decomposition reaction
b)
single displacement reaction
c)
synthesis reaction
d)
double displacement reaction
95.
What kind of chemical reaction is this:
2 H₂ + O₂ → 2 H₂O
2 H₂ + O₂ → 2 H₂O
a)
decomposition reaction
b)
synthesis reaction
c)
combustion reaction
d)
single displacement reaction
96.
What kind of chemical reaction is this:
CH₄ + 2 O₂ → CO₂ + 2 H₂O
CH₄ + 2 O₂ → CO₂ + 2 H₂O
a)
Combustion reaction
b)
double displacement reaction
c)
synthesis reaction
d)
single displacement reaction
97.
What kind of chemical reaction is this:
2 Fe + 6 NaBr → 2 FeBr₃ + 6 Na
2 Fe + 6 NaBr → 2 FeBr₃ + 6 Na
a)
single displacement reaction
b)
double displacement reaction
c)
synthesis reaction
d)
decomposition reaction
98.
What kind of chemical reaction is this:
Pb + O₂ --> PbO₂
Pb + O₂ --> PbO₂
a)
synthesis reaction
b)
decomposition reaction
c)
combustion reaction
d)
single displacement reaction
99.
What kind of chemical reaction is this:
2CO + O₂ --> 2CO₂
2CO + O₂ --> 2CO₂
a)
synthesis reaction
b)
decomposition reaction
c)
combustion reaction
d)
displacement reaction
100.
What kind of chemical reaction is this:
Ca(OH)₂ + H₂SO₄ --> CaSO₄ + 2H₂O
Ca(OH)₂ + H₂SO₄ --> CaSO₄ + 2H₂O
a)
double displacement reaction
b)
single displacement reaction
c)
combustion reaction
d)
synthesis reaction
101.
What is the volume of a mole of hydrogen at STP?
a)
41.02 L
b)
20.21 L
c)
1.01 L
d)
22.41 L
102.
What amount of H2O is produced when 3.51g of C2H6 reacts with an excess of O2?
_ C2H6 + _ O2 -> _ CO2 + _ H2O
_ C2H6 + _ O2 -> _ CO2 + _ H2O
a)
6.308g
b)
13.78g
c)
6.31g
d)
13.709g
103.
If 63.1 L of methanol is burned at STP, what volume of H2O will be produced?
_ CH3OH + _ O2 -> _ CO2 + _ H2O
_ CH3OH + _ O2 -> _ CO2 + _ H2O
a)
126 L
b)
48.2 L
c)
5.63 L
d)
24.7 L
104.
What volume of H3PO4 forms when 4 L of POCl3 reacts? The density of POCl3 is 1.67 g/mL and the density of H3PO4 is 1.83 g/mL.
a)
2333.2 L
b)
2 L
c)
2000 L
d)
2.33 L
105.
How many molecules of HCl will react with 41.34g of Ca?
_ Ca + _ HCl -> _ CaCl2 + _ H2
_ Ca + _ HCl -> _ CaCl2 + _ H2
a)
1.242 x 1023 molecules
b)
2.342 x 1024 molecules
c)
2.342 x 1023 molecules
d)
1.242 x 1024 molecules
106.
A reaction had a theoretical yield of 30.0g of KCl. Only 27.8g of KCl formed. What is the percent yield of this reaction?
a)
92.7%
b)
.927%
c)
93%
d)
92.66%
107.
3.98g of FeO and 2.47g of CuCl were used in this reaction. What is the limiting reactant and the excess reactant? What is the theoretical yield of FeCl2?
_ FeO + _ CuCl -> _ FeCl2 + _ Cu2O
_ FeO + _ CuCl -> _ FeCl2 + _ Cu2O
a)
ER = FeO
LR = CuCl
TY = 1.60g FeCl2
LR = CuCl
TY = 1.60g FeCl2
b)
ER = CuCl
LR = FeO
TY = 1.58g FeCl2
LR = FeO
TY = 1.58g FeCl2
c)
ER = CuCl
LR = FeO
TY = 1.55g FeCl2
LR = FeO
TY = 1.55g FeCl2
d)
ER = FeO
LR = CuCl
TY = 1.58g FeCl2
LR = CuCl
TY = 1.58g FeCl2
108.
If 52.3g of HCl and 97.2g of KOH were used with an excess of KOH, what amount of the excess reactant is left over?
a)
16.7g KOH
b)
16.78g KOH
c)
17.0g KOH
d)
16.8g KOH
109.
Once the excess reactant runs out, the reaction stops.
a)
True
b)
False
110.
This reactant produces the smallest amount of product.
a)
Limiting Reactant
b)
Excess Reactant
111.
The actual yield tends to be less than the theoretical yield.
a)
True
b)
False
112.
Which formula is associated with the ideal gas law?
a)
d=m/v
b)
PV=nRT
c)
PE=mgh
d)
E=hv
113.
Which law combines the laws of Boyle, Charles, and Lussac?
a)
Ideal Gas Law
b)
Dalton's Gas Law
c)
Combined Gas Law
d)
Charles Law
114.
When converting temperature from Celsius to Kelvin add 283.
a)
True
b)
False
115.
What is the formula for Dalton's Law?
a)
PTotal=P1+P2+...Pn
b)
P1T2=P2T1
c)
PV=nRT
d)
None of the above
116.
What two things in Lussacs law have a relationship?
a)
Volume and Temperature
b)
Pressure and Volume
c)
Pressure and Temperature
d)
Moles and Pressure
117.
Charles law is the relationship between temperature and volume?
a)
True
b)
False
118.
Pressure is _______ proportional to volume in Boyle's law.
a)
Inversely
b)
Directly
c)
Not
119.
At STP what is 1 mole equal to?
a)
22.41L
b)
397.8L
c)
2222.22L
d)
21.81L
120.
What is the greenhouse effect?
a)
Heat from the sun being trapped within the atmosphere.
b)
Plants growing because of heat trapped in a greenhouse.
c)
Paint on the side of a building fading to a light green color.
d)
Heat from the moon becoming trapped in a house.
121.
In a heating curve the transfer of heat does not always result in a temperature increase.
a)
True
b)
False
122.
A _______ is dissolved in a ___________ to produce a __________.
a)
solute, solvent, solution
b)
miscible, immiscible, solution
c)
liquid, air, solid
d)
proton, neutron, atom
123.
A solution is prepared by dissolving 29.98 grams of ammonium dichromate, (NH4)2Cr2O7 in water and diluting it to 400.0mL. What is the molarity?
a)
1.9876 M (NH4)2Cr2O7
b)
.295 M (NH4)2Cr2O7
c)
.2975 M (NH4)2Cr2O7
d)
74.95 M (NH4)2Cr2O7
124.
Vinegar contains 5.0 grams of acetic acid, CH3COOH, in 100.0 mL of solution. Calculate the molarity of acetic acid in vinegar.
a)
.0895 M CH3COOH
b)
23.88 M CH3COOH
c)
.00083 M CH3COOH
d)
.83 M CH3COOH
125.
A homogeneous mixture is uniform throughout and all particles are evenly dispersed.
a)
True
b)
False
126.
The Molarity formula is :
M= Moles of solute/ Liters of solution
M= Moles of solute/ Liters of solution
a)
True
b)
False
127.
The amount of a substance in a given quantity of solution is a ___________.
a)
Solution
b)
Concentration
c)
Solvent
d)
Base
128.
What is a solution that contains less solute than a saturated solution and is able to dissolve additional solute?
a)
monounsaturated solution
b)
supersaturated solution
c)
saturated solution
d)
unsaturated solution
129.
What solution cannot dissolve any more solute under the given conditions?
a)
monounsaturated solution
b)
supersaturated solution
c)
saturated solution
d)
unsaturated solution
130.
What solution holds more dissolved solute than what is required to reach equilibrium at a given temperature?
a)
monounsaturated solution
b)
supersaturated solution
c)
saturated solution
d)
unsaturated solution
131.
What are the steps in making a solution?
a)
1. get a graduated cylinder and fill with 20 mL of water
2. add solute
3. stir with stirring rod
2. add solute
3. stir with stirring rod
b)
1. measure out solute
2. place solute in a beaker
3. add tap water to the top of beaker
4. stir with a stirring rod
2. place solute in a beaker
3. add tap water to the top of beaker
4. stir with a stirring rod
c)
1. find and measure out mass of solute needed
2. place solute into volumetric flask of desired volume
3. add distilled water to fill line
4. put cap on flask and shake to mix
2. place solute into volumetric flask of desired volume
3. add distilled water to fill line
4. put cap on flask and shake to mix
d)
1. find and measure out mass of solute needed
2.place solute into a weighing dish
3. add tap water and stir
2.place solute into a weighing dish
3. add tap water and stir
132.
A solution of AgNO3 contains 29.66 grams of solute in 100.0 mL of solution. What is the molarity of the solution?
a)
.1746 M AgNO3
b)
2.34 M AgNO3
c)
1.746 M AgNO3
d)
1.666 M AgNO3
133.
Equilibrium is when the rate of the forward reaction is the same as the rate of the reverse reaction.
a)
True
b)
False
134.
What does it mean to be a reverse reaction?
a)
The reaction goes backward
b)
The products can make reactants and the reactants can make products
c)
The reaction goes forward
d)
The reaction does not occur
135.
LeChatelier's Principle is if a system at equilibrium is subjected to a stress, the equilibrium will shift to minimize the effects of the stress.
a)
False
b)
True
136.
The following reaction is in equilibrium:
2SO2(g) + O2(g) ↔ 2SO3(g)
What will the result be of an increase of pressure
2SO2(g) + O2(g) ↔ 2SO3(g)
What will the result be of an increase of pressure
a)
Forward reaction favored
b)
Shift right
c)
Products favored
d)
All of the above
137.
The following reaction is in equilibrium:
H2 + I2 ↔ 2HI
Which way will the reaction shift if HI is added to the reaction
H2 + I2 ↔ 2HI
Which way will the reaction shift if HI is added to the reaction
a)
Reverse reaction is favored
b)
Forward reaction is favored
138.
Reverse reaction is favored, is the same as:
a)
Shift left
b)
Shift right
c)
Products favored
d)
None
139.
The following reaction is in equilibrium:
PCl3 + Cl2 ↔ PCl5
What effect will an increase of Cl2 have on PCl3?
PCl3 + Cl2 ↔ PCl5
What effect will an increase of Cl2 have on PCl3?
a)
Decrease
b)
Increase
140.
The following is in equilibrium:
4HCl + O2 ↔ 2H2O + 2Cl2 + heat
Which direction will this reaction shift if heat is added.
4HCl + O2 ↔ 2H2O + 2Cl2 + heat
Which direction will this reaction shift if heat is added.
a)
Shift right
b)
Shift left
141.
What is Keq?
a)
Equilibrium constant
b)
Pressure constant
c)
Temperature constant
d)
Time constant
142.
2NO2(g) ↔ N2O4(g)
What is the equilibrium constant expression for this equation?
What is the equilibrium constant expression for this equation?
a)
[N2O4]/[NO2]2
b)
[NO2]2/[N2O4]
143.
What substances are kept out of equilibrium constant expressions?
a)
Solids
b)
Aqueous
c)
Gases
d)
None of the above
144.
CaCO3(s) ↔ CaO(s) + O2(g)
Choose the correct equilibrium constant expression for the given equilibrium reaction.
Choose the correct equilibrium constant expression for the given equilibrium reaction.
a)
[O2]
b)
[CaO]x[O2]/[CaCO3]
c)
[CaCO3]/[CaO]x[O2]
d)
None of the above
145.
If Keq equals 3 x 10-3 then which side is favored?
a)
Reactants
b)
Products
c)
None
d)
Both
146.
HCl + OH- ↔ Cl- + H2O
Which substance is the acid?
Which substance is the acid?
a)
HCl
b)
OH-
c)
Cl-
d)
H2O
147.
HCl + OH- ↔ Cl- + H2O
Which substance is the base?
Which substance is the base?
a)
HCl
b)
OH-
c)
Cl-
d)
H2O
148.
HCl + OH- ↔ Cl- + H2O
Which substance is the conjugate base?
Which substance is the conjugate base?
a)
HCl
b)
OH-
c)
Cl-
d)
H2O
149.
HCl + OH- ↔ Cl- + H2O
Which substance is the conjugate acid?
Which substance is the conjugate acid?
a)
HCl
b)
OH-
c)
Cl-
d)
H2O
150.
Whose definition of an acid is "release H+ ions in aqueous solutions?
a)
Bronsted-Lowry
b)
Arrhenius
c)
Lewis
d)
None of the above
151.
Whose definition of a base is "substance that donates an e- pair"
a)
Bronsted-Lowry
b)
Arrhenius
c)
Lewis
d)
None of the above
152.
Whose definition of an acid is "donates a proton to another substance"
a)
Bronsted-Lowry
b)
Arrhenius
c)
Lewis
d)
None of the above
153.
A substance with a pH of 9 is a(n):
a)
Acid
b)
Base
c)
Neutral
d)
None of the above
154.
A substance with a pH of 16 is a(n):
a)
Acid
b)
Base
c)
Neutral
d)
None of the above
155.
A substance with a pH of 2 is a(n)
a)
Acid
b)
Base
c)
Neutral
d)
None of the above
156.
If the hydronium ion concentration of a solution is 1.63 x 10-8 M, what is the hydroxide concentration?
a)
6.13 x 10-7
b)
6.13 x 10-9
c)
6.13 x 10-4
d)
6.13 x 10-6
157.
The hydronium ion concentration in a solution is 1.87 x 10-3 mol/L. What is [OH-]?
a)
5.35 x 10-12
b)
6.35 x 10-12
c)
5.35 x 10-3
d)
6.35 x 10-3
158.
How much HCl would you need to dissolve in 1.0L of water so that [OH-] = 6.0 x 10-12 M?
a)
1.7 x 10-3 moles
b)
1.7 x 10-5 moles
c)
7.1 x 10-3 moles
d)
7.1 x 10-5 moles
159.
What is the pH of a 0.15M solution of HClO4, a strong acid?
a)
0.82
b)
0.28
c)
8.2
d)
2.8
160.
Calculate the pH of a 0.0316 M solution of the strong base RbOH.
a)
3.16 x 10-13
b)
6.13 x 10-4
c)
12.5
d)
8.5
161.
A solution has a hydronium ion concentration of 1.0 x 10-9 M. What is its pH?
a)
8.0
b)
9.0
c)
10.0
d)
11.0
162.
What is the hydronium ion concentration of a weak acid with a pH of 4.7?
a)
[2.0x10-5]
b)
[3.11x105]
c)
[2.23x10-6]
d)
[1.1x107]
163.
What is the hydroxide ion concentration in a solution of pH 8.72?
a)
[4.32x10-7]
b)
[5.00x10-6]
c)
[6.98x10-8]
d)
[3.47x108]
164.
The pH of a solution is 9.5. What is [H3O+]?
What is [OH-]?
What is [OH-]?
a)
[4.4x10-6] and [4.5x106]
b)
[2.3x102] and [6.7x10-3]
c)
[3.2x10-10] and [3.1x10-5]
d)
[5.2x102] and [7.5x10-2]
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