Unit 6 Study Guide
6.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
Al + Fe3O4  Al2O3 + Fe
A) 1
B) 3
C) 6
D) 9
E) 12
1.
All of the following are clues that a chemical reaction
has taken place except
A) A color change occurs.
B) A solid forms.
C) The reactant is smaller.
D) Bubbles form.
E) A flame occurs.
2.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
Sn + NaOH  Na2SnO2 + H2
A) 1
B) 2
C) 3
D) 4
E) 5
7.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
CH3OH + O2  CO2 + H2O
A) 1
B) 2
C) 3
D) 4
E) 6
3.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
Na2S2O3 + I2  NaI + Na2S4O6
A) 1
B) 2
C) 3
D) 4
E) 6
8.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
P4O10 + H2O  H3PO4
A) 10
B) 6
C) 4
D) 2
E) 1
4.
You are asked to balance the chemical equation
H2 + O2  H2O. How many of the following ways are correct
ways to balance this equation?
I. 2H2 + O2  2H2O
II. H2 + 1 2 O2  H2O
III. 4H2 + 2O2  4H2O
IV. H2 + O2  H2O2
A) 0
B) 1
C) 2
D) 3
E) 4
9.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
NO2 + H2O  HNO3 + NO
A) 1
B) 2
C) 3
D) 4
E) 5
10.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
MnO2 + HCl  MnCl2 + Cl2 + H2O
A) 5
B) 4
C) 3
D) 2
E) 1
5.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
Pb(NO3)2 + K2CO3  PbCO3 + KNO3
A) 5
B) 4
C) 3
D) 2
E) 1
Page 1
16.
Consider a reaction given by the equation aA + bB  cC
+ dD. In this equation A, B, C, D represent chemicals, and a, b, c,
d represent coefficients in the balanced equation. For a given
reaction, how many values are there for the quantity “c/d”?
A) 1
B) 2
C) 3
D) 4
E) an infinite number
11.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
PCl5 + H2O  H3PO4 + HCl
A) 1
B) 2
C) 3
D) 4
E) 5
Use the following to answer questions 17-23:
12.
Balance the following equation in standard form and
determine the sum of the coefficients.
LiAlH4(s) + AlCl3(s)  AlH3(s) + LiCl(s)
A) 8
B) 9
C) 10
D) 11
E) 12
When the following equations are balanced using the smallest
possible integers, what is the number in front of the underlined
substance in each case?
13.
Which of the following statments is not true of balancing
a chemical equation?
A) Subscripts in the reactants must be conserved in the
products.
B) Coefficients are used to balance the atoms on both
sides.
C) The law of conservation of matter must be
followed.
D) Phases are often shown for each compound but are
not critical to balancing an equation.
E) All of the above statements (a-d) are true.
17.
Pb(s) + AgNO3(aq)  Pb(NO3)2 + Ag(s)
A) 1
B) 2
C) 4
D) 5
E) 6
18.
S(s) + O2(g)  SO2(g)
A) 1
B) 2
C) 3
D) 4
E) 5
19.
N2(g) + O2(g)  N2O3
A) 1
B) 2
C) 3
D) 4
E) 6
20.
Al2O3(s) + H2SO4(aq)  Al2(SO4)3(aq) + H2O(l)
A) 1
B) 2
C) 3
D) 6
E) 9
21.
Sr(s) + P4(s)  Sr3P2(s)
A) 2
B) 3
C) 6
D) 12
E) 18
22.
C2H6(g) + O2(g)  CO2(g) + H2O(g)
A) 4
B) 7
C) 8
D) 10
E) 14
14.
Balance the following equation in standard form and
determine the sum of the coefficients.
FeO(s) + O2 (g )  Fe2O3 (s)
A)
B)
C)
D)
E)
3
4
6
7
14
15.
Consider the reaction represented by the unbalanced
equation NH3 + O2  NO + H2O. For every 2.42 mol of NH3
that reacts, _______ mol of O2 is required.
A) 2.42
B) 3.03
C) 9.68
D) 1.94
E) none of these
Page 2
23.
Li(s) + O2(g)  Li2O(s)
A) 1
B) 2
C) 3
D) 4
E) 5
29.
When ethane (C2H6) is reacted with oxygen in the air, the
products are carbon dioxide and water. This process requires
__________ mol of oxygen for every 2.46 mol of ethane.
A) 2.46
B) 6.15
C) 8.61
D) 17.22
E) none of these
24.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
KClO3  KCl + KClO4
A) 1
B) 2
C) 3
D) 4
E) 5
Use the following to answer questions 30-32:
When the following equations are balanced using the smallest
possible integers, what is the number in front of the underlined
substance in each case?
25.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
NBr3 + NaOH  N2 + NaBr + HOBr
A) 1
B) 2
C) 3
D) 4
E) 5
26.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
C2H6 + O2  CO2 + H2O
A) 1
B) 2
C) 4
D) 6
E) 7
30.
Sb(s) + O2(g)  Sb2O5(s)
A) 1
B) 2
C) 4
D) 6
E) 12
31.
C4H10(g) + O2(g)  CO2(g) + H2O(g)
A) 2
B) 4
C) 6
D) 8
E) 10
32.
CH3OH(l) + O2(g)  CO2(g) + H2O(g)
A) 1
B) 2
C) 4
D) 6
E) 12
33.
Which of the following statements about chemical
reactions is false?
A) In balancing a chemical equation, all subscripts
must be conserved.
B) When one coefficient is doubled, the rest of the
coefficients in the balanced equation must also be
doubled.
C) The subscripts in a balanced equation tell us the
number of atoms in a molecule.
D) An individual coefficient in a balanced equation is
meaningless.
E) The phases in a chemical reaction tell us the nature
of the reactants and products.
27.
When the following equation is balanced using the
smallest possible integers, what is the number in front of the
substance in bold type?
SiCl4 + H2O  SiO2 + HCl
A) 1
B) 2
C) 3
D) 4
E) 5
28.
When table sugar is burned in air, carbon dioxide and
water vapor are products, as shown by the following unbalanced
chemical equation:
C12H22O11(s) + O2(g)  CO2(g) + H2O(g)
How many moles of oxygen are required to react completely with
7.37 mol of sugar?
A) 88.4
B) 7.37
C) 129
D) 177
E) none of these
34.
When the equation Si(s) + HF(aq)  SiF4(g) + H2(g) is
balanced, what is the coefficient for HF?
A) 0
B) 1
C) 2
D) 3
E) 4
Page 3
35.
The factors that most commonly cause chemical
reactions to occur are all the following except
A) formation of a solid
B) formation of a gas
C) formation of water
D) transfer of electrons
E) a decrease in temperature
41.
An aqueous solution of ammonium sulfate is allowed to
react with an aqueous solution of lead (II) nitrate.
The net ionic equation contains which of the following species
(when balanced in standard form)?
36.
A substance that, when dissolved in water, produces a
solution that conducts electric current very efficiently is called
A) a strong electrolyte
B) a weak electrolyte
C) a strong ion
D) an electrical solute
E) none of these
39.
An aqueous solution of ammonium sulfate is allowed to
react with an aqueous solution of lead (II) nitrate.
What is the coefficient of the solid in the balanced equation (in
standard form)?
A) 1
B) 2
C) 3
D) 4
E) 6
40.
An aqueous solution of ammonium sulfate is allowed to
react with an aqueous solution of lead (II) nitrate.
The complete ionic equation contains which of the following
species (when balanced in standard form)?
B)
2NH 4 ( aq)
3Pb2 (aq)

D) NO3 ( aq )
C)
E)
B)
2SO 24 (aq)
C)
2NO3 ( aq)
E)
38.
An aqueous solution of ammonium sulfate is allowed to
react with an aqueous solution of lead(II) nitrate.
Identify the solid in the balanced equation.
A) (NH4)2SO4
B) Pb(NO3)2
C) PbSO4
D) NH4NO3
E) There is no solid formed when the two solutions are
mixed.
2SO 24 (aq)
2NH 4 ( aq)
D)
37.
When a precipitation reaction occurs, the ions that do not
form the precipitate
A) evaporate
B) are cations only
C) form a second insoluble compound in the solution
D) are left dissolved in the solution
E) none of these
A)
A)
Na  (aq)
Page 4
Pb 2 (aq)
NO3 (aq )
42.
Which drawing best represents the mixing of aqueous
calcium chloride with aqueous potassium sulfate when they are
mixed in stoichiometric amounts (neither reactant is limiting)?
A)
43.
An aqueous solution of sodium carbonate is reacted with
an aqueous solution of calcium chloride.
Identify the solid in the balanced equation.
A) Na2CO3
B) CaCl2
C) NaCl
D) CaCO3
E) There is no solid formed when the two solutions are
mixed.
44.
An aqueous solution of sodium carbonate is reacted with
an aqueous solution of calcium chloride.
What is the coefficient of the solid in the balanced equation (in
standard form)?
A) 5
B) 4
C) 3
D) 2
E) 1
B)
45.
An aqueous solution of sodium carbonate is reacted with
an aqueous solution of calcium chloride.
The complete ionic equation contains which of the following
species (when balanced in standard form)?
C)
B)
Na  (aq)
2CO32 (aq)
C)
2Na  (aq)
D)
Cl (aq)
E)
3Ca 2 (aq)
A)
46.
An aqueous solution of sodium carbonate is reacted with
an aqueous solution of calcium chloride.
The net ionic equation contains which of the following species
(when balanced in standard form)?
D)
E)
A)
CO32 ( aq)
B)
2Na  (aq)
C)
2Cl (aq)
D)
Cl (aq)
E)
2Ca 2 (aq)
47.
The scientist who discovered the essential nature of acids
through solution conductivity studies is
A) Priestley
B) Boyle
C) Einstein
D) Mendeleev
E) Arrhenius
Page 5
53.
The reaction 2K(s) + Br2(l)  2KBr(s) is a(n)
______________ reaction.
A) precipitation
B) acid-base
C) oxidation-reduction
D) double-displacement
E) single-replacement
48.
When the following equation is balanced, what is the
coefficient for H2O?
Ca(OH)2(aq) + H3PO4(aq)  Ca3(PO4)2(s) + H2O(l)
A) 2
B) 3
C) 4
D) 6
E) 8
54.
The reaction AgNO3(aq) + NaCl(aq)  AgCl(s) +
NaNO3(aq) is a(n) ______________ reaction.
A) precipitation
B) acid-base
C) oxidation-reduction
D) single-replacement
E) none of these
49.
An aqueous solution of potassium chloride is mixed with
an aqueous solution of sodium nitrate.
Identify the solid in the balanced equation.
A) KCl
B) NaNO3
C) KNO3
D) NaCl
E) There is no solid formed when the two solutions are
mixed.
55.
The equation 2C2H6 + 7O2  4CO2 + 6H2O is an
oxidation-reduction reaction. True or false, and why?
A) True; the carbon is oxidized, and the oxygen is
reduced.
B) True; the carbon is reduced, and the oxygen is
oxidized.
C) True; the carbon is oxidized, and the hydrogen is
reduced.
D) True; the oxygen is reduced, and the hydrogen is
oxidized.
E) False
50.
An aqueous solution of potassium chloride is mixed with
an aqueous solution of sodium nitrate.
The molecular equation contains which one of the following terms
(when balanced in standard form)?
A) KCl(s)
B) KNO3(aq)
C) KNa(aq)
D) ClNO3(aq)
E) NaCl(s)
56.
The reaction HCl(aq) + KOH(aq)  H2O(l) + KCl(aq) is
a(n) ______________ reaction.
A) precipitation
B) acid-base
C) oxidation-reduction
D) single-replacement
E) none of these
51.
An aqueous solution of potassium chloride is mixed with
an aqueous solution of sodium nitrate.
The complete ionic equation contains which of the following
species (when balanced in standard form)?
B)
2K  (aq)
3NO3 ( aq )
C)
Cl (aq)
A)
D)
E)
57.
How many electrons are transferred in the following
oxidation-reduction reaction?
Zn(s) + 2AgNO3(aq)  Zn(NO3)2(aq) + 2Ag(s)
A) 1
B) 2
C) 3
D) 4
E) 5
2Na  (aq)
2KNO3 (aq)
52.
An aqueous solution of potassium chloride is mixed with
an aqueous solution of sodium nitrate.
The net ionic equation contains which of the following species
(when balanced in standard form)?
B)
2K  (aq)
3NO3 ( aq )
C)
2KNO3 (aq)
A)
D)
E)
58.
How many of the following are oxidation-reduction
reactions?
I. reaction of a metal with a nonmetal
II. synthesis
III. combustion
IV. precipitation
V. decomposition
A) 1
B) 2
C) 3
D) 4
E) 5
2Na  (aq)
No net ionic equation exists for this reaction.
Page 6
59.
65.
The equation 2Al(s) + 2Br2(l)  2AlBr3(s) is a(n)
______________ reaction.
A) oxidation-reduction and synthesis
B) oxidation-reduction only
C) synthesis only
D) decomposition
E) combustion
In what type of reaction is water always a product?
A) precipitation
B) acid-base
C) oxidation
D) decomposition
E) synthesis
60.
Classify the following reaction:
2Mg(s) + O2(g)  2MgO(s)
A) oxidation-reduction
B) combustion
C) synthesis
D) two of the above
E) a-c are all correct.
66.
The equation 2Ag2O(s)  4Ag(s) + O2(g) is a(n)
______________ reaction.
A) oxidation-reduction
B) synthesis
C) decomposition
D) combustion
E) two of these
61.
Classify the following reaction:
HNO3(aq) + KOH(aq)  KNO3(aq) +H2O(l)
A) oxidation-reduction
B) combustion
C) precipitation
D) acid-base
E) two of the above
67.
62.
When the following equation is balanced in standard
form, what is the coefficient in front of the underlined substance?
C2H6(g) + O2(g)  CO2(g) + H2O(l)
A) 1
B) 2
C) 3
D) 4
E) 5
2.
True or false? A catalyst is a substance that speeds up a
reaction without being consumed.
A) True
B) False
3.
True or false? A minimum energy called the activation
energy is needed for a reaction to occur.
A) True
B) False
63.
A reaction that involves a transfer of electrons is called
a(n) ______________ reaction.
A) precipitation
B) acid-base
C) oxidation-reduction
D) double-displacement
E) none of these
64.
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)
A) oxidation-reduction
B) synthesis
C) decomposition
D) combustion
E) two of these
4.
True or false? At equilibrium, the concentrations of all
reactants and products are constant.
A) True
B) False
5.
True or false? At equilibrium, the concentrations of all
reactants and products are equal.
A) True
B) False
Which of the following statements is not true?
A) When a metal reacts with a nonmetal, an ionic
compound is formed.
B) A metal-nonmetal reaction can always be assumed
to be an oxidation-reduction reaction.
C) Two nonmetals can undergo an oxidation-reduction
reaction.
D) When two nonmetals react, the compound formed is
ionic.
E) A metal-nonmetal reaction involves electron
transfer.
6.
Given the reaction A(g) + B(g)
C(g) + D(g). You
have the gases A, B, C, and D at equilibrium. Upon adding gas A,
the value of K
A) increases because when A is added, more products
are made, increasing the product-to-reactant ratio
B) decreases because A is a reactant, so the product-toreactant ratio decreases
C) does not change because A does not figure into the
product-to-reactant ratio
D) does not change as long as the temperature is
constant
E) depends on whether the reaction is endothermic or
exothermic
7.
Write the equilibrium expression for the reaction
3O2(g)
2O3(g)
Page 7
8.
Consider the general reaction
aA + bB
11.
cC + dD
2NO(g) + O2(g)
Choose the correct equilibrium expression below.
A)
K
B)
K
C)
K
D)
E)
C
B)
C)
D)
E)
10.
F2(g)
2NO2(g)
at a certain temperature, the equilibrium concentrations were
found to be [NO2] = 5.1  10–3 M, [O2] = 1.0  10–2 M,and [NO]
= 2.0  10–3 M. Calculate the value of the equilibrium constant
from these data (delete units).
A) 6.5  102
B) 12.7  104
C) 2.6  102
D) 1.5  10–3
E) none of these
D
[c ] [ d ]
[a]A [b]B
[C]c [D]d
[A]a [B]b
[A]a [B]b
[C]c [D]d
[a]A [b]B
K C D
[c ] [ d ]
[cC][dD]
K
[aA][bB]
12.
Write the equilibrium expression for the following
reaction:
S(s) + O2(g)
SO2(g)
[SO ]
2
[O ]
2
[O ]
2
B) K =
[SO ]2
2
[SO ]
2
C) K =
[O ]2
2
[SO ]2
2
D) K =
[O ]
2
9.
The correct equilibrium expression for the reaction of
sulfur dioxide gas with oxygen gas to produce sulfur trioxide gas
is
A)
For the reaction
[SO ]
3
[SO ][O ]
2
2
[SO ]2
3
[SO ]2 [O ]
2
2
[SO ]
3
[SO ]2 [O ]
2
2
[O ][SO ]2
2
2
[SO ]2
3
A)
K=
E)
none of these
13.
Which of the following is an example of a homogeneous
equilibrium reaction?
A) 2CO(g) + O2(g)
2CO2(g)
B) PCl5(s)
PCl3(l) + Cl2(g)
C) 2KClO3(s)
2KCl(s) + 3O2(g)
D) CaCO3(s)
CaO(s) + CO2(g)
E) 6CO2(g) + 6H2O(g)
C6H12O6(s) + 6O2(g)
none of these
For the reaction
14.
Which of the following is an example of a heterogeneous
equilibrium reaction?
A) N2O4(g)
2NO2(g)
B) H2(g) + F2(g)
2HF(g)
C) C2H2(g) + 2Br2(g)
C2H2Br4(g)
D) N2(g) + 3H2(g)
2NH3(g)
E) MgO(s) + CO2(g)
MgCO3(s)
2F(g)
at a particular temperature, the concentrations at equilibrium were
observed to be [F2] = 2.2  10–2 mol/L and [F] = 2.0  10–4
mol/L. Calculate the value of the equilibrium constant from these
data. (The units are deleted.)
A) 4.4  10–2
B) 1.7
C) 5.5  105
D) 1.8  10–6
E) none of these
Page 8
15.
Choose the correct equilibrium expression for the
following reaction.
2A(s) + 3B(l)
C(aq) + 4D(aq)
A)
[A]2 [B]3
[C][D]4
B)
[C] [D]4
C)
D)
E)
28.
Consider the following equilibrium:
2H2(g) + X2(g)
2H2X(g) + energy
The equilibrium expression is
A)
[2H2 X]
[2H 2 ][X2 ]
[2H 2 X]
[2H 2 ]  [X 2 ]
[C][4D]4
[2A]2 [3B]3
[C][D]4
[A]2 [B]3
B)
C)
[H 2 X]2
[H 2 ]2  [X 2 ]
none of these
D)
[H 2 X]2
[H 2 ]2 [X 2 ]
E)
none of these
Use the following to answer questions 19-22:
Consider the reaction 2H2(g) + O2(g)
2H2O(g) at some
equilibrium position. Using the following choices, indicate what
will happen if the changes below are made.
29.
Consider the following equilibrium:
2H2(g) + X2(g)
2H2X(g) + energy
Addition of X2 to this system at equilibrium
A) will cause [H2] to decrease
B) will cause [X2] to increase
C) will cause [H2X] to increase
D) will have no effect
E) cannot possibly be carried out
a. shifts to the left
b. shifts to the right
c. no change
19.
Additional H2O(g) is injected into the reaction vessel.
20.
Some H2(g) is removed from the reaction vessel.
21.
The size of the reaction vessel is decreased.
22.
Some He(g) is injected into the reaction vessel.
30.
Consider the following equilibrium:
2H2(g) + X2(g)
2H2X(g) + energy
Addition of argon to this system at equilibrium
A) will cause [H2] to decrease
B) will cause [X2] to increase
C) will cause [H2X] to increase
D) will have no effect
E) cannot possibly be carried out
Use the following to answer questions 23-27:
Consider the reaction system CH4(g) + 2O2(g)
CO2(g) +
2H2O(g) + energy, and use the following choices to describe what
happens when the changes below are made to the system at
equilibrium.
31.
Consider the following equilibrium:
2H2(g) + X2(g)
2H2X(g) + energy
Decreasing the volume of the container for this system at
equilibrium will cause
A) an increase in the amount of H2X
B) an increase in the amounts of H2 and X2
C) an increase in the amount of H2 but not X2
D) no change
E) X2 to dissociate
a. shifts to the left
b. shifts to the right
c. no change
23.
O2(g) is removed from the reaction vessel.
24.
CO2(g) is removed from the reaction vessel.
25.
He(g) is added to the reaction vessel.
26.
The temperature is increased.
27.
CH4(g) is added to the reaction vessel.
Page 9
32.
In the presence of ultraviolet light, the "inert" gas xenon
(Xe) will react with fluorine (F2) gas to produce solid XeF4. What
is the equilibrium expression for this reaction?
A)
B)
C)
D)
E)
36.
above
A)
B)
C)
D)
E)
[XeF4 ]
[Xe][F2 ]
[XeF4 ]
[Xe][F2 ]2
1
[F2 ]
1
[Xe][F2 ]2
1
[Xe][F2 ]
B)
C)
38.
Raising the pressure by decreasing the volume of the
container
A) will cause [A] to increase
B) will cause [B] to increase
C) will have no effect
D) cannot be determined
E) none of the above
[H 2 ][I 2 ]
[HI]2
39.
Which of the following is true when the equilibrium
constant for a reaction is relatively large?
A) It will take a short time to reach equilibrium.
B) It will take a long time to reach equilibrium.
C) The equilibrium lies to the left.
D) The equilbrium lies to the right.
E) two of these
[H 2 ][I 2 ]
[HI]2
[HI]
[H 2 ]
D)
[HI]2
[H 2 ][I 2 ]
E)
[HI]2
[H 2 ]
will cause [A] to increase
will cause [C] to increase
will have no effect
cannot be determined
none of the above
37.
Placing the equilibrium mixture in an ice bath (thus
lowering the temperature)
A) will cause [A] to increase
B) will cause [B] to increase
C) will have no effect
D) cannot be determined
E) none of the above
33.
Consider the following equilibrium:
H2(g) + I2(s)
2HI(g)
The equilibrium expression is
A)
Addition of chemical B to an equilibrium mixture of the
40.
Consider a system of four gases. The equilibrium
concentration of each product is 2.7 M. The equilibrium
concentrations of the reactants are equal. The equilibrium is shown
here:
A+B
34.
True or false? The concentrations of pure solids or pure
liquids involved in a chemical reaction are not included in the
equilibrium expression for the reaction.
A) True
B) False
C+D
K = 2.6
What is the equilibrium concentration of gas A?
A) 2.8 M
B) 19.0 M
C) 7.0 M
D) 1.7 M
E) 0.60 M
Use the following to answer questions 35-38:
41.
Given the equation A(g)
B(g) + 2C(g). At a particular
temperature, K = 1.4  105.
For the reaction
2SO2(g) + O2(g)
35.
If you mixed 1.2 mol B, 0.050 mol C, and 0.003 mol A
in a 1-L container, in which direction would the reaction initially
proceed?
A) to the left
B) to the right
C) The mixture is in the equilibrium state.
D) cannot tell from the information given
2SO3(g)
at a certain temperature, the equilibrium concentrations were
observed to be [SO2] = 0.733 M, [O2] = 7.50  10–2 M, and [SO3]
= 0.650 M. Calculate the value of K for this system at this
temperature.
A) 11.8
B) 16.1
C) 7.69
D) 140
E) 10.5
Page 10
42.
For the reaction
CO(g) + H2O(g)
49.
Given the solubility products (Ksp)
BaSO4
1.5  10-9
CoS
5.0  10-22
PbSO4
1.3  10-2
AgBr
5.0  10-13
which of the following compounds is the most soluble (in
mol/L)?
A) BaSO4
B) CoS
C) PbSO4
D) AgBr
E) BaCO3
CO2(g) + H2(g)
K = 3.88 at a certain temperature. If at this temperature in a
certain experiment the equilibrium concentrations are [H2] = 1.9
M, [CO2] = 1.8 M, and [H2O] = 0.26 M, calculate [CO].
A) 0.29 M
B) 1.9 M
C) 3.7 M
D) 3.4 M
E) none of these
43.
Write the balanced equation for the dissolving of
PbCl2(s) in water.
50.
The solubility of Fe(OH)2 in water at a certain
temperature is 7.9  10–6 mol/L. The value of Ksp of Fe(OH)2 at
this temperature is
A) 7.9  10–6
B) 2.0  10–15
C) 4.9  10–16
D) 1.2  10–10
E) none of these
44.
Write the balanced equation for the dissolving of Ag2S(s)
in water.
45.
Write the balanced equation for the dissolving of
Fe3(PO4)2 in water.
46.
The solubility of BaCO3(s) in water at a certain
temperature is 3.8  10–5 mol/L. Calculate the value of Ksp for
BaCO3(s) at this temperature.
A) 3.8  10–5
B) 7.6  10–5
C) 1.4  10–9
D) 6.2  10–3
E) none of these
51.
The molar solubility of PbI2 at a certain temperature is
1.5  10–3 M. Calculate the value of Ksp for PbI2.
A) 1.5  10–3
B) 3.4  10–9
C) 1.4  10–8
D) 4.5  10–6
E) none of these
47.
The solubility of Mg(OH)2(s) in water at a certain
temperature is 1.0  10–4 mol/L. Calculate the value of Ksp for
Mg(OH)2(s) at this temperature.
A) 1.0  10–4
B) 1.0  10–12
C) 1.0  10–8
D) 4.0  10–12
E) none of these
52.
Calculate the concentration of the silver ion in a saturated
solution of silver chloride, AgCl (Ksp = 1.6  10-10).
A) 5.4  10-4
B) 1.3  10-5
C) 1.6  10-10
D) 8.0  10-11
E) none of these
48.
The Ksp for ZnS(s) is 2.9  10–22 at a certain
temperature. The solubility of ZnS(s) in water at this temperature
is
A) 2.9  10–22
B) 1.7  10–11
C) 1.5  10–22
D) 5.8  10–22
E) none of these
53.
The concentration of Ag+ in a saturated solution of
Ag2CrO4 is 1.6  10-4 M. What is the Ksp value for Ag2CrO4?
A) 2.0  10-12
B) 2.6  10-8
C) 4.1  10-12
D) 5.1  10-8
E) 1.6  10-11
54.
The solubility of ZnS(s) in water at a certain temperature
is 1.4  10–11 mol/L. The value of the Ksp of ZnS is
A) 2.0  10–22
B) 1.4  10–11
C) 3.7  10–6
D) 7.0  10–12
E) 2.8  10–11
Page 11
55.
The solubility in mol/L of Ag2CrO4 is 1.2  10–4 M at a
certain temperature. What is the Ksp for this compound?
A) 1.2  10–4
B) 1.7  10–12
C) 6.9  10–12
D) 2.9  10–8
E) 5.8  10–8
56.
Silver chromate, Ag2CrO4, has a Ksp of 8.7  10–12 at a
certain temperature. What is the solubility in mol/L of silver
chromate?
A) 1.3  10–4
B) 8.7  10–12
C) 2.2  10–12
D) 1.6  10–4
E) 4.7  10–24
57.
The solubility of Cd(OH)2 in water at a certain
temperature is 1.8  10–5 mol/L. The Ksp value for Cd(OH)2 is
A) 2.3  10–14
B) 1.8  10–5
C) 5.8  10–15
D) 6.5  10–10
E) 3.2  10–10
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
C
A
B
D
D
D
D
E
C
B
E
D
A
D
B
A
B
A
C
C
C
B
B
C
B
E
D
A
C
C
D
C
A
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
Page 12
E
E
A
D
C
A
B
D
B
D
E
C
A
E
D
E
B
C
E
C
A
A
B
B
D
B
E
D
D
C
D
A
E
67.
E
2.
3.
4.
5.
6.
7.
A
A
A
B
D
8.
9.
10.
11.
12.
13.
14.
15.
B
B
D
A
A
A
E
B
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
a
a
b
c
a
b
c
a
b
D
K
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
[O3 ]2
[O 2 ]3
Page 13
A
D
A
D
E
A
B
A
D
A
D
D
E
D
PbCl2(s)
Pb2+(aq) + Cl-(aq)
Ag2S(s)
2Ag+(aq) + S2-(aq)
Fe3(PO4)2(s)
3Fe2+(aq) + 2PO43-(aq)
C
D
B
C
B
C
B
A
A
C
A
A