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Chapter Test B
Chapter: Acid-Base Titration and pH
In the space provided, write the letter of the term or phrase that best
completes each statement or best answers each question.
PART I
______ 1. The pH scale generally ranges from
a. 0 to 1.
b. 1 to 1.
c. 0 to 7.
d. 0 to 14.
______ 2. During the titration of HCl with NaOH, a very rapid change in pH
occurs
a. when the first addition of known solution is made.
b. when roughly equivalent amounts of H3O ions and OH ions
become present.
c. at several points.
d. at no point.
______ 3. A water solution is neutral if
a. it contains no H3O ions.
b. it contains no ionized water molecules.
c. it contains no H3O ions or OH ions.
d. the concentrations of H3O ions and OH ions are equal.
______ 4. The antilog of a number N is
a. the inverse of N.
b. the square root of N.
c. 10 raised to the power of N.
d. N raised to the 10th power.
______ 5. Universal indicators
a. are mixtures of several indicator solutions.
b. are pure substances.
c. have very brief color-change intervals.
d. work well only for acidic solutions.
______ 6. A useful pH range for an indicator in neutralizations involving strong
acids and weak bases is
a. 1.2 to 3.0.
b. 3.1 to 4.6.
c. 6.0 to 7.6.
d. 9.5 to 11.0.
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Chapter Test B, continued
______ 7. An acid-base titration determines the solution volumes that are
a. chemically equivalent.
b. of equal molarity.
c. of equal mass.
d. of equal molality.
______ 8. In acidic solutions, an indicator that is a weak acid, HIn, is primarily in
the form
a. In.
b. In.
c. InOH.
d. HIn.
PART II
Write the correct term (or terms) in the space provided.
9. Pure water partially breaks down into ions in a process called
.
10. If [H3O] in a solution is less than [OH], the solution is
.
11. The pH range over which an indicator changes color is called the indicator’s
.
12. The negative of the common logarithm of the hydronium ion concentration is
called
.
13. The product of [H3O] and [OH] in a water solution equals
.
14. The sum of the pH and the pOH of a neutral solution at 25°C is
.
15. As the concentration of hydronium ions increases, a solution becomes more
acidic and the pH
.
16. In a titration, an indicator changes color at the
of the titration.
17. When a weak acid is titrated with a strong base, the pH of the solution at the
equivalence point is
than 7.
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Modern Chemistry
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Chapter Test
SHORT ANSWER Answer the following questions in the space provided.
1. Refer to the energy diagram below to answer the following questions.
D ---
J
C
Bf-----'­
A'---------'
Course of reaction--)
d
a. Which letter represents the energy of the activated complex?
(a) A
(b) B
C
b. Which letter represents the energy of the reactants?
(a) A
(b) B
d
the amount of energy at C minus the amount of energy at B
the amount of energy at D minus the amount of energy at A
the amount of energy at D minus the amount of energy at B
the amount of energy at D minus the amount of energy at C
d. Which of the following represents the quantity of activation energy for the reverse
reaction?
(a)
(b)
(c)
( d)
b
(c) C
(d) D
c. Which of the following represents the quantity of activation energy for the forward
reaction?
(a)
(b)
(c)
(d)
C
(c) C
(d) D
the amount of energy at C minus the amount of energy at B
the amount of energy at D minus the amount of energy at A
the amount of energy at D minus the amount of energy at B
the amount of energy at D minus the amount of energy at C
e. Which of the following represents the energy change for the forward reaction?
(a)
(b)
(c)
( d)
the amount of energy at C minus the amount of energy at B
the amount of energy at B minus the amount of energy at C
the amount of energy at D minus the amount of_energy_at B
the amount of energy at B minus the amount of energy at A
MODERN CHEMISTRY
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REACTION KINETICS
137
Name ________________ Date _______ Class _______
CHAPTER 17 REVIEW
Reaction Kinetics
SHORT ANSWER Answer the following questions in the space provided.
1. Below is an energy diagram for a particular process. One curve represents the energy profile for the
uncatalyzed reaction, and the other curve represents the energy profile for the catalyzed reaction.
Course of reaction______......,.
_a__ a. Which curve has the greater activation energy?
(a) curve 1
(b) curve 2
( c) Both are equal.
__c_ b. Which curve has the greater energy change, M?
(a) curve 1
(b) curve 2
( c) Both are equal.
b_ c. Which curve represents the catalyzed process?
_::.
(a) curve 1
(b) curve 2
MODERN CHEMISTRY
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REACTION KINETICS
139
Name ________________ Date _______ Class _______
CHAPTER 18 REVIEW
Chemical Equilibrium
l1HU•1@fj
SHORT ANSWER
Answer the foll o wi ng qu e s t io n s in the s p ace provided.
1. _:,:d_ Raising the temperature of any equilibrium system always
(a) favors the forward reaction.
(b) favors the reverse reaction.
(c) favors the exothermic reaction.
(d) favors the endothermic reaction.
2. Consider the following equilibrium equation: CH3 0H(g)
+ 101 kJ � CO(g) + 2H2(g).
_bee.__ a. Increasing [CO] will
(a) increase [H2].
(b) decrease [H2].
(c) not change [H2].
(d) cause [H2] to fluctuate.
b _ b. Raising the temperature will cause the equilibrium of the system to
_;;;c.
(a) favor the reverse reaction.
(b) favor the forward reaction.
(c) shift back and forth.
(d) remain as it was before.
_;;;c.a_ c. Raising the temperature will
(a)
(b)
( c)
(d)
increase the value of K.
decrease the value of K.
not change the value of K.
make the value of K fluctuate.
MODERN CHEMISTRY
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CHEMICAL EQUILIBRIUM
145
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Chapter Test A
Chapter: Chemical Equilibrium
In the space provided, write the letter of the term or phrase that best completes
each statement or best answers each question.
______ 1. A 15.0 mL volume of 0.0100 M Pb(NO3)2 is added to 15.0 mL of
0.0100 M NaI. A precipitate is formed, and equilibrium is established. The
Ksp equilibrium expression for the dissolution of PbI2 is
a. [Pb2][I]2.
b. [Pb][I2].
c. [Pb2][2I]2.
d. 2[Pb2][I].
______ 2. What is the ion product for the PbI2 reaction in question 1?
a. 1.00 108
b. 1.25 107
c. 1.00 106
d. 2.5 105
______ 3. What is the equilibrium expression for the following equation?
Fe(OH)3(aq) ^ Fe3(aq) 3OH(aq)
[Fe3][OH]
a. [Fe(OH)3]
[Fe3][OH]3
b. [Fe(OH)3]
[Fe(OH)3]
c. [Fe3][OH]3
[Fe(OH)3]
d. [Fe3][OH]
______ 4. In a bottle of unopened cola, the CO2 gas dissolved in the liquid is in
equilibrium with the CO2 gas above the liquid. The dissolved gas reacts
with water molecules in the cola to form carbonic acid, which also
dissociates into carbon dioxide and water. Which chemical equation(s)
best describe this equilibrium system?
a. CO2(g) ^ CO2(l)
b. CO2(g) ^ CO2(aq) and CO2(l) H2O(l) ^ H2CO3(aq)
c. CO2(g) ^ CO2(aq)
d. CO2(g) ^ CO2(aq) and CO2(aq) H2O(l) ^ H2CO3(aq)
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Chapter Test A, continued
______ 5. The Haber process, N2(g) 3H2(g) ^ 2NH3(g) 92 kJ, is operated at
temperatures of about 500°C because
a. a higher temperature would favor the products.
b. K is a maximum at 500°C.
c. the forward reaction rate is too slow at lower temperatures.
d. K is equal to 1 at 500°C.
______ 6. Which of the following would not affect the aqueous equilibrium
reaction represented by the equation below?
HNO2(aq) ^ H(aq) NO
2 (aq)
a. the addition of NaNO3(s)
b. an increase in H concentration
c. the addition of NaNO2(s)
d. a decrease in NO
2 concentration
______ 7. Consider the equilibrium system represented by the equation below.
2
H2O(l) 2CrO2
4 (aq) ^ Cr2O7 (aq) 2OH (aq)
yellow
orange
If the hydroxide ions were removed, how would the color change?
a. to darker yellow
b. to lighter orange
c. to darker orange
d. not at all
______ 8. The Fe ion present in acid mine drainage is colorless and surrounded
by water molecules. If phenanthroline (Phe) is added, the solution
turns orange as a colored complex is formed according to the equation
Fe3 H2O Phe ^ Fe3 Phe H2O. The color is commonly used
as an indicator of the Fe ion concentration. What would an increase
in color from light to dark orange indicate in this system?
a. an applied stress that shifted the equilibrium to favor the reverse
reaction
b. an applied stress that shifted the equilibrium to favor the forward
reaction
c. an increase in the rate of the reverse reaction
d. addition of water to the system
______ 9. The solubility product constant expression includes
a. a concentration of zero for undissolved salt.
b. the concentrations of dissolved and undissolved salt.
c. an exponent corresponding to the charge on each ion.
d. the concentrations of dissociated ions.
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______10. In a reaction that goes nearly to completion,
a. the re-formation of reactants is much slower than the formation of
the products.
b. the rate of the reverse reaction is faster than the rate of the forward
reaction.
c. the re-formation of reactants is much faster than the rate of
formation of the products.
d. the forward reaction rate increases.
______11. Which of the following Keq expressions is correct for the formation of
ammonia, NH3, from its elements, as represented by the equation
3H2 N2 ^ 2NH3 92 kJ?
[NH3]2
a. 3
[H2] [N2]
[H2]3[N2]
b. [NH3]2
[NH3]
c. [H2][N2]
[H2][N2]
d. [NH3]
______12. When you calculate the Ksp of calcium fluoride, CaF2, if the
concentration of the F ion is 4.2 104 M, then the concentration
of the Ca2 ion is
a. 2.1 104 M.
b. 8.4 104 M.
c. 4.2 104 M.
d. 3.7 1011 M.
______13. Which of the following salts is least soluble?
a. Ag2CO3
Ksp 8.4 1012
b. Ag2CrO4
Ksp 1.1 1012
c. AgI
Ksp 1.5 1016
d. AgBr
Ksp 5.4 1013
______14. Consider the reaction represented by the equation 2NO(g) O2(g) ^
2NO2(g). If the volume of the reaction chamber is decreased, then the
a. forward reaction will be favored.
b. reverse reaction will be favored.
c. initial pressure of NO2 will decrease.
d. initial pressure of O2 will remain constant.
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______15. Consider the reaction represented by the equation Ag2SO4(aq) ^
2Ag(aq) SO2
4 (aq). You can shift the equilibrium to favor the
reverse reaction by adding
a. CaCl2.
b. AgNO3.
c. Na2SO4.
d. Both (b) and (c)
______16. A chemical reaction that is at equilibrium always has
a. a high Keq value.
b. a forward reaction rate that equals the reverse reaction rate.
c. equal concentrations of reactants and products.
d. Both (a) and (b)
______ 17. Which of these is true about the chemical equation below?
reactants e products
a. The concentration of the products is greater than the concentration
of the reactants.
b. Keq of the forward reaction has a low value.
c. The reaction favors the products.
d. Keq is equal to 1.
______18. In which of the following reactions, described by the equations below,
will an increase in pressure have no effect on the equilibrium of the
system?
a. 2NO2(g) ^ N2O4(g)
b. 2NOCl(g) ^ 2NO(g) Cl2(g)
c. H2O(g) CO(g) ^ H2(g) CO2(g)
d. N2(g) 3H2(g) ^ 2NH3(g)
______19. The common-ion effect promotes
a. dissolution.
b. precipitation.
c. boiling.
d. ionization.
______20. What is the acid ionization expression for the equation
HA(aq) H2O(l) ^ H3O(aq) A(aq)?
[A][H3O]
a. [HA][H2O]
[A]
b. [HA][H2O]
[A][H3O]
c. [HA]
d. [A ][H3O][HA][H2O]
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Chapter Test A, continued
______21. The reaction represented by the equation BH(aq) H2O(l) ^
H3O(aq) B(aq) is an example of a(n)
a. cation hydrolysis reaction.
b. anion hydrolysis reaction.
c. conjugated reaction.
d. pH reaction.
______22. What is the value of Kw?
a. 1 1014
b. 1 1014
c. 1 107
d. 14 1014
______23. An example of a good buffer solution is one that contains
a. HCl and NaCl.
b. HNO2 and NaCl.
c. HNO2 and NaNO2.
d. CH3COOH and NaCl.
______24. When H3O ions are added to an aqueous solution of acetic acid,
a. the reaction forms more CH3COO.
b. the reaction forms more water.
c. the reaction forms more CH3COOH.
d. nothing happens.
______25. Which of the following is a conjugate acid-base pair in the reaction
represented by the equation below?
H2PO
4 H2O ^ H3PO4 OH
a.
b.
c.
d.
H2PO
4 and H2O
H2PO
4 and OH
H2PO4 and H3PO4
None of the above
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Chapter Test B
Chapter: Chemical Equilibrium
PART I In the space provided, write the letter of the term or phrase that best
completes each statement or best answers each question.
______ 1. What is the effect on concentration if more CO(g) is added to the
following equilibrium system?
2CO(g) O2(g) ^ 2CO2(g)
a.
b.
c.
d.
[CO2] increases and [O2] decreases.
Both [CO2] and [O2] increase.
Both [CO2] and [O2] decrease.
Both [CO2] and [O2] remain the same.
______ 2. Consider the following equation for the ionization of acetic acid:
CH3COOH(aq) H2O(l) ^ H3O(aq) CH3COO(aq)
What is the equation for the acid ionization constant, Ka, for this
system?
a. [H3O][CH3COO]
[H3O][CH3COO]
b. [CH3COOH]
[H3O][CH3COO]
c. [CH3COOH][H2O]
[CH3COOH]
d. [H3O][CH3COO]
______ 3. Adding the salt of a weak base to a solution of the weak base
a. lowers the concentration of the nonionized base and of OH.
b. lowers the concentration of the nonionized base and raises the
concentration of OH.
c. raises the concentration of the nonionized base and of OH.
d. raises the concentration of the nonionized base and lowers the
concentration of OH.
______ 4. A very high value for K indicates that
a. reactants are favored.
b. products are favored.
c. equilibrium is reached slowly.
d. equilibrium has been reached.
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Chapter Test B, continued
______ 5. How do Ka values for weak and strong acids compare?
a. Ka(weak) Ka(strong).
b. Ka(weak) Ka(strong).
c. Ka(weak) Ka(strong).
d. Ka is not defined for weak acids.
______ 6. A reversible reaction is one in which
a. only the forward reaction takes place.
b. only the reverse reaction takes place.
c. the products can react to reform the reactants.
d. None of the above
______ 7. If the ion product for two ions whose solutions have just been mixed
is greater than the value of Ksp,
a. precipitation occurs.
b. decomposition occurs.
c. the solution is unsaturated.
d. equilibrium cannot be achieved.
PART II
Write the correct term (or terms) in the space provided.
8. Salts of a weak acid and a strong base produce solutions that are
.
9. The equation for the self-ionization of water is
.
10. Hydrolysis is a reaction between water and
.
11. Equilibrium is a
state.
12. The equilibrium expression for the reaction AgCl(s) ^ Ag(aq) Cl(aq) is
.
13. The
is the phenomenon in which the
addition of a charged particle common to two solutes decreases the solute
concentration.
14. When small amounts of acids or bases are added to a solution of a weak acid
and its salt, pH
.
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