Spring Final Review
1. ) Of the following substances, only __________ has London dispersion forces as the only
intermolecular force.
A) CH3OH
B) NH3
C) H2S
D) Kr
E) HCl
Answer: D
2. A sample of potassiumchromate (49.0 g) is dissolved in 100 g of water at 100 °C, with
precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no
precipitate is observed. This solution is __________.
A) hydrated
B) placated
C) saturated
D) unsaturated
E) supersaturated
3. Calculate the freezing point (0 °C) of a 0.15500 m aqueous solution of glucose. The molal
freezing-point-depression constant of water is 1.86 °C/m.
A) 0.0286 °C
B) 0.106 °C
C) -0.0562 °C
D) -0.102 °C
E) -0.2883 °C Answer
4. The phrase "like dissolves like" refers to the fact that __________.
A) gases can only dissolve other gases
B) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes
C) solvents can only dissolve solutes of similar molar mass
D) condensed phases can only dissolve other condensed phases
E) polar solvents dissolve nonpolar solutes and vice versa
Answer: B
5. A solution with a concentration higher than the solubility is __________.
A) is not possible
B) is unsaturated
C) is supercritical
D) is saturated
E) is supersaturated
Answer: E
6. A 0.100 m solution of which one of the following solutes will have the lowest vapor pressure?
A)KMnO4
B) Ca(ClO4)2
C) Al(OH)3
D) glucose
E) KCl
Answer: C
7. A reaction was found to be second order in carbon monoxide concentration. The rate of the
reaction __________ if the [CO] is halved, with everything else kept the same.
A) doubles
B) remains unchanged
C) triples
D) decreases by a factor of 4
E) is reduced by a factor of 2
Answer: D
8. If the rate law for the reaction
3A + 2B  products
is first order in A and second order in B, then the rate law is rate = __________.
A)
k  A   B 
2
3
B) k[A] [B]
C) k[A] [B]2
2
D) k[A] [B]
2
2
E) k[A] [B]
9. The overall order of a reaction is 1. The units of the rate constant for the reaction are
__________.
A) M-2/s
1 1
B) M s
C) 1 s
D) 1 M
2
E) s M
Answer: c
The data in the table below were obtained for the reaction:
2ClO2 (aq)  2OH  (aq)  ClO3 (aq)  ClO 2  (aq)  H 2O(l)
10. What is the order of the reaction with respect to OH-?
A) 1
B) 0
C) 2
D) 3
E) 4
Answer: A
11. Which one of the following graphs shows the correct relationship between concentration and
time for a reaction that is second order in [A]?
A)
B)
C)
D)
E)
Answer: C
12. The reaction A(aq)  B(aq) is first order in [A]. A solution is prepared with [A] = 1.22 M.
The following data are obtained as the reaction proceeds:
1
The rate constant for this reaction is __________ s .
A) 0.23
B) 1.0
C) 0.17
D) 0.12
E) 0.12
Answer: D
13. The value of Keq for the equilibrium H2(g) + I2(g) ↔ 2HI(g)
is 794 at 25 °C. What is the value of Keq for the equilibrium below?
1/2H2(g) + 1/2I2(g) ↔ HI(g)
A) 397
B) 0.035
C) 28
D) 1588
E) 0.0013
Answer: C
14. Which of the following expressions is the correct equilibrium-constant expression for the
reaction below?
HF(aq) + H2O(l) ↔ H3O+(aq) + F-(aq)


A) [HF][H 2O] / {H3O ][F ]
B) 1 / HF


C) [H3O ][F ] / [HF][H 2O]


D) [H3O ][F ] / [HF]

E) [F ] / [HF]
Answer: D
15. Consider the following reaction at equilibrium:
2NH3(g) ↔N2(g) + 3H2(g)
ΔH° = +92.4 kJ
H
Le Chatelier's principle predicts that the moles of 2 in the reaction container will increase with
__________.
A) some removal of NH3 from the reaction vessel (V and T constant)
B) a decrease in the total pressure (T constant)
C) addition of someN2 to the reaction vessel (V and T constant)
D) a decrease in the total volume of the reaction vessel (T constant)
E) an increase in total pressure by the addition of helium gas (V and T constant)
Answer: B
16. The conjugate base of HSO4- is __________.

A) OH
B) H 2 SO 4
2
C) SO 4

D) HSO 4
H SO 
E) 3 4
Answer: C
17. What is the pH of an aqueous solution at 25.0 °C in which [OH-] is 0.0025 M?
A) +2.60
B) -2.60
C) +11.4
D) -11.4
E) -2.25
Answer: C
18. Calculate the concentration (in M) of hydronium ions in a solution at 25.0 °C with a pOH of
4.223.
A) 5.98 X 10-5
10
B) 1.67 10
C) 1.67 10
19
D) 5.99  10
4
E) 1.00 10
Answer: B
7
19. An aqueous solution contains 0.100 M NaOH at 25.0 °C. The pH of the solution is
__________.
A) 0.100
B) 1.00
C) 13.00
D) 7.00
E) -1.00
nswer: C
3
20. The acid-dissociation constant, Ka, for gallic acid is 4.57 10 What is the base-dissociation
constant, Kb, for the gallate ion?
3
A) 4.57 10
12
B) 2.19  10
5
C) 5.43 10
6
D) 7.8110
2
E) 2.9110
Answer: B
21. A Br  nsted-Lowry acid is defined as a substance that __________.
A) increases [H+] when placed in H2O
B) decreases [H+] when placed in H2O
C) increases [OH-] when placed in H2O
D) acts as a proton acceptor
E) acts as a proton donor
Answer: E
22. The molar concentration of hydroxide ion in pure water at 25 °C is __________.
A) 1.00
B) 0.00
14
C) 1.0 10
D) 1.0  10
E) 7.00
7
23. ) Of the following acids, __________ is not a strong acid.
A) HNO2
B) H2SO4
C) HNO3
D)HClO4
E) HCl
Answer: A
24. In which of the following aqueous solutions does the weak acid exhibit the highest
percentage ionization?
A) 0.01 M HC2H3O2 (Ka = 1.8 X10-5)
B) 0.01 M HNO2 (Ka = 4.5 X10-4)
C) 0.01 M HF (Ka = 6.8 X 10-4)
D) 0.01 MHClO (K= 3.0 X10-8)
E) These will all exhibit the same percentage ionization.
Answer: C
25. A 0.1 M solution of __________ has a pH of 7.0.
A) Na2S
B) KF
C) NaNO3
D) NH4Cl
E) NaF
Answer: C
26. Calculate the pH of a solution prepared by dissolving 0,150 mol of benzoic acid (HBz) and
0.300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic
acid is 6.50 X 10-5.
A) 2.516
B) 3.892
C) 4.488
D) 10.158
E) 4.195
nswer: C
27. A 25.0 mL sample of 0.723 M HClO4is titrated with a 0.273M KOH solution. What is the
[H+] (molarity) before any base is added?
A) 0.439
7
B) 1.00 10
C) 0.723
13
D) 2.8110
E) 0.273
Answer: C
27. A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273M KOH solution. The [H+]
concentration after the addition of 10.0 ml of KOH is __________ M.
A) 0.438
7
B) 1.00 10
C) 0.723
13
D) 2.8110
E) 0.273
Answer: A
28. A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The [H+]
concentration at the equivalence point is __________ M.
A) 0.439
7
B) 1.00 10
C) 0.723
13
D) 2.8110
E) 0.273
Answer: B
29. Which one of the following pairs cannot be mixed together to form a buffer solution?
A) C5H5N, C5H5NHCl
B) HC2H3O2, NaOH
C) KOH, HI
D)NH2CH3,HCl
E) NaClO, HNO3
Answer: C
30. The loss of electrons by an element is called __________.
A) reduction
B) oxidation
C) disproportionation
D) fractionation
E) sublimation
Answer: B
31. _________ is the oxidizing agent in the reaction below.
Cr 2 O 7 2 6S 2 O 32 14H   2Cr 3  3S 4 O 6 2 7H 2 O
A)
Cr 2 O 7 2 
S O 2
B) 2 3

C) H
3
D) Cr
S O 2
E) 4 6
Answer: A
32. What is the oxidation number of potassium in KMnO4?
A) 0 Answer: B
B) +1
C) +2
D) -1
E) +3
33. The electrode at which reduction occurs is called the __________.
A) oxidizing agent
B) cathode
C) reducing agent
D) anode
E) voltaic cell
Answer: B
34. In a voltaic cell, electrons flow from the __________ to the __________.
A) salt bride, anode
B) anode, salt bridge
C) cathode, anode
D) salt bridge, cathode
E) anode, cathode
Answer: E
35. The standard cell potential (E°cell) for the voltaic cell based on the reaction below is
__________ V.
Cr (s)  3Fe3 (aq)  3Fe2 (aq)  Cr 3 (aq)
A) -1.45
B) +2.99
C) +1.51
D) +3.05
E) +1.57
Answer: C
CaCO 3
36. The balanced net ionic equation for precipitation of
when aqueous solutions of
Na 2 CO 3 and CaCl 2
are mixed is __________.
A)
2Na + (aq)  CO32 (aq)  Na 2 CO 3 (aq)
+

B) 2 Na (aq)  2Cl (aq)  2NaCl (aq)
+

C) Na (aq)  Cl (aq)  NaCl (aq)
D)
E)
Ca 2+ (aq)  CO 32 (aq)  CaCO 3 (s)
Na 2 CO 3 (aq)  CaCl 2 (aq)  2NaCl (aq)  CaCO 3 (s)
Answer: D
37. The spectator ions in the reaction between aqueous perchloric acid and aqueous barium
hydroxide are __________.


A) OH and ClO 4
+


2+
B) H ,OH ,ClO 4 ,and Ba
+

C) H and OH
+
2+
D) H and Ba

2+
E) ClO 4 and Ba
Answer: E
38. Which of the following are strong acids?
HI
HNO 3
HF
HBr
A) HF , HBr
HI , HNO 3 , HF , HBr
B)
C) HI , HF , HBr
D) HNO 3 , HF , HBr
HI , HNO 3 , HBr
E)
Answer: E
39. Which of the following is soluble in water at 25 °C?
A)
Fe 3 (PO 4 ) 2
B) Fe(OH) 2
Fe(NO 3 ) 2
C)
FeCO 3
D)
E) FeS
Answer: C
40. Which combination will produce a precipitate?
NaC 2 H 3 O 2 (aq) and HCl (aq)
A)
B) NaOH (aq) and HCl (aq)
AgNO 3 (aq) and Ca(C 2 H 3 O 2 ) 2 (aq)
C)
KOH (aq) and Mg(NO 3 ) 2 (aq)
D)
E) NaOH (aq) and HCl (aq)
Answer: D
41. With which of the following will the ammonium ion form an insoluble salt?
A) chloride
B) sulfate
C) carbonate
D) sulfate and carbonate
E) none of the above
Answer: E
42. Which one of the following is a diprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
Answer: E
43. In which reaction does the oxidation number of hydrogen change?
A)
B)
C)
HCl (aq)  NaOH (aq)  NaCl (aq)  H 2O (l)
2 Na (s)  2H 2 O (l)  2 NaOH (aq)  H 2 (g)
CaO (s)  H 2 O (l)  Ca(OH) 2 (s)
2 HClO 4 (aq)  CaCO 3 (s)  Ca(ClO 4 )
D)
SO 2 (g)  H 2 O (l)  H 2 SO 3 (aq)
E)
Answer: B
2
(aq)  H 2 O (l)  CO 2 (g)
Answer: D