Acids And Bases, A Molecular Look Exam Prep Chapter 15 - Solution Bank | Chemistry Molecular Nature 8e by Neil D. Jespersen. DOCX document preview.
Chemistry: Molecular Nature of Matter, 8e (Jespersen)
Chapter 15 Acids and Bases, a Molecular Look
1) The conjugate acid of HPO42- is
A) H2PO4.
B) H3PO4.
C) PO43-.
D) PO42-.
E) H2PO4-.
Diff: 1
Section: 15.1
2) The conjugate base of HPO42- is
A) H2PO4.
B) H3PO4.
C) PO43-.
D) PO42-.
E) H2PO4-.
Diff: 1
Section: 15.1
3) The conjugate base of H2SO4 is
A) SO42-.
B) H3O+.
C) OH-.
D) HSO4-.
E) H2SO3.
Diff: 1
Section: 15.1
4) The conjugate base of H2AsO4- is
A) H2AsO4
B) H3AsO4
C) HAsO4-
D) HAsO42-.
E) AsO43-.
Diff: 1
Section: 15.1
5) The conjugate acid of NH3 is
A) NH4
B) NH3+
C) H+
D) H3O+
E) NH4+
Diff: 1
Section: 15.1
6) The conjugate acid of H2AsO4- is
A) H2AsO4
B) H3AsO4
C) HAsO4-
D) HAsO42-
E) AsO43-
Diff: 1
Section: 15.1
7) Which species is amphiprotic?
A) PO43-(aq)
B) HCl(g)
C) HSO4-(aq)
D) Cl-(aq)
E) CO32-(aq)
Diff: 1
Section: 15.1
8) Which species is amphoteric?
A) HNO3(aq)
B) Cl-(g)
C) CO32-(aq)
D) HSO3-(aq)
E) PO43-(aq)
Diff: 1
Section: 15.1
9) Which species is amphiprotic?
A) AsO43-(aq)
B) HBr(aq)
C) HF(aq)
D) SO42-(aq)
E) HCO3-(aq)
Diff: 1
Section: 15.1
10) Which species does not have a conjugate base?
A) H2O
B) H3O+
C) NH4+
D) HCO3-
E) F-
Diff: 1
Section: 15.1
11) Which species does not have a conjugate acid?
A) HCO2
B) H2O
C) HCl
D) OH-
E) NH2-
Diff: 1
Section: 15.1
12) Which species has a conjugate base?
A) Cl-
B) SO42-
C) CN-
D) OH-
E) CO32-
Diff: 1
Section: 15.1
13) In the reaction, HClO3 + N2H4 
ClO3- + N2H5+, which species are a conjugate acid-base pair?
A) HClO3, N2H4
B) N2H4, ClO3-
C) HClO3, N2H5+
D) N2H4, N2H5+
E) ClO3-, N2H5+
Diff: 1
Section: 15.1
14) In the reaction, HClO3 + N2H4 ClO3- + N2H5+, which two species are acids?
A) HClO3, N2H4
B) HClO3, ClO3-
C) HClO3, N2H5+
D) N2H4, N2H5+
E) ClO3-, N2H5+
Diff: 1
Section: 15.1
15) In the reaction, HClO3 + N2H4 ClO3- + N2H5+, which two species are bases?
A) HClO3, N2H4
B) HClO3, ClO3-
C) HClO3, N2H5+
D) N2H4, N2H5+
E) ClO3-, N2H4
Diff: 1
Section: 15.1
16) In the reaction, H2PO4- + HAsO42- HPO42- + H2AsO4-, which species are a conjugate acid-base pair?
A) H2PO4-, HAsO42-
B) H2PO4-, H2AsO4-
C) H2PO4-, HPO42-
D) HAsO42-, HPO42-
E) HPO42-, H2AsO4-
Diff: 1
Section: 15.1
17) In the reaction, H2PO4- + HAsO42- HPO42- + H2AsO4-, which two species are acids?
A) H2PO4-, HAsO42-
B) H2PO4-, H2AsO4-
C) H2PO4-, HPO42-
D) HAsO42-, HPO42-
E) HPO42-, H2AsO4-
Diff: 1
Section: 15.1
18) In the reaction, H2PO4- + HAsO42- HPO42- + H2AsO4-, which two species are bases?
A) H2PO4-, HAsO42-
B) H2PO4-, H2AsO4-
C) H2PO4-, HPO42-
D) HAsO42-, HPO42-
E) HPO42-, H2AsO4-
Diff: 1
Section: 15.1
19) In the reaction, HSO4- + HS- H2S + SO42-, which species are a conjugate acid-base pair?
A) HSO4-, HS-
B) HSO4-, H2S
C) HS-, H2S
D) HS-, SO42-
E) H2S, SO42-
Diff: 1
Section: 15.1
20) In the reaction, HSO4- + HS- H2S + SO42-, which two species are acids?
A) HSO4-, HS-
B) HSO4-, H2S
C) HS-, H2S
D) HS-, SO42-
E) H2S, SO42-
Diff: 1
Section: 15.1
21) In the reaction, HSO4- + HS- H2S + SO42-, which two species are bases?
A) HSO4-, HS--
B) HSO4-, H2S
C) HS-, H2S
D) HS-, SO42-
E) H2S, SO42-
Diff: 1
Section: 15.1
22) In the reaction, HSO4- + CN- HCN + SO42-, which species are a conjugate acid-base pair?
A) HSO4-, CN-
B) CN-, HCN
C) CN-, SO42-
D) HCN, SO42-
E) HCN, HSO4-
Diff: 1
Section: 15.1
23) In the reaction, HSO4- + CN- HCN + SO42-, which two species are acids?
A) HSO4-, CN-
B) HSO4-, HCN
C) CN-, HCN
D) CN-, SO42-
E) SO42-, HCN
Diff: 1
Section: 15.1
24) In the reaction, HSO4- + CN- HCN + SO42-, which two species are both bases?
A) HSO4-, CN-
B) HSO4-, HCN
C) SO42-, HCN
D) CN-, HCN
E) CN-, SO42-
Diff: 1
Section: 15.1
25) For the system
NH2OH + CH3NH3+ CH3NH2 + NH3OH+
the position of the equilibrium lies to the left. Which is the strongest acid in the system?
A) NH2OH
B) CH3NH3+
C) CH3NH2
D) NH3OH+
E) NH2OH and CH3NH3+ are equal in acid strength, and are the strongest acids in the system.
Diff: 1
Section: 15.2
26) For the system
HC6H5O + C4H7O2- C6H5O- + HC4H7O2
the position of the equilibrium lies to the left. Which is the strongest acid in the system?
A) HC6H5O
B) C4H7O2-
C) C6H5O-
D) HC4H7O2
E) HC4H7O2 and C4H7O2- are equal in acid strength, and are the strongest acids in the system
Diff: 1
Section: 15.2
27) For the system
NH2OH + CH3NH3+ CH3NH2 + NH3OH+
the position of the equilibrium lies to the left. Which is the weakest base in the system?
A) NH2OH
B) CH3NH3+
C) CH3NH2
D) NH3OH+
E) CH3NH2 and NH3OH+ are equal in base strength and are the weakest bases in the system
Diff: 1
Section: 15.2
28) For the system
HC6H5O + C4H7O2- C6H5O- + HC4H7O2
the position of the equilibrium lies to the left. Which is the strongest base in the system?
A) HC6H5O
B) C4H7O2-
C) C6H5O-
D) HC4H7O2
E) HC4H7O2 and C4H7O2- are equal in acid strength, and are the strongest acids in the system
Diff: 1
Section: 15.2
29) Given the following substances, listed in order of increasing acid strength,
HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)
Which species listed below is the strongest base?
A) Cl-(aq)
B) OCl-(aq)
C) H2C2O4(aq)
D) NO2-(aq)
E) OCN-(aq)
Diff: 1
Section: 15.2
30) Given the following substances, listed in order of increasing acid strength,
HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)
Which species listed below is the weakest base?
A) C2H3O2-(aq)
B) OCl-(aq)
C) H2C2O4(aq)
D) Cl-(aq)
E) OCN-(aq)
Diff: 1
Section: 15.2
31) Given the following substances, listed in order of increasing acid strength,
HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)
Which species listed below is the strongest base?
A) Cl-(aq)
B) HOCl(aq)
C) C2O42-(aq)
D) NO2-(aq)
E) OCN-(aq)
Diff: 1
Section: 15.2
32) Given the following substances in order of increasing acid strength,
HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)
Which species listed below is the weakest base of that set?
A) C2H3O2-(aq)
B) OCl-(aq)
C) HC2O4-(aq)
D) HNO2(aq)
E) OCN-(aq)
Diff: 1
Section: 15.2
33) Given that X is the same atom for each of the following, which is the strongest oxyacid?
A) O
║
H—O—X—O—H
B) O
║
H—O—X—O—H
│
O—H
C) O
║
X—O—H
║
O
D) O
║
H—O—X—O—H
│
H
E) O
║
H—O—X—H
│
H
Diff: 1
Section: 15.3
34) Given that X is the same atom for each of the following, which is the strongest oxyacid?
A) O
║
H—O—X—O—H
B) O
║
X—O—H
║
O
C) O
║
H—O—X—O—H
║
O
D) O
║
H—O—X═O
║
O
E) O
║
H—O—X—O—H
│
H
Diff: 1
Section: 15.3
35) Given that X is the same atom for each of the following, which is the weakest oxoacid?
A) O
║
H—O—X—O—H
B) O—H
│
H—O—X—O—H
│
O—H
C) O
║
X—O—H
║
O
D) O
║
H—O—X—O—H
║
O
E) O
║
H—O—X═O
║
O
Diff: 1
Section: 15.3
36) Given that X is the same atom for each of the following, which is the strongest oxoacid?
A) O
║
X—O—H
║
O
B) O
║
H—O—X—O—H
║
O
C) O
║
H—O—X═O
║
O
D) O
║
H—O—X—O—H
│
H
E) O
║
H—O—X—H
│
H
Diff: 1
Section: 15.3
37) Which species would be expected to be the most acidic?
A) HClO
B) HClO2
C) HClO3
D) HClO4
E) Cl-
Diff: 1
Section: 15.3
38) Which species is the weakest acid?
A) HBr
B) HCl
C) HF
D) HI
E) H2Se
Diff: 1
Section: 15.3
39) Which species is the strongest acid?
A) H2O
B) H2S
C) H2Se
D) H2Te
E) HCl
Diff: 1
Section: 15.3
40) Which species is the strongest organic acid?
A) CCl3-COOH
B) CH3-COOH
C) CH2Cl-COOH
D) CBr3-COOH
E) CBrCl2-COOH
Diff: 1
Section: 15.3
41) For the reaction, CO2 + H2O H2CO3, which of the following statements is incorrect?
A) CO2 is a Brønsted-Lowry acid and H2O is a Brønsted-Lowry base.
B) H2CO3 forms a coordinate covalent bond by a Lewis acid-base reaction.
C) CO2 is a Lewis acid and H2O is a Lewis base.
D) The lone pairs in the H2O molecule are used to form a new bond with the carbon in the CO2 molecule.
E) Both A and D
Diff: 2
Section: 15.4
42) NH3 can react with BF3, forming NH3—BF3. In this reaction,
A) the NH3 is a Brønsted-Lowry base, accepting a proton from the BF3 molecule.
B) the NH3 is a Lewis base, donating a proton to the BF3 molecule.
C) the NH3 is a Brønsted-Lowry acid, donating a proton to the BF3 molecule.
D) the BF3 molecule is a Lewis acid, accepting an electron pair from the NH3 molecule to form a coordinate covalent bond.
E) the BF3 molecule is a Lewis base, donating an electron pair to the NH3 molecule to form a coordinate covalent bond.
Diff: 1
Section: 15.4
43) SO2 can react with OH-, forming HSO3-. In this reaction,
A) the SO2 is a Brønsted-Lowry acid, accepting a proton from the OH- ion.
B) the SO2 is a Lewis acid, accepting a proton from the OH- ion.
C) the OH- ion is a Brønsted-Lowry base, donating a proton to the SO2 molecule.
D) the OH- ion is a Lewis base, donating an electron pair to the SO2 molecule to form a coordinate covalent bond.
E) the OH- ion is a Lewis acid, accepting an electron pair from the SO2 molecule to form a coordinate covalent bond.
Diff: 2
Section: 15.4
44) The F- ion can react with BF3, forming the BF4- anion. In this reaction,
A) the F- ion is a Brønsted-Lowry base, accepting a proton from the BF3 molecule.
B) the F- ion is a Lewis base, donating a proton to the BF3 molecule.
C) the F- ion is a Brønsted-Lowry acid, donating a proton to the BF3 molecule.
D) the BF3 molecule acts as a Lewis acid, accepting an electron pair from the F- ion to form a coordinate covalent bond.
E) the BF3 molecule acts as a Lewis base, donating an electron pair to the F- ion to form a coordinate covalent bond.
Diff: 2
Section: 15.4
45) CO2 can react with OH-, forming HCO3-. In this reaction,
A) the CO2 is a Brønsted-Lowry acid, accepting a proton from the OH- ion.
B) the CO2 is a Lewis acid, accepting a proton from the OH- ion.
C) the OH- ion is a Brønsted-Lowry base, donating a proton to the CO2 molecule.
D) the OH- ion is a Lewis acid, accepting an electron pair from the CO2 molecule to form a coordinate covalent bond.
E) the OH- ion is a Lewis base, donating an electron pair to the CO2 molecule to form a coordinate covalent bond.
Diff: 2
Section: 15.4
46) Which pair of reactants will yield H2SO4 as one of its products?
A) SO2 + OH-
B) SO3 + OH-
C) SO2 + H2O
D) SO42- + OH-
E) SO3 + H2O
Diff: 2
Section: 15.4
47) Which pair of reactants will yield H2SO3 as one of its products?
A) SO2 + OH-
B) SO3 + OH-
C) SO2 + H2O
D) SO42- + OH-
E) SO3 + H2O
Diff: 2
Section: 15.5
48) Which 0.1 M solution would be the most acidic?
A) Al(NO3)3 (aq)
B) Ca(NO3)2 (aq)
C) KNO3 (aq)
D) Mg(NO3)2 (aq)
E) Zn(NO3)2 (aq)
Diff: 2
Section: 15.5
49) Which 0.1 M solution would be the most acidic?
A) ZnCl2 (aq)
B) CdCl2 (aq)
C) FeCl3 (aq)
D) AuCl3 (aq)
E) NaCl (aq)
Diff: 2
Section: 15.5
50) Which 0.1 M solution would be the least acidic?
A) ZnCl2 (aq)
B) CdCl2 (aq)
C) FeCl3 (aq)
D) NiCl2 (aq)
E) CuCl2 (aq)
Diff: 2
Section: 15.5
51) Five solutions were prepared by dissolving 0.00100 mole of each of the following compounds in enough water to make 1.000 liter of solution. Which one of these compounds would make the most acidic solution?
A) CO2
B) P4O6
C) P4O10
D) SO2
E) SO3
Diff: 2
Section: 15.5
52) Which of the following would form an acidic solution when added to water?
A) CO2 (g)
B) Na2O (s)
C) CaO (s)
D) H2O (g)
E) None of these
Diff: 1
Section: 15.5
53) Which of the following would form an acidic solution when added to water?
A) SO2 (g)
B) Na2O (s)
C) MgO (s)
D) H2O (g)
E) None of these
Diff: 1
Section: 15.5
54) Which of the following would form a basic solution when added to water?
A) CO2 (g)
B) Na2O (s)
C) SO3 (g)
D) H2O (g)
E) P4O6 (g)
Diff: 1
Section: 15.5
55) Which of the following would form a basic solution when added to water?
A) NO2 (g)
B) K2O (s)
C) SO3 (g)
D) H2O (g)
E) P4O6 (g)
Diff: 2
Section: 15.5
56) Which solution should be the least acidic?
A) Al(NO3)3 (aq)
B) Ga(NO3)3 (aq)
C) AgNO3 (aq)
D) Cu(NO3)2 (aq)
E) Zn(NO3)2 (aq)
Diff: 2
Section: 15.5
57) Which solution should be the most acidic?
A) Zn(NO3)2 (aq)
B) Cd(NO3)2 (aq)
C) Ga(NO3)3 (aq)
D) Hg(NO3)2 (aq)
E) Al(NO3)3 (aq)
Diff: 2
Section: 15.5
58) Which solution should be the least acidic?
A) Al(NO3)3 (aq)
B) Cd(NO3)2 (aq)
C) Ga(NO3)3 (aq)
D) KNO3 (aq)
E) Zn(NO3)2 (aq)
Diff: 2
Section: 15.5
59) Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution. Which one of these compounds would make the most acidic solution?
A) CO2
B) P4O6
C) P4O10
D) SO2
E) SO3
Diff: 2
Section: 15.5
60) Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution. Which one of these compounds would make the most acidic solution?
A) Na2O
B) BaO
C) Ga2O3
D) Al2O3
E) P4O6
Diff: 2
Section: 15.5
61) Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution. Which one of these compounds would make the most acidic solution?
A) Na2O
B) BaO
C) Ga2O3
D) Al2O3
E) P4O6
Diff: 2
Section: 15.5
62) The step in the sol-gel process that forms oxygen bridges while forming water molecules can be best classified as
A) an acid-base reaction.
B) sintering.
C) an evaporation process.
D) annealing.
E) metallurgy.
Diff: 2
Section: 15.6
63) Ceramic material made by the sol-gel process involve the reaction of
A) water and acids.
B) ethanol and water.
C) water and metal oxides.
D) acids and metal alkoxides.
E) water and metal alkoxides.
Diff: 2
Section: 15.6
64) What is the formula for the conjugate base of NH3(aq)?
Diff: 1
Section: 15.1
65) What is the formula for the conjugate acid of the OH-(aq) ion?
Diff: 1
Section: 15.1
66) What is the formula for the conjugate acid of the HCO3-(aq) ion?
Diff: 1
Section: 15.1
67) What is the formula for the conjugate base of the HCO3-(aq) ion?
Diff: 1
Section: 15.1
68) What is the formula for the conjugate base of HNO3(aq)?
Diff: 1
Section: 15.1
69) In the reaction, HClO3(aq) + N2H4(aq) ClO3-(aq) + N2H5+(aq), list the species that are conjugate acid-base pairs.
Diff: 1
Section: 15.1
70) In the reaction, HSO4-(aq) + OH-(aq) SO42-(aq) + H2O(l), list the species that are conjugate acid-base pairs.
Diff: 1
Section: 15.1
71) Explain why the anion HCO3- can be classified as an amphoteric species.
Diff: 1
Section: 15.1
72) The strongest base that can exist in aqueous solution is ________.
Diff: 1
Section: 15.2
73) The strongest acid that can exist in aqueous solution is ________.
Diff: 1
Section: 15.2
74) For the system
NH2OH(aq) + CH3NH3+(aq) CH3NH2(aq) + NH3OH+(aq)
the position of the equilibrium lies to the left. What is the strongest acid in this reaction?
Diff: 2
Section: 15.2
75) For the system
NH2OH(aq) + CH3NH3+(aq) CH3NH2(aq) + NH3OH+(aq)
the position of equilibrium lies to the left. What is the strongest base in this reaction?
Diff: 2
Section: 15.2
76) For the system
H3PO4(aq) + COOH-(aq) HCOOH(aq) + H2PO4-(aq)
the position of equilibrium lies to the right. What is the strongest acid in this reaction?
Diff: 2
Section: 15.2
77) For the system
H3PO4(aq) + COOH-(aq) HCOOH(aq) + H2PO4-(aq)
the position of equilibrium lies to the right. What is the strongest base in this reaction?
Diff: 2
Section: 15.2
78) Three oxoacids with the formulas shown are listed in order of decreasing acid strength:
HZO3 > HYO3 > HXO3
What is the formula for the strongest conjugate base of these acids?
Diff: 1
Section: 15.2
79) Three binary acids with the formulas shown are listed in order of decreasing acid strength:
HZ > HY > HX
What is the formula for the strongest conjugate base of these acids?
Diff: 1
Section: 15.2
80) Which one of the two species, H2Se or H3As, is the stronger Brønsted-Lowry acid?
Diff: 1
Section: 15.3
81) Which one of the two species, HF(aq) or HI(aq), is the weaker Brønsted-Lowry acid?
Diff: 1
Section: 15.3
82) Which one of the two species, H2S or HBr, is the stronger Brønsted-Lowry acid?
Diff: 1
Section: 15.3
83) The sulfide ion can react with the sulfur trioxide molecule to produce a thiosulfate ion, as shown below.
Which reactant is functioning as the Lewis base?
Diff: 1
Section: 15.3
84) Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.
Diff: 2
Section: 15.3
85) Selenium atoms can react with the sulfite ion to produce a selenosulfate ion, as shown below.
Which reactant is functioning as the Lewis base?
Diff: 2
Section: 15.4
86) The oxide ion can react with the carbon dioxide molecule to produce a carbonate ion, as shown be low.
Which reactant is functioning as the Lewis acid?
Diff: 2
Section: 15.4
87) Explain how NH3 can be both a Brønsted-Lowry base and a Lewis base, at the same time.
Diff: 1
Section: 15.4
88) Which solution is more acidic, AlCl3(aq) or InCl3(aq)?
Diff: 2
Section: 15.5
89) Would a solution of Al(NO3)3 be expected to form an acidic or basic solution in water?
Diff: 1
Section: 15.5
90) Would adding CaO to water be expected to form an acidic or basic solution?
Diff: 2
Section: 15.5
91) What effect would bubbling CO2 gas through a solution of distilled water have on the pH of a solution?
Diff: 2
Section: 15.5
92) What effect would bubbling SO3 gas through a solution of distilled water have on the pH of a solution?
Diff: 2
Section: 15.5
93) In order to make a ceramic material with uniform composition and high structural integrity, the ________ process is preferred over the traditional heating process, which causes sintering.
Diff: 2
Section: 15.6
94) Which process for making ceramics, sol-gel or sintering, results in a more uniform and stronger ceramic material?
Diff: 2
Section: 15.6
95) A xerogel is formed through the sol-gel process, from evaporation of the solvent from a wet gel. What will form if this zerogel is heated to high temperatures?
Diff: 1
Section: 15.6
96) The conjugate base of NH3 is NH4OH(aq).
Diff: 1
Section: 15.1
97) The conjugate acid of Cl-(aq) is HCl(aq).
Diff: 1
Section: 15.1
98) NH4Cl(aq) is one of the conjugate bases of Cl-(aq).
Diff: 1
Section: 15.1
99) The H2PO4-(aq) ion is amphiprotic in water solution.
Diff: 1
Section: 15.1
100) O2- ion is produced by the dissociation of MgO when it is dissolved in water. The O2- ion acts as a strong acid.
Diff: 1
Section: 15.1
101) All oxides are acidic when added to water.
Diff: 1
Section: 15.5
102) Most ceramics have high melting points and are brittle .
Diff: 1
Section: Chemistry Outside the Classroom 16.1
103) A useful property of most ceramics is that they are very hard and resistant to wear.
Diff: 1
Section: Chemistry Outside the Classroom 16.1
104) Explain why the strong acids HNO3 and HCl both have the same relative acid strength in water.
Diff: 2
Section: 15.2
105) Water can be purified by many ways, including by distillation. A student distills water in a lab experiment, in which she is going to work with pH and acid/base properties. She obtains a pH meter, and discovers that her distilled water sample has an acidic pH reading. Knowing that neutral water should be neither acidic nor basic, the student assumes that the pH meter is not calibrated, but after calibrating it again, it reads a similar pH. What could explain the student's observations?
Diff: 2
Section: 15.5
106) What is the difference between a xerogel and aerogel solid made using the sol-gel process?
Diff: 2
Section: 15.66
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