General Chemistry Ebbing Gammon Ch. 15
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Transcript of General Chemistry Ebbing Gammon Ch. 15
Chapter 15 - Acids and Bases
1.Which of the following reactions is not readily explained by the Arrhenius concept of acids and bases?
A)
HCl(g) + NH3(g) NH4Cl(s)
B)
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
C)
HClO4(aq) + H2O(l) H3O+(aq) + ClO4-(aq)
D)
HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2-(aq)
E)
H3O+(aq) + OH-(aq) 2H2O(l)
ANS:APTS:1DIF:easyREF:15.1
OBJ:Define acid and base according to the Arrhenius concept.
TOP:acidsandbases | acid-baseconceptsNOT:REVISED
2.Which of the following statements is/are consistent with the Arrhenius concept of acids and bases?
1.
An Arrhenius acid will increase the concentration of hydronium ion in an aqueous or nonaqueous solvent.
2.
All Arrhenius acids are strong electrolytes in water.
3.
All strong acid-strong base reactions have the same heat of reaction (DH) per mole of water formed.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
1, 2 and 3
ANS:CPTS:1DIF:easyREF:15.1
OBJ:Define acid and base according to the Arrhenius concept.
TOP:acidsandbases | acid-baseconcepts
3.Which of the following statements does not describe a characteristic of an Arrhenius acid?
A)
An Arrhenius acid reacts with an Arrhenius base to produce a salt.
B)
An Arrhenius acid turns red litmus blue.
C)
An Arrhenius acid is an electrolyte.
D)
An Arrhenius acid reacts with CaCO3 to produce CO2.
E)
An Arrhenius acid tastes sour.
ANS:BPTS:1DIF:easyREF:15.1
OBJ:Define acid and base according to the Arrhenius concept.
TOP:acidsandbases | acid-baseconcepts
KEY:ArrheniusconceptofacidsandbasesMSC:general chemistry
4.Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?
A)
Br
B)
HF
C)
H2SO3
D)
H3O+
E)
HNO3
ANS:APTS:1DIF:easyREF:15.1
OBJ:Define acid and base according to the Arrhenius concept.
TOP:acidsandbases | acid-baseconcepts
5.Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?
A)
CHCl3
B)
HNO3
C)
H2SO4
D)
H3O+
E)
HClO4
ANS:APTS:1DIF:easyREF:15.1
OBJ:Define acid and base according to the Arrhenius concept.
TOP:acidsandbases | acid-baseconcepts
6.Which of the following statements is correct concerning the neutralization of sulfurous acid by a strong base?
2OH(aq) + H2SO3(aq) SO32(aq) + 2H2O(l)
A)
H2SO3 is both an Arrhenius acid and a BrnstedLowry acid.
B)
H2SO3 is a BrnstedLowry acid, but not an Arrhenius acid.
C)
H2SO3 is neither an Arrhenius acid nor a BrnstedLowry acid.
D)
H2SO3 is an Arrhenius acid, but not a BrnstedLowry acid.
E)
H2SO3 is a Lewis base.
ANS:APTS:1DIF:easyREF:15.2
OBJ:Define acid and base according to the BrnstedLowry concept.
TOP:acidsandbases | acid-baseconcepts
KEY:Brnsted-Lowry concept of acids and basesMSC:general chemistry
7.Which of the following statements is/are consistent with the Brnsted-Lowry concept of acids and bases?
1.
A conjugate acid-base pair may differ by only one proton.
2.
A base is defined as a hydroxide ion donor.
3.
Brnsted-Lowry acid-base reactions are restricted to aqueous solutions.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
ANS:APTS:1DIF:easyREF:15.2
OBJ:Define acid and base according to the BrnstedLowry concept.
TOP:acidsandbases | acid-baseconcepts
8.Which are the BrnstedLowry bases in the following equilibrium?
CH3COO(aq) + H2O(l) CH3COOH(aq) + OH(aq)
A)
CH3COO and OH
B)
H2O and OH
C)
H2O, CH3COOH, and OH
D)
CH3COO and CH3COOH
E)
H2O and CH3COOH
ANS:APTS:1DIF:easyREF:15.2
OBJ:Identify acid and base species. (Example 15.1)
TOP:acidsandbases | acid-baseconcepts
KEY:Brnsted-Lowry concept of acids and basesMSC:general chemistry
9.Which of the following pairs of species is not a conjugate acidbase pair?
A)
HOCl, OCl
B)
HNO2, NO2+
C)
O2, OH
D)
HSO4, SO42
E)
H2CO3, HCO3
ANS:BPTS:1DIF:easyREF:15.2
OBJ:Identify acid and base species. (Example 15.1)
TOP:acidsandbases | acid-baseconcepts
KEY:Brnsted-Lowry concept of acids and basesMSC:general chemistry
10.What is a conjugate acidbase pair for the following equilibrium?
H2O(l) + HPO42(aq) H2PO4(aq) + OH(aq)
A)
H2O is an acid and HPO42 is its conjugate base.
B)
HPO42 is an acid and OH is its conjugate base.
C)
H2O is an acid and OH is its conjugate base.
D)
HPO42 is an acid and H2PO4 is its conjugate base.
E)
HPO42 is an acid and H2O is its conjugate base.
ANS:CPTS:1DIF:moderateREF:15.2
OBJ:Identify acid and base species. (Example 15.1)
TOP:acidsandbases | acid-baseconcepts
KEY:Brnsted-Lowry concept of acids and basesMSC:general chemistry
11.What is the conjugate base of H2PO4(aq)?
A)
PO43
B)
H3O+
C)
HPO42-
D)
H3P
E)
H3PO4
ANS:CPTS:1DIF:moderateREF:15.2
OBJ:Identify acid and base species. (Example 15.1)
TOP:acidsandbases | acid-baseconcepts
12.What is a conjugate acidbase pair for the following equilibrium?
H2O(l) + NH4+(aq) NH3(aq) + H3O+(aq)
A)
H2O is an acid and NH3 is its conjugate base.
B)
H2O is an acid and H3O+ is its conjugate base.
C)
NH4+ is an acid and NH3 is its conjugate base.
D)
H2O is a base and NH3 is its conjugate acid.
E)
H2O is a base and NH4+ is its conjugate acid.
ANS:CPTS:1DIF:moderateREF:15.2
OBJ:Identify acid and base species. (Example 15.1)
TOP:acidsandbases | acid-baseconcepts
KEY:Brnsted-Lowry concept of acids and basesMSC:general chemistry
13.Which of the following species is amphiprotic in aqueous solution?
A)
CH3NH2
B)
H3O+
C)
NH4+
D)
F-
E)
H2O
ANS:EPTS:1DIF:moderateREF:15.2
OBJ:Define amphiprotic species.TOP:acidsandbases | acid-baseconcepts
14.Which of the following species cannot act as a Lewis base?
A)
H2S
B)
S2
C)
Al3+
D)
SH
E)
H2O
ANS:CPTS:1DIF:easyREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
15.Which of the following species cannot act as a Lewis base?
A)
H2O2
B)
OH
C)
O2
D)
H2O
E)
Be2+
ANS:EPTS:1DIF:easyREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
16.Which of the following species cannot act as a Lewis base?
A)
NH3
B)
NH4+
C)
N3
D)
NH2
E)
NH2
ANS:BPTS:1DIF:easyREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
17.Which of the following species cannot act as a Lewis acid?
A)
H+
B)
H
C)
K+
D)
Mg2+
E)
Al3+
ANS:BPTS:1DIF:easyREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
18.In the reaction
CuO(s) + SO2(g) CuSO3(s),
A)
O2 acts as a Lewis base and SO2 acts as a Lewis acid.
B)
O2 acts as a Lewis base and Cu2+ acts as a Lewis acid.
C)
CuO is the Lewis acid and CuSO3 is its conjugate base.
D)
SO2 is the Lewis acid and CuSO3 is its conjugate base.
E)
Cu2+ acts as a Lewis acid and SO32 acts as a Lewis base.
ANS:APTS:1DIF:easyREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
19.Consider the following reaction:
AgBr(s) + 2CN(aq) Ag(CN)2(aq) + Br(aq)
The species that are acting as a Lewis acid and Lewis base, respectively, are
A)
Br and CN.
B)
Ag+ and CN.
C)
AgBr and Ag(CN)2.
D)
Ag(CN)2 and Ag+.
E)
Ag+ and Br.
ANS:BPTS:1DIF:easyREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
20.Which of the following is not an example of an acidbase reaction?
A)
Al(OH)3(s) + 3H+(aq) Al3+(aq) + 3H2O(l)
B)
C2H6(g) C2H4(g) + H2(g)
C)
MgO(s) + CO2(g) MgCO3(s)
D)
Al(OH)3(s) + OH(aq) Al(OH)4(aq)
E)
CN(aq) + H2O(l) HCN(aq) + OH(aq)
ANS:BPTS:1DIF:moderateREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
21.Which of the following is/are an appropriate classification of the reaction given below?
KOH(aq) + CO2(g) KHCO3(aq)
1.
The above reaction may be classified as an Arrhenius acid-base reaction.
2.
The above reaction may be classified as a Brnsted-Lowry acid-base reaction.
3.
The above reaction may be classified as a Lewis acid-base reaction.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
none
ANS:CPTS:1DIF:moderateREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
22.Which of the following species cannot act as a Lewis acid?
A)
BeCl2
B)
H+
C)
Ag+
D)
BF3
E)
NH4+
ANS:EPTS:1DIF:moderateREF:15.3
OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)
TOP:acidsandbases | acid-baseconcepts
KEY:LewisconceptofacidsandbasesMSC:general chemistry
23.Which acid has the strongest conjugate base in aqueous solution?
A)
HF
B)
HNO3
C)
HClO4
D)
HI
E)
H2SO4
ANS:APTS:1DIF:easyREF:15.4
OBJ:Understand the relationship between the strength of an acid and that of its conjugate base.TOP:acidsandbases | acidandbasestrength
24.Which of the following concerning the relative strength of acids and bases is/are correct?
1.
As the acidity of the acid decreases, the basicity of the conjugate base increases.
2.
The hydronium ion is the strongest acid that can be found in aqueous solution.
3.
All acids classified as strong acids in aqueous solution have the same acidity in a more acidic solvent like acetic acid.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
ANS:DPTS:1DIF:easyREF:15.4
OBJ:Understand the relationship between the strength of an acid and that of its conjugate base.TOP:acidsandbases | acidandbasestrength
25.Which of the following acids has the weakest conjugate base in aqueous solution?
A)
CH3COOH
B)
HOCl
C)
HF
D)
HNO2
E)
HClO4
ANS:EPTS:1DIF:easyREF:15.4
OBJ:Understand the relationship between the strength of an acid and that of its conjugate base.TOP:acidsandbases | acidandbasestrength
26.Which of the following acids has the strongest conjugate base?
A)
HClO
B)
HClO4
C)
HClO2
D)
HClO3
E)
HCl
ANS:APTS:1DIF:easyREF:15.5
OBJ:Understand the relationship between the strength of an acid and that of its conjugate base.TOP:acidsandbases | acidandbasestrength
KEY:relativestrengthsofacidsandbasesMSC:general chemistry
27.The acid strength decreases in the series HBr > HSO4 > CH3COOH > HCN > HCO3. Which of the following is the strongest base?
A)
SO42
B)
CO32
C)
CH3COO
D)
Br
E)
CN
ANS:BPTS:1DIF:easyREF:15.4
OBJ:Understand the relationship between the strength of an acid and that of its conjugate base.TOP:acidsandbases | acidandbasestrength
KEY:relativestrengthsofacidsandbasesMSC:general chemistry
28.What is the leveling effect?
A)
All bases are 100% ionized in water.
B)
All acids are 100% ionized in solvents other than water.
C)
All strong acids are 100% ionized in water.
D)
An acid with a higher concentration in water has a lower pH than an acid with a lower concentration in water.
E)
A base with a higher concentration in water has a lower pH than a base with a lower concentration in water.
ANS:CPTS:1DIF:easyREF:15.4
OBJ:Understand the relationship between the strength of an acid and that of its conjugate base.TOP:acidsandbases | acidandbasestrength
KEY:relativestrengthsofacidsandbasesMSC:general chemistry
29.Which of the following reactions is not product-favored?
A)
NaOH(aq) Na+(aq) + OH(aq)
B)
NH3(aq) + H2O(l) NH4+(aq) + OH(aq)
C)
HClO4(aq) + H2O(l) H3O+(aq) + ClO4(aq)
D)
HCl(aq) + H2O(l) H3O+(aq) + Cl(aq)
E)
H2SO4(aq) + H2O(l) H3O+(aq) + HSO4(aq)
ANS:BPTS:1DIF:easyREF:15.4
OBJ:Decide whether reactants or products are favored in an acidbase reaction. (Example 15.3)TOP:acidsandbases | acidandbasestrength
KEY:relativestrengthsofacidsandbasesMSC:general chemistry
30.Given equal concentrations of the following acids, which exhibits the greatest amount of ionization in water?
A)
nitrous acid
B)
chlorous acid
C)
ascorbic acid
D)
hydrobromic acid
E)
citric acid
ANS:DPTS:1DIF:easyREF:15.4
OBJ:Decide whether reactants or products are favored in an acidbase reaction. (Example 15.3)TOP:acidsandbases | acidandbasestrength
31.Which of the following statements is true concerning an aqueous solution of the weak base NH3?
A)
OH is a stronger base than NH3.
B)
OH is a stronger acid than NH4+.
C)
NH4+ is a stronger acid than H3O+.
D)
NH3 is a weaker base than H2O.
E)
H2O is a stronger acid than H3O+.
ANS:APTS:1DIF:easyREF:15.4
OBJ:Decide whether reactants or products are favored in an acidbase reaction. (Example 15.3)TOP:acidsandbases | acidandbasestrength
KEY:relativestrengthsofacidsandbasesMSC:general chemistry
32.Which of the following statements is true concerning an aqueous solution of the strong acid HBr?
A)
Br is a stronger acid than H2O.
B)
Br is a stronger base than OH.
C)
H3O+ is a stronger acid than HBr.
D)
H2O is a stronger acid than HBr.
E)
H2O is a stronger base than Br.
ANS:EPTS:1DIF:easyREF:15.4
OBJ:Decide whether reactants or products are favored in an acidbase reaction. (Example 15.3)TOP:acidsandbases | acidandbasestrength
KEY:relativestrengthsofacidsandbasesMSC:general chemistry
33.Rank the following in order of decreasing acid strength in aqueous solution: HCl, HOCl, HOBr, HOI.
A)
HCl > HClO > HBrO > HIO
B)
HIO > HBrO > HClO > HCl
C)
HCl > HIO > HBrO > HClO
D)
HClO > HCl > HBrO > HIO
E)
HClO > HBrO > HCl > HIO
ANS:APTS:1DIF:easyREF:15.5
OBJ:Understand the periodic trends in the strengths of the binary acids HX.
TOP:acidsandbases | acidandbasestrength
34.Which of the following statements is incorrect?
A)
One reason why HCl is a stronger acid than HF is that the HCl bond is weaker than the HF bond.
B)
F is a stronger base than Cl.
C)
One reason why HCl is a stronger acid than HF is that Cl is more electronegative than F.
D)
The acids HBr and HI both appear equally strong in water.
E)
One reason why HCl is a stronger acid than HF is that Cl has a larger atomic radius than F.
ANS:CPTS:1DIF:easyREF:15.5
OBJ:Understand the periodic trends in the strengths of the binary acids HX.
TOP:acidsandbases | acidandbasestrength
KEY:molecularstructureandacidstrength
MSC:general chemistry
35.Which solution has the highest pH?
A)
0.10 M HBr(aq)
B)
0.10 M HI(aq)
C)
0.10 M HF(aq)
D)
0.10 M HCl(aq)
E)
0.10 M HClO4(aq)
ANS:CPTS:1DIF:moderateREF:15.6
OBJ:Understand the periodic trends in the strengths of the binary acids HX.
TOP:acidsandbases | acidandbasestrength
KEY:molecularstructureandacidstrength
MSC:general chemistry
36.Which of the following is the strongest acid in aqueous solution?
A)
H3AsO4
B)
H3PO4
C)
H3PO3
D)
H3SbO4
E)
H3AsO3
ANS:BPTS:1DIF:easyREF:15.5
OBJ:Understand the rules for determining the relative strengths of oxoacids.
TOP:acidsandbases | acidandbasestrength
KEY:molecularstructureandacidstrength
MSC:general chemistry
37.Rank the following in order of decreasing acid strength: H2O, H2S, H2Se, H2Te
A)
H2Te > H2Se > H2S > H2O
B)
H2O > H2S > H2Se > H2Te
C)
H2Se > H2Te > H2S > H2O
D)
H2S > H2Te > H2Se > H2O
E)
H2Se > H2S > H2Te > H2O
ANS:APTS:1DIF:easyREF:15.5
OBJ:Understand the rules for determining the relative strengths of oxoacids.
TOP:acidsandbases | acidandbasestrength
38.Which of the following is the strongest acid?
A)
HClO2
B)
HCl
C)
HClO4
D)
HClO
E)
HClO3
ANS:CPTS:1DIF:easyREF:15.5
OBJ:Understand the rules for determining the relative strengths of oxoacids.
TOP:acidsandbases | acidandbasestrength
KEY:molecularstructureandacidstrength
MSC:general chemistry
39.Which of the following solutes, dissolved in 1.0 kg of water, would be expected to provide the fewest particles and to freeze at the highest temperature?
A)
0.10 mol HClO
B)
0.10 mol HClO3
C)
0.10 mol HClO2
D)
0.10 mol HClO4
E)
0.10 mol HCl
ANS:APTS:1DIF:difficultREF:15.5
OBJ:Understand the rules for determining the relative strengths of oxoacids.
TOP:acidsandbases | acidandbasestrength
KEY:molecularstructureandacidstrength
MSC:general chemistry
40.Rank H3PO4, H2PO4, and HPO42 in order of increasing acid strength.
A)
HPO42 < H2PO4 < H3PO4
B)
H2PO4 < HPO42 < H3PO4
C)
H2PO4 < H3PO4 < HPO42
D)
HPO42 < H3PO4 < H2PO4
E)
H3PO4 < H2PO4 < HPO42
ANS:APTS:1DIF:easyREF:15.5
OBJ:Understand the relative acid strengths of a polyprotic acid and its anions.
TOP:acidsandbases | acidandbasestrength
KEY:molecularstructureandacidstrength
MSC:general chemistry
41.The ionization constant of water at a temperature above 25C is 1.71014. What is the pH of pure water at this temperature?
2H2O(l) H3O+(aq) + OH(aq)
A)
7.88
B)
5.68
C)
6.88
D)
13.85
E)
7.00
ANS:CPTS:1DIF:moderateREF:15.8
OBJ:Define self-ionization (or autoionization).
TOP:acidsandbases | self-ionizationofwaterandpH
KEY:self-ionizationofwaterMSC:general chemistry
42.The autoionization of water, as represented by the equation below, is known to be endothermic. Which of the following correctly states what occurs as the temperature of water is raised?
H2O(l) + H2O(l) H3O+(aq) + OH(aq)
A)
The pH of the water decreases, and the water becomes more acidic.
B)
The pH of the water decreases, and the water remains neutral.
C)
The pH of the water increases, and the water remains neutral.
D)
The pH of the water does not change, and the water remains neutral.
E)
The pH of the water increases, and the water becomes more acidic.
ANS:BPTS:1DIF:difficultREF:15.6
OBJ:Define self-ionization (or autoionization).
TOP:acidsandbases | self-ionizationofwaterandpH
KEY:self-ionizationofwaterMSC:general chemistry
43.The equilibrium constant for the autonionization of water (shown below) increases with increasing temperature, from 1.01 x10-14 at 25C to 5.31 x10-14 at 50C.
H2O(l) + H2O(l) H3O+(aq) + OH(aq)
Which of the following statements is consistent with this behaviour?
A)
The autoionization of water is an endothermic reaction.
B)
The autoionization of water is an exothermic reaction.
C)
The hydronium ion concentration at equilibrium increases with increasing temperature.
D)
The hydronium ion concentration at equilibrium decreases with increasing temperature.
E)
Both A and C.
ANS:EPTS:1DIF:difficultREF:15.6
OBJ:Define self-ionization (or autoionization).
TOP:acidsandbases | self-ionizationofwaterandpH
44.What is the equilibrium concentration of amide ion (NH2) in liquid ammonia at 25C? ("am"=dissolvedinammonia)
2NH3(l) NH4+(am) + NH2(am); Kc = 1.8 1024 at 25C
A)
2.6 1012 M
B)
3.6 1024 M
C)
1.3 1012 M
D)
1.8 1024 M
E)
9.0 1025 M
ANS:CPTS:1DIF:moderateREF:15.6
OBJ:Define the ion-product constant for water.
TOP:acidsandbases | self-ionizationofwaterandpHMSC:general chemistry
45.What is the hydronium-ion concentration in a solution formed by combining 750mL of 0.10MNaOH with 250mL of 0.30MHCl?
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)
A)
0.075 M
B)
1.7 1013 M
C)
1.0 107 M
D)
0.30 M
E)
0.10 M
ANS:CPTS:1DIF:difficultREF:15.6
OBJ:Define the ion-product constant for water.
TOP:acidsandbases | self-ionizationofwaterandpH
KEY:self-ionizationofwaterMSC:general chemistry
46.At 20C, the ion-product constant of water, Kw, is
6.8810
15
. What is the pH of pure water at 20C?
A)
7.000
B)
6.501
C)
7.181
D)
7.081
E)
none of these
ANS:DPTS:1DIF:moderateREF:15.8
OBJ:Define the ion-product constant for water.
TOP:acidsandbases | self-ionizationofwaterandpH
47.The concentration of H3O+ in a solution is 7104 M at 25C. What is its hydroxide-ion concentration?
A)
7 104 M
B)
1 1010 M
C)
2 1010 M
D)
3 1010 M
E)
1 1011 M
ANS:EPTS:1DIF:easyREF:15.7
OBJ:Calculate the concentrations of H3O+ and OH in solutions of a strong acid or base. (Example 15.4)TOP:acidsandbases | solutionsofastrongacidorbase
MSC:general chemistry
48.At 25C a solution has a hydroxide-ion concentration of 4.94105 M. What is its hydronium-ion concentration?
A)
4.94 1019 M
B)
1.00 107 M
C)
1.00 1014 M
D)
4.94 105 M
E)
2.02 1010 M
ANS:EPTS:1DIF:easyREF:15.7
OBJ:Calculate the concentrations of H3O+ and OH in solutions of a strong acid or base. (Example 15.4)TOP:acidsandbases | solutionsofastrongacidorbase
MSC:general chemistry
49.What is the hydronium-ion concentration of a 0.0087MLiOH solution?
A)
1.1 1012 M
B)
8.7 103 M
C)
1.0 1014 M
D)
1.0 107 M
E)
8.7 1017 M
ANS:APTS:1DIF:easyREF:15.7
OBJ:Calculate the concentrations of H3O+ and OH in solutions of a strong acid or base. (Example 15.4)TOP:acidsandbases | solutionsofastrongacidorbase
MSC:general chemistry
50.What is the hydronium-ion concentration of a 0.0038MBa(OH)2 solution?
A)
7.6 103 M
B)
3.8 103 M
C)
1.3 1012 M
D)
2.6 1012 M
E)
1.0 107 M
ANS:CPTS:1DIF:moderateREF:15.7
OBJ:Calculate the concentrations of H3O+ and OH in solutions of a strong acid or base. (Example 15.4)TOP:acidsandbases | solutionsofastrongacidorbase
MSC:general chemistry
51.Which of the following expressions is not equivalent to pH?
A)
log [H+(aq)]
B)
C)
14.0 pOH
D)
E)
log Kw
ANS:EPTS:1DIF:easyREF:15.8
OBJ:Define pH.TOP:acidsandbases | solutionsofastrongacidorbase
KEY:pHofasolutionMSC:general chemistry
52.A solution in which the pH is 1.5 would be described as
A)
neutral.
B)
very acidic.
C)
slightly basic.
D)
slightly acidic.
E)
very basic.
ANS:BPTS:1DIF:easyREF:15.8
OBJ:Define pH.TOP:acidsandbases | solutionsofastrongacidorbase
KEY:pHofasolutionMSC:general chemistry
53.A solution has a hydroxide-ion concentration of 0.0030M. What is the pOH of the solution?
A)
11.48
B)
2.52
C)
7.00
D)
8.19
E)
5.81
ANS:BPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
54.What is the pH of a 0.051 M HClO4 solution?
A)
15.29
B)
2.98
C)
12.71
D)
1.29
E)
11.02
ANS:DPTS:1DIF:easyREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
55.What is the pOH of a 0.044 M HI solution?
A)
3.12
B)
12.64
C)
10.88
D)
15.36
E)
1.36
ANS:BPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
56.What is the pH of the final solution when 25 mL of 0.025 M HCl has been added to 35mL of 0.040MHCl at 25C?
A)
3.22
B)
1.78
C)
1.47
D)
2.69
E)
3.39
ANS:CPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
57.What is the pH of a 0.0042 M hydrochloric acid solution?
A)
5.47
B)
11.62
C)
7.00
D)
8.53
E)
2.38
ANS:EPTS:1DIF:easyREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
58.The hydronium-ion concentration of a solution is 2.5106 M. What is the pH of the solution?
A)
6.81
B)
3.77
C)
2.00
D)
5.60
E)
10.60
ANS:DPTS:1DIF:easyREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
59.At 25C, what is the pH of a 10.0 M HBr solution?
A)
1.000
B)
0.000
C)
10.000
D)
1.000
E)
14.000
ANS:DPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
60.Which aqueous solution has the lowest pH?
A)
0.30 M HCl
B)
0.30 M NaOH
C)
0.30 M NH3
D)
0.30 M Ba(OH)2
E)
0.30 M H2SO4
ANS:EPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofaweakacidorbase
61.What pH should a solution have if its pH is about the same as that of vinegar?
A)
about 8
B)
about 11
C)
about 1
D)
about 6
E)
about 3
ANS:EPTS:1DIF:easyREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofaweakacidorbaseMSC:general chemistry
62.A solution has a pH value of 3.76. What is the pOH for this solution?
A)
7.00
B)
3.72
C)
3.76
D)
1.74
E)
10.24
ANS:EPTS:1DIF:easyREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
63.Which solution has the highest pH?
A)
0.1 M Ba(OH)2
B)
0.1 M CH3COOH
C)
0.1 M HCl
D)
0.1 M NH3
E)
0.1 M NaOH
ANS:APTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
64.The pOH of a solution is 5.22. What is the pH of the solution?
A)
5.22
B)
8.78
C)
6.03
D)
7.00
E)
2.68
ANS:BPTS:1DIF:easyREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
65.What is the pH of a 0.0035 M Ba(OH)2 solution?
A)
9.04
B)
11.54
C)
2.46
D)
11.85
E)
2.15
ANS:DPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
66.What is the pOH of a 0.0055 M Ba(OH)2 solution?
A)
9.49
B)
11.74
C)
12.04
D)
1.96
E)
2.26
ANS:DPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
67.A solution has a hydronium-ion concentration of 0.0082 M. What is its pOH?
A)
2.09
B)
16.09
C)
9.20
D)
4.80
E)
11.91
ANS:EPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
68.A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?
A)
15.37
B)
12.63
C)
17.15
D)
7.00
E)
1.37
ANS:BPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
69.What is the pOH of a 0.065 M HNO3 solution?
A)
12.81
B)
11.27
C)
15.19
D)
1.19
E)
2.73
ANS:APTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
70.What is the pH of a 0.0086 M LiOH solution?
A)
9.24
B)
11.93
C)
2.07
D)
4.76
E)
16.07
ANS:BPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
71.What is the pOH of a 0.0092 M CsOH solution?
A)
2.04
B)
16.04
C)
9.31
D)
4.69
E)
11.96
ANS:APTS:1DIF:easyREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
72.What is the pH of a solution prepared by dissolving 0.739 g of NaOH(s) in 4.50L of water?
A)
1.733
B)
12.267
C)
7.000
D)
11.613
E)
2.387
ANS:DPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
73.What is the pOH of a solution prepared by dissolving 0.287 g of KOH(s) in 7.00L of water?
A)
10.864
B)
3.136
C)
2.291
D)
11.709
E)
7.000
ANS:BPTS:1DIF:moderateREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
74.What is the pH of a solution prepared by dissolving 0.365 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 6.00L? (R=0.0821Latm/(Kmol))
A)
2.566
B)
11.434
C)
1.788
D)
7.000
E)
12.212
ANS:APTS:1DIF:difficultREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
75.What is the pOH of a solution prepared by dissolving 0.465 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 4.50 L? (R=0.0821Latm/(Kmol))
A)
12.317
B)
7.000
C)
1.683
D)
11.664
E)
2.336
ANS:DPTS:1DIF:difficultREF:15.8
OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
76.Which of the following solutions has the highest hydroxide-ion concentration?
A)
0.1 M HCl
B)
a solution with pH = 5
C)
0.1 M H2SO4
D)
pure water
E)
a solution with pOH = 12
ANS:DPTS:1DIF:moderateREF:15.8
OBJ:Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP:acidsandbases | solutionsofastrongacidorbase
77.A solution has a pH of 10.20 at 25C. What is the hydroxide-ion concentration at 25C?
A)
3.8 M
B)
2.2 102 M
C)
1.6 104 M
D)
6.3 1011 M
E)
1.0 107 M
ANS:CPTS:1DIF:moderateREF:15.8
OBJ:Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
78.A solution has a pOH of 5.36. What is its hydroxide-ion concentration?
A)
1.8 104 M
B)
5.4 M
C)
2.3 109 M
D)
4.4 106 M
E)
4.7 103 M
ANS:DPTS:1DIF:easyREF:15.8
OBJ:Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
79.The pOH of a solution is 5.06. What is its hydronium-ion concentration?
A)
1.1 105 M
B)
1.1 109 M
C)
8.7 106 M
D)
5.06 M
E)
6.3 103 M
ANS:BPTS:1DIF:moderateREF:15.8
OBJ:Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
80.The pH of a solution of a strong base is 10.27 at 25C. What is its hydronium-ion concentration?
A)
2.9 103 M
B)
1.9 104 M
C)
1.4 104 M
D)
5.4 1011 M
E)
1.4 102 M
ANS:DPTS:1DIF:easyREF:15.8
OBJ:Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
81.What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.15MHCl with 300.mL of 0.090MNaOH at 25C?
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
A)
1.7 1013 M
B)
0.090 M
C)
1.7 1012 M
D)
0.054 M
E)
1.0 107 M
ANS:CPTS:1DIF:moderateREF:15.8
OBJ:Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry
82.Which solution would cause blue litmus to turn red?
A)
a solution of pH 10
B)
a solution of 0.01 M NH3
C)
a solution of pOH 4
D)
a solution of 0.005 M CH3COOH
E)
a solution of 0.10 M NaOH
ANS:DPTS:1DIF:moderateREF:15.8
OBJ:Describe the determination of pH by a pH meter and by acidbase indicators.
TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution
MSC:general chemistry