Chapter 15 1 Which The Following Concerning The Relative Strength

subject Type Homework Help
subject Pages 9
subject Words 3145
subject Authors Darrell Ebbing, Steven D. Gammon

Unlock document.

This document is partially blurred.
Unlock all pages and 1 million more documents.
Get Access
page-pf1
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)
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 (H) per
mole of water formed.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
1, 2 and 3
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.
page-pf2
Test Bank General Chemistry, 10th edition 2
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
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
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 BrønstedLowry acid.
B)
H2SO3 is a BrønstedLowry acid, but not an Arrhenius acid.
C)
H2SO3 is neither an Arrhenius acid nor a BrønstedLowry acid.
D)
H2SO3 is an Arrhenius acid, but not a BrønstedLowry acid.
E)
H2SO3 is a Lewis base.
7. Which of the following statements is/are consistent with the Brønsted-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.
Brønsted-Lowry acid-base reactions are restricted to aqueous solutions.
page-pf3
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
8. Which are the BrønstedLowry 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
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
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.
page-pf4
11. What is the conjugate base of H2PO4(aq)?
A)
PO43
B)
H3O+
C)
HPO4−
D)
H3P
E)
H3PO4
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.
13. Which of the following species is amphiprotic in aqueous solution?
A)
CH3NH2
B)
H3O+
C)
NH4+
D)
F
E)
H2O
14. Which of the following species cannot act as a Lewis base?
A)
H2S
B)
S2
C)
Al3+
D)
SH
E)
H2O
page-pf5
15. Which of the following species cannot act as a Lewis base?
A)
H2O2
B)
OH
C)
O2
D)
H2O
E)
Be2+
16. Which of the following species cannot act as a Lewis base?
A)
NH3
B)
NH4+
C)
N3
D)
NH2
E)
NH2
17. Which of the following species cannot act as a Lewis acid?
A)
H+
B)
H
C)
K+
D)
Mg2+
E)
Al3+
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.
page-pf6
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.
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)
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 Brønsted-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
page-pf7
Test Bank General Chemistry, 10th edition 7
22. Which of the following species cannot act as a Lewis acid?
A)
BeCl2
B)
H+
C)
Ag+
D)
BF3
E)
NH4+
23. Which acid has the strongest conjugate base in aqueous solution?
A)
HF
B)
HNO3
C)
HClO4
D)
HI
E)
H2SO4
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
25. Which of the following acids has the weakest conjugate base in aqueous solution?
A)
CH3COOH
B)
HOCl
C)
HF
D)
HNO2
E)
HClO4
page-pf8
Test Bank General Chemistry, 10th edition 8
26. Which of the following acids has the strongest conjugate base?
A)
HClO
B)
HClO4
C)
HClO2
D)
HClO3
E)
HCl
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
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.
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)
page-pf9
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
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+.
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.
page-pfa
Test Bank General Chemistry, 10th edition 10
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
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.
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)
36. Which of the following is the strongest acid in aqueous solution?
A)
H3AsO4
B)
H3PO4
C)
H3PO3
D)
H3SbO4
E)
H3AsO3
page-pfb
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
38. Which of the following is the strongest acid?
A)
HClO2
B)
HCl
C)
HClO4
D)
HClO
E)
HClO3
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
page-pfc
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
41. The ionization constant of water at a temperature above 25°C is 1.7 1014. 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
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.

Trusted by Thousands of
Students

Here are what students say about us.

Copyright ©2022 All rights reserved. | CoursePaper is not sponsored or endorsed by any college or university.