Quiz
Chapter 14- acid base equilibria
Questions in this quiz (68)
1According to the Arrhenius concept, an acid is a substance that __________.
- AA) is capable of donating one or more H+
- BB) causes an increase in the concentration of H+ in aqueous solutions
- CC) can accept a pair of electrons to form a coordinate covalent bond
- DD) reacts with the solvent to form the cation formed by autoionization of that solvent
- EE) tastes bitter
2A BrØnsted-Lowry base is defined as a substance that __________.
- AA) increases [H+] when placed in H2O
- BB) decreases [H+] when placed in H2O
- CC) increases [OH-] when placed in H2O
- DD) acts as a proton acceptor
- EE) acts as a proton donor
3A BrØnsted-Lowry acid is defined as a substance that __________.
- AA) increases Ka when placed in H2O
- BB) decreases [H+] when placed in H2O
- CC) increases [OH-] when placed in H2O
- DD) acts as a proton acceptor
- EE) acts as a proton donor
4Which one of the following is a BrØnsted -Lowry acid?
- AA) (CH3)^3NH+
- BB) CH3COOH
- CC) HF
- DD) HNO2
- EE) all of the above
5A substance that is capable of acting as both an acid and as a base is __________.
- AA) autosomal
- BB) conjugated
- CC) amphoteric
- DD) saturated
- EE) miscible
66) Which one of the following is a BrØnsted -Lowry base?
- AA) (CH3)3N
- BB) CH3COOH
- CC) HF
- DD) HNO2
- EE) none of the above
7The molar concentration of hydronium ion in pure water at 25°C is __________.
- AA) 0.00
- BB) 1.0 × 10-7
- CC) 1.0 × 10-14
- DD) 1.00
- EE) 7.00
8The magnitude of Kw indicates that __________.
- AA) water autoionizes very slowly
- BB) water autoionizes very quickly
- CC) water autoionizes only to a very small extent
- DD) the autoionization of water is exothermic
9In basic solution, __________.
- AA) [H3O+] = [OH-]
- BB) [H3O+] > [OH-]
- CC) [H3O+] < [OH-]
- DD) [H3O+] = 0 M
- EE) [OH-] > 7.00
10Which solution below has the highest concentration of hydroxide ions?
- AA) pH = 3.21
- BB) pH = 12.6
- CC) pH = 7.93
- DD) pH = 9.82
- EE) pH = 7.00
11Which solution below has the highest concentration of hydronium ions?
- AA) pH = 3.21
- BB) pH = 12.6
- CC) pH = 7.93
- DD) pH = 9.82
- EE) pH = 7.00
12Which one of the following statements regarding Kw is false?
- AA) pKw is 14.00 at 25°C
- BB) The value of Kw is always 1.0 × 10-14.
- CC) Kw changes with temperature.
- DD) The value of Kw shows that water is a weak acid.
- EE) Kw is known as the ion product of water.
13 The hydride ion, H-, is a stronger base than the hydroxide ion, OH-. The product(s) of the reaction of hydride ion with water is/ are __________.
- AA) H3O+ (aq)
- BB) OH- (aq) + H2 (g)
- CC) OH- (aq) + 2H+ (aq)
- DD) no reaction occurs
- EE) H2O2 (aq)
14An aqueous solution contains 0.10 M NaOH. The solution is __________.
- AA) very dilute
- BB) highly colored
- CC) basic
- DD) neutral
- EE) acidic
15Nitric acid is a strong acid. This means that __________.
- AA) aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH-(aq)
- BB) HNO3 does not dissociate at all when it is dissolved in water
- CC) HNO3 dissociates completely to H+(aq) and NO3-(aq) when it dissolves in water
- DD) HNO3 produces a gaseous product when it is neutralized
- EE) HNO3 cannot be neutralized by a weak base
16Of the following acids, __________ is a strong acid.
- AA) HNO2
- BB) H2CO3
- CC) HBrO3
- DD) HClO
- EE) HF
17Of the following acids, __________ is not a strong acid.
- AA) HNO2
- BB) H2SO4
- CC) HNO3
- DD) HClO4
- EE) HCl
18Which one of the following is the weakest acid?
- AA) HF (Ka = 6.8 × 10-4)
- BB) HClO (Ka = 3.0 × 10-8)
- CC) HNO2 (Ka = 4.5 × 10-4)
- DD) HCN (Ka = 4.9 × 10-10)
- EE) Acetic acid (Ka = 1.8 × 10-5)
19The Ka of hypochlorous acid (HClO) is 3.0 × 10-8 at 25.0°C. What is the % ionization of hypochlorous acid in a 0.015 M aqueous solution of HClO at 25.0°C?
- AA) 4.5 × 10-8
- BB) 14
- CC) 2.1 × 10-5
- DD) 0.14
- EE) 1.4 × 10-3
20In which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization?
- AA) 0.01 M HC2H3O2 (Ka = 1.8 × 10-5)
- BB) 0.01 M HNO2 (Ka = 4.5 × 10-4)
- CC) 0.01 M HF (Ka = 6.8 × 10-4)
- DD) 0.01 M HClO (Ka = 3.0 × 10-8)
- EE) These will all exhibit the same percentage ionization.
21In which of the following aqueous solutions does the weak acid exhibit the lowest percentage ionization?
- AA) 0.01 M HC2H3O2 (Ka = 1.8 × 10-5)
- BB) 0.01 M HNO2 (Ka = 4.5 × 10-4)
- CC) 0.01 M HF (Ka = 6.8 × 10-4)
- DD) 0.01 M HClO (Ka = 3.0 × 10-8)
- EE) These will all exhibit the same percentage ionization.
22HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-?
- AA) HA (aq) + H2O (l) --> H2A+ (aq) + OH- (aq)
- BB) A- (aq) + H3O+ (aq) --> HA (aq) + H2O (l)
- CC) HA (aq) + OH- (aq) --> H2O (l) + H+ (aq)
- DD) A- (aq) + H2O (l) --> HA (aq) + OH- (aq)
- EE) A- (aq) + OH- (aq) --> HOA2- (aq)
23Using the data in the table, which of the conjugate acids below is the weakest acid?
- AA) HClO
- BB) HCO3-
- CC) H2S
- DD) NH3CH3+
- EE) H2S and HClO
24A 0.0035 M aqueous solution of a particular compound has pH = 2.46. The compound is __________.
- AA) a weak base
- BB) a weak acid
- CC) a strong acid
- DD) a strong base
- EE) a salt
25Which of the following aqueous solutions has the lowest [OH-]?
- AA) a solution with a pH of 3.0
- BB) a 1 × 10-4 M solution of HNO3
- CC) a solution with a pOH of 12.0
- DD) pure water
- EE) a 1 × 10-3 M solution of NH4Cl
26Which of the following aqueous solutions has the highest [OH-]?
- AA) a solution with a pH of 3.0
- BB) a 1 × 10-4 M solution of HNO3
- CC) a solution with a pOH of 12.0
- DD) pure water
- EE) a 1 × 10-3 M solution of NH4Cl
27Of the following substances, an aqueous solution of __________ will form basic solutions.
NH4Cl Cu(NO3)2 K2CO3 NaF- AA) NH4Cl, Cu(NO3)2
- BB) K2CO3, NH4Cl
- CC) NaF only
- DD) NaF, K2CO3
- EE) NH4Cl only
28A 0.1 M aqueous solution of __________ will have a pH of 7.0 at 25.0°C.
NaOCl KCl NH4Cl Ca(OAc)2- AA) NaOCl
- BB) KCl
- CC) NH4Cl
- DD) Ca(OAc)2
- EE) KCl and NH4Cl
29Of the compounds below, a 0.1 M aqueous solution of __________ will have the highest pH.
- AA) KCN, Ka of HCN = 4.0 × 10-10
- BB) NH4NO3, Kb of NH3 = 1.8 × 10-5
- CC) NaOAc, Ka of HOAc = 1.8 × 10-5
- DD) NaClO, Ka of HClO = 3.2 × 10-8
- EE) NaHS, Kb of HS- = 1.8 × 10-7
30A 0.1 M solution of __________ has a pH of 7.0.
- AA) Na2S
- BB) KF
- CC) NaNO3
- DD) NH4Cl
- EE) NaF
3152) An aqueous solution of __________ will produce a basic solution.
- AA) NH4ClO4
- BB) KBr
- CC) NaCl
- DD) NaHSO4
- EE) Na2SO3
32Of the following, which is the strongest acid?
- AA) HIO
- BB) HIO4
- CC) HIO2
- DD) HIO3
- EE) The acid strength of all of the above is the same.
33Of the following, which is the weakest acid?
- AA) HIO
- BB) HIO4
- CC) HIO2
- DD) HIO3
- EE) The acid strength of all of the above is the same.
34Which of the following acids will be the strongest?
- AA) H2SO4
- BB) HSO4-
- CC) H2SO3
- DD) H2SeO4
- EE) HSO3-
35In the gas phase reaction below, NH3 is acting as a(n) __________ base but not as a(n) __________ base.
- AA) Arrhenius, BrØnsted-Lowry
- BB) BrØnsted-Lowry, Lewis
- CC) Lewis, Arrhenius
- DD) Lewis, BrØnsted-Lowry
- EE) Arrhenius, Lewis
36What is the conjugate acid of NH3?
- AA) NH3
- BB) NH2+
- CC) NH3+
- DD) NH4+
- EE) NH4OH
37What is the conjugate acid of CO3-2?
- AA) CO2-2
- BB) HCO2-2
- CC) H2CO3
- DD) HCO3-
- EE) none of the above
38The conjugate base of HSO4- is __________.
- AA) OH-
- BB) H2SO4
- CC) SO42-
- DD) HSO4+
- EE) H3SO4+
39The conjugate base of H2PO4- is __________.
- AA) PO4-3
- BB) H2PO4
- CC) H3PO4
- DD) HPO4-2
- EE) none of the above
40The conjugate acid of HSO4- is __________.
- AA) SO42-
- BB) H2SO4
- CC) HSO4+
- DD) H+
- EE) HSO3+
41What is the conjugate base of OH-?
- AA) O2
- BB) O-
- CC) H2O
- DD) O2-
- EE) H3O+
42What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion?
- AA) 8.400
- BB) 5.600
- CC) 9.000
- DD) 3.980
- EE) 7.000
43What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion?
- AA) 8.40
- BB) 5.60
- CC) 9.00
- DD) 3.98
- EE) 7.00
44What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion?
- AA) 8.40
- BB) 5.60
- CC) 9.00
- DD) 3.98
- EE) 7.00
45Calculate the concentration (in M) of hydronium ions in a solution at 25.0°C with a pOH of 4.223.
- AA) 5.98 × 10-5
- BB) 1.67 × 10-10
- CC) 1.67 × 104
- DD) 5.99 × 10-19
- EE) 1.00 × 10-7
46An aqueous solution contains 0.100 M NaOH at 25.0°C. The pH of the solution is __________.
- AA) 0.100
- BB) 1.00
- CC) 13.00
- DD) 7.00
- EE) -1.00
47An aqueous solution contains 0.150 M HCl at 25.0°C. The pH of the solution is __________.
- AA) 0.150
- BB) 1.00
- CC) 13.00
- DD) 7.00
- EE) 0.82
48HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 4.93 at 25.0°C. The Ka of HZ is
- AA) 1.2 × 10-5
- BB) 6.9 × 10-9
- CC) 1.4 × 10-10
- DD) 9.9 × 10-2
- EE) 2.8 × 10-12
49The pH of a 0.60 M aqueous solution of formic acid, HCHO2, at 25.0°C is 1.98. What is the value of Ka for formic acid?
- AA) 2.0 × 10-5
- BB) 1.8 × 10-4
- CC) 6.0 × 10-5
- DD) 3.5 × 10-4
- EE) none of the above
50A 0.15 M aqueous solution of the weak acid HA at 25.0°C has a pH of 5.35. The value of Ka for HA is __________.
- AA) 3.0 × 10-5
- BB) 1.8 × 10-5
- CC) 7.1 × 10-9
- DD) 1.3 × 10-10
- EE) 3.3 × 104
51The Ka of hypochlorous acid (HClO) is 3.00 × 10-8. What is the pH at 25.0°C of an aqueous solution that is 0.0200 M in HClO?
- AA) +2.45
- BB) -2.45
- CC) -9.22
- DD) +9.22
- EE) +4.61
52The acid-dissociation constants of sulfurous acid (H2SO3) are Kal = 1.7 × 10-2 and
Ka2 = 6.4 × 10-8 at 25.0°C. Calculate the pH of a 0.163 M aqueous solution of sulfurous acid.- AA) 4.53
- BB) 1.28
- CC) 1.86
- DD) 6.21
- EE) 1.93
53The acid-dissociation constants of phosphoric acid (H2PO3) are Kal = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.2 × 10-13 at 25.0°C. What is the pH of a 2.5 M aqueous solution of phosphoric acid?
- AA) 1.82
- BB) 0.40
- CC) 2.51
- DD) 0.86
- EE) 0.13
54The pH of a 0.55 M aqueous solution ammonia, NH3, at 25.0°C is 11.50. What is the value of Kb for NH3?
- AA) 2.0 × 10-9
- BB) 1.1 × 10-9
- CC) 6.0 × 10-5
- DD) 1.8 × 10-5
- EE) none of the above
55The pH of a 0.30 M solution of a weak acid is 2.67. What is the Ka for this acid?
- AA) 2.1 × 10-4
- BB) 4.4 × 10-4
- CC) 1.5 × 10-4
- DD) 6.6 × 10-4
- EE) none of the above
56Z- is a weak base. An aqueous solution of NaZ is prepared by dissolving 0.350 mol of NaZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 8.93 at 25.0°C. The Kb of Z- is __________.
- AA) 1.2 × 10-5
- BB) 6.9 × 10-9
- CC) 2.1 × 10-10
- DD) 9.9 × 10-2
- EE) 2.8 × 10-12
57The acid-dissociation constant, Ka, for gallic acid is 4.57 × 10-3. What is the base-dissociation constant, Kb, for the gallate ion?
- AA) 4.57 × 10-3
- BB) 2.19 × 10-12
- CC) 5.43 × 10-5
- DD) 7.81 × 10-6
- EE) 2.19 × 102
58The base-dissociation constant, Kb, for pyridine, C5H5N, is 1.4 × 10-9. The acid-dissociation constant, Ka, for the pyridinium ion, C5H5NH+, is __________.
- AA) 1.0 × 10-7
- BB) 1.4 × 10-23
- CC) 7.1 × 10-4
- DD) 1.4 × 10-5
- EE) 7.1 × 10-6
59The Ka for HCN is 4.9 × 10-10. What is the value of Kb for CN-?
- AA) 2.0 × 10-5
- BB) 4.0 × 10-6
- CC) 4.9 × 104
- DD) 4.9 × 10-24
- EE) 2.0 × 109
60 The base-dissociation constant of ethylamine (C2H5NH2) is 6.4 × 10-4 at 25.0 °C. The [H+] in
a 1.6 × 10-2 M solution of ethylamine is __________ M.- AA) 3.5 × 10-12
- BB) 2.9 × 10-3
- CC) 3.1 × 10-12
- DD) 3.2 × 10-3
- EE) 11.46
61Calculate the pH of a 0.100 M aqueous solution of NH3. The Kb of NH3 is 1.77 × 10-5.
- AA) 8.95
- BB) 11.12
- CC) 2.88
- DD) 12.12
- EE) 1.87
62The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?
- AA) 11.11
- BB) 2.89
- CC) 1.3 × 10-3
- DD) 7.8 × 10-12
- EE) 3.9 × 10-11
63Calculate the pH of 0.586 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 × 10-4.
- AA) 1.82
- BB) 12.18
- CC) 5.41
- DD) 8.59
- EE) 12.42
64A solution of acetic acid is 2.0% dissociated at 25.0°C. What was the original concentration (in M) of the acetic acid solution? The Ka at 25.0 °C for acetic acid is 1.8 × 10-5.
- AA) 3.6 x 10-7
- BB) 0.045
- CC)
- DD)
65What is the pH of a sodium acetate solution prepared by adding 0.820 grams of sodium acetate to 100.0 ml of water at 25.0°C? The Ka at 25.0°C for acetic acid is 1.8 × 10-5.
- AA) 8.87
- BB) 1.476 x 10-3
- CC) 2.87
- DD) 11.13
66In the reaction
BF3 + F- → BF4-
BF3 acts as a Br∅nsted-Lowry acid.- ATrue
- BFalse
67An acid containing the COOH group is called a carbo-oxy acid.
- ATrue
- BFalse
68A Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor.
- ATrue
- BFalse
Information
- Description
- originally chapter 16
- Author
- Dawn G
- Language
- English
- Views
- 544
- Tags
- Rating
- No ratings yet Rate this quiz