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Chapter 14- acid base equilibria

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originally chapter 16
Dawn G
Quiz by Dawn G, updated more than 1 year ago
Dawn G
Created by Dawn G almost 8 years ago
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Question 1

Question
According to the Arrhenius concept, an acid is a substance that __________.
Answer
  • A) is capable of donating one or more H+
  • B) causes an increase in the concentration of H+ in aqueous solutions
  • C) can accept a pair of electrons to form a coordinate covalent bond
  • D) reacts with the solvent to form the cation formed by autoionization of that solvent
  • E) tastes bitter

Question 2

Question
A BrØnsted-Lowry base is defined as a substance that __________.
Answer
  • 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

Question 3

Question
A BrØnsted-Lowry acid is defined as a substance that __________.
Answer
  • A) increases Ka 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

Question 4

Question
Which one of the following is a BrØnsted -Lowry acid?
Answer
  • A) (CH3)^3NH+
  • B) CH3COOH
  • C) HF
  • D) HNO2
  • E) all of the above

Question 5

Question
A substance that is capable of acting as both an acid and as a base is __________.
Answer
  • A) autosomal
  • B) conjugated
  • C) amphoteric
  • D) saturated
  • E) miscible

Question 6

Question
6) Which one of the following is a BrØnsted -Lowry base?
Answer
  • A) (CH3)3N
  • B) CH3COOH
  • C) HF
  • D) HNO2
  • E) none of the above

Question 7

Question
The molar concentration of hydronium ion in pure water at 25°C is __________.
Answer
  • A) 0.00
  • B) 1.0 × 10-7
  • C) 1.0 × 10-14
  • D) 1.00
  • E) 7.00

Question 8

Question
The magnitude of Kw indicates that __________.
Answer
  • A) water autoionizes very slowly
  • B) water autoionizes very quickly
  • C) water autoionizes only to a very small extent
  • D) the autoionization of water is exothermic

Question 9

Question
In basic solution, __________.
Answer
  • A) [H3O+] = [OH-]
  • B) [H3O+] > [OH-]
  • C) [H3O+] < [OH-]
  • D) [H3O+] = 0 M
  • E) [OH-] > 7.00

Question 10

Question
Which solution below has the highest concentration of hydroxide ions?
Answer
  • A) pH = 3.21
  • B) pH = 12.6
  • C) pH = 7.93
  • D) pH = 9.82
  • E) pH = 7.00

Question 11

Question
Which solution below has the highest concentration of hydronium ions?
Answer
  • A) pH = 3.21
  • B) pH = 12.6
  • C) pH = 7.93
  • D) pH = 9.82
  • E) pH = 7.00

Question 12

Question
Which one of the following statements regarding Kw is false?
Answer
  • A) pKw is 14.00 at 25°C
  • B) The value of Kw is always 1.0 × 10-14.
  • C) Kw changes with temperature.
  • D) The value of Kw shows that water is a weak acid.
  • E) Kw is known as the ion product of water.

Question 13

Question
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 __________.
Answer
  • A) H3O+ (aq)
  • B) OH- (aq) + H2 (g)
  • C) OH- (aq) + 2H+ (aq)
  • D) no reaction occurs
  • E) H2O2 (aq)

Question 14

Question
An aqueous solution contains 0.10 M NaOH. The solution is __________.
Answer
  • A) very dilute
  • B) highly colored
  • C) basic
  • D) neutral
  • E) acidic

Question 15

Question
Nitric acid is a strong acid. This means that __________.
Answer
  • A) aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH-(aq)
  • B) HNO3 does not dissociate at all when it is dissolved in water
  • C) HNO3 dissociates completely to H+(aq) and NO3-(aq) when it dissolves in water
  • D) HNO3 produces a gaseous product when it is neutralized
  • E) HNO3 cannot be neutralized by a weak base

Question 16

Question
Of the following acids, __________ is a strong acid.
Answer
  • A) HNO2
  • B) H2CO3
  • C) HBrO3
  • D) HClO
  • E) HF

Question 17

Question
Of the following acids, __________ is not a strong acid.
Answer
  • A) HNO2
  • B) H2SO4
  • C) HNO3
  • D) HClO4
  • E) HCl

Question 18

Question
Which one of the following is the weakest acid?
Answer
  • A) HF (Ka = 6.8 × 10-4)
  • B) HClO (Ka = 3.0 × 10-8)
  • C) HNO2 (Ka = 4.5 × 10-4)
  • D) HCN (Ka = 4.9 × 10-10)
  • E) Acetic acid (Ka = 1.8 × 10-5)

Question 19

Question
The 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?
Answer
  • A) 4.5 × 10-8
  • B) 14
  • C) 2.1 × 10-5
  • D) 0.14
  • E) 1.4 × 10-3

Question 20

Question
In which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization?
Answer
  • A) 0.01 M HC2H3O2 (Ka = 1.8 × 10-5)
  • B) 0.01 M HNO2 (Ka = 4.5 × 10-4)
  • C) 0.01 M HF (Ka = 6.8 × 10-4)
  • D) 0.01 M HClO (Ka = 3.0 × 10-8)
  • E) These will all exhibit the same percentage ionization.

Question 21

Question
In which of the following aqueous solutions does the weak acid exhibit the lowest percentage ionization?
Answer
  • A) 0.01 M HC2H3O2 (Ka = 1.8 × 10-5)
  • B) 0.01 M HNO2 (Ka = 4.5 × 10-4)
  • C) 0.01 M HF (Ka = 6.8 × 10-4)
  • D) 0.01 M HClO (Ka = 3.0 × 10-8)
  • E) These will all exhibit the same percentage ionization.

Question 22

Question
HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-?
Answer
  • A) HA (aq) + H2O (l) --> H2A+ (aq) + OH- (aq)
  • B) A- (aq) + H3O+ (aq) --> HA (aq) + H2O (l)
  • C) HA (aq) + OH- (aq) --> H2O (l) + H+ (aq)
  • D) A- (aq) + H2O (l) --> HA (aq) + OH- (aq)
  • E) A- (aq) + OH- (aq) --> HOA2- (aq)

Question 23

Question
Using the data in the table, which of the conjugate acids below is the weakest acid?
Image:
166ce573-29f4-4cae-8304-ac2ec251fdeb (image/png)
Answer
  • A) HClO
  • B) HCO3-
  • C) H2S
  • D) NH3CH3+
  • E) H2S and HClO

Question 24

Question
A 0.0035 M aqueous solution of a particular compound has pH = 2.46. The compound is __________.
Answer
  • A) a weak base
  • B) a weak acid
  • C) a strong acid
  • D) a strong base
  • E) a salt

Question 25

Question
Which of the following aqueous solutions has the lowest [OH-]?
Answer
  • A) a solution with a pH of 3.0
  • B) a 1 × 10-4 M solution of HNO3
  • C) a solution with a pOH of 12.0
  • D) pure water
  • E) a 1 × 10-3 M solution of NH4Cl

Question 26

Question
Which of the following aqueous solutions has the highest [OH-]?
Answer
  • A) a solution with a pH of 3.0
  • B) a 1 × 10-4 M solution of HNO3
  • C) a solution with a pOH of 12.0
  • D) pure water
  • E) a 1 × 10-3 M solution of NH4Cl

Question 27

Question
Of the following substances, an aqueous solution of __________ will form basic solutions. NH4Cl Cu(NO3)2 K2CO3 NaF
Answer
  • A) NH4Cl, Cu(NO3)2
  • B) K2CO3, NH4Cl
  • C) NaF only
  • D) NaF, K2CO3
  • E) NH4Cl only

Question 28

Question
A 0.1 M aqueous solution of __________ will have a pH of 7.0 at 25.0°C. NaOCl KCl NH4Cl Ca(OAc)2
Answer
  • A) NaOCl
  • B) KCl
  • C) NH4Cl
  • D) Ca(OAc)2
  • E) KCl and NH4Cl

Question 29

Question
Of the compounds below, a 0.1 M aqueous solution of __________ will have the highest pH.
Answer
  • A) KCN, Ka of HCN = 4.0 × 10-10
  • B) NH4NO3, Kb of NH3 = 1.8 × 10-5
  • C) NaOAc, Ka of HOAc = 1.8 × 10-5
  • D) NaClO, Ka of HClO = 3.2 × 10-8
  • E) NaHS, Kb of HS- = 1.8 × 10-7

Question 30

Question
A 0.1 M solution of __________ has a pH of 7.0.
Answer
  • A) Na2S
  • B) KF
  • C) NaNO3
  • D) NH4Cl
  • E) NaF

Question 31

Question
52) An aqueous solution of __________ will produce a basic solution.
Answer
  • A) NH4ClO4
  • B) KBr
  • C) NaCl
  • D) NaHSO4
  • E) Na2SO3

Question 32

Question
Of the following, which is the strongest acid?
Answer
  • A) HIO
  • B) HIO4
  • C) HIO2
  • D) HIO3
  • E) The acid strength of all of the above is the same.

Question 33

Question
Of the following, which is the weakest acid?
Answer
  • A) HIO
  • B) HIO4
  • C) HIO2
  • D) HIO3
  • E) The acid strength of all of the above is the same.

Question 34

Question
Which of the following acids will be the strongest?
Answer
  • A) H2SO4
  • B) HSO4-
  • C) H2SO3
  • D) H2SeO4
  • E) HSO3-

Question 35

Question
In the gas phase reaction below, NH3 is acting as a(n) __________ base but not as a(n) __________ base.
Image:
a1925955-ff09-4d49-a988-1de6ac4b0de4 (image/png)
Answer
  • A) Arrhenius, BrØnsted-Lowry
  • B) BrØnsted-Lowry, Lewis
  • C) Lewis, Arrhenius
  • D) Lewis, BrØnsted-Lowry
  • E) Arrhenius, Lewis

Question 36

Question
What is the conjugate acid of NH3?
Answer
  • A) NH3
  • B) NH2+
  • C) NH3+
  • D) NH4+
  • E) NH4OH

Question 37

Question
What is the conjugate acid of CO3-2?
Answer
  • A) CO2-2
  • B) HCO2-2
  • C) H2CO3
  • D) HCO3-
  • E) none of the above

Question 38

Question
The conjugate base of HSO4- is __________.
Answer
  • A) OH-
  • B) H2SO4
  • C) SO42-
  • D) HSO4+
  • E) H3SO4+

Question 39

Question
The conjugate base of H2PO4- is __________.
Answer
  • A) PO4-3
  • B) H2PO4
  • C) H3PO4
  • D) HPO4-2
  • E) none of the above

Question 40

Question
The conjugate acid of HSO4- is __________.
Answer
  • A) SO42-
  • B) H2SO4
  • C) HSO4+
  • D) H+
  • E) HSO3+

Question 41

Question
What is the conjugate base of OH-?
Answer
  • A) O2
  • B) O-
  • C) H2O
  • D) O2-
  • E) H3O+

Question 42

Question
What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion?
Answer
  • A) 8.400
  • B) 5.600
  • C) 9.000
  • D) 3.980
  • E) 7.000

Question 43

Question
What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion?
Answer
  • A) 8.40
  • B) 5.60
  • C) 9.00
  • D) 3.98
  • E) 7.00

Question 44

Question
What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion?
Answer
  • A) 8.40
  • B) 5.60
  • C) 9.00
  • D) 3.98
  • E) 7.00

Question 45

Question
Calculate the concentration (in M) of hydronium ions in a solution at 25.0°C with a pOH of 4.223.
Answer
  • A) 5.98 × 10-5
  • B) 1.67 × 10-10
  • C) 1.67 × 104
  • D) 5.99 × 10-19
  • E) 1.00 × 10-7

Question 46

Question
An aqueous solution contains 0.100 M NaOH at 25.0°C. The pH of the solution is __________.
Answer
  • A) 0.100
  • B) 1.00
  • C) 13.00
  • D) 7.00
  • E) -1.00

Question 47

Question
An aqueous solution contains 0.150 M HCl at 25.0°C. The pH of the solution is __________.
Answer
  • A) 0.150
  • B) 1.00
  • C) 13.00
  • D) 7.00
  • E) 0.82

Question 48

Question
HZ 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
Answer
  • A) 1.2 × 10-5
  • B) 6.9 × 10-9
  • C) 1.4 × 10-10
  • D) 9.9 × 10-2
  • E) 2.8 × 10-12

Question 49

Question
The 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?
Answer
  • A) 2.0 × 10-5
  • B) 1.8 × 10-4
  • C) 6.0 × 10-5
  • D) 3.5 × 10-4
  • E) none of the above

Question 50

Question
A 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 __________.
Answer
  • A) 3.0 × 10-5
  • B) 1.8 × 10-5
  • C) 7.1 × 10-9
  • D) 1.3 × 10-10
  • E) 3.3 × 104

Question 51

Question
The 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?
Answer
  • A) +2.45
  • B) -2.45
  • C) -9.22
  • D) +9.22
  • E) +4.61

Question 52

Question
The 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.
Answer
  • A) 4.53
  • B) 1.28
  • C) 1.86
  • D) 6.21
  • E) 1.93

Question 53

Question
The 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?
Answer
  • A) 1.82
  • B) 0.40
  • C) 2.51
  • D) 0.86
  • E) 0.13

Question 54

Question
The 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?
Answer
  • A) 2.0 × 10-9
  • B) 1.1 × 10-9
  • C) 6.0 × 10-5
  • D) 1.8 × 10-5
  • E) none of the above

Question 55

Question
The pH of a 0.30 M solution of a weak acid is 2.67. What is the Ka for this acid?
Answer
  • A) 2.1 × 10-4
  • B) 4.4 × 10-4
  • C) 1.5 × 10-4
  • D) 6.6 × 10-4
  • E) none of the above

Question 56

Question
Z- 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 __________.
Answer
  • A) 1.2 × 10-5
  • B) 6.9 × 10-9
  • C) 2.1 × 10-10
  • D) 9.9 × 10-2
  • E) 2.8 × 10-12

Question 57

Question
The acid-dissociation constant, Ka, for gallic acid is 4.57 × 10-3. What is the base-dissociation constant, Kb, for the gallate ion?
Answer
  • A) 4.57 × 10-3
  • B) 2.19 × 10-12
  • C) 5.43 × 10-5
  • D) 7.81 × 10-6
  • E) 2.19 × 102

Question 58

Question
The base-dissociation constant, Kb, for pyridine, C5H5N, is 1.4 × 10-9. The acid-dissociation constant, Ka, for the pyridinium ion, C5H5NH+, is __________.
Answer
  • A) 1.0 × 10-7
  • B) 1.4 × 10-23
  • C) 7.1 × 10-4
  • D) 1.4 × 10-5
  • E) 7.1 × 10-6

Question 59

Question
The Ka for HCN is 4.9 × 10-10. What is the value of Kb for CN-?
Answer
  • A) 2.0 × 10-5
  • B) 4.0 × 10-6
  • C) 4.9 × 104
  • D) 4.9 × 10-24
  • E) 2.0 × 109

Question 60

Question
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.
Answer
  • A) 3.5 × 10-12
  • B) 2.9 × 10-3
  • C) 3.1 × 10-12
  • D) 3.2 × 10-3
  • E) 11.46

Question 61

Question
Calculate the pH of a 0.100 M aqueous solution of NH3. The Kb of NH3 is 1.77 × 10-5.
Answer
  • A) 8.95
  • B) 11.12
  • C) 2.88
  • D) 12.12
  • E) 1.87

Question 62

Question
The 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)?
Answer
  • A) 11.11
  • B) 2.89
  • C) 1.3 × 10-3
  • D) 7.8 × 10-12
  • E) 3.9 × 10-11

Question 63

Question
Calculate the pH of 0.586 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 × 10-4.
Answer
  • A) 1.82
  • B) 12.18
  • C) 5.41
  • D) 8.59
  • E) 12.42

Question 64

Question
A 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.
Answer
  • A) 3.6 x 10-7
  • B) 0.045
  • C)
  • D)

Question 65

Question
What 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.
Answer
  • A) 8.87
  • B) 1.476 x 10-3
  • C) 2.87
  • D) 11.13

Question 66

Question
In the reaction BF3 + F- → BF4- BF3 acts as a Br∅nsted-Lowry acid.
Answer
  • True
  • False

Question 67

Question
An acid containing the COOH group is called a carbo-oxy acid.
Answer
  • True
  • False

Question 68

Question
A Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor.
Answer
  • True
  • False
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