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CHM 112 > Chpt 11 Iconic Equilibra > Flashcards

Chpt 11 Iconic Equilibra Flashcards

1
Q

QUESTION

A

OPTION 1

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2
Q
  1. What is the main characteristic of electrolytes?
A

a) They dissociate into charged particles.

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3
Q
  1. Which of the following is an example of a strong electrolyte?
A

a) NaCl

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4
Q
  1. The Van’t Hoff factor (i) is a correction factor necessary for which type of solutions?
A

a) Electrolyte solutions

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5
Q
  1. What is the degree of dissociation of an electrolyte?
A

a) The fraction of dissociation of the electrolyte

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6
Q
  1. The Van’t Hoff factor (i) for a dissociating electrolyte is always:
A

a) Greater than 1

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7
Q
  1. What does the percent degree of dissociation refer to?
A

a) The percentage of solute that dissociates into ions.

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8
Q
  1. For a given solution, what determines the degree of dissociation?
A

a) Nature of the solute

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9
Q
  1. The degree of dissociation of acetic acid in a 1 M solution is:
A

a) 0.4%

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10
Q
  1. What effect does decreasing the concentration of a solute have on its degree of dissociation?
A

a) The degree of dissociation increases.

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11
Q
  1. Which of the following solutes is considered a weak electrolyte?
A

a) CH₃COOH

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12
Q
  1. Which factor primarily determines the dissociation of an electrolyte in a solution?
A

a) Nature of the solute and solvent

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13
Q
  1. What is the effect of temperature on the dissociation of electrolytes?
A

a) It may either increase or decrease dissociation depending on the substance.

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14
Q
  1. What is the difference between dissociation and ionization?
A

a) Ionization is the dissociation of particles into charged ions.

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15
Q
  1. Which of the following is an example of dissociation without ionization?
A

a) PCl₅ → PCl₄⁺ + Cl⁻

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16
Q
  1. In concentrated solutions, ionization can be incomplete due to the formation of:
A

a) Ion pairs

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17
Q
  1. Which of the following solutions would have no electrical conductivity?
A

a) A solution containing only ion pairs

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18
Q
  1. The ionization equilibrium constant is represented as:
A

a) Kₐ

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19
Q
  1. For weak electrolytes, the ionic concentrations are:
A

a) Low

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20
Q
  1. What is the main assumption for calculating the ionization equilibrium constant for weak electrolytes?
A

a) The activity coefficient is close to unity.

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21
Q
  1. The solubility of a sparingly soluble salt is calculated based on:
A

a) Its solubility product (Ksp)

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22
Q
  1. What type of equilibrium exists in a saturated solution of a sparingly soluble salt?
A

a) Heterogeneous equilibrium

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23
Q
  1. For a salt with the formula AB, the equilibrium for its solubility is represented by:
A

a) AB(s) ⇌ A⁺(aq) + B⁻(aq)

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24
Q
  1. What is the solubility product (Ksp) used to describe?
A

a) The equilibrium between a solid salt and its ions in solution

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25
Q
  1. In a solution of a 1:1 salt like NaCl, the solubility product (Ksp) is equal to:
A

a) S²

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26
Q
  1. For a salt with the formula FeCl₂, what would be the relationship between the solubility (S) and the ions produced?
A

a) The concentration of Fe²⁺ ions is S, and the concentration of Cl⁻ ions is 2S.

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27
Q
  1. The solubility of a slightly soluble salt can be affected by:
A

a) The presence of common ions

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28
Q
  1. In which case will a salt’s solubility decrease due to the common ion effect?
A

a) When the concentration of one of the ions already present in the salt increases.

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29
Q
  1. The concentration of ions in a saturated solution of a slightly soluble salt is:
A

a) Directly proportional to the solubility

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30
Q
  1. Which factor does NOT significantly affect the solubility of a salt?
A

a) The size of the ions

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31
Q
  1. What is the solubility of a salt with a Ksp value of 1.6 × 10⁻⁹, assuming it dissociates into two ions?
A

a) 4.0 × 10⁻⁵ mol/L

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32
Q
  1. What is the common ion effect in solubility?
A

A) The solubility of an ionic salt decreases when a common ion is added.

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33
Q
  1. What happens when chloride ion is added to a saturated solution of silver chloride?
A

A) The equilibrium shifts to the left, and some silver chloride precipitates.

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34
Q
  1. Which of the following is a correct description of the solubility product (Ksp)?
A

A) Ksp is the product of the concentrations of the ions in a saturated solution.

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35
Q
  1. What occurs when the ionic product exceeds Ksp?
A

A) Precipitation of the salt occurs.

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36
Q
  1. How does the solubility product principle apply to the precipitation of salts?
A

A) Precipitation occurs when the ionic product exceeds Ksp.

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37
Q
  1. Which of the following substances will reduce the solubility of silver chromate (Ag2CrO4) in solution?
A

A) The addition of a common ion like Ag+.

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38
Q
  1. What is the primary purpose of the solubility product principle?
A

A) To predict the formation of a precipitate in a solution.

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39
Q
  1. In a solution of Ag2CrO4, what happens if NaCl is added?
A

A) The solubility of Ag2CrO4 decreases due to the common ion effect.

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40
Q
  1. What happens when NH3 is added to a saturated solution of AgCl?
A

A) The solubility of AgCl increases due to the formation of a complex ion.

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41
Q
  1. How is the concentration of an ion affected when the solubility product is exceeded?
A

A) The concentration of the ion will decrease as the salt precipitates.

42
Q
  1. What is the effect of adding NaNO3 to a saturated solution of AgCl?
A

A) The solubility of AgCl will decrease due to the common ion effect.

43
Q
  1. What does the solubility product constant (Ksp) indicate in an equilibrium system?
A

A) It represents the maximum concentration of ions that can exist in a saturated solution.

44
Q
  1. What is the solubility of silver chromate (Ag2CrO4) in pure water at 25°C if Ksp = 9.0 × 10^-12?
A

A) 6.92 × 10^-4 mol/dm^3.

45
Q
  1. Which factor increases the solubility of a slightly soluble salt?
A

A) Addition of a complexing agent like NH3.

46
Q
  1. What happens to the solubility of ZnS in the presence of a common ion like Zn2+?
A

A) The solubility decreases.

47
Q
  1. What is the effect of the presence of NaOH in a solution of H2SO4 (sulfuric acid)?
A

A) NaOH neutralizes the acid and forms a salt.

48
Q
  1. What is the correct dissociation of H2SO4 in water?
A

A) H2SO4 → H+ + HSO4^- → 2H+ + SO4^2-.

49
Q
  1. What is the definition of a polyprotic acid?
A

A) An acid that can donate more than one proton per molecule.

50
Q
  1. What is the amphoteric behavior of water?
A

A) Water can act as both an acid and a base.

51
Q
  1. What is the ionization constant of H2SO4 in its first dissociation step?
A

A) k1 > k2 > k3.

52
Q
  1. Which of the following is true about weak acids in water?
A

A) Weak acids are only slightly ionized in water.

53
Q
  1. How does NH3 act as a base in water?
A

A) NH3 accepts a proton to form NH4+.

54
Q
  1. What is the result when CO2 dissolves in water?
A

A) It forms H2CO3, which increases the H+ concentration.

55
Q
  1. Which of the following compounds acts as an acid in water according to the Brønsted-Lowry definition?
A

A) HCl.

56
Q
  1. What is the Brønsted-Lowry definition of an acid?
A

A) A substance that donates a proton.

57
Q
  1. What is a conjugate base?
A

A) The species formed when an acid donates a proton.

58
Q
  1. What type of reaction occurs when an acid and a base react together according to Brønsted-Lowry?
A

A) A proton transfer (neutralization).

59
Q
  1. How does NH4Cl act in water?
A

A) It forms NH4+ and Cl-, making the solution acidic.

60
Q
  1. What is the main feature of a Lewis acid-base reaction?
A

A) A Lewis acid accepts an electron pair from a Lewis base.

61
Q
  1. In the reaction between Na2S and H2O, what type of solution is formed?
A

A) A basic solution due to the production of OH- ions.

62
Q
  1. According to the Lewis definition of acids and bases, an acid is a substance that:
A

a) Accepts an electron pair

63
Q
  1. What is the ion product constant (Kw) of water at 25°C?
A

a) 1.0 x 10^-14

64
Q
  1. A solution with a pH of 3 is:
A

a) Acidic

65
Q
  1. The pH scale was introduced by:
A

a) Sorensen

66
Q
  1. What is the pOH of a solution with an OH- concentration of 1 x 10^-4 M?
A

a) 10

67
Q
  1. Which of the following acids has the smallest ionization constant (Ka)?
A

a) HCN

68
Q
  1. A weak acid, such as acetic acid, dissociates in water to form:
A

a) H+ and Ac- ions

69
Q
  1. The formula for calculating pH is:
A

a) -log[H+]

70
Q
  1. Which of the following is a characteristic of a strong acid?
A

a) High dissociation in water

71
Q
  1. The dissociation constant for a weak base is known as:
A

a) Kb

72
Q
  1. The relationship between pH and pOH is:
A

a) pH + pOH = 14

73
Q
  1. In a neutral solution at 25°C, the concentration of H+ ions is:
A

a) 1 x 10^-7 M

74
Q
  1. Which of the following bases has the largest ionization constant (Kb)?
A

a) Pyridine

75
Q
  1. The ionization of a weak acid is described by:
A

a) Ka = [H+][Ac-] / [HAc]

76
Q
  1. What is the pH of a 0.010 M HCl solution?
A

a) 2

77
Q
  1. Which of the following compounds is considered a weak base?
A

a) NH3

78
Q
  1. The degree of ionization (α) of a weak acid is defined as:
A

a) x / C

79
Q
  1. The concentration of OH- ions in a neutral solution is:
A

a) 1 x 10^-7 M

80
Q
  1. The pKa of an acid is related to:
A

a) Its strength

81
Q
  1. What is the relationship between pKa and acid strength?
A

a) The smaller the pKa, the stronger the acid

82
Q
  1. A solution of NaOH in water increases the concentration of:
A

a) OH- ions

83
Q
  1. For a weak acid with a very small Ka value, the degree of ionization is:
A

a) Very small

84
Q
  1. What happens when a base is added to water?
A

a) OH- concentration increases

85
Q
  1. The degree of ionization is represented by:
A

a) α

86
Q
  1. The concentration of H+ ions in a solution with pH = 9 is:
A

a) 1 x 10^-9 M

87
Q
  1. Which of the following is true for a neutral solution at 25°C?
A

a) [H+] = [OH-]

88
Q
  1. In an acid-base titration, an indicator is used to:
A

a) Detect the end point of the reaction

89
Q
  1. What is the pH of a solution with an H+ concentration of 1 x 10^-8 M?
A

a) 8

90
Q
  1. The ionization constant for water is represented by:
A

a) Kw

91
Q
  1. Which of the following is true about a weak acid solution?
A

a) It has a small Ka value

92
Q
  1. What is the ionization constant (K) for a weak acid, as described in the text?
A

a) K = 85 x 10^-9

93
Q
  1. What is the degree of ionization of hydrogen acetate in a solution?
A

a) 1.8 x 10^-4

94
Q
  1. Which of the following indicators changes color in the pH range 3.1 to 4.4?
A

a) Methyl orange

95
Q
  1. What is the acid color of methyl orange in an acidic solution?
A

a) Red

96
Q
  1. Which of the following is the correct equilibrium for a weak acid indicator in water?
A

a) HIn ⇌ H+ + In-

97
Q
  1. What causes the shift in the equilibrium of an indicator in an acidic solution?
A

a) Excess H+ ions suppress ionization

98
Q
  1. In an alkaline medium, what happens to the ionization of an indicator?
A

a) It increases

99
Q
  1. What type of acid-base indicator is typically used for titrations involving strong acids and weak bases?
A

a) Methyl orange

100
Q
  1. What is the effect of salt hydrolysis on the pH of a solution?
A

a) It can produce a weak acid or weak base

101
Q
  1. In a titration of a strong acid with a weak base, the equivalence point will be: a) Acidic
A

b) Neutral

CHM 112 (7 decks)

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