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CHEM 1110 > Chapter 10 > Flashcards

Chapter 10 Flashcards

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1
Q

A _______ is any substance that can donate a proton (H+ ion) to some other substance. In other words, this is a proton (H+ ion) donor.

A

Bronsted-Lowry acid

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2
Q

A _______ base is any substance that can accept a proton (H+ ion) from some other substance. In other words, this is a proton (H+ ion) acceptor.

A

Bronsted-Lowry base

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3
Q

A substance that can accept a proton from another species is a _______.

A

Bronsted-Lowry base

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4
Q

The hydrogen ion is also called a ______.

A

proton

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5
Q

An _____ is a hydrogen-containing compound that in water, produces hydrogen ions (H+).

A

Arrhenius acid

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6
Q

An ______ is a hydroxide-containing compound that in water, produces hydroxide ions (OH-).

A

Arrhenius base

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7
Q

Arrhenius bases are also called _______.

A

hydroxide bases

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8
Q

_____ is the production of hydrogen ions from a molecular compound that has been dissolved in a solution.

A

Ionization

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9
Q

______ is the production of ions from an ionic compound that has been dissolved in a solution.

A

Dissociation

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10
Q

_______ is the process in which individual positive and negative ions are produced from a molecular compound that is dissolved in a solution.

A

Ionization

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11
Q

_______ is the process in which individual positive and negative ions are released from an ionic compound that is dissolved in a solution.

A

Dissociation

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12
Q

_____ and ______ are coupled together in a chemical reaction. Proton donation from an acid can only take place when there is an acceptor base present. It is impossible to have a Bronsted-Lowry acid without a Bronsted-Lowry base.

A

Acids and bases

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13
Q

The real acidic species in an aqueous solution is not the proton (H+ ion) but the ______. The formation of this is due to the strong attraction between the hydrogen ion of the acid and the polar water molecule. The type of bond formed is called a _________ bond because both bonding electrons are supplied by the oxygen atom.

A 
hydronium ion (H3O+);
a coordinate covalent bond
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14
Q

The bond between a water molecule and a proton (when a hydronium ion is formed) is called _________.

A

a coordinate covalent bond

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15
Q

TRUE or FALSE:
The bonding electrons between a water molecule and a proton (when a hydronium ion is formed) are furnished equally. In other words, one electron is contributed by the oxygen atom and one electron is contributed by the proton.

A

False - protons don’t have electrons to contribute

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16
Q 
TRUE or FALSE:
Hydroiodic acid (HI) can be classified correctly as either an Arrhenius acid or a Bronsted-Lowry acid.
A

True

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17
Q

TRUE or FALSE:

Ammonia (NH3) can be classified correctly as either Arrhenius base or a Bronsted-Lowry base.

A

False - it is a Bronsted-Lowry base but not an Arrhenius base

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18
Q

A ______ is two species, one an acid and one a base, that differ from each other through the loss of gain of a proton (H+ ion).

A

conjugate acid-base pair

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19
Q

A _______ is the species formed when a proton (H+ ion) is added to a Bronsted-Lowry base.

A

conjugate acid

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20
Q

A _______ is the species that remains when a proton (H+ ion) is removed from a Bronsted-Lowry acid.

A

conjugate base

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21
Q

A ______ is a substance that can either lose or accept a proton and thus can function as either a Bronsted-Lowry acid or Bronsted-Lowry base.

A

amphiprotic substance

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22
Q

Depending on the other species present in the reaction, _____ can act as either a Bronsted-Lowry base or a Bronsted-Lowry acid. Any ion or molecule that can behave as either an acid or a base is said to be amphiprotic.

A

water

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23
Q

A ______ is a molecule that can either accept or donate a proton. Therefore, it can act as either a Bronsted-Lowry acid or a Bronsted-Lowry base – depending on the given conditions of the solution.

A

amphiprotic species

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24
Q

The _____ mixture of a Bronsted-Lowry acid-base reaction always contains 2 acids and 2 bases.

A

equilibrium

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25
Q

The acid in a conjugate pair always has ______ H atom and is one unit more ______ that the conjugate base.

A

one more;

positive

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26
Q

The base in the conjugate pair always has ____ H atom and is one unit more _____ that the conjugate acid.

A

one less;

negative

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27
Q

A _____ is an acid that can donate only one proton (H+ ion) in an acid-base reaction.

A

monoprotic acid

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28
Q

A ______ is an acid that can donate 2 protons (H+ ions) in an acid-base reaction.

A

diprotic acid

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29
Q

A ______ is an acid that can donate 3 protons (H+ ions) in an acid-base reaction.

A

triprotic acid

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30
Q

A base that can accept 2 protons is a ______.

A

diprotic base

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31
Q

TRUE or FALSE:

The species HPO4- and H3PO4 are conjugates of each other.

A

False - they differ by more than one proton

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32
Q

Diprotic and triprotic acids are both examples of _______.

A

polyprotic acids

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33
Q

A ______ is an acid that can donate 2 or more protons (H+ ions) in an acid-base reaction.

A

polyprotic acid

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34
Q

What are the 3 rules in chemical formula writing that convey whether or not a hydrogen-containing substance is an acid?

A
  1. If a molecule is an acid, start the chemical formula with H.
  2. If the molecule is not an acid, do not begin the chemical formula with H.
  3. If a molecule is an acid but not every hydrogen atom is involved in the acid-base reaction, only the acidic hydrogen atom(s) are listed first and separately from the non-acidic hydrogen atoms.
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35
Q

The transfer of the protons from ______ is always stepwise – that is, __ proton is transferred at a time in a sequential way.

A

polyprotic acids;

1

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36
Q

When a double arrow for a system at equilibrium have unequal lengths, the longer arrow denotes the direction in which the _________ lies.

A

equilibrium

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37
Q

A ____ is a base that can accept 2 or more protons (H+ ions) in an acid-base reaction.

A

polyprotic base

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38
Q

A ______ is an acid that reacts completely with water to produce solutions in which 100% (or nearly 100%) of all acid molecules have transferred their proton (H+ ion) to water.

A

strong acid

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39
Q

A ______ is an acid that reacts incompletely with water to produce solutions in which only a small percentage of all acid molecules have transferred their proton (H+ ion) to water.

A

weak acid

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40
Q

What are the 6 strong acids?

A 
hydrochloric acid;
hydrobromic acid;
hydroiodic acid;
nitric acid;
sulfuric acid;
perchloric acid
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41
Q

What is the chemical symbol for hydrochloric acid?

A

HCl

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42
Q

What is the chemical symbol for hydrobromic acid?

A

HBr

43
Q

What is the chemical symbol for hydroiodic acid?

A

HI

44
Q

What is the chemical symbol for nitric acid?

A

HNO3

45
Q

What is the chemical symbol for sulfuric acid?

A

H2SO4

46
Q

What is the chemical symbol for perchloric acid?

A

HClO4

47
Q

____ and ______ relate to the extent of proton transfer not the concentration of the acid or base.

A

strong and weak

48
Q

____ and _____ make reference to the relative concentration of an acid or base.

A

concentrated or dilute

49
Q

__________ are experimentally determined values that are used to quantify the strength of acids and bases.

A

Dissociation constants

50
Q

An ________ is an expression that describes the equilibrium that exists between a weak acid (HA) and its conjugate base (A-). The symbol Ka is used to represent this.

A

acid dissociation constant

51
Q

A ______ is an expression that describes the equilibrium that exists between a weak base (B) and it’s conjugate acid (BH+). The symbol Kb is used to represent this.

A

base dissociation constant

52
Q

Why does the Kb expression not include the concentration of water?

A

Equilibrium expressions do not include water because the concentration of water is constant.

53
Q

A very important fact you need to remember about polyprotic acids is that the second proton is not as ______ transferred as the first.

A

easily

54
Q

For polyprotic bases, the ____ proton is not as easily gained as the first.

A

second

55
Q

A _____ is any ionic compound that contains either a metal or a polyatomic ion as the cation and a nonmetal or a polyatomic ion as the anion.

A

salt

56
Q

The exception to the salt rule is ____; ionic compounds containing this are bases, not salts.

A

OH-

57
Q

There are no weak or strong salts because all salts completely ______.

A

dissociate

58
Q

A salt is an ______ compound that contains _________.

A

ionic;

metal or polyatomic cation and nonmetal or polyatomic anion.

59
Q

TRUE or FALSE:

Salts with limited solubility in water only partially dissolve. Such salts are also called weak salts.

A

False - there are no such things as weak salts.

60
Q

TRUE or FALSE:

Sr(OH)2 is a salt.

A

False - Sr is a metallic ion but OH- is the one polyatomic ion that is the exception to the salt rule. Sr(OH)2 is a base.

61
Q

A reaction between as acid and a hydroxide base is called a _____ and the products of this reaction are always a salt and water.

A

neutralization reaction

62
Q

A ______ is a reaction in which two reactants exchange parts with each other to form two different products.

A

double-replacement reaction

63
Q

______ happens every time an acid and a base react completely with each other, regardless of whether the acid and base are strong or weak.

A

Neutralization

64
Q

The process wherein water molecules react with each other to form ions is called _______.

A

self-ionization

65
Q

TRUE or FALSE:

Water is a molecular compound that can react with itself to form ions.

A

True - this process is called self-ionization

66
Q

TRUE or FALSE:

Water can act as a proton acceptor (base).

A

True - water is amphiprotic so it can act as a base or an acid.

67
Q

The equilibrium constant (Keq) for the self-ionization of water is called the _______ (or _______). It is denoted by the symbol Kw and has a numerical value of 1.00 x 10^-14.

A

ion product constant for water (or self-ionization constant)

68
Q

A solution with equal concentrations of the H3O+ and the OH- ions is a ______.

A

neutral solution

69
Q

A solution with a higher concentration of the H3)+ than the OH- ions is a ______.

A

acidic solution

70
Q

A solution with a higher concentration of the OH- than the H3O+ ions is a _____ (aka ______).

A

basic solution (alkaline solution)

71
Q

A ____ is defined as the negative logarithm of a number or -log

A

p function

72
Q

The ____ is the negative logarithm (-log) of the molar hydronium ion concentration, [H3O+], in an aqueous solution.

A

pH

73
Q

A mathematical operation that takes the negative of the logarithm of a number is called _____.

A

p function

74
Q

The ____ is the negative logarithm of the molar hydroxide ion concentration.

A

pOH

75
Q

When taking the _____ of a number, keep as many digits past the decimal as there are significant figures in the original number.

A

logarithm

76
Q

When taking the ____ of a number, keep as many digits (in total) as there are past the decimal point in the original number.

A

antilog

77
Q

The ____ is the negative logarithm of the molar hydroxide ion concentration, [OH-], in an aqueous solution.

A

pOH

78
Q

_____ are species that form ions and whose aqueous solutions conduct electricity.

A

Electrolytes

79
Q

_______ are species that do not form ions and whose aqueous solutions do not conduct electricity.

A

Nonelectrolytes

80
Q

________ are species that completely dissociate or ionize into ions in aqueous solutions.

A

Strong electrolytes

81
Q

_______ are species that dissociate or ionize only partially into ions in aqueous solutions.

A

Weak electrolytes

82
Q

A reaction between water and salt that produces either hydronium or hydroxide ions is referred to as ________.

A

hydrolysis reaction

83
Q

TRUE or FALSE:

The Ph of an aqueous solution to which acid has been added will be above 7.

A

False

84
Q

When a salt is added to water and no hydronium or hydroxide is formed, the pH of the resulting solution will be ______.

A

neutral

85
Q

The reaction of the anion from a salt with water to produce the conjugate acid of the anion and hydroxide ion is called _______.

A

basic hydrolysis

86
Q

The reaction of the cation from a salt with water to produce the conjugate base of the cation and hydronium ion is called _____.

A

acidic hydrolysis

87
Q

What are the products formed in an acid hydrolysis reaction?

A

H3O+ and a weak base

88
Q

Other than water, what is required as a chemical reactant in a base hydrolysis?

A

the conjugate base of a weak acid - a proton acceptor

89
Q

Not all salts undergo hydrolysis. What are the 5 rules?

A
  1. The metal ion is never involved in the hydrolysis reaction.
  2. The conjugate bases of strong acids are very weak bases.
  3. The conjugate bases of weak acids vary in strength.
  4. If the ammonium ion (NH4+) is present in a salt, then acidic hydrolysis can occur. If it contains a weak conjugate base from a strong acid, the anion will not associate with water.
  5. If the ammonium ion (NH4+) is present in a salt, then acidic hydrolysis can occur. If it contains a conjugate base from a weak acid, both the anion and cation can react with water.
90
Q

Any solution that contains a _______ is a buffered solution.

A

weak acid-conjugate base pair

91
Q

A _____ is an aqueous solution that can resist changes in pH when small amounts of either an acid or base are added to it.

A

buffer

92
Q

TRUE or FALSE:

The pH of an unbuffered solution will become more acidic when an acid is added.

A

True

93
Q

What factors determine the pH of a buffer?

A

The identity of the buffering species and their concentrations.

94
Q

An ______ will have a pH <7. It will be made up of a weak acid and its conjugate base.
(example: acetic acid and sodium acetate)

A

acidic buffer

95
Q

A _____ will have a pH of >7. It will be made up of a weak base and its conjugate acid.
(example: ammonia and ammonium chloride)

A

basic buffer

96
Q

Regardless of which type of buffer, all buffers must contain a ______ derived from either a weak acid or a weack base.

A

conjugate acid-base pair

97
Q

The____ for an acid is the -log of the acid dissociation constant (Ka) of this acid.

A

pKa

98
Q

A ____ is an electronic instrument used to measure the pH (acidity or basicity) of a liquid. It consists of a special measuring probe (a glass electrode) connected to an electronic meter that measures and displays the reading.

A

pH meter

99
Q

An ______ is a neutralization reaction in which a known volume of a strong acid or a base with a known concentration is completely reacted with a measured volume of a base or an acid of unknown concentration.

A

acid-base titration

100
Q

The point at which equal amounts of acid and base have completely reacted is called the _____ of the titration.

A

equivalence point or end point

101
Q

An ______ is a compound, usually either a naturally occurring or man-made dye, that changes color as the pH changes.

A

acid-base indicator

102
Q

What should you use to make a quick pH determination for a solution?

A

a pH meter

103
Q

Why do we need to use the titration method for determining the concentration of a weak acid? Can we also use this technique for strong acids?

A

The pH of the solution tells us the concentration of hydronium - not the concentration of the weak acid because weak acids do not ionize completely. Yes, you can use the technique for strong acids because they will undergo neutralization with a strong base nad have an endpoint pH of 7.

CHEM 1110 (10 decks)

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