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Anachem 101 > Acids and Bases Part 2 > Flashcards

Acids and Bases Part 2 Flashcards

1
Q

TRUE or FALSE

When dissolved in water, an oxoacid yields one or more H⁺ ions and an oxoanion.

A

TRUE

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2
Q

TRUE or FALSE

When dissolved in water, an oxoacid yields only one H⁺ ions and an oxoanion.

A

FALSE

When dissolved in water, an oxoacid yields ONE OR MORE H⁺ ions and an oxoanion.

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3
Q

TRUE or FALSE

names of oxoacids are related to the names of the corresponding oxoanions

A

TRUE

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4
Q

TRUE or FALSE

names of oxoacids are not related in anyway to the names of the corresponding oxoanions

A

FALSE

names of oxoacids are related to the names of the corresponding oxoanions

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5
Q

With the -ite or -ate ending of the anion name replaced by _____ ?

A

-ous acid or -ic acid

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6
Q

The acid with fewer oxygens has an ___ ending

A

-ous

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7
Q

The acid with more oxygens has an ____ ending

A

-ic

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8
Q

TRUE or FALSE

The acid with fewer oxygens has an -ic ending

A

FALSE

The acid with fewer oxygens has an -ous ending

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9
Q

TRUE or FALSE

The acid with more oxygens has an -ous ending

A

FALSE

The acid with more oxygens has an -ic ending

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10
Q

TRUE or FALSE

The acid with more oxygens has an -ic ending

A

TRUE

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11
Q

TRUE or FALSE

The acid with fewer oxygens has an -ous ending

A

TRUE

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12
Q

The compound HNO₂, is called?

A

Nitrous acid because it has fewer oxygens and yields the nitrite ion (NO₂⁻) when dissolved in water

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13
Q

TRUE or FALSE

Nitrous acid has fewer oxygens and yields the nitrite ion (NO₂⁻)

A

TRUE

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14
Q

TRUE or FALSE

The compound HNO₂, is called Nitrous acid because it has more oxygens and yields the nitrite ion (NO₂⁻)

A

FALSE

The compound HNO₂, is called Nitrous acid because it has FEWER oxygens and yields the nitrite ion (NO₂⁻) when dissolved in water

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15
Q

The compound HNO₂, is called Nitrous acid yields the ____ when dissolved in water?

A

nitrite ion (NO₂⁻)

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16
Q

TRUE or FALSE

HNO₃ is called nitric acid

A

TRUE

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17
Q

TRUE or FALSE

HNO₃ is called nitric acid because it has more oxygens and yields the nitrate ion (NO₃⁻) when dissolved in water.

A

TRUE

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18
Q

HNO₃ is called what?

A

nitric acid

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19
Q

What does HNO₃ yields when dissolved in water?

A

nitrate ion (NO₃⁻)

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20
Q

An acid and a base are mixed in the right stoichiometric proportions, both acidic and basic properties disappear

A

neutralization reaction

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21
Q

Neutralization reaction produces _____ and ____

A

water, ionic salt

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22
Q

Anion of the salt (A⁻) comes from the _____?

A

acid

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23
Q

Cation of the salt (M⁺) comes from the _____?

A

base

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24
Q

TRUE or FALSE

Salts are generally strong electrolytes in aqueous solution

A

TRUE

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25
Q

TRUE or FALSE

Salts are generally weak electrolytes in aqueous solution

A

FALSE

Salts are generally STRONG electrolytes in aqueous solution

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26
Q

TRUE or FALSE

We can write the neutralization reaction of a strong acid with a strong base as an ionic equation

A

TRUE

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27
Q

Canceling the ions that appear on both sides of the ionic equation, A⁻ and M⁺, gives what?

A

net ionic equation

Canceling the ions that appear on both sides of the ionic equation, A⁻ and M⁺, gives the net ionic equation

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28
Q

Describes the reaction of any strong acid with any strong base in water

A

net ionic equation

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29
Q

An important aspect of clinical biochemistry is information on a ________ and blood gas homeostasis.

A

patient’s acid-base balance

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30
Q

An important aspect of clinical biochemistry is information on a patient’s acid-base balance and _________.

A

blood gas homeostasis

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31
Q

These data often are used to assess patients in life-threatening situations.

A

information on a patient’s acid-base balance and blood gas homeostasis

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32
Q

Exchange of gases, carbon dioxide and oxygen, together with the body’s mechanisms to maintain acid-base balance.

A

Blood gases and pH

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33
Q

A substance that can yield a hydrogen ion (H⁺) or hydronium ion when dissolved in water.

A

ACID

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34
Q

A substance that can yield hydroxyl ions (OH⁻).

A

BASE

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35
Q

The negative log of the ionization constant

A

pK

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36
Q

Also the pH in which the protonated and unprotonated forms are present in equal concentrations

A

pK

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37
Q

pK is also the ______ in which the protonated and unprotonated forms are present in equal concentrations

A

pH

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38
Q

TRUE or FALSE

pK is the negative log of the ionization constant

A

TRUE

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39
Q

TRUE or FALSE

pK is the positive log of the ionization constant

A

FALSE

pK is the NEGATIVE log of the ionization constant

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40
Q

TRUE or FALSE

Strong acids have pK values of less than 3.0, whereas strong bases have pK values greater than 9.0

A

TRUE

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41
Q

TRUE or FALSE

Strong acids have pK values of less than 9.0, whereas strong bases have pK values greater than 3.0

A

FALSE

Strong acids have pK values of LESS THAN 3.0, whereas strong bases have pK values GREATER THAN 9.0.

42
Q

Raising the pH above the pK will cause the acid to dissociate and yield an H⁺

43
Q

Lowering the pH below the pK will cause the base to release OH⁻

44
Q

TRUE or FALSE

For bases, Raising the pH above the pK will cause the acid to dissociate and yield an H⁺

A

FALSE

For acids

45
Q

TRUE or FALSE

For acids, Lowering the pH below the pK will cause the base to release OH⁻

A

FALSE

For base

46
Q

For acids, raising the pH above the pK will cause the acid to dissociate and yield an ____?

47
Q

For base, lowering the pH below the pK will cause the base to release ____?

A

OH⁻ Hydroxide

48
Q

Combination of a weak acid or weak base and its salt

49
Q

Is a system that resists changes in pH

50
Q

H2CO3

A

Carbonic acid

51
Q

HCO3-+ H+

A

Bicarbonate

52
Q

TRUE or FALSE

Bicarbonate-carbonic acid buffer system uses HCO₃⁻ and H₂CO₃ to minimize pH changes in plasma and erythrocytes.

53
Q

A buffer system that uses HCO₃⁻ and H₂CO₃ to minimize pH changes in plasma and erythrocytes.

A

Bicarbonate-carbonic acid buffer system

54
Q

What does bicarbonate-carbonic acid buffer system uses to minimize pH changes in plasma and erythrocytes.

A

HCO₃⁻ and H₂CO₃

55
Q

Why does bicarbonate-carbonic acid buffer system uses HCO₃⁻ and H₂CO₃?

A

To minimize pH changes in plasma and erythrocytes.

56
Q

It is the most important buffer system in plasma.

A

Bicarbonate-carbonic acid buffer system

57
Q

TRUE or FALSE

The effectiveness of a buffer depends on the pK of the buffering system and the pH of the environment in which it is placed.

58
Q

Fill in the blanks.

The _________ of a buffer depends on the ____ of the buffering system and the ___ of the environment in which it is placed.

A

effectiveness, pK, pH

59
Q

TRUE or FALSE

In plasma, the bicarbonate–carbonic acid system, having a pK of 6.1, is one of the principal buffers.

60
Q

TRUE or FALSE

In serum, the bicarbonate–carbonic acid system, having a pK of 6.1, is one of the principal buffers.

A

FALSE

In PLASMA

61
Q

In plasma, is one of the principal buffers

A

having a pK of 6.1

62
Q

The average normal ratio of HCO₃⁻ to CO₂ is 20:1

A

REGULATION

63
Q

TRUE or FALSE

Any change in the bicarbonate concentration or the dissolved carbon dioxide concentration (includes H₂CO₃) would result in a change in blood pH.

A

TRUE

Average normal ratio of HCO₃⁻ to CO₂ is 20:1

64
Q

In regulation. what is the average normal ratio of HCO₃⁻ to CO₂

65
Q

pH=pK’ + log cA-/cHA

A

Henderson-Hasselbalch Equation

66
Q

In Henderson-Hasselbalch Equation:

A⁻ is proton acceptor, or ____?

67
Q

TRUE or FALSE

In Henderson-Hasselbalch Equation:

A⁻ is proton acceptor, or base (e.g., HCO₃⁻),

68
Q

TRUE or FALSE

In Henderson-Hasselbalch Equation:

HA is proton donor, or weak acid

69
Q

TRUE or FALSE

In Henderson-Hasselbalch Equation:

HA is proton donor, or weak acid (e.g., H₂CO₃)

70
Q

Fill in the blanks.

In Henderson-Hasselbalch Equation:

_____ is proton donor, or weak acid

71
Q

Fill in the blanks.

In Henderson-Hasselbalch Equation:

HA is _______, or weak acid

A

proton donor

72
Q

Fill in the blanks.

In Henderson-Hasselbalch Equation:

HA is proton donor, or ______

73
Q

TRUE or FALSE

pK’ is pH at which there is an equal concentration of protonated and unprotonated species

74
Q

Fill in the blanks.

pK’ is pH at which there is an equal concentration of ________ and unprotonated species

A

protonated

75
Q

Fill in the blanks.

pK’ is pH at which there is an equal concentration of protonated and ________ species

A

unprotonated

76
Q

TRUE or FALSE

The lungs regulate pH through retention or elimination of CO2 by changing the rate and volume of ventilation.

77
Q

TRUE or FALSE

The lungs regulate pH through retention or elimination of Oxygen by changing the rate and volume of ventilation.

A

FALSE

CO2

The lungs regulate pH through retention or elimination of CO2 by changing the rate and volume of ventilation.

78
Q

TRUE or FALSE

The lungs regulate pH through retention or elimination of CO2 by leaving the rate and volume of ventilation.

A

FALSE

changing the rate

The lungs regulate pH through retention or elimination of CO2 by changing the rate and volume of ventilation.

79
Q

TRUE or FALSE

The kidneys regulate pH by excreting acid, primarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.

80
Q

TRUE or FALSE

The kidneys regulate pH by taking acid, primarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.

A

FALSE

excreting acid

The kidneys regulate pH by EXCRETING acid, primarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.

81
Q

TRUE or FALSE

The kidneys regulate pH by taking acid, secondarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.

A

FALSE

primarily

The kidneys regulate pH by taking acid, PRIMARILY in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.

82
Q

In Henderson-Hasselbalch Equation:

numerator (HCO3⁻) denotes what function?

A

kidney function

83
Q

In Henderson-Hasselbalch Equation:

denominator (pCO2, which represents H2CO3) denotes what function?

A

lung function

84
Q

TRUE or FALSE

In plasma and at body temperature (37°C), the pK of the bicarbonate buffering system is 6.1

85
Q

TRUE or FALSE

Normal value of pH 7.34-7.44 (7.35-7.45)

86
Q

Normal value of pH

A

7.34-7.44 (7.35-7.45)

87
Q

A pH below the reference range (7.34)

88
Q

A pH above the reference range (7.44)

89
Q

What suffix refers to a process in the body?

90
Q

What suffix refers to the corresponding state in blood ?

91
Q

TRUE or FALSE

-osis is the cause of the -emia

92
Q

Two important organs in the body for regulating blood gas and pH

A

Lungs and kidneys

93
Q

Acts to maintain acid-base balance

A

respiratory system

94
Q

Oxygen is removed from oxyhemoglobin in the tissues. This allows for the acceptance of hydrogen ions, forming _______?

A

carboxyhemoglobin

95
Q

TRUE or FALSE

Oxygen is removed from oxyhemoglobin in the tissues.

96
Q

Fill in the blanks.

Oxygen is _________ from _______ in the tissues.

A

removed, oxyhemoglobin

97
Q

TRUE or FALSE

In the lungs, carboxyhemoglobin recombines with bicarbonate to form carbonic acid

98
Q

In the lungs, carboxyhemoglobin recombines with bicarbonate to form what type of acid?

A

carbonic acid

99
Q

Which breaks down to form carbon dioxide and water.

A

carbonic acid

100
Q

The carbon dioxide is then expired by ___________.

A

respiration

Anachem 101 (5 decks)

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