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Anachem 101 > Acids and Bases Part 2 > Flashcards

Acids and Bases Part 2 Flashcards

(100 cards)

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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
TRUE or FALSE Salts are generally weak electrolytes in aqueous solution
FALSE Salts are generally STRONG electrolytes in aqueous solution
26
TRUE or FALSE We can write the neutralization reaction of a strong acid with a strong base as an ionic equation
TRUE
27
Canceling the ions that appear on both sides of the ionic equation, A⁻ and M⁺, gives what?
net ionic equation Canceling the ions that appear on both sides of the ionic equation, A⁻ and M⁺, gives the net ionic equation
28
Describes the reaction of any strong acid with any strong base in water
net ionic equation
29
An important aspect of clinical biochemistry is information on a ________ and blood gas homeostasis.
patient’s acid-base balance
30
An important aspect of clinical biochemistry is information on a patient’s acid-base balance and _________.
blood gas homeostasis
31
These data often are used to assess patients in life-threatening situations.
information on a patient’s acid-base balance and blood gas homeostasis
32
Exchange of gases, carbon dioxide and oxygen, together with the body’s mechanisms to maintain acid-base balance.
Blood gases and pH
33
A substance that can yield a hydrogen ion (H⁺) or hydronium ion when dissolved in water.
ACID
34
A substance that can yield hydroxyl ions (OH⁻).
BASE
35
The negative log of the ionization constant
pK
36
Also the pH in which the protonated and unprotonated forms are present in equal concentrations
pK
37
pK is also the ______ in which the protonated and unprotonated forms are present in equal concentrations
pH
38
TRUE or FALSE pK is the negative log of the ionization constant
TRUE
39
TRUE or FALSE pK is the positive log of the ionization constant
FALSE pK is the NEGATIVE log of the ionization constant
40
TRUE or FALSE Strong acids have pK values of less than 3.0, whereas strong bases have pK values greater than 9.0
TRUE
41
TRUE or FALSE Strong acids have pK values of less than 9.0, whereas strong bases have pK values greater than 3.0
FALSE Strong acids have pK values of LESS THAN 3.0, whereas strong bases have pK values GREATER THAN 9.0.
42
Raising the pH above the pK will cause the acid to dissociate and yield an H⁺
For acids
43
Lowering the pH below the pK will cause the base to release OH⁻
For base
44
TRUE or FALSE For bases, Raising the pH above the pK will cause the acid to dissociate and yield an H⁺
FALSE For acids
45
TRUE or FALSE For acids, Lowering the pH below the pK will cause the base to release OH⁻
FALSE For base
46
For acids, raising the pH above the pK will cause the acid to dissociate and yield an ____?
H⁺
47
For base, lowering the pH below the pK will cause the base to release ____?
OH⁻ Hydroxide
48
Combination of a weak acid or weak base and its salt
BUFFER
49
Is a system that resists changes in pH
BUFFER
50
H2CO3
Carbonic acid
51
HCO3-+ H+
Bicarbonate
52
TRUE or FALSE Bicarbonate-carbonic acid buffer system uses HCO₃⁻ and H₂CO₃ to minimize pH changes in plasma and erythrocytes.
TRUE
53
A buffer system that uses HCO₃⁻ and H₂CO₃ to minimize pH changes in plasma and erythrocytes.
Bicarbonate-carbonic acid buffer system
54
What does bicarbonate-carbonic acid buffer system uses to minimize pH changes in plasma and erythrocytes.
HCO₃⁻ and H₂CO₃
55
Why does bicarbonate-carbonic acid buffer system uses HCO₃⁻ and H₂CO₃?
To minimize pH changes in plasma and erythrocytes.
56
It is the most important buffer system in plasma.
Bicarbonate-carbonic acid buffer system
57
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.
TRUE
58
# 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.
effectiveness, pK, pH
59
TRUE or FALSE In plasma, the bicarbonate–carbonic acid system, having a pK of 6.1, is one of the principal buffers.
TRUE
60
TRUE or FALSE In serum, the bicarbonate–carbonic acid system, having a pK of 6.1, is one of the principal buffers.
FALSE In PLASMA
61
In plasma, is one of the principal buffers
having a pK of 6.1
62
The average normal ratio of HCO₃⁻ to CO₂ is 20:1
REGULATION
63
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.
TRUE Average normal ratio of HCO₃⁻ to CO₂ is 20:1
64
In regulation. what is the average normal ratio of HCO₃⁻ to CO₂
20:1
65
pH=pK' + log cA-/cHA
Henderson-Hasselbalch Equation
66
In Henderson-Hasselbalch Equation: A⁻ is proton acceptor, or ____?
base
67
TRUE or FALSE In Henderson-Hasselbalch Equation: A⁻ is proton acceptor, or base (e.g., HCO₃⁻),
TRUE
68
TRUE or FALSE In Henderson-Hasselbalch Equation: HA is proton donor, or weak acid
TRUE
69
TRUE or FALSE In Henderson-Hasselbalch Equation: HA is proton donor, or weak acid (e.g., H₂CO₃)
TRUE
70
# Fill in the blanks. In Henderson-Hasselbalch Equation: _____ is proton donor, or weak acid
HA
71
# Fill in the blanks. In Henderson-Hasselbalch Equation: HA is _______, or weak acid
proton donor
72
# Fill in the blanks. In Henderson-Hasselbalch Equation: HA is proton donor, or ______
weak acid
73
TRUE or FALSE pK’ is pH at which there is an equal concentration of protonated and unprotonated species
TRUE
74
# Fill in the blanks. pK’ is pH at which there is an equal concentration of ________ and unprotonated species
protonated
75
# Fill in the blanks. pK’ is pH at which there is an equal concentration of protonated and ________ species
unprotonated
76
TRUE or FALSE The lungs regulate pH through retention or elimination of CO2 by changing the rate and volume of ventilation.
TRUE
77
TRUE or FALSE The lungs regulate pH through retention or elimination of Oxygen by changing the rate and volume of ventilation.
FALSE CO2 The lungs regulate pH through retention or elimination of CO2 by changing the rate and volume of ventilation.
78
TRUE or FALSE The lungs regulate pH through retention or elimination of CO2 by leaving the rate and volume of ventilation.
FALSE changing the rate The lungs regulate pH through retention or elimination of CO2 by changing the rate and volume of ventilation.
79
TRUE or FALSE The kidneys regulate pH by excreting acid, primarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.
TRUE
80
TRUE or FALSE The kidneys regulate pH by taking acid, primarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.
FALSE excreting acid The kidneys regulate pH by EXCRETING acid, primarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.
81
TRUE or FALSE The kidneys regulate pH by taking acid, secondarily in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.
FALSE primarily The kidneys regulate pH by taking acid, PRIMARILY in the ammonium ion, and by reclaiming HCO₃⁻ from the glomerular filtrate.
82
In Henderson-Hasselbalch Equation: numerator (HCO3⁻) denotes what function?
kidney function
83
In Henderson-Hasselbalch Equation: denominator (pCO2, which represents H2CO3) denotes what function?
lung function
84
TRUE or FALSE In plasma and at body temperature (37°C), the pK of the bicarbonate buffering system is 6.1
TRUE
85
TRUE or FALSE Normal value of pH 7.34-7.44 (7.35-7.45)
TRUE
86
Normal value of pH
7.34-7.44 (7.35-7.45)
87
A pH below the reference range (7.34)
acidosis
88
A pH above the reference range (7.44)
alkalosis
89
What suffix refers to a process in the body?
-osis
90
What suffix refers to the corresponding state in blood ?
-emia
91
TRUE or FALSE -osis is the cause of the -emia
TRUE
92
Two important organs in the body for regulating blood gas and pH
Lungs and kidneys
93
Acts to maintain acid-base balance
respiratory system
94
Oxygen is removed from oxyhemoglobin in the tissues. This allows for the acceptance of hydrogen ions, forming _______?
carboxyhemoglobin
95
TRUE or FALSE Oxygen is removed from oxyhemoglobin in the tissues.
TRUE
96
# Fill in the blanks. Oxygen is _________ from _______ in the tissues.
removed, oxyhemoglobin
97
TRUE or FALSE In the lungs, carboxyhemoglobin recombines with bicarbonate to form carbonic acid
TRUE
98
In the lungs, carboxyhemoglobin recombines with bicarbonate to form what type of acid?
carbonic acid
99
Which breaks down to form carbon dioxide and water.
carbonic acid
100
The carbon dioxide is then expired by ___________.
respiration

Anachem 101 (5 decks)

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