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Chem > Chapter 9; Acids and Bases, pH, and Buffers > Flashcards

Chapter 9; Acids and Bases, pH, and Buffers Flashcards

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1
Q

what is the acid base homeostasis range

A

7.35 - 7.45
proper organ function requires blood pH

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2
Q

what is the pH balance range

A

0 - 14

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3
Q

what is the range of pH for blood pH

A

6.6 - 8.0

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4
Q

protons, H+, cause fluids to be

A

acidic

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5
Q

in blood pH what does having more than 7.4 pH lead to

A

7.4 - 7.8 = alkalosis
7.8 - 8.0 = death

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6
Q

in blood pH what does having less than 7.4 pH lead to

A

7.4 - 6.8 = acidosis
6.8 - 6.6 = death

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7
Q

what is the range of blood pH for it to be acidosis

A

pH < 7.35

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8
Q

what is the range of blood pH for it to be alkalosis

A

pH > 7.45

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9
Q

what is the blood pH ranges

A

6.6 - 8.0

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10
Q

what does cellular metabolism produce in acid base homeostasis in the blood

A

substances that affect blood pH such as CO2 and H+ ions

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11
Q

how is blood pH maintained in acid base homeostasis in the blood

A
  • increasing respiration to exhale more CO2 or
  • shifting buffer equilibrium to consume more H+
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12
Q

what do acids produce in aqueous solutions

A

hydronium ions, H subscript 3 O+ ; H3O+

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13
Q

what is the formula for hydronium ions

A

H3O+

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14
Q

what is the hydroxide ion formula

A

OH-

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15
Q

what do bases produce in aqueous solutions

A

hydroxide ions, OH-

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16
Q

according to the Arrhenius definition what are the two conditions

A
  • an acid is a substance that produces hydronium ions, H3O+
  • and a base is a substance that produces hydroxide ions, OH-, in aqueous solution
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17
Q

what are group 1A hydroxide salts in ionic compounds containing hydroxide ions being bases

A

NaOH, KOH
soluble in water
strong electrolytes
dissolve entirely to produce ions in water
(contains hydroxide ions, OH, are bases)

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18
Q

what are 2A hydroxide salts in ionic compounds containing hydroxide ions being bases

A

Ca(OH)2, Mg(OH)2
slightly soluble in water
weak electrolytes (not many ions)
dissolve slightly to produce few ions in water
(containing hydroxide ions, OH, are bases)

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19
Q

ionic compounds composed of hydroxide ion (OH-) are bases because they produce

A

solvated hydroxide ions in solution

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20
Q

are soluble hydroxide ion salts (group 1A salts strong or weak electrolytes

A

strong

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21
Q

are slightly soluble hydroxide ion salts (group 2A salts) strong or weak electrolytes

A

weak

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22
Q

in the Bronsted-Lowry theory of acids and bases, how are an acid and base differentiated

A

acid: a proton (H+) donor
base: a proton (H+) acceptor

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23
Q

hydrochloric acid, HCl, donates a proton to a water molecule, acts as a

A

base by accepting the proton

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24
Q

in bronsted lowry theory what is the term of neutral acid loses proton to form

A

conjugate base
(one fewer H+ and, a -1 charge; compared to formula of acid

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25
Q

in bronsted Lowry theory what is the term when water acts as a base, accepting proton to form

A

conjugate acid
(one more H+, a +1 charge; compared to formula of base)

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26
Q

observation; in the bronsted Lowry theory what differentiate an acid from a base

A

acid ; with water the acids are only two molecules typically with a hydrogen at the front. e.g. HCl + H20 -> H30+ + Cl-
base; the base has more than two elements when reacting with water.
e.g. NH3 + H2O <–> OH- + NH4+

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27
Q

what does a neutral base combine with/ accepts to produce its conjugate acid according to the bronsted Lowry theory

A

H+
base + H+ (<-,->) conjugate acid

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28
Q

neutral water donates a proton to form its conjugate base

A

H+
one fewer H+, and thus, a -1 charge

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29
Q

according to the Bronsted Lowry theory, can water accept and/or donate a proton

A

can accept or donate

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30
Q

can water act as an acid or a base according to the bronsted Lowry theory

A

both

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31
Q

what is the term under the bronsted Lowry theory for any substance that can act as an acid or a base

A

amphoteric compound

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32
Q

in a conjugate acid-base pair; an acid and its conjugate base or a base and its conjugate acid are called a conjugate acid-base pair

A

yes

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33
Q

can all H+ be donated

A

usually indicated at the beginning of the formula
e.g
HCl -> Cl- chloride ion
HC2H3O2 -> C2H3O2- acetate ion

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34
Q

the strength of an acid depends on the ….

A

extent to which the acid donates a proton to water

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35
Q

the strength of a base depends on the extent to which…

A

the base accepts a proton from water

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36
Q

strong acids dissociate in water […] to form a conjugate base and hydronium ions

A

completely

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37
Q

is HCl really strong

A

yes, the only strong acid produced in the human body

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38
Q

strong acids are highly […] when concentrated but are safe to handle as […] solutions

A

corrosive
dilute

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39
Q

what are the common strong acids

A

HNO3 nitric acid
H2SO4 sulfuric acid
HCLO4 perchloric acid
HCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid

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40
Q

in a solution, what does the strong acid contain mostly and very little of

A

mostly H3O+ and the conjugate base, and very little of the acid

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41
Q

why are strong acids strong electrolytes

A

base they produce many ions in solution

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42
Q

what groups make up strong bases

A

1A and 2A metal ions with hydroxide ions

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43
Q

do strong bases (groups 1A and 2A) completely dissociate in aqueous solutions

A

yes, producing hydroxide ions and cations (conjugate acids)

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44
Q

are strong bases (1A and 2A) strong electrolytes

A

if soluble

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45
Q

strong bases (1A and 2A) are […] corrosive when concentrated; can be handled safely as […] solutions

A

highly
dilute

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46
Q

what are common strong bases

A

Ba(OH)2 Barium hydroxide
Ca(OH)2 Calcium hydroxide
LiOH Lithium hydroxide
KOH Potassium hydroxide
NaOH Sodium hydroxide
Sr(OH)2 Strontium hydroxide
appear to contain OH

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47
Q

strong acids […] ionize, where weak acids only […] ionize

A

completely
partially

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48
Q

weak acids and weak bases are characterized

A
  • little dissociation in water; produce ions in aqueous solution; are weak electrolytes
  • reaction with water is reversible.
  • at equilibrium reactants>products
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49
Q

a weak acid, and similarly a weak base, undergo a reversible reaction with water that, at equilibrium, favors the […]

A

reactants

50
Q

what are e.g. of weak acids

A

CH3COOH
H3PO4
H2CO3
any acid not listed in the six common strong acids

51
Q

what are some weak bases

A

NH3
CH3NH2

52
Q

what is Le Chatelier’s principle

A

reaction shifts in direction that counteracts a disturbance
- forward reaction enhanced (a shift to the right) until a new equilibrium is attained)
- reverse reaction enhanced (a shift to the left) until a new equilibrium is attained

53
Q

what is Le CHatelier’s principle important in reactions for

A

weak acid and weak base reactions

54
Q

what are biochemical pathways in Le Chatelier’s principle

A

reactions are approaching equilibrium

55
Q

how to identify a weak strong or non electrolyte through pictures

A

weak; some + and - charges while others have no indication of charge
strong; equal number of + and - charged particles
non; no indication at all of charges

56
Q

e.g. of weak acids

A
  • organic acids; acetic acid (HC2H3O2) & citric acid (H3C6H5O7)
  • inorganic acids; carbonic acid (H2CO3), phosphoric acid (H3PO4), and hydrofluoric acid (HF)
  • any acid not listed in the six common acids
57
Q

is ammonia, NH3, a weak or strong base

A

weak

58
Q
A
59
Q

what does pH measure

A

concentration of hydronium ions (H3O+) in aqueous solution

60
Q

Low pH levels indicate
High pH levels indicate
high or low acid concrentrations

A
  • high acid concentration
  • low acid concentration
61
Q

H3O+ = molar concentration (mole/L) of

A

H3O+

62
Q

OH- = molar concentration of

A

OH-

63
Q

pH < 7 is

A

acidic
[H3O+] > [OH-]
brackets indicate concentration of hydroxide ions

64
Q

pH > 7 is

A

basic (alkaline)
[H3O+] < [OH-]
brackets indicate molar concentration

65
Q

PH = 7 is

A

neutral
[H3O+] = [OH-]
brackets indicate molar concentration

66
Q

what is auto ionization of water

A

occurs when very few water molecules react with other water molecules to produce hydronium ions and hydroxide ions
e.g. H2O + H2O <–> OH- + H3O+

67
Q

the increase or decrease of any reactant or product in the solid or liquid phase regarding equilibrium have any effect

A

no

68
Q

what does a catalyst do to a reaction

A

speed it up

69
Q

in pure water at 25 degrees celsius what is the power of 10 for M in H3O+

A

1.0 x 10^-7 M

70
Q

In pure water at 25 degrees celsius what is the power of 10 in M for OH-

A

1.0 x 10^-7 M

71
Q

what is the power of 10 for K subscript w Kw

A

Kw = 10^-14
which is
Kw = [H3O+] x [OH-]

72
Q

Kw is

A

ion product constant for water

73
Q

when acid or base is added to water, auto ionization of water shifts, but Kw is

A

constant. Kw = 10^-14

74
Q

when hydronium ion […], hydroxide must […] under the ion product constant

A

increase
decrease

75
Q

when adding acid to water; what does [H3O+] increases from 1x10^-7 M to

A

1x10^-6 M

76
Q

how to calculate the pH from the hydronium ion concentration

A

pH = -log subscript 10 [H3O+]
for pure water,
pH = -log subscript 10 [1x10^-7]

77
Q

when calculating pH from the hydronium ion concentration what is pH of an aqueous solution

A

the logarithm of the hydronium ion concentration multiplied by -1

78
Q

to find the [OH-] hydroxide ion

A

pH + pOH = 14

79
Q

pH decreases as what increases

A

hydronium ions;
H3O+

80
Q

the more hydronium ions [H3O+] the more the solution is

A

acidic

81
Q

the more hydroxide ions [OH-} the more the solution is

A

basic

82
Q

for the pH to be more acidic or more basic what doe the pH reflect on

A

H3O+

83
Q

what is the equation of finding the H3O+ concentration when only given pH

A

[H3O+] = 10^-pH

84
Q

what is the equation of finding the OH- concentration when only given pH

A

14 - pH = pOH
[OH-] = 10^-pOH

85
Q

when an acid is combined with a base, a neutral product is formed, and a […] reaction has occurred

A

neutralization

86
Q

in an acid base neutralization reaction what type of replacement reaction occurs

A

double replacement

87
Q

what reacts with stomach acid (HCl) and neutralizes the acid

A

antacids

88
Q

what are the common bases used in neutralization reactions

A

ionic compounds containing
- hydroxide ion, OH-
- hydrogen carbonate ion, HCO3-
- carbonate ion, CO subscript 3 charge -2

89
Q

sodium and chloride ions are unchanged during the reaction; they remain in solution as

A

spectator ions

90
Q

acids with more than one acidic proton are known as

A

polyprotic acids
e.g.
sulfuric acid, H2SO4
phosphoric acid, H3PO4
citric acid, H3C6H5O7

91
Q

in neutralization reactions with polyprotic acids,

A
  • all acidic protons can be donated in a neutralization reaction
  • one hydroxide ion is needed to neutralize each acidic proton
  • combine the spectator ions in a ratio that forms a neutral salt for the ionic compound
92
Q

in a hydrogen carbonate and carbonate ion containing bases; ionic compounds hydrogen carbonate, HCO3-, and carbonate ion, CO3-

A
  • are weak bases
  • are frequently used in neutralization reactions, and
  • can react with acids to produce water an ionic compound and CO2 gas
93
Q

in a neutralization reaction what do the reaction of an acid with a hydroxide ion containing base produce

A

water and a dissolved salt

94
Q

what is the net reaction in a neutralization reaction that produces water and a salt

A

H+ + OH- -> H2O

95
Q

in a neutralization reaction that produces water and a salt; how is the solution neutral

A

when an equal number of moles of hydroxide ions, OH-, and protons, H+, are combined

96
Q

a buffer is a solution that […] change in pH when small amounts of acid or base are added

A

resists

97
Q

what is pH range in buffer components

A

maintained by buffer depends on identity of the weak acid

98
Q

what is buffer capacity in buffer components

A

depends on the concentration of the buffer components

99
Q

in buffer components the strength of the acid + its conjugate base is in similar concentrations

A

yes
weak acid + conjugate base = conjugate base
strong acid + conjugate base = stronger buffer

100
Q

a buffer resists changes in pH because the equilibrium shifts in response to the […] or […] of H3O+, maintaining the concentration of H3O+. the addition of hydroxide ion is equivalent to the removal of hydronium ion, H3O+

A

addition
removal

101
Q

what is respiratory acidosis

A

breathing weak and shallow so CO2 is not exhaled
causes a shift to the right, increasing [H3O+] and decreasing pH

102
Q

what is metabolic acidosis

A

kidneys do not release sufficient HCO3- to support normal shift to the left
leads to increasing [H3O+] and decreasing pH

103
Q

for treatment what is respiratory or metabolic acidosis

A

IV infusion of HCO3- causing a shift to the left

104
Q

what is respiratory alkalosis in treatment

A

breathing into a paper bag to increase blood CO2 and shift equilibrium to right

105
Q

what is metabolic alkalosis in treatment

A

IV infusion of dilute HCl causing a shift to right

106
Q

a buffer contains either a

A

weak acid and its conjugate base,
or
a weak base and its conjugate acid.

107
Q

what is the charge of SO4

A

-2

108
Q

what is the charge of NO3 (nitrate)

A

-1

109
Q

what is the charge of PO3

A

-3

110
Q

what is the charge of ClO

A

-1

111
Q

what is the charge of HPO4

A

-2

112
Q

what is the charge of NO2

A

-1

113
Q

What is the charge of PO4 (phosphate)

A

-3

114
Q

what is the charge of SO3

A

-2

115
Q

what is the charge of NH4

A

+1

116
Q

what is the charge H3O

A

+1

117
Q

when finding the net ionic equation for the reaction

A

break down each molecule that is aquatic

118
Q

A strong acid can react with a weak base in the buffer to form a weak acid, which produces

A

A few H+ ions in solution and therefore only a little change in pH

118
Q

what are common buffers

A

CH3COOH - acetic acid/acetate buffer
H2CO3 - carbonic acid/hydrogen carbonate buffer

119
Q

during exercise, [H3O+] increases or decreases, causing a shift to the left, producing more H2CO3, shifting left again to produce more CO2, which is exhaled by increasing ventilation

A

increase
kidneys can support the shift to the left by releasing additional HCO3- into the blood

Chem (12 decks)

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