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z - CHM040 - Biomolecules > Chapter 2: Water: The Medium of Life > Flashcards

Chapter 2: Water: The Medium of Life Flashcards

1
Q

water and its ionization products, hydrogen ions and hydroxide ions, are __ __ of the __ and __ of many biomolecules

A
  • critical determinants
  • structure and functioning
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2
Q

represents an energized condition essential to biological mechanisms of energy transformation

A

difference in concentration of hydrogen ions on opposite sides of membrane

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3
Q

for a substance of this molecular weight that is neither metallic nor ionic, water has a substantially higher what?

A
  • higher boiling point
  • melting point
  • heat of vaporization
  • surface tension
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4
Q

__ __ of attraction between H2O molecules are high

A

intermolecular forces

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5
Q

Where is the maximum density of water found

A

liquid state

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6
Q

occur when two atoms in a molecule have substantially different electronegativity : one atom attracts electrons more than another, becoming more negative, while the other atom becomes more positive

A

permanent dipoles

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7
Q

__ __ in water is key to its properties

A

hydrogen bonding

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8
Q

the solvent properties of water are derived from its __ __

A

polar nature

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9
Q

H-bonding is __

A

cooperative

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10
Q

H2O molecule serving as an H-bond donor becomes a better H-bond __

A

acceptor

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11
Q

Properties of Water

A
  1. high dielectric constant
  2. forms H bonds with polar solutes
  3. hydrophobic interactions
  4. interaction with amphiphilic molecules
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12
Q
  • ability of water to surround ions in dipole interactions and diminish their attraction for each other
  • attractions between water molecules interacting with ions are much greater than tendency of oppositely charged ions to attract one another
A

high dielectric constant

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13
Q

examples of polar functional groups

A
  • hydroxyl
  • amines
  • carbonyl
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14
Q

apparent affinity of nonpolar structures for one another

A

hydrophobic interactions

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15
Q

in actuality, the “attraction” between nonpolar solutes is an ____ process due to a net decrease in order

A

entropy-driven

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16
Q

compounds containing both strongly polar and strongly nonpolar groups

A

amphiphilic molecules

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17
Q

what disturbs the structure of liquid water, thereby changing its properties?

A

presence of dissolved substances

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18
Q

physical changes that result from adding solute to a solvent

A

Colligative properties

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19
Q

Colligative Properties of Water

A
  1. freezing point depression
  2. boiling point elevation
  3. vapor pressure lowering
  4. osmotic pressure effects
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20
Q

by imposing local order on water molecules, solutes make it more difficult for water to assume its __ __ (__) or escape into the atmosphere (__ or __)

A
  • crystalline lattice (freeze)
  • boil or vaporize
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21
Q

point at which the water is in a state of equilibrium, with the same number of water molecules transitioning from liquid to gas and from gas to liquid

A

vapor pressure

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22
Q

pressure necessary to push water back through the membrane at a rate exactly equaled by the water influx

A

osmotic pressure of the solution

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23
Q

when equilibrium is disturbed, the rates of the forward and reverse reactions change to relieve that stress and reestablish equilibrium

A

Le Chatelier’s principle

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24
Q

before equilibrium is reached, the concentrations of the reactants and products __

A

change

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25
Q

initially, reactants have a __ rate of reaction than the rate of reaction of the products

A

faster

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26
Q

at equilibrium, the rate of the forward reaction is __ to the rate of the reverse reaction

A

equal

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27
Q

As F- and H3O+ products build up, the rate of __ __ increases, while the rate of __ __ decreases

A
  • reverse reaction
  • forward reaction
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28
Q

Effects of Concentration Changes on Equilibrium:
Add reactant

A
  • increases forward reaction rate
  • shift in direction: products
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29
Q

Effects of Concentration Changes on Equilibrium:
Remove reactant

A
  • decreases forward reaction rate
  • shift in direction: reactants
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30
Q

Effects of Concentration Changes on Equilibrium:
Add product

A
  • increases reverse reaction rate
  • shift in direction: reactants
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31
Q

Effects of Concentration Changes on Equilibrium:
Remove product

A
  • decreases reverse reaction rate
  • shift in direction: products
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32
Q

state in which oxygen is not available in sufficient amounts at the tissue level to maintain adequate homeostasis

A

Hypoxia

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33
Q

a person living at a high altitude can have __ more red blood cells than someone at sea level

A

50%

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34
Q

pure water

A

[OH-] = [H+]

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35
Q

[H+] = [OH-]

A

neutral

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36
Q

[H+] > [OH-]

A

acidic

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37
Q

[H+] < [OH-]

A

basic

38
Q

Kw

A

ionization constant

39
Q

what is the ionization constant

A

1.0 x 10^-14

40
Q

Significant figures of M = __ __ of pH

A

decimal places

41
Q

according to the early days, what is the taste of acid and base

A

acid = sour
base = bitter

42
Q

acid reacts with __ to make __

A
  • carbonate
  • CO2
43
Q

base reacts with __ to make __

A
  • fats
  • soap
44
Q

acid reacts with __ to produce __

A
  • metals
  • H2
45
Q

base __ __ with metals

A

do not react

46
Q

acid turns __ litmus __

A
  • blue
  • red
47
Q

base turns __ litmus __

A
  • red
  • blue
48
Q

acid reacts with base to make __ and __

A

salt and water

49
Q

proposed the first definition of acids and bases

A

Svante Arrhenius

50
Q

According to Svante Arrhenius,
acids are substances that dissociate in water to produce __ __ and bases are substances that dissociate in water to produce __ __

A
  • H+ ions
  • OH- ions
51
Q

The Arrhenius definition for acids and bases only refers to compounds __ _ __

A

dissolved in water

52
Q

revised Arrhenius’ acid-base theory to include other solvents besides water

A
  • Johannes Bronsted
  • Thomas Lowry
53
Q

According to the Bronsted-Lowry definition, an acid is a hydrogen containing species that __ _ __, and a base is any substance that __ _ __

A
  • donates a proton
  • accepts a proton
54
Q
  • contains one more H atom and one more + charge than the base that formed it
  • formed when an acid donates a proton to a base
A

conjugate acid

55
Q
  • contains one less H atom and one more - charge than the acid that formed it
  • left over substance after acid loses its hydrogen ion
A

conjugate base

56
Q

used to represent the ionization of strong acids

A

single arrow

57
Q

used to represent ionization of weak acids because an equilibrium is created

A

double arrows

58
Q

6 strong acids

A
  1. perchloric acid
  2. hydrochloric acid
  3. hydrobromic acid
  4. hydroiodic acid
  5. nitric acid
  6. sulfuric acid
59
Q

perchloric acid

A

HClO4

60
Q

hydrochloric acid

A

HCl

61
Q

hydrobromic acid

A

HBr

62
Q

hydroiodic acid

A

HI

63
Q

nitric acid

A

HNO3

64
Q

sulfuric acid

A

H2SO4

65
Q

6 strong bases

A
  1. lithium hydroxide
  2. sodium hydroxide
  3. potassium hydroxide
  4. calcium hydroxide
  5. strontium hydroxide
  6. barium hydroxide
66
Q

lithium hydroxide

A

LiOH

67
Q

sodium hydroxide

A

NaOH

68
Q

potassium hydroxide

A

KOH

69
Q

calcium hydroxide

A

Ca(OH)2

70
Q

strontium hydroxide

A

Sr(OH)2

71
Q

barium hydroxide

A

Ba(OH)2

72
Q

completely dissociate into their ions when they are mixed with water

A

strong acids

73
Q

rule of thumb is that a strong acid is __ dissociated in solutions of __ or __

A
  • 100%
  • 1.0M or less
74
Q

bases which completely dissociate in water into the cation and OH-

A

strong bases

75
Q

hydroxides of the group _ and _ metals usually are considered to be strong bases

A

I and II

76
Q

primary organs that regulate the pH of body fluids

A
  • lungs
  • kidneys
77
Q

present to prevent large fluctuations in pH

A

buffers

78
Q

strong acid is one where __ __ of the compound occurs

A

complete dissociation

79
Q

weak acid is one where __ __ of the compound ocurs

A

incomplete dissociation

80
Q
  • dissociate poorly in water
  • release protons, but only a small fraction of their molecules dissociate (ionize)
A

weak acids

81
Q

what combination is used in buffers

A

acid-base conjugate pair

82
Q

ability to resist pH change

A

buffer capacity

83
Q

the more concentrated the components of a buffer, the __ the buffer capacity

A

greater

84
Q

the rest of the CO2 dissolves in body fluids such as __ and __ forming __ __

A
  • plasma and saliva
  • carbonic acid H2CO3
85
Q

as a weak acid, carbonic acid dissociates to give __ and __

A
  • HCO3 (bicarbonate)
  • H3O+
86
Q
  • caused by an overproduction of acid that builds up in the blood or an excessive loss of bicarbonate from the blood
  • caused by a buildup of carbon dioxide in the blood that results from poor lung function or depressed breathing
A

Acidosis

87
Q

abnormal pathophysiological condition characterized by the buildup of excess base or alkali in the body.

A

Alkalosis

88
Q

Renal responses to acidosis

A
  1. secretion of H+
  2. activity of buffers in tubular fluid
  3. removal of CO2
  4. reabsorption of NaHCO3
89
Q

Renal responses to alkalosis

A
  1. rate of H+ secretion declines
  2. tubule cells do not reclaim bicarbonates in tubular fluid
  3. collecting system transports HCO3- out into tubular fluid while releasing strong acid (HCl) into peritubular fluid
90
Q

Measure of its ability to store electrical energy

A

dielectric constant

z - CHM040 - Biomolecules (15 decks)

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