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Z Biomolecules (Biochemistry) > Module 2: Water > Flashcards

Module 2: Water Flashcards

1
Q

formula for Finding pH

A

pH= -log (H^+)

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2
Q

formula for finding pOH

A

pOH= -log (OH^-)

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3
Q

Formula for finding H^+

A

H^+= 10^-ph

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4
Q

Formula for finding OH^+

A

OH^-= 10^-ph

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5
Q

finding pH/pOH given one of them

A

pH= 14-pOH or pOH= 14-pH

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6
Q

organisms are __% to __% water

A

70% to 90% water

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7
Q

Normal metabolic activity can occur only when cells are at least ____ H2O

A

65%

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8
Q

water and its ionization products, ______ and ______, are critical determinants of the structure and function of many biomolecules.

A
  • hydrogen ions
  • hydroxide ions
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9
Q

What are the properties of water?

A
  • Hydrogen bonding in water is key
    to its properties.
  • Water forms H bonds with polar solutes
  • Interactions with amphiphilic molecules
  • Hydrophobic Interactions
  • The solvent properties of water
    derive from its polar nature
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10
Q

Because of its highly polar nature, water is an
excellent solvent for various compounds

A

THE SOLVENT PROPERTIES OF WATER DERIVE FROM
ITS POLAR NATURE

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11
Q

Water’s ability to surround ions in dipole interactions and diminish their attraction for each other

A

Water has a high dielectric constant

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12
Q

excellent solvent properties of water stem from its ability to readily form hydrogen bonds with the polar functional groups on these compounds, such as hydroxyls, amines, and carbonyls

A

Water Forms H Bonds with Polar Solutes

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13
Q

Water Forms H Bonds with Polar Solutes:
excellent solvent properties of water stem from its
ability to readily form hydrogen bonds with the polar functional groups on these compounds, such as ____, ___, and __

A

hydroxyls, amins and carbonyls

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14
Q
  • apparent affinity of nonpolar structures for one another
A

Hydrophobic Interactions

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15
Q

Compounds containing both strongly polar and strongly nonpolar groups

A

Interaction with amphiphilic molecules

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16
Q
  • the physical changes that result from adding solute to a solvent
  • The presence of dissolved substances disturbs the structure of
    liquid water, thereby changing its properties.
A

Colligative properties

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17
Q

Example of colligative properties (in water)

A

▪ Freezing point depression
▪ boiling point elevation
▪ vapor pressure lowering
▪ Osmotic pressure effects

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18
Q
  • the freezing point of a solution is less than the freezing point of the pure solvent
  • means that a solution must be cooled to a lower temperature than the pure solvent in order for freezing to occur.
A
  • Freezing point depression
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19
Q

refers to the increase in the boiling point of a solvent upon the addition of a solute

A

Boiling point elevation

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20
Q

The vapor pressure of a pure solvent is greater than the vapor pressure of a solution containing a non volatile liquid. This lowered vapor pressure leads to boiling point elevation

A

Vapor pressure lowering

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21
Q

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

A

Osmotic pressure solution

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22
Q

the minimum pressure that must be applied to a solution to halt the flow of solvent molecules through a semipermeable membrane

A

Osmotic pressure

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23
Q

a compound in which molecules of one component are physically trapped within the crystal structure of another.
- Cagelike

A

Clathrate

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24
Q

a proton is transferred from one water molecule to another to produce a hydronium ion (H₃O⁺) and a hydroxide ion (OH⁻)

A

Autoionization of water

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25
Q

Equilibrium expression for Autoionization of water

A

Kw = [H₃O⁺][OH⁻]

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26
Q

Equilibrium expression for Autoionization of water:
Kw

A

autoionization constant for water

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27
Q

a state in which opposing forces or influences are balanced.

A

Equilibrium

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28
Q

quantitative measure of the acidity or basicity of aqueous or other liquid solutions

A

pH

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29
Q

who devised pH scale?

A

Søren Sørensen, a danish biochemist

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30
Q

Acidic pH range

A

less than pH 7

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31
Q

Neutral pH range

A

pH 7

32
Q

base/ basic pH range

A

greater than pH 7

33
Q

Substances that are almost completely dissociated to form ions in solution

A

strong electrolytes

34
Q

examples of electrolytes

A

salts such as NaCl and K2SO4,
strong acid such as HCl
strong bases such as NaOH

35
Q

Proton acceptors

A

base

36
Q

proton donors

A

Acids

37
Q

Substances with only a slight tendency to dissociate to form ions in solution

A

weak electrolytes

38
Q

are solutions that tend to resist changes in their pH as acid or base is added.

A

buffers

39
Q

Buffer system is composed of;

A
  • Weak acid and its conjugate base
40
Q

serves to buffer the intracellular fluid of cells at physiological pH because pK2 lies near this pH value

A

Phosphate system

41
Q

defined as a breathing rate more rapid than necessary for normal CO2 elimination from the body, can result in an inappropriately low [CO2(g)] in the blood.

A

Hyperventilation

42
Q

is the opposite of hyperventilation and is characterized by an inability to excrete CO2 rapidly enough to meet
physiological needs.

A

Hypoventilation

43
Q

Hypoventilation results in _____

A

respiratory acidosis

44
Q

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

A

Le Châtelier’s principle

45
Q

proposed the first definition of
acids and bases

A

Svante Arrhenius

46
Q

Defines acid as follows: “An acid is a hydrogen containing species that donates a proton.
A base is any substance that accepts a proton.”

A

Brønsted-Lowry Definition

47
Q

theory stating that any compound that can transfer a proton to any other compound is an acid

A

Brønsted-Lowry theory

48
Q

who revised Arrhenius’s acid-base theory

A

Johannes Brønsted and Thomas Lowry

49
Q
  • the act of making a substance neutral
  • the reaction between an acid and a base, which produces a salt and water
A

Neutralization

50
Q

a method or process of determining the concentration of a dissolved substance in terms of the smallest amount of reagent of known concentration required to bring about a given effect in reaction with a known volume of the test solution

A

titration

51
Q

equation of neutralization

A

NaOH + HCl → H2O (water) and NaCl (salt)

52
Q

First line of defense againts pH shift

A

Chemical buffer

53
Q

Seconf line of defense againts pH shift

A

Physiological buffer

54
Q

types of Chemical buffer system (in the body)

A
  1. Bicarbonate buffer
  2. Phosphate buffer
  3. Protein buffer
55
Q

types of Physiological buffer

A
  1. Respiratory mechanism (CO2 excretion)
  2. Renal mechanism (H+ excretion)
56
Q

maintaining the pH homeostasis of blood

A

Bicarbonate buffer system

57
Q

free and terminal amino acids
– Respond to pH changes by accepting or releasing H+

A

Protein buffer; Amino acids

58
Q
  • Binds CO2
  • Binds and transports hydrogen and oxygen
  • Maintains blood pH as hemoglobin changes from oxyhemoglobin to
    deoxyhemoglobin
A

Protein buffer; Hemoglobin

59
Q

how does bicarbonate buffer lowers pH

A
  • lowers pH by releasing H+
  • raises pH by binding H+
60
Q

how does bicarbonate function with respiratory and urinary systems?

A

– to lower pH, kidneys excrete HCO3
– to raise pH, kidneys excrete H+ and lungs excrete CO2

61
Q

consists of acidic phosphate ions and alkaline phosphate ions that work to neutralize pH

A

Phosphate buffer

62
Q

a description of the process wherein protein compounds consume small amounts of acids or bases.

A

Protein buffers

63
Q

is a substance that when placed in water increases the hydrogen ion concentration

A

Arrhenius acid

64
Q

is a substance that donates a proton.

A

Bronsted-Lowry acid

65
Q

is a substance that serves as an electron pair acceptor

A

Lewis acid

66
Q

an example of a arrhenius, Bronsted-Lowry, and Lewis acid.

A

Carbonic acid

67
Q

Physiological buffer systems (in the body parts)

A
  • lungs
  • kidneys
68
Q

-Provide O2 to cells and remove CO2
- Exhalation of carbon dioxide

A

Respiratory regulation

69
Q
  • Can eliminate large amounts of fixed acid
  • If kidneys fail, pH balance fails
  • Can conserve and produce bicarbonate ions
A

Renal Regulation

70
Q
  • Only regulated by the kidney.
  • Primary base in the body is HCO3
  • The kidney can retain or excrete HCO3 as needed
A

Base excretion

71
Q

involves the enzyme carbonate
dehydratase (carbonic anhydrase)

A

Renal carbonate regeneration

72
Q

Renal Renal carbonate regeneration involves the enzyme _______ _____ (_______ ______)

A
  • carbonate dehydratase
  • (carbonic anhydrase)
73
Q

3 responses of renal regulaion in acidosis

A

A. increased reabsorption of the filtered HCO3^-
B. increased excretion of titratable acids, and
C. increased production of ammonia

74
Q

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

A

Alkalosis

75
Q
  • ## occurs when acid builds up or when bicarbonate (a base) is lost
A

Acidosis

Z Biomolecules (Biochemistry) (12 decks)

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