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Cell > Water. pH, Buffers and Acid-Base Balance > Flashcards

Water. pH, Buffers and Acid-Base Balance Flashcards

1
Q

The ff are properties of ____:

Ability to Solvate Organic and Inorganic Molecules

Nucleophile

Ability to Ionize→Tendency to Dissociate

A

Water

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2
Q

T/F: Water acts both as an acid and base, thus impacts pH

A

True

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3
Q

Water molecules from dipoles due to

A

strong electronegativity of oxygen, the O atom attracts electrons away from the H nuclei creating a partial charge between O (-) and H (+). T

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4
Q

feature that allows water to weaken the forces between charged and polar molecules.

A

dielectric constanst

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5
Q

Water has a low dielectrict constant (T/F)

A

False; high

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6
Q

Water decreases the force of attraction between charged and polar species relative to water- free environments with (lower/higher) dielectric constants

A

Lower

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7
Q

Water has a high viscosity, surface tension, and

boiling point due to

A

hydrogen bonds

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8
Q

The oxygen atoms of aldehydes, ketones, and amides provide

lone pairs of electrons that can serve as hydrogen____.

A

acceptors

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9
Q

Alcohols, carboxylic acids, and amines can serve as as hydrogen donors of unshielded hydrogen atoms for formation of hydrogen bonds

A

False: donors and acceptors

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10
Q

° Carbonyl carbons in amides, esters, aldehydes, and ketones.
° The phosphorus atoms of phospho-esters.

Electrophiles or nucleophiles?

A

Electrohpiles

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11
Q

° The oxygen atoms of phosphates, alcohols, and carboxylic acids ° The sulfur of thiols
° The nitrogen atom of amines

Electrophiles or nucleophiles?

A

Nucleophiles

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12
Q

Thermodynamics that govern the equilibrium point of a reaction
determines the rate at which it will proceed toward its equilibrium point (t/f)

A

False; does not

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13
Q

Covalent and non-covalent bonds stabilize biologic molecules (t/f)

A

truw

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14
Q

A ____ bond is the stronger bond that holds biologic molecules
together. ____ have a lesser magnitude of force

A

Covalent; non-covalent

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15
Q

Tendency of nonpolar compounds to self-associate in aqueous

environments

A

hydrophobic interactions

Minimizes disruption of energetically favorable interactions
between surrounding water molecules
− Hydrogens of non-polar groups do not form H-bonds
− Water molecules adjacent to hydrophobic group are restricted in
forming H-bonds

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16
Q

Salt bridges: electrostatic interactions between oppositely charged groups

A

Electrostatic interactions

Act over a larger distance than H-bonds
° Facilitate binding of charged molecules and ions to proteins and
nucleic acids

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17
Q

Come from attraction between transient dipoles
° Transient dipoles due to the distance between atoms or
molecules

A

Van der Waals forces

Weaker but more numerous than H-bonds
° Acts in a shorter distance

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18
Q

Determine the bonds in DNA:

___ hold together each DNA strand
___ between nucleotide base pairing
___ between stacked purine and pyrimidine bases

A

covalent, h bond, van der waals

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19
Q

Buffer systems in the body

A

chemical buffering system protein buffering system, respiratory and renal

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20
Q

Chemical buffering systems

A

bicarbonate, phosphate, proteins

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21
Q

The Hydrogen ion concentration in the body and its balance in the body fluid systems

A

Acid-base balance

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22
Q

Acid-base balance is controled by

A

buffers

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23
Q

ph level that is normal arterial ph ofour body

A

7.4

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24
Q

What do buffers do

A

Instead of eliminating excessive Hydrogen ions, they are trapped until balance is reestablished.

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25
Q

Most important buffer system in the ECF because it can regulate acid base balance within seconds

A

Bicarbonate buffer system

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26
Q

regulates bicarbonate buffer syste,

A

carbonic anhydrase

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27
Q 
Consists of:
− Acid: H2CO3 (Carbonic Acid)
° Easily dissociates to CO2 and water OR to H+ and HCO3-
Base: HCO3- (Bicarbonate ion)
Salt: NaHCO3 (Sodium Bicarbonate)
Enzyme: Carbonic Anhydrase
A

Bicarbonate buffer system

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28
Q

Bicarbonate Buffer: in order restore balance

in the presence of strong acid,

1) hydrogen concentration increases or decreases?
2) system shifts to left or right?
3) producing more or less CO2?

A

1) increases
2) left
3) more

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29
Q

Bicarbonate Buffer: in order restore balance

in the presence of strong base, strong base reacts with H2CO3

1) producing more or less HCO3-?
2) system shifts to left or right?

A

1) more

2) right

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30
Q

Why is bicarbonate buffer strongest in lung alveoli and kidney tubules

A

carbonic anhydrase is present in the ECF of these areas

31
Q

Equation to quantify amounts

A

Henderson-HAssebach Equation = pH = pKa + log (concentration of conjugate base/concentation of weak acid)

32
Q

ph level of acidosis

A

6.8 < pH < 7.4

33
Q

ph level of akalosis

A

7.4

34
Q

high HCO3-, low PCO2

A

alkolatic

35
Q

low HCO3-, high PCO2

A

acidotic

36
Q

A buffer can be considered as efficient if

A

the concentration of the acid and the base are equal

37
Q

Main buffer system in ICF

A

Phosphate Buffer Systwm

Acid: H2PO4- (Dihydrogen Phosphate)
Base: HPO4-2 (Hydrogen Phosphate)
Salt: Na2HPO4 (Disodium Phosphate)

38
Q

why is phosphate buffer system active in ICF

A

− Abundant in the tubular fluids in kidneys (ICF)

− Higher concentration of phosphate in proximal tubules

39
Q

phosphate system has a better efficiency in titration curve compared to bicarbonate

A

True; However, this is not used as often because this system is only
abundant in the tubular fluid of the kidneys

40
Q

Protein pK is near intracellular pH
● Slow buffer, might take several hours before steady state is achieved
● Abundant in ICF and ECF

A

Protein Buffer SYstem

41
Q

Protein buffer has effective ICF buffers because molecules are ___

A

molecules are ampotheric

42
Q

ECF buffer of protein bfufer

A

hemoglobin (Facilitates exchange of O2 and CO2 from lungs to tissue and vice versa)

Buffer for CO2 and H+
° 10% of CO2 is dissolved in the plasma
° 20% of CO2 is combined with Hemoglobin, forming
Carbaminohemoglobin
􏰀 The Carbaminohemoglobin produced is then released to
the lungs
° 70% reacts with H2O to form HCO3-

43
Q

protein buffeR: The HCO3- produced goes out to the ECF in exchange for

A

chloride ions

44
Q

acts within a few minutes to eliminate CO2 from the body

A

respiratory control

45
Q

Respiratory control uses ____ system becuase this is usually done in the lungs

A

bicarbonate buffer system

46
Q

High metabolic activity→__ low or high CO2→low or hhigh ___ H+ ion in the body

A

high, highh

47
Q

Increase in CO2 will push the equation to the (left or right), (decreasing/increasing) H+ ions, thereby inducing a more (acidic/basic) environment

A

right; increasing; acidic

48
Q

A decrease in ventilation will decrease/increase the CO2 inside the body because more/less CO2 is blown off, which decreases/increases H+ concentration in the body

A

increase; less; increases

49
Q

this mechanism is applied to regulate changes in PCO2 and H+

A

Negative feedback control

50
Q

Feedback control mechanism: increase in concentration of H+ = (1) in Alveolar ventilation = (2) PCO2 in blood→ Alveolar ventilation rate will not (3) anymore because
concentration of H+ is not that (4) anymore

A

increasel decrease; decrease; high

51
Q

Hyperventilation/ respiratory alkalosis:

(1) in ventilation means an (2) in CO2 blown away, which (3) CO2 in the body, thereby (4) H+ (acidity) in the body

A

increase; increase; decrease; decrease

52
Q

Fever
− Anxiety
− Severe asthma
− High altitude position

are causes of

A

hyperventilation / respiratory alkalosis:

53
Q

respiratory acidosis: (1) in ventilation means a (2) in CO2 blown away, which (3) CO2 in the body, thereby (4) H+ (acidity) in the body

A

decrease, decrease, increase, increase

54
Q

Chronic Obstructive Pulmonary Disease
− Chest wall tumors
− Narcotic use

causes of

A

Causes of respiratory acidosis

55
Q

The slowest buffer system (hours to days)

A

renal

56
Q

how does renal eliminate excess of acid or base

A

altering ph of urine

57
Q

end arteries; filters blood

A

glomerulus

58
Q

where urine is concentrated before it leaves

the body

A

tubular systems

59
Q

Renal control uses the ____ system

A

Bicarbonate

Carbonate anhydrase can be found in the tubular cells

60
Q

Cells of the tubules (tubular cells) surrounded by interstitial fluid

A

Bicarbonate system

Tubular lumen - area where urine is concentrated in

61
Q

Processes of Bicarbonate System (3)

A

Filtration of HCO3-, Active Secretion H+ and Active. Reabsorption of HCO3-

Filtration of HCO3-: Bicarbonate ions are continuously filtered in the urine.
− Active secretion H+: Hydrogen ions are continuously secreted into the urine.
° They can also leave via the phosphate buffer system and via the ammonia buffer system.
° Active secretion occurs since H+ ions would have to go against the concentration gradient (low concentration→high concentration).
° This process allows the acid to be removed from the blood.
− Active reabsorption of HCO3-: Bicarbonate is actively reabsorbed
through the bicarbonate buffer system
° In the proximal tubule cells of the kidney.

62
Q

Involves active secretion and reabsorption

A

steady state (bicarbonate system)

General process:
° Carbon dioxide can pass through any cell.
° CO2 can enter tubular cells from the interstitial fluid or from the
tubular lumen.
° Inside the cells: CO2 + H2O → H2CO3 → HCO3- + H+
􏰀 Carbonic acid is produced by the enzyme carbonic anhydrase.
􏰀 Carbonic acid rapidly dissociates into bicarbonate and hydrogen ions, then bicarbonate is actively reabsorbed back in the system.
􏰀 For every active reabsorption of bicarbonate, there is a hydrogen ion that is secreted.

However, there is still a lot of hydrogen ions that we need to secrete or buffer so there is no acid-base imbalance.

63
Q

Excretion of excess H+ can be buffered through 2 more systems

A

Renal control (Bicarbonate system)

64
Q

System in renal control:

High phosphate in tubular lumen → whenever hydrogen ions are excreted, filtered hydrogen phosphate buffers the process so that hydrogen can be excreted.

A

phosphate buffer system

65
Q

Ammonium is secreted from the tubular cells which then buffers
with the hydrogen ion to become ammonia (NH4) which is then excreted through the urine

A

ammonia buffer system

66
Q

metabolic abnormalities depend on the amount of ____ in the body

A

bicarbonate

67
Q

Metabolic Alkalosis

(decreased/increased) amount of bicarbonate:
° Hydrogen ion concentration (decreased/increased) to reach equilibrium
° As a result, pH (decreased/increased)

A

increased; decreased; increased

68
Q

Metabolic Acidosis
(decreased/increased) amount of bicarbonate:
° Hydrogen ion concentration (decreased/increased)
° As a result, pH (decreased/increased)

A

decreased, increase, decrease

69
Q

Metabolic abnormality that leads to
° Vomiting gastric contents that are acidic
° Ingestion of alkaline drugs (ex. peptic ulcer)

A

metabolic alkalosis

70
Q

Metabolic abnormality that leads to
− Situations that lead to metabolic acidosis
° Diarrhea
° Vomiting intestinal contents that are alkaline ° Starvation
° Diabetic ketoacidosis

A

metaboic acidosis

71
Q

Electric force (F) between oppositely charged particles is inversely proportionate to the dielectric constant ε.

A

coulombs law

72
Q

ucleophilic attack by water typically results in the cleavage of the amide, glycoside, or ester bonds that hold

A

hydrolysis

73
Q

catalyze the hydrolysis of proteins into their component amino acids.

A

proteases

74
Q

catalyze the hydrolysis of the phosphoester bonds in DNA and RNA.

A

nucleases

Cell (6 decks)

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