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Biochemistry > Physiological pH Buffers > Flashcards

Physiological pH Buffers Flashcards

1
Q

T/F: [ ] of a gas is = to the pressure of the gas

A

T

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2
Q

The [ ] of any gas in fluids will be expressed in terms of _____

A

pressure (P)

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3
Q

Borderline hemoglobin saturation to support normal brain function:

A

85%

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4
Q

More acidic pH for hemoglobin leads to…

A

decrease in oxygen carrying ability

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5
Q

Factors that influence pH:

A
  • physical activity
  • metabolism
  • protein degradation
  • diseases
  • diseases of lungs and kidneys
  • drugs
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6
Q

How does physical activity affect pH?

A
  • muscles produce lactic acid which is excreted in urine
  • excessive exercise can results in large amounts of lactic acid and kidneys can’t excrete it
  • pH will drop
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7
Q

How does metabolism affect pH?

A
  • can release acids or bases

- ex: protein degradation creates ammonia (base)

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8
Q

How do diseases (ex: diabetes) affect pH?

A
  • can’t make enough insulin
  • oxidize fats instead of carbs: makes acid
  • not well controlled diabetes = drop in pH
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9
Q

How do diseases of lungs and kidneys affect pH?

A
  • cause pH to change b/c these organs are highly involved in regulating pH
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10
Q

How do drugs affect pH?

A
  • large number of drugs available to treat different types of diseases are either acidic or basic
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11
Q

Arrhenius theory:

A
  • acid: release H+ when placed in water

- base: releases OH- when placed in water

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12
Q

Bronsted Lowry theory:

A
  • acid: donates H+
  • base: accepts H+
  • reaction is reversible
  • conjugate acid: comes from the base
  • conjugate base: comes from the acid
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13
Q

Lewis theory:

A
  • acid: accepts pair of e-

- base: donates pair of e-

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14
Q

pKa and pKb measures the strength of…

A

acids and bases

- tells us how much H+ of acid or OH- of base is released

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15
Q

More H+ released in solution = ______

A

stronger the acid

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16
Q

More OH- released in solution = _____

A

stronger the base

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17
Q

Ka = (formula)

A

[ionized form]/[unionized form]

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18
Q

Relationship between Ka and strength of acid:

A

direct relationship

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19
Q

pKa is the _______ of Ka

A

negative log

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20
Q

Stronger acids will have a _____ pKa

A

smaller

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21
Q

Relationship between pKa and acid strength:

A

inverse relationship

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22
Q

Buffers help keep pH of solution…

A

constant

23
Q

pH of body:

A

7.4

24
Q

Buffers are made up of..

A

weak acid and its salt (vice versa w/ base)

25
Q

Def of salt:

A

charged compound that contains anion of acid/cation of base

- results from reaction between acid and base

26
Q

Acetate buffer is an…

A

acidic buffer

27
Q

Ammonia buffer is a…

A

basic buffer

28
Q

Mixing of acid and base together results in…

A

water and base

29
Q

Neutral form:

A

not charged

30
Q

Protonated form:

A

has H+ attached (no charge)

31
Q

Deprotonated form:

A

loses H+ (positive charge)

32
Q

Midpoint of titration:

A
  • max resistance range
  • equal amounts of salt and acid/base
  • pKa/pKb of acid/base
33
Q

Why would a pH not change as much after the initial addition of a base to an acidic solution?

A

solution now has some salt in it, which creates a buffering system that will resist changes in pH

34
Q

More salt created in a solution =

A

more resistance to change until there are no more of initial solution molecules left

35
Q

T/F: to buffer a solution at specific pH, select acid/base whose pKa is greater than or equal to target pH

A

T

36
Q

Henderson buffer equation for acids:

A

pH = pKa + log[Ac-]/[HAc]

37
Q

Henderson buffer equation for bases:

A

pH = pKw-pKb+log[B]/[HB+]

38
Q

Two ions that are in the blood that act as physiological buffers:

A
  • carbonic acid (H2CO3)

- dihydrogen phosphate (H2PO4-)

39
Q

Carbonic acid has a pKa of…

A

6.1

40
Q

Salt of carbonic acid is…

A
  • bicarbonate anion (HCO3-)
41
Q

Dihydrogen phosphate has a pKa of…

A

6.7

42
Q

Salt of dihydrogen phosphate is…

A

HPO42-

43
Q

Dihydrogen phosphate loses ____ protons

A

3

- titration curve has 3 midpoints

44
Q

T/F: [dihydrogen phosphate} is high, so it has a high buffering power in regulating pH

A

F, has low [dihydrogen phosphate] so it has limited buffering power

45
Q

Bicarbonate ion plays a _____ important role in regulating pH than dihydrogen phosphate

A

more important

- more [bicarbonate]

46
Q

Acidosis:

A

pt have blood pH less than 7.4

47
Q

2 causes of acidosis:

A
  • respiratory

- metabolic

48
Q

Respiratory issues (diseases of lung/respiratory system) can cause acidosis b/c…

A

may not be able to efficiently eliminate CO2 from blood and will drop pH

49
Q

Metabolic issues (exercise/diabetes) can cause acidosis b/c…

A
  • release of acidic substances into blood stream from organs
50
Q

Alkalosis:

A

pt have blood pH greater than 7.4

51
Q

T/F: hyperventilation causes alkalosis

A

T

52
Q

Vomiting, excess intake of Tums/baking soda causes…

A
  • alkalosis

- eliminates excessive amounts of H+

53
Q

Kidney disease causes alkalosis b/c…

A
  • body can’t eliminate excessive amounts of bicarb
54
Q

Alkalosis impairs…

A

calcium ion balance, which leads to muscle cramps and cardiac arrhythmia

Biochemistry (9 decks)

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