CGIER 38 - The importance of pH in biological functions Flashcards

1
Q

where are acid base groups found and name an example of each

A

NH2 COOH

found in macromolecules and smaller molecules

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2
Q

pH of blood

A

7.35-7.45
pH too low - acidosis
pH too high - alkylosis

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3
Q

Arrhenius definition of acid

A

ionise in water to give H+

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4
Q

Arrhenius definition of base

A

ionise in water to give OH-

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5
Q

Lewis base

A

donate a pair of electrons

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6
Q

lewis acid

A

accept a pair of electrnos

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7
Q

Bronsted Lowry definition of acid

A

H+ donor

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8
Q

Bronsted Lowry definition of base

A

H+ acceptor

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9
Q

How is pH of blood maintained

A

by buffer systems - chemical equilibria that can resist serious changes in pH upon addition of acids or bases (chemical acid-base equilibrium system that shifts left or right depending on how much acid or base is added - uses lewis definition)

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10
Q

amphoteric

A

depending on where it finds itself it can act as an acid or base e.g. H2O
in the presence of an acid it acts as a base and vice versa

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11
Q

weak acid examples

A
weak acid =/= diluted strong acid
HF
HCN
HNO2
HCOOH
CH3COOH
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12
Q

Strong bases

A

NaOH
KOH
Ba(OH)2
Li(OH)

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13
Q

weak bases

A

NH3, CH3NH2, C6H5NH2

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14
Q

strong acids

A

HClO4 > HI > HBr > HCl > H2SO4 > HNO3

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15
Q

arrhenius definition of weak acid

A

will ionise partially

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16
Q

arrhenius definition of weak base

A

will ionise partially

17
Q

if an acid is strong the conjugate base must be

A

weak

18
Q

if the base is strong the conjugate acid is

A

weak

19
Q

dissociation constant with weak acid/base

A

keep the weak base as the denominator for the equilibrium but remove the acid
for acid keep the weak acid but remove the base

20
Q

pure water conducts…

A

Pure water conducts electricity (slightly) due to autodissociation

21
Q

anything above 7 is ..

A

alkaline

22
Q

anything below 7 is..

A

acidic

23
Q

Kw

A

dissociation of water

[H30+][OH-]

24
Q

Ka

A

[H30+][A-] / [HA]

25
Q

Kb

A

[HA][OH-] / [A-]

26
Q

Ka in terms of Kw and Kb

A

Kw/Kb

27
Q

Kb in terms of Ka and Kw

A

Kw/Ka

28
Q

Kw in terms of Ka and Kb

A

Ka x Kb

29
Q

pH for acid and pOH for base

A

𝐩𝐇=βˆ’π₯𝐨𝐠𝟏𝟎[𝐇+]

π©πŽπ‡=βˆ’π₯𝐨𝐠𝟏𝟎[πŽπ‡]

30
Q

pH + pOH =

A

14

31
Q

Who introduced the concept of pH

A

Arnold Beckman,

32
Q

pH of saliva

A

6.5-7.5

33
Q

pH of upper stomach

A

4-6.5

34
Q

pH of lower stomach

A

1.5-4.0

35
Q

pH of Duodenum

A

7-8.5

36
Q

pH of small intestine and large intestine

A

4-7