LEC1: pH and Buffers Flashcards

1
Q

where can a buffer be useful?

A

+/- 1 pH unit around the pKa

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2
Q

formula for dissociation constant of an acid?

A
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3
Q

how do weak acids/abses act as buffers?

A

weak acids & bases only partially dissociate into charged species
buffers provide a reservoir of acid that consumes added base, reservoir of base that consumes added acid
therefore dampen pH changes

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4
Q

what do acids and bases tend to do, what is each’s effect on pH?

A

acids donate protons, cause a decrease in pH
bases accept protons, cause an increase in pH by removing protons from H2O

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5
Q

what do acids/bases each do re: proton exchange?

A

acids donate protons
bases accept protons

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6
Q

what is pH for pure water under normal conditions?

A

pH = 7

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7
Q

what is the definition of pH?

A

pH = -log[H+]

pH is the measure of the H+ion concentration

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8
Q

what is the effect of buffers on pH?

A

buffers dampen pH changes

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9
Q

what is the Ka?

A

dissociation constant of an acid

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10
Q

what does this curve show?

A

concentration curve for buffer

shows relationship between acid added/base added (x axis) & pH (y axis)

see small changes to pH when add base (to the R) or acid (to the L) because this is where buffer is useful

see if add a LOT of base or acid, the conjugate acid/base is exhausted, buffer is no longer useful as a buffer

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11
Q

what is Henderson-Hasselbach equation?

A
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12
Q

what is the pKa of a weak acid?

A

the pH at which 1/2 of the molecules are dissociated into ions

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13
Q

what is the maximum buffering capacity of a weak acid?

A

1 pH unit above/below the pKa

here, both acid and conjugate base are present, can consume added ions

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14
Q

how is an acid and a base when each is above its pKa?

A

acid above its pka: unprotonated, charged

base above its pKa: unprotonated, neutral

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15
Q

what buffers human blood?

A

bicarbonate buffering system

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16
Q

what is the Henderson-Hasselbach equation for the formation of bicarbonate?

A
17
Q

what does this graph represent?

A

titration curve of carbonic acid/bicarbonate system

pH = 6.1 is known neutral state; see that between pH=5.1-7.1, small changes in pH

18
Q

what is the pH of blood?

A

7.4

19
Q

at physiologic pH of blood, what is ratio of bicarbonate:carbonic acid? explain

A

[H2CO3] to [HCO3-] is 1:20

physiological mechanisms can regulate this concentration

1) [H2CO3] modulates with breathing rate, affecting CO2levels in the blood - rxn becomes more acidic
2) [HCO3-] modulates by changing the rate of its elimination by the **kidney **- rxn becomes more basic

20
Q

when does a drug get absorbed?

A

if a drug is a weak acid, aka **protonated & uncharged, **it can be absorbed into the stomach

21
Q

describe how aspirin works, the form its found in in the stomach

A

pH of the stomach = 1.5

aspirin is a weak acid, pH= 3.5

therefore at pH = 1.5, aspirin will be protonated and uncharged, and therefore can cross membrane > stomach & intestines

protonated form is 100x more abundant than charged form

22
Q

what is charge of each part of an amino acid? & what is amino acid’s charged at pH=7?

A

weakly basic amino group, pKa = 9-10

weakly acidic carboxyl group, pKa = 2

overall, at pH=7, charge of an amino acid=0

23
Q

structure of an amino acid?

A
24
Q

what does it mean that amino acids are optical isomers?

A

their stereoisomers are nonsuperimposable mirror images

25
Q

what is the simplest amino acid? how is it found in nature?

A

glycine; R group = H

overall charge is positive, both groups are protonated, if in highly acidic environment

overall charge is **neutral **in physiologic form (normal!)

overall charge is negative, both groups are unprotonated, if in highly basic environment

26
Q

what is this? explain what is happening

A

represents the acidic/basic propteries of an amino acid w/ an uncharged R-group, aka glycine

see 2 regions where it behaves as a buffer:

1) pK1, the pKa of carboxyl group
2) pK2, the pKa of the amino group

27
Q

what is the isoelectric point?

A

the pH in which the amino acid is electrically neutral - charges balance

28
Q

what is the pI of amino acids w/ R groups that cannot be ionized?

A

6

29
Q

how are amino acids re: protonation, charge, at physiological pH?

A

carboxyl group is unprotonated, negative charged

amino group is protonated, positively charged

30
Q

how does the body control the level of CO2 in blood?

A

[H2CO3] modulates with breathing rate, affecting CO2 levels in the blood

Henderson-Hasselbalch rxn becomes more acidic

31
Q

how does the body control bicarbonate concentration?

A

[HCO3-] modulates by changing the rate of its elimination by the kidney

H-H rxn becomes more basic

32
Q

how does a buffer reduce the effect of added acid or base on the pH of a solution?

A

buffers dampen pH changes by providing a reservoir of acid that consumes added base / a reservoir of base that consumes added acid

at +/- 1 pH unit above or below a weak acid’s pKa, added ions are consumed by buffer

33
Q

why is the maximum buffering capacity of a weak acid at +/- 1 pH unit of its pKa?

A

because in this pH range both the acid and its conjugate base are present and can consume the added ions

34
Q

is a weak acid charged or uncharged at 2 pH units above its pKa?

A

charged

35
Q

is a weak base charged or uncharged at 2 pH units above its pKa?

A

neutral

36
Q

why is the carbonic acid/bicarbonate system an effective buffer of blood even though its combined pKa is more than 1 more pH unit below that of blood pH?

A

the combined pKa of carbonic acid/bicarbonate = 6.1

blood pH=7.4

works b/c components can be regulated by physiological mechanisms