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mcat chem > acid base chemistry > Flashcards

acid base chemistry Flashcards

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1
Q

arrhenius acid

A

acids dissociate into H+ in solution
must contain H
Hbr, H2CO3, H3PO4

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2
Q

arrhenius base

A

bases dissociate into OH- in solution
- bases must contain OH
- BaOH, KOH, NaOH

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3
Q

bronstead lowery acids

A

proton donor , after donating proton it becomes its conjugate base

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4
Q

bronstead lowery base

A

proton acceptor
- NH3, after accepting it becomes its conjugate acid

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5
Q

lewis acid

A

e- acceptors

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6
Q

lewis base

A

e- donors

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7
Q

amphoteric compounds

A

can act as acids or bases (can either accept or donate hydrogen)

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8
Q

pH

A

-log[h+]

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9
Q

poH

A

-log[oh-]

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10
Q

kw

A

1.0E-14 = [h][oh]
ka*kb
ionization constant of water
- do not include pure liquiids (h2o)

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11
Q

pkw

A

ph+poh= 14

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12
Q

find h+ from ph

A

10^-pH

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13
Q

henderson hassalbach eqn

A

pH= pka + log cb/a

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14
Q

strong acids

A

when dissolved will dissolve 100%

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15
Q

weak acids

A

will dissociate into hydronium and conjugate base to reach equllibrium

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16
Q

ka

A

acid dissociation constant [h+][a-]/[ha]
- proportional to amount of h+ in solution

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17
Q

pka

A

-log(ka)

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18
Q

buffer

A
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19
Q

when pH = pka

A

buffer region
- ha= a-
same amount of HA and A-
*apply to hendelson hasselbach eqn

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20
Q

zwitter ion

A

2 ion charge (at least two charged groups) usually zero
has both + and - charges on same molecule

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21
Q

pH<pKA

A

acidic solution
- molecule accepts protons (positive charge )

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22
Q

ph>pka

A

less available h+ and molecule gives away h+ –> deprotinated

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23
Q

pH= pKa

A

uncharged buffer zone
half molecules are protinated, half deprotinated

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24
Q

PI

A

point where aminoacid has net charge of 0

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25
Q

PI of typical amino acid

A

Pka1 + pka2/ 2

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26
Q

pI of basic amino acid

A

pka2 +pka3/ 2

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27
Q

PI of acidic amino acid

A

use lower 2 pKa to calculate average

28
Q

what perameter is kw dependent on

A

temperature , higher kw = higher temp

29
Q

what is the concentration of H+ in pure water solution

A

1.0E-7 mol

30
Q

kb

A

base dissociation constant
[bh+][oh-]/[b]
ratio of conjugate acid and hydroxide to original base

31
Q

weak acid

A

does not fully dissociate in water and forms h+ and CB and reaches equillibrium
smaller ka

32
Q

strong acids (memorize).

A

So –> h2so4
I –> HI
Brought –> HBr
No –> HNO3
Clean –> HCl
Clothes –> HClO4, HClO3

33
Q

strong bases (memorize)

A

LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2

34
Q

dissociation of a generic acid

A

HA (aq) + H20 (l) <–> H3o+ + A-

35
Q

physiological pH

A

7.35 to 7.45

36
Q

when doing ice tables

A

[x][x]/[molarity of original acid] = Ka
M-x (x is negligable)

37
Q

bicarbonate buffer system

A

primary buffer of blood pH (extracellular)

38
Q

metabolic acidosis

A

excess of H+
- h+ combine with bicarbonate to form carbonic acid
H+ + co3- –> h2CO3 –> h2O + CO2
- bicarbonate decreases
- carbonic acid increases and dissociates into carbon dioxide and water
- carbon dioxide is eliminated and exhaled from lungs

39
Q

how does the body adjust levels of CO2 elimination

A

Hyper and Hypoventilation

40
Q

hypoventilation

A

co2 is not being expelled and accumulates
co2 + h2o –> carbonic acid –> H+ and hco3-
- H+ goes up

41
Q

henderson- hasselbach eqn

A

pH = pKa + log [a-]/[ha]

42
Q

titrations

A

a technique where a solution of known concentration is used to determine the concentration of an unknown solution

43
Q

endpoint

A

color change and amount of known solution is required to reach

44
Q

equivalence point

A

end point of acid base titration , when original acid or base has been neutralized by added acid go bases
- middle of steep point
- moles of base = moles of acid

45
Q

when has an acid reached neutralization

A

when all acid has lost its proton

46
Q

monoprotic acdis

A

singular acidic h+

47
Q

example of diprotic acid

A

H2SO4

48
Q

polyprotic acid

A

more than once acidic h+

49
Q

polyprotic acid

A

more than once acidic h+
- neutralize multiple protons with multiple curves

50
Q

normality

A

the number of protons a molecule of acid can release in solution
ex: normality of h2so4 is 2

51
Q

N

A

moles of equivelents / L of solution
- equivelents is acidic protons or OH ions

52
Q

neutralization equation

A

N (acid) * V (acid) = N (base) * V (base)

53
Q

normality for monoprotic acid

A

molarity = normality

54
Q

indicators

A

weak acids or bases that take on different colors depending on their protonation state

55
Q

phenopthalein

A

colorless when protonated and pink when deprotonated

56
Q

how to chose indicator

A

make the pH of indicator same as pKa of acid or base you are predicting the solution to have

57
Q

half equivelence point

A

where half of the acidic protons are deprotinated
- half exsist as original acid and half are deprotinated
- horizontal regions of graph
- ph= pka

58
Q

difference in moles of acid and base for equivalence point and half equivalence point

A

eq pt: when moles acid = moles base
1/2 eq pt: when moles of acid = moles of CB

59
Q

location of equivilence pt on a titration curve

A

steep middle portion

60
Q

location of half eq pt

A

horizontal regions

61
Q

isoelectric point

A

charge is o

62
Q

isoelectric point

A

charge is o

63
Q

how many equivelence pts are there for a triprotic acid

A

3

64
Q

respiratory alkilosis

A

hyperventaliation
- decrease in co2 so increase in hco3-

65
Q

metabolic alkilosis

A

increase in bicarbonate

66
Q

metabolic acidosis

A

increase in h2co3

mcat chem (11 decks)

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