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Pharmaceutics I > Week 1 > Flashcards

Week 1 Flashcards

1
Q

Is benzocaine acidic or basic?

A

basic

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2
Q

is amphetamine acidic or basic?

A

basic

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3
Q

is acetaminophen acidic or basic?

A

acidic

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4
Q

is clotrimazole acidic or basic?

A

basic

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5
Q

T/F any drug with acid-base character will always exist in both acidic and basic forms

A

True

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6
Q

The amount of drug in either unionized or ionized form depends on the ___ of the acid and the ___ of the medium

A

pka, ph

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7
Q

T/F acids/bases both exist in both charged and uncharged forms

A

True

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8
Q

the ionized form of a drug is more _____ soluble than the unionized form

A

water

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9
Q

the unionized form of a drug is more _____ soluble than the ionized form

A

lipid

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10
Q

the acidic form of a drug is greater when pH is?

A

less than 7

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11
Q

the basic form of a drug is greater when pH is?

A

greater than 7

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12
Q

define drug absorption

A

movement of drug from site of administration into the bloodstream

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13
Q

in order for drugs to cross lipophilic barriers, some of it is requires to be in its _____ form. Why?

A

unionized

unionized form is more lipid soluble, so it can cross the lipid bilayer

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14
Q

drug absorption is greatly dependent on? (what form of drug)

A

amount of drug in unionized form at site of absorption

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15
Q

Define renal drug excretion

A

elimination of drug from the body by the kidney

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16
Q

if a drug is being excreted from the body, which soluble form is more easily excreted?

A

water soluble compounds

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17
Q

if a drug is in its unionized form in the kidneys, what outcome can happen a part from excretion?

A

Unionized drug can be reabsorbed into circulation to provide its therapeutic effect again

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18
Q

if a drug is in its ionized form in the kidneys, what is the outcome?

A

ionized drug is excreted in the urine

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19
Q

who’s concept describes an acid as a substance which generates a hydrogen proton (H+)?

A

Arrhenius Concept

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20
Q

who’s concept describes a base as a substance which generates a hydroxide anion (OH-)

A

Arrhenius Concept

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21
Q

who’s concept describes a neutralization reaction as resulting in the formation of water and salt?

A

Arrhenius Concept

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22
Q

what is the flaw in the Arrhenius Concept?

A

some basic substances do not have OH-

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23
Q

who’s concept describes an acid as a substance which is capable of donating a hydrogen proton to a conjugate base?

A

Bronsted-Lowry Concept

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24
Q

who’s concept describes a base as a substance which is capable of accepting a hydrogen proton (H+) producing a conjugate acid?

A

Bronsted-Lowry Concept

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25
Q

who’s concept describes a neutralization reaction being when the reaction between acid and base results in the formation of a conjugate base and conjugate acid?

A

Bronsted-Lowry Concept

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26
Q

what does it mean to say water is amphoteric

A

can function as both a proton acceptor and proton donor

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27
Q

who’s concept describes an acid as a substance which is capable of accepting an electron pair?

A

Lewis Concept

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28
Q

who’s concept describes a base as a substance which is capable of donating an electron pair?

A

Lewis Concept

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29
Q

who’s concept describes a neutralization reaction as a reaction between an acid and base forming an addition product as the electrons from the electron donating base are picked up by the electron accepting acid?

A

Lewis Concept

30
Q

Reaction between an acid and base results in the formation of a?

A

conjugate base and

conjugate acid

31
Q

what is molarity?

A

concentration measured by the number of moles of solute per liter of solution

32
Q

what does the pH tell you about an aqueous solution?

A 
the concentration of a hydrogen proton (H+) or
hydronium anion (H3O+) already in the medium
33
Q

each whole pH value is ___ times more acidic/basic than the following value, for example, an acid with a pH of 2 is ____ times more acidic than a solution with a pH of 5

A

ten, 1000

34
Q

what information does the pOH scale provide?

A

the concentration of OH- ions in a solution

35
Q

how do you calculate pOH given the pH?

A

pOH= 14-pH

36
Q

T/F almost every acid and base encountered in pharmacy is a strong acid or strong base

A

False, weak acid or weak base

37
Q

what is Le Chatelier’s principle?

A

if a chemical system at equilibrium experiences a change, than the equilibrium shifts to counteract the change and a new equilibrium is established

38
Q

a larger Ka means that the acid has a ______ tendency to donate its H+, meaning its a stronger or weaker acid?

A

stronger, stronger acid

39
Q

the lower the pKa value the ____ the acid

A

stronger

40
Q

the higher the pKa value the ____ the acid

A

weaker

41
Q

what does the pKa value tell you? is it a value that is changeable?

A

how willing/unwilling an acid is to donate a proton when dissolved in water
no

42
Q

what does the pH value tell you? is it a value that is changeable?

A

the concentration of hydrogen proton in the solution

yes

43
Q

what is a polyprotic compound?

A

a molecule that contains several different ionizable groups

44
Q

how many protons can a diprotic acid donate?

A

two hydrogen protons

45
Q

how many protons can a triprotic acid donate?

A

three hydrogen protons

46
Q

the stronger an acid, the ____ its conjugate base will be

A

weaker

47
Q

the weaker an acid, the ____ its conjugate base will be

A

stronger

48
Q

the weaker the acid, the ___ time it spends in acid form and ____ time it spends in conjugate base form

A

more, less

49
Q

an aliphatic carboxylic group (R-COOH) is a common weak acid or base?

A

acid

50
Q

an aromatic carboxylic group (benzene ring with COOH attached) is a common weak acid or base?

A

acid

51
Q

a phenol group (benzene ring with OH attached) is a common weak acid or base?

A

acid

52
Q

a sulfonamide group (R-SOONH2) is a common weak acid or base?

A

acid

53
Q

an imide group (O=C-NH-C=O) is a common weak acid or base?

A

acid

54
Q

a thiol group (R-SH) is a common weak acid or base?

A

acid

55
Q

what is the Henderson-Hasselbalch equation?

A

pH = pKa + log [Conj, Base] / [Acid]

56
Q

when the pH of the medium is equal to the pKa of the acid, the drug exists __% in the ionized form and __% in the unionized form

A

50,50

57
Q

a primary amine (R-NH2) is a common weak acid or base?

A

weak base

58
Q

a secondary amine (R-NH-R) is a common weak acid or base?

A

weak base

59
Q

a tertiary amine (R-N-R)
I
R
is a common weak acid or base?

A

weak base

60
Q

a pyridine (benzene ring with one carbon replaced by N) is a common weak acid or base?

A

weak base

61
Q

an imidazole (pentagon ring with two Ns replacing C) is a common weak acid or base?

A

weak base

62
Q

what does Kb measure?

A

weak base strength

63
Q

the pKa for a weak base is actually the pKa of the ________ of that base

A

conjugate acid

64
Q

the lower the pKa the ___ the acid and the ___ the base

A

stronger, weaker

65
Q

the higher the pKa value the ___ the acid and the ___ the base

A

weaker, stronger

66
Q

The stronger an acid, the ____ its conjugate base will be

A

weaker

67
Q

the stronger a base, the ____ its conjugate acid will be

A

weaker

68
Q

a pKa less than two is a strong or weak acid?

A

strong

69
Q

a pKa greater than 12 is a strong or weak base?

A

strong

70
Q

a pKa greater than 3 is a strong or weak acid?

A

weak

71
Q

a pKa less than 11 is a strong or weak base?

A

weak

Pharmaceutics I (6 decks)

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