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PHYSICAL PHARMACY > Exercise3 > Flashcards

Exercise3 Flashcards

1
Q

Defined in a quantitative terms as the concentration of solute in a saturated solution in a certain temperature

A

SOLUBILITY

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2
Q

In a qualitative way, it can be defined as the spontaneous interaction of two or more substances to form a homogeneous molecule dispersion

A

SOLUBILITY

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3
Q

intrinsic material property that can be altered only by chemical modification of the molecule

A

SOLUBILITY

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4
Q

extrinsic material property that can be influenced by various chemical, physical, or crystallographic means such as complexation, particle size, surface properties, solid-state modification, or solubilization enhancing formulation strategies.

A

DISSOLUTION

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5
Q

A. SOLUBILITY OF SOLIDS IN LIQUIDS

A

ALUMINUM SULFATE
ASCORBIC ACID
CALCIUM STEARATE

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6
Q

A. SOLUBILITY OF SOLIDS IN LIQUIDS
water:1:3 (freely soluble)
ethyl alcohol: insoluble
chloroform: insoluble
ether: insoluble

A

ALUMINUM SULFATE

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7
Q

A. SOLUBILITY OF SOLIDS IN LIQUIDS
water: 1:3 (freely soluble)
ethyl alcohol: 1:50 (sparingly soluble)
chloroform: insoluble
ether: insoluble

A

ASCORBIC ACID

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8
Q

A. SOLUBILITY OF SOLIDS IN LIQUIDS
water: insoluble
(dissolves 0.004g/100mL at 15oC)
ethyl alcohol: insoluble
chloroform: insoluble
ether: insoluble

A

CALCIUM STEARATE

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9
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
benzene + chloroform

A

MISCIBLE

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10
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
water+alcohol

A

MISCIBLE

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11
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
(6 C’s or less) are soluble in water

A

LOW MOLECULAR WEIGHT ALCOHOL

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12
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
(6 C’s pr more) are not soluble in water

A

HIGHER MOLECULAR WEIGHT ALCOHOLS

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13
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
water+phenol

A

PARTIALLY MISCIBLE

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14
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
the critical temperature above which the components of a mixture are miscible in all proportions

A

UPPER CRITICAL SOLUTION TEMPERATURE (UCST) or UPPER CONSOLUTE TEMPERATURE

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15
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
all combinations of phenol and water are completely miscible at

A

66.8C

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16
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
water + mineral oil

A

IMMISCIBLE

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17
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
water + peppermint oil

A

IMMISCIBLE

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18
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
water + benzyl benzoate

A

IMMISCIBLE

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19
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
water + ether

A

PARTIALLY MISCIBLE

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20
Q

B. SOLUBILITY OF LIQUIDS IN LIQUIDS
addition of ______ , respectively shall increase the miscibility of water between non-polar solvents

A

GLYCERIN, PEG, ACETONE

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21
Q

refers to the mutual solubilities of the component in liquid-liquid system

A

MISCIBILITY

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22
Q

TYPES OF MISCIBILITY

A

COMPLETE MISCIBILITY
PARTIAL MISCIBILITY
IMMISCIBLE

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23
Q

TYPES OF MISCIBILITY
water and alcohol, glycerin and alcohol

A

COMPLETE MISCIBILITY

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24
Q

TYPES OF MISCIBILITY
ether and water, phenol and water

A

PARTIAL MISCIBILITY

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25
Q

TYPES OF MISCIBILITY
water and liquid petroleum

A

IMMISCIBLE

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26
Q

added to water to form hydroalcoholic solutions of various concentrations

A

ALCOHOL

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27
Q

TYPES OF MISCIBILITY
mixed with water to form dilute solution known as aromatic waters

A

VOLATILE OILS

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28
Q

TYPES OF MISCIBILITY
volatile oils mixed with water to form dilute solution known

A

AROMATIC WATERS

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29
Q

TYPES OF MISCIBILITY
added to alcohol to yield spirits and elixirs

A

VOLATILE OILS

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30
Q

TYPES OF MISCIBILITY
combined in collodions

A

ETHER AND ALCOHOL

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31
Q

C. EFFECT OF TEMPERATURE

A

POSITIVE HEAT
NEGATIVE HEAT

32
Q

C. EFFECT OF TEMPERATURE
solubility increases with increasing temperature. most of the salts show ___

A

POSITIVE HEAT

33
Q

C. EFFECT OF TEMPERATURE
solubility increases with decreasing temperature. salts like calcium sulfate and calcium hydroxide show ___

A

NEGATIVE HEAT

34
Q

C. EFFECT OF TEMPERATURE
most of salts show

A

POSITIVE HEAT

35
Q

C. EFFECT OF TEMPERATURE
salts like calcium hydroxide show

A

NEGATIVE HEAT

36
Q

C. EFFECT OF TEMPERATURE
when heat is neither absorbed nor given off, the solubility is not affected by variation of temperature as is nearly the case with sodium chloride

A

NEGATIVE HEAT

37
Q

D. EFFECT ON OTHER SUBSTANCE
It is a phenomenon by which gases are often liberate from solutions in which they are dissolved by th introduction of an electrolyte such as sodium chlorid and sometimes by a non-electrolyte such as sucrose

A

SALTING OUT

38
Q

D. EFFECT ON OTHER SUBSTANCE
The resultant escape of gas is due to the attraction of th salt ions or the highly polar non-electrolyte for the wate molecules, which reduces the density environment adjacent to the gas molecules

A

SALTING OUT

39
Q

Influence of Foreign Substances:
The addition of a substance to a binary liquid system produ ternary system, i.e., one having three components.

A

1- If the added material is soluble in only one of the components, the mutual solubility of the liquid pair is decrease

40
Q

Influence of Foreign Substances:
The addition of a substance to a binary liquid system produ ternary system, i.e., one having three components.

A

• 2- If the original binary mixture has an upper critical sol temp., the temperature is raised by addition of of the component
• 3- if it has a lower consolute temp., it is lowered by the additi the third component.
For example, if naphthalene is added to a mixture of pheno water, it dissolves only in the phenol and raises the constant temperature

41
Q

added to a phenol-water mixture, it dissolves only in water and raises the consolute temp.

A

POTASSIUM CHLORIDE

42
Q

When the third substance is soluble in both of the liquids to roughly the same extent, the mutual solubility of the liquid pair increased, an upper critical solution temp

A

LOWERED

43
Q

When the third substance is soluble in both of the liquids to roughly the same extent, the mutual solubility of the liquid pair increased, lower critical solution temp.

A

RAISED

44
Q

E. EFFECT OF PH
protonation of the anion can dramatically increase the solubility of the salt.

A

LOW PH

45
Q

This refers to the effect of adding an ion common to on already in equilibrium in a solubility reaction is t lower the solubility of the salt.

A

COMMON-ION EFFECT

46
Q

It is responsible for the reduction in the solubililty of a ionic precipitate when a soluble compoun combining one of the ions of the precipitate is adde to the solution in equilibrium with the precipitate.

A

COMMON ION EFFECT

47
Q

Importance of Solubility to Pharmacy

A
  • Permits the pharmacist to choose the best solvent medium for a drug or combination of drugs.
  • Helps in overcoming difficulties which arise: in the preparation of pharmaceutical solution
  • Serves as standard or test of purity.
48
Q

“Like dissolves Like”
dissolve ionic solutes and other polar substances.

A

POLAR SOLVENTS

49
Q

can dissolve non pola solutes like oils and fats, carbon tetrachloride benzene, mineral oil, alkaloidal bases and fatt acids.

A

NON POLAR COMPOUNDS

50
Q
  1. Factors Affecting Solubility of Drugs
A
  • Physicochemical properties of the solute and the solvent
  • Temperature
  • Pressure
  • ph of the solution
  • Presence of other substance to aid solubility
51
Q

a) Physicochemical properties of the drug

A

Ionized vs. Unionized forms

Particle size

Crystalline state

Drug complexes

52
Q

lower ionic strength favors solubility; solubility occurs faster with salt

A

Ionized vs. Unionized forms

53
Q

smaller particles increase surface al in contact resulting to solubility

A

PARTICLE SIZE

54
Q

amorphous form favors solubility

A

Crystalline state

55
Q

complexes like cyclodextrins enhance absorption

A

Drug complexes

56
Q

the solubility of a gas is expressed by Henry’s Law,. which states that at
constant temp, the concentration of dissolved gas is proportional to the partial pressure of the gas above the solution at equilibrium.

A

EFFECT OF PRESSURE

57
Q

Solubility of a gas increases directly as the pressure of the gas in the solution is increased and conversely, that the solubility of the gas decreases so that sometimes the gas escapes with violence when the pressure above the solution is released.

A

Importance of Henry’s law in pharmacy:

58
Q

This phenomenon is commonly effervescent solutions when the
recognize stop in container is removed.

A

EFFECT OF PRESSURE

59
Q

dissolve rapidly in a low pH environment.

A

WEAKLY BASIC DRUGS

60
Q

Solubility decreases with increasing pH

A

WEAK BASES

61
Q

dissolve well in a high pH environment.

A

WEAKLY ACIDIC DRUGS

62
Q

Solubility increases with increasing pH

A

WEAK ACIDS

63
Q

Frequently a solute is more soluble in a mixture of solvents than in one solvent alone. This phenomenon is known as cosolvency, and the solvents that, in combination, increase the solubility of the solute are called

A

CONSOLVENTS

64
Q

energy is released into the surroundings as heat. As a result, the temperature of the surroundings increases.

A

EXOTHERMIC

65
Q

energy is absorbed from the surroundings. As a result, the temperature of the surroundit

A

ENDOTHERMIC

66
Q

Obey Raoult’s law at every range of concentration; neither heat is evolved nor absorbed during dissolution

A

IDEAL SOLUTION

67
Q

total volume of solution is equal to sum of volumes o.
the components

A

IDEAL SOLUTION

68
Q

Examples: Dilute solutions; benzene + toluene; n-hexane + n-heptane; chlorobenzene + bromobenzene; ethyl bromide + ethyl iodide; n-butyl chloride + n-butyl bromide

A

IDEAL SOLUTION

69
Q

Do not obey Raoult’s law at every range of concentration;

A

NON IDEAL SOLUTION

70
Q

Either heat is evolved or absorbed during dissolution

Either volume of solution is increased after dissolutior or decreased during dissolution

A

NON IDEAL SOLUTION

71
Q

Examples: Acetone tethanol; water + methanol; water + ethanol; acetone + benzene; cyclohexane + ethanol

A

NON IDEAL SOLUTION

72
Q

Examples: Acetone + aniline; acetone + chloroform; chloroform + diethyl ether; water + HCl; acetic acid + pyridine; chloroform + benzene

A

NON IDEAL SOLUTION

73
Q

reduced in solution that contains an ion in common with that salt

A

solubility of a sparingly soluble salt

74
Q

AgCl + H20 = soluble
AgCl + H20 + NaCl • AgCl (ppt) + NaCl (aq. Solin)
Except: CuCl + H20 • CuCl (ppt) + H20
CuCl + H20 + 2HCl • CuCl + H20

A

COMMON ION EFFECT

75
Q

The solubility of a sparingly soluble salt is reduced in solution that contains an ion in common with that salt

A

COMMON ION EFFECT

76
Q

as the concentration of solute in a saturated solution in a certain temperature

A

SOLUBILITY IN QUANTITATIVE TERM

77
Q

defined as the spontaneous interaction of two or more substances to form a homogeneous molecule dispersion

A

SOLUBILITY IN QUALITATIVE TERM

PHYSICAL PHARMACY (1 decks)

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