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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
TYPES OF MISCIBILITY water and liquid petroleum
IMMISCIBLE
26
added to water to form hydroalcoholic solutions of various concentrations
ALCOHOL
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TYPES OF MISCIBILITY mixed with water to form dilute solution known as aromatic waters
VOLATILE OILS
28
TYPES OF MISCIBILITY volatile oils mixed with water to form dilute solution known
AROMATIC WATERS
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TYPES OF MISCIBILITY added to alcohol to yield spirits and elixirs
VOLATILE OILS
30
TYPES OF MISCIBILITY combined in collodions
ETHER AND ALCOHOL
31
C. EFFECT OF TEMPERATURE
POSITIVE HEAT NEGATIVE HEAT
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C. EFFECT OF TEMPERATURE solubility increases with increasing temperature. most of the salts show ___
POSITIVE HEAT
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C. EFFECT OF TEMPERATURE solubility increases with decreasing temperature. salts like calcium sulfate and calcium hydroxide show ___
NEGATIVE HEAT
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C. EFFECT OF TEMPERATURE most of salts show
POSITIVE HEAT
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C. EFFECT OF TEMPERATURE salts like calcium hydroxide show
NEGATIVE HEAT
36
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
NEGATIVE HEAT
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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
SALTING OUT
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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
SALTING OUT
39
Influence of Foreign Substances: The addition of a substance to a binary liquid system produ ternary system, i.e., one having three components.
1- If the added material is soluble in only one of the components, the mutual solubility of the liquid pair is decrease
40
Influence of Foreign Substances: The addition of a substance to a binary liquid system produ ternary system, i.e., one having three components.
• 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
added to a phenol-water mixture, it dissolves only in water and raises the consolute temp.
POTASSIUM CHLORIDE
42
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
LOWERED
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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.
RAISED
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E. EFFECT OF PH protonation of the anion can dramatically increase the solubility of the salt.
LOW PH
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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.
COMMON-ION EFFECT
46
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.
COMMON ION EFFECT
47
Importance of Solubility to Pharmacy
- 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
"Like dissolves Like" dissolve ionic solutes and other polar substances.
POLAR SOLVENTS
49
can dissolve non pola solutes like oils and fats, carbon tetrachloride benzene, mineral oil, alkaloidal bases and fatt acids.
NON POLAR COMPOUNDS
50
3. Factors Affecting Solubility of Drugs
- Physicochemical properties of the solute and the solvent - Temperature - Pressure - ph of the solution - Presence of other substance to aid solubility
51
a) Physicochemical properties of the drug
Ionized vs. Unionized forms Particle size Crystalline state Drug complexes
52
lower ionic strength favors solubility; solubility occurs faster with salt
Ionized vs. Unionized forms
53
smaller particles increase surface al in contact resulting to solubility
PARTICLE SIZE
54
amorphous form favors solubility
Crystalline state
55
complexes like cyclodextrins enhance absorption
Drug complexes
56
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.
EFFECT OF PRESSURE
57
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.
Importance of Henry's law in pharmacy:
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This phenomenon is commonly effervescent solutions when the recognize stop in container is removed.
EFFECT OF PRESSURE
59
dissolve rapidly in a low pH environment.
WEAKLY BASIC DRUGS
60
Solubility decreases with increasing pH
WEAK BASES
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dissolve well in a high pH environment.
WEAKLY ACIDIC DRUGS
62
Solubility increases with increasing pH
WEAK ACIDS
63
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
CONSOLVENTS
64
energy is released into the surroundings as heat. As a result, the temperature of the surroundings increases.
EXOTHERMIC
65
energy is absorbed from the surroundings. As a result, the temperature of the surroundit
ENDOTHERMIC
66
Obey Raoult's law at every range of concentration; neither heat is evolved nor absorbed during dissolution
IDEAL SOLUTION
67
total volume of solution is equal to sum of volumes o. the components
IDEAL SOLUTION
68
Examples: Dilute solutions; benzene + toluene; n-hexane + n-heptane; chlorobenzene + bromobenzene; ethyl bromide + ethyl iodide; n-butyl chloride + n-butyl bromide
IDEAL SOLUTION
69
Do not obey Raoult's law at every range of concentration;
NON IDEAL SOLUTION
70
Either heat is evolved or absorbed during dissolution Either volume of solution is increased after dissolutior or decreased during dissolution
NON IDEAL SOLUTION
71
Examples: Acetone tethanol; water + methanol; water + ethanol; acetone + benzene; cyclohexane + ethanol
NON IDEAL SOLUTION
72
Examples: Acetone + aniline; acetone + chloroform; chloroform + diethyl ether; water + HCl; acetic acid + pyridine; chloroform + benzene
NON IDEAL SOLUTION
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reduced in solution that contains an ion in common with that salt
solubility of a sparingly soluble salt
74
AgCl + H20 = soluble AgCl + H20 + NaCl • AgCl (ppt) + NaCl (aq. Solin) Except: CuCl + H20 • CuCl (ppt) + H20 CuCl + H20 + 2HCl • CuCl + H20
COMMON ION EFFECT
75
The solubility of a sparingly soluble salt is reduced in solution that contains an ion in common with that salt
COMMON ION EFFECT
76
as the concentration of solute in a saturated solution in a certain temperature
SOLUBILITY IN QUANTITATIVE TERM
77
defined as the spontaneous interaction of two or more substances to form a homogeneous molecule dispersion
SOLUBILITY IN QUALITATIVE TERM

PHYSICAL PHARMACY (1 decks)

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