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Drug Delivery > Test #2 > Flashcards

Test #2 Flashcards

1
Q

Coarse Dispersion

A

Greater than 500nm

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2
Q

Colloidal Dispersion

A

Less than 500nm

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3
Q

Phase separation depends on:

A

Temperature and composition

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4
Q

Common Solvents

A
  • Purified water
  • Alcohol
  • Dehydrated alcohol
  • Rubbing alcohol
  • Glycerin
  • Propylene glycol
  • Oils
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5
Q

Common Solutes include:

A
  • Drugs
  • Flavors and Sweeteners
  • Colorants
  • Preservatives
  • Stabilizers
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6
Q

Solutions include:

A
  • Syrups
  • Elixirs
  • Tinctures
  • Spirits
  • Aromatic Waters
  • Injectables
  • I.V. Drug infusion
  • Oral drug solutions
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7
Q

Colligative Properties

A
  • Osmotic pressure
  • Vapor pressure
  • Boiling point
  • Freezing point
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8
Q

Additive properties:

A
  • Molecular weight
  • Mass of a solution
  • Volume
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9
Q

Constitutive properties:

A
  • Solubility

- Interfacial energy

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10
Q

Properties of an ideal solution:

A
  • Intermolecular bonding is equivalent
  • No heat absorbed or evolved when mixed
  • No change in volume when mixed
  • Vapor pressure is proportional to molar fraction
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11
Q

Raoults Law:

A

Partial pressure of a volatile solution is equal to VAPOR PRESSURE OF PURE CONSTITUENT (Po) * MOLE FRACTION (X)

Pi=PioXi

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12
Q

Non-ideal solutions:

A
  • In vapor: intermolecular interaction is negligible

- For real solutions (A-A, B-B, A-B) activity coefficient is 1

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13
Q

High activity coefficient =

A

Weaker interaction with solvent

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14
Q

Low activity coefficient=

A

Stronger interactions with solvent

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15
Q

Activity =

A

Activity coefficient (Yi) * Mole fraction (Xi)

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16
Q

Henry’s Law:

A

Psolute = kCsolute
k=Henry’s law constant
Csolute=Concentration of solute

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17
Q

Dissolution Enhancement Methods:

A
  • Gentle heating
  • Particle size reduction
  • Using solubilizing agents
  • Using agitation
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18
Q

Molarity:

A

Moles/liter

Temperature dependent

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19
Q

Molality:

A

Moles/kilogram

NOT temperature dependent

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20
Q

Percent by weight (w/w)%:

A

Grams of solute/100g of solution

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21
Q

Percent by volume (v/v)%:

A

Milliliters of solute/100ml of solution

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22
Q

Percent weight by volume (w/v)%:

A

Grams of solute/100ml of solution

23
Q

Ratio strength:

A

Grams/ml

24
Q

Pharmaceutical advantages of a salt compared to it’s parent drug:

A
  • Solubility
  • Bioavailability
  • Physical stability
  • Chemical stability
  • Mechanical properties
  • Ease of crystallization
  • Taste
  • Melting point
25
Q

Ph=pKa where on ionization curve?

A

At 50%

26
Q

At 1 unit above or below pH on ionization curve you are at:

A

91%, 9%

27
Q

At 2 units above or below pH on ionization curve you are at:

A

99%, 1%

28
Q

Solubility:

A

Amount of solute that can be dissolved in a unit volume of a solvent to for a saturated solution

29
Q

Unsaturated solution:

A

Solution with concentration below equilibrium solubility

30
Q

Supersaturated solution:

A

Solution that contains a solute at a concentration higher than that of a saturated solution
*It is unstable - excess solute tends to leave solution in bubbles or crystals, etc…

31
Q

Intrinsic Solubility:

A

Equilibrium solubility of the drug molecule

32
Q

Apparent solubility:

A

Sum of all species of the drug in solution

33
Q

Solubility of a gas:

A

Concentration of gas that is in equilibrium with the pure gas

34
Q

Solubility of gases change with what?

A
  • Decrease in pressure

- Increase in temperature

35
Q

What happens when you add an electrolyte like NaCl to an aqueous solution of a gas?

A

You decrease it’s solubility - it salts out

36
Q

Activity of a drug can be thought of as:

A

Effective concentration

37
Q

What affects activity?

A
  • Melting temperature

- Heat of fusion

38
Q

What does NOT affect activity?

A

-Solvent

39
Q

Does Hsoln depend on the solvent in the Van’t Hoff equation?

A

YES!

40
Q

Does Hf in the Van’t Hoff equation depend on solvent?

A

No!

41
Q

Can Hsoln in Van’t Hoff equation be a negative value?

A

Yes!

42
Q

Can Hf in the Van’t Hoff equation be a negative value?

A

No, it is always positive

43
Q

What do co-solvents do?

A
  • Increase solubility of drugs with poor aqueous solubility

- Reduce the H-bond density of water

44
Q

What factors affect solubility?

A
  • pH
  • Temperature
  • Solid form
  • Particle size
  • Solvent
  • Pressure
45
Q

Acidic drugs precipitate out where?

A

In the stomach

46
Q

Basic drugs precipitate out where?

A

In the intestine

47
Q

Drugs in a co-solvent precipitate out where?

A

In the blood

48
Q

Salting out:

A

Ions STRENGTHEN solvent structure to make it more difficult to insert drug

49
Q

Salting-In:

A

Ions WEAKEN solvent structure to make it easier to insert drug molecules

50
Q

Solubility of a drug depends on:

A
  • Salt concentration

- Type of salt

51
Q

Effects related to Ionic Strength:

A
  • Solubility (salting-in/salting-out)

- Activity of ions (Ksp of salt, pH of solution, etc…)

52
Q

The state of a solvent can be:

A
  • Solid
  • Liquid
  • Super critical fluid
  • Gas
53
Q

True or False: Mole fraction and molality are both independent of temperature.

A

TRUE!

54
Q

True or False: For dilute aqueous solutions molarity and molality values are essentially equivalent.

A

TRUE!

Drug Delivery (1 decks)

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