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43 Cards in this Set
- Front
- Back
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Boyle's Law
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PV= k
-constant temp |
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Charles Law
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V= kT
-constant pressure |
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Gay-Lussac's Law
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P=kT
-constant volume |
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Ideal Gas Law assumptions
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no intermolecular interactions
elastic collisions no energy exchange |
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Pharmaceutics
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science of dosage form design
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Dosage Form
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physical form of drug intended for administration
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what does a dosage form contain?
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active drug
excipients |
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heat
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form of energy transferred from one place to another due to temperature difference
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calorie
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amount of heat energy to raise 1 g of water 1 C
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state of a system can be defined by which four values?
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n, P, V, T
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endothermic rxn
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enthalpy change > 0
heat flow from surroundings into system |
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exothermic rxn
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enthalpy change < 0
heat flows from system to surroundings |
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first law of thermodynamics
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energy must be conserved from one form to another
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second law of thermodynamics
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every system wants to reach an equilibrium
process by which system reaches equilibrium is via entropy entropy is always increasing |
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third law of thermodynamics
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entropy of a pure crystalline substance is zero at absolute zero
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Gibbs Free Energy minimized when
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system reaches equilibrium at constant pressure and temperature
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Gibbs Free Energy = 0 when...
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system at equilibrium
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Absorption
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transition from low to high energy state
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Emission
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transition from high to low energy state
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true solution
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mixtures of 2+ components that form a homogenous molecular dispersion
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what concentrations change with temperature?
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% w/v, % v/v, M
-i.e. anything with volume |
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assumptions of dilute aqueous solutions
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%w/w = %w/v
m = M |
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relationship between vapor pressure and boiling point
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high vapor pressure --> low boiling point
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relationship between vapor pressure and temperature
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increased vapor pressure w/ increased temperature
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Properties of Ideal Solution
(in terms of entropy, enthalpy, and volume change) |
enthalpy of mixing = 0
volume change upon mixing = 0 entropy change of mixing is NOT zero --> not enthalphy driven, but entropy driven |
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Negative Deviation (of ideal solutions)
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solvent-solute interactions stronger than solute-solute and solvent-solvent
-lower than predicted |
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Positive Deviation (of ideal solutions)
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solvent-solute interactions weaker than solute-solute and solvent-solvent
-higher than predicted |
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Behaviors of Real Solutions
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-follows Raoult's Law as a solvent
-follows Henry's Law as a solute |
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relationship between solubility and dissolution rate
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increased solubility with increased dissolution rate
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relationship between dissolution rate and oral absorption rate
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increased oral absorption rate with increased dissolution rate
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when do undersaturated solutions crystallize?
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-decreased temperature
-solvent evaporation |
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relationship between melting point and solubility
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increased melting point--> lower solubility (if structures otherwise similar)
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buffer capacity
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concentration of strong base required to change pH by one unit
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methods of buffer preparation
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combine HA and A- directly
add strong base to weak acid or strong acid to weak base |
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what does diffusivity depend on?
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solute, temperature, medium
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rheology
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science that describes flow and deformation of matter under stress
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viscocity
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resistance of fluid material to flow under stress
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relationship between viscocity and resistance
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high viscocity--> greater resistance
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shear
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movement of material relative to parallel layer
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shear stress
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force/unit area to bring about flow
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shear rate
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difference in velocity between two planes of liquids separated by a distance
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how do you make something spread faster or thinner?
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increase the shear rate
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slope of rheogram
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viscoity
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