Term
| the speed of a reaction is propotional to a paramater called the |
|
Definition
|
|
Term
| Energy necessary for the reaction to take place. can be reduced by catalyst |
|
Definition
|
|
Term
| units of rate constants for first order kinetics |
|
Definition
|
|
Term
| The study of drug stability under stress factors |
|
Definition
| Accelerated stability testing |
|
|
Term
| (T/F) Increase in temperature results in faster degradation rates of drugs |
|
Definition
|
|
Term
| quick estimate of drug stabilities |
|
Definition
|
|
Term
| the speed of many chemical reactions increases by ____to_____ times with 10 degrees Celsius rise in temperature |
|
Definition
|
|
Term
| The average Q10 for most drug degradations, can be used to do quick estimates of drug shelf lives. |
|
Definition
|
|
Term
| (T/F) shelf life decreases as temperature decreases |
|
Definition
| False-shelf life INCREASES as temperature decreases |
|
|
Term
| substance that increases the rate of a reaction with changing itself, decreases Ea subsequently increasing the rate constant |
|
Definition
|
|
Term
| T/F Many drugs in aqueous solution degrade faster because of the presence of water. |
|
Definition
|
|
Term
| When H30+ ions participate in the drug degradation, also has a slope of -1 in a plot of logk vs. pH. |
|
Definition
|
|
Term
| When OH- ions participate in the drug degradation process, a plot of logk vs pH has a slope of 1. |
|
Definition
|
|
Term
| When H2O molecules participate in the drug degradation process. |
|
Definition
|
|
Term
| When HA (Acid form) of buffer substance in aqueous solutions participates in drug degradation. Slope is not equal to 1 in a graph of logk vs. pH |
|
Definition
|
|
Term
| When A- (base form) of buffer substance in aqueous solutions participates in the drug degradation process. slope is not equal to 1 in a graph of logk vs. pH |
|
Definition
|
|
Term
| Stability is highest when the rate constant (k) is __________ |
|
Definition
|
|
Term
| T/F Light enery can not provide the energy of activation |
|
Definition
|
|
Term
| The cause of many photochemical drug degradations |
|
Definition
|
|
Term
| ________________ containers are used to protect drug substances from photodegradation |
|
Definition
|
|
Term
| Color that gives best protection from UV light |
|
Definition
|
|
Term
| Gives reasonable protection from UV light but not much against infrared light |
|
Definition
|
|
Term
| Which form is generally more pharmacologically active, D (dextro) or L (levo) |
|
Definition
|
|
Term
| Racemization usually follows _______ _________ kinetics |
|
Definition
|
|
Term
| Drugs containing _________ groups usually undergo hydrolysis. |
|
Definition
|
|
Term
| Most drugs have greater stabilities in pH of |
|
Definition
|
|
Term
| T/F OH- ions have greater catalytic effect than H3O+ ions |
|
Definition
|
|
Term
| may be added to reduce minor changes in pH that would induce significant degradation of the active ingredient |
|
Definition
|
|
Term
| Major cause of product instability |
|
Definition
|
|
Term
| used by drug companies to displace air from containers to avoid oxidation of drug formulations |
|
Definition
| Nitrogen and Carbon Dioxide |
|
|
Term
| T/F Decreases in temperature accelerate the rate of oxidation |
|
Definition
| False, INCREASES in temperature accelerate the rate of oxidation |
|
|
Term
| Oxidation rates may be affected by: |
|
Definition
| Temperature, Radiation, and Catalyst |
|
|
Term
| T/F Trace amounts of heavy metals will prevent oxidation of drug products. |
|
Definition
| False, trace amounts of heavy metals will CATALYZE oxidation of drug products ex: cupric, chromic, ferrous, ferric ions) |
|
|
Term
| used to sequester metal ions |
|
Definition
|
|
Term
| Ions that catalyze oxidation reactions |
|
Definition
|
|
Term
| Useful in increasing the stability of drug formulations undergoing chain reaction mediated oxidation |
|
Definition
| Antioxidants, ex: for aqueous ascorbic acid, sodium sulfite, and thiosulfate for oil: ascorbyl palmitate, hydroquinone, and alpha-tocopherol |
|
|
Term
| T/F Reductions are less common than oxidation |
|
Definition
|
|
Term
| how "non-changing" and drug products remains over a given length of time |
|
Definition
|
|
Term
| Five types of stability that must be considered for drug products |
|
Definition
1. Chemical
2. Physcial
3. Microbiological
4. Therapeutic
5. Toxicological
(CPMTT) |
|
|
Term
| Time the formulation remains within the desired potency and integrity when stored at recommended conditions. |
|
Definition
|
|
Term
| can be redispersed homogenously with moderate shaking and can be poured easily throught its shelf life, Crystal form, partical size, and physiological availability should be maintained throughout its shelf life |
|
Definition
|
|
Term
| resdispersed homogenously to its orginal state with moderate shaking, gross physical stability should be maintained |
|
Definition
|
|
Term
| Clarity, Color, and Odor are retained throughout its shelf life |
|
Definition
|
|
Term
| Retain their origianl size, shape, weight, and color throughout their shelf life. |
|
Definition
|
|
Term
| Should not soften, stick, harden, or crack throughout shelf life. should remain microbiologically uncontaminated over time |
|
Definition
|
|
Term
| High viscosity suspension that should maintain consistency throughout shelf life. |
|
Definition
|
|
Term
| The active ingredient in formulation has a potency less than pre-established goal, usually 90% of original potency |
|
Definition
|
|
Term
| Overtime a toxic degradation byproduct may form at unacceptable levels |
|
Definition
|
|
Term
| Most common solvent in pharmaceutical work |
|
Definition
|
|
Term
| Concentration of the solute in equilibrium with undissolved solute in a given solvent and temperature, the maximum extent to which solute can dissolve |
|
Definition
|
|
Term
| T/F Drug must be in solution before it can be absorbed and exert therapeutic action |
|
Definition
|
|
Term
| solute and solvent showed a SPONTANEOUS reaction to form a homogenous mixture such that nor more solute can be mixed with solvent. |
|
Definition
|
|
Term
| solute and solvent showed a SPONTANEOUS reaction to form a homogenous mixture such that more solute can be mixed with the solvent |
|
Definition
|
|
Term
| Solute and Solvent showed a NONSPONTANEOUS reaction to form homogenous mixture such that solute concentration exceeds solubility |
|
Definition
|
|
Term
|
Definition
| moles of solute in 1L solution |
|
|
Term
|
Definition
| Moles of solute in 1kg solvent |
|
|
Term
|
Definition
| gram-equivalent weight of solute in 1L solution |
|
|
Term
|
Definition
| moles of solute per solution total number of moles |
|
|
Term
| concentration of dissolved gas in equilibrium with gas above the the solution. |
|
Definition
| Solubility of gas in liquid |
|
|
Term
| Solubility of gas ___________ as pressure above the solution increases |
|
Definition
|
|
Term
| As temperature increases, the solubility of most gases __________. |
|
Definition
|
|
Term
| Addition of salts to dissolved gas solutions results in _________ gas solubility |
|
Definition
| decreasing, because the added salts compete for solvent molecules and mroe gas is released from the solution |
|
|
Term
| Gases that react with solvent ___________ their solubility |
|
Definition
| increase, ex: HCl gas, ammonia, CO2 |
|
|
Term
| ___________ miscibility is seen when liquids mix in all prportions |
|
Definition
|
|
Term
| ______________ miscibility: where completely dissolved solutions are seen only at certain temperatures and compositions. |
|
Definition
|
|
Term
| _________ solutions, solubility depends on heat of fusion and the melting point of the solute. |
|
Definition
|
|
Term
| Solutes and Solvents in Ideal Solutions are __________ chemicals |
|
Definition
|
|
Term
| example of ideal solution |
|
Definition
| naphthalene dissolved in benzene or toluene |
|
|
Term
| ___________ solutions also account for complexation, hydrogen bonding, and ionization |
|
Definition
|
|
Term
| Most pharmaceutical solutions are |
|
Definition
|
|
Term
| occurs when solute reacts with another substance in the solution to form a complex. Can either increase or decrease solubility |
|
Definition
|
|
Term
| Compounds with what functional groups can form hydrogen bonds with water, thereby increasing solubility |
|
Definition
|
|
Term
| T/F Aqueous solubility decreases with solute increase in carbon chains |
|
Definition
|
|
Term
| T/F The lower the melting point the lower the aqueous solubility |
|
Definition
| False, the HIGHER the melting point, the lower the aqueous solubility |
|
|
Term
| Chain branching of hydrophobic groups _________ aqueous solubility |
|
Definition
|
|
Term
| T/F Hydrophilic substituents increase aqueous solubility |
|
Definition
|
|
Term
| Solubility of solute is increased when salt is added |
|
Definition
|
|
Term
| Solubility of solute is decreased when salt is added |
|
Definition
|
|
Term
| Compounds which dissociate to a small extent in water |
|
Definition
|
|
Term
| When a common ion is added to a solution of sparingly soluble salt, the solubility is affected |
|
Definition
|
|
Term
| endothermic system, ∆Hsol is ____________. solubility __________with increasing temperature |
|
Definition
|
|
Term
| Exothermic solution: ∆Hsol is ___________, solubility _________ with increasing temperature |
|
Definition
|
|
Term
| No change in the system heat: ∆Hsol is ____________ and the solubility is _____ _____________ |
|
Definition
|
|
Term
| T/F ionized weak acids and bases have theoretically very high solubilities |
|
Definition
|
|
Term
| Acids are more soluble at _____pH |
|
Definition
|
|
Term
| Bases are more soluble at ______pH |
|
Definition
|
|
Term
| T/F solubility of strong electrolytes generally decreases as dielectric constant and/or polarity of solvent decrease |
|
Definition
|
|
