Term
|
Definition
Absorption, distribution, metabolism, excretion
What happens to a drug when it enters the body |
|
|
Term
| What are the two routes of drug administration? |
|
Definition
| Extravascular and intravascular |
|
|
Term
| What are the two ways for intravascular drug administration? |
|
Definition
| Intravenous and intra-arterial |
|
|
Term
| What is a benefit to intravascular drug administration? |
|
Definition
| 100% of drug is available to the circulatory system |
|
|
Term
| List examples of extravascular drug administration |
|
Definition
| Oral, transdermal, suppositories, sublingual, subcutaneous, intramuscular, hypodermic |
|
|
Term
| If a drug is injected, is it 100% available to the circulatory system? |
|
Definition
| No, not necessarily. Intramuscular injection is not 100% absorbed. |
|
|
Term
|
Definition
| The peak concentration of drug in the body |
|
|
Term
| Will a drug concentration ever reach zero? |
|
Definition
No, due to half life, it theoretically never reaches zero.
After a while (4 half lives or so) we just pretend that it is zero. |
|
|
Term
| Describe the graph for an intravascular drug concentration in the body |
|
Definition
| Starts at Cmax and then approaches zero |
|
|
Term
| Describe the graph for an extravascular drug concentration in the body |
|
Definition
| Slowly increases as drug is absorbed to Cpeak (at Tmax) then reduces to approach zero |
|
|
Term
| What is Cpeak? When does Cpeak happen? |
|
Definition
| Cpeak is when an extravascular drug is at its highest blood concentration. The time this occurs is called Tmax |
|
|
Term
| What are the steps of oral absorption? |
|
Definition
Drug in stomach:
1. Disintegration
2. Dissolution (going into solution)
Then a percentage passes epithelium into circulation |
|
|
Term
| What factors affect absorption through GI epithelium? |
|
Definition
1. MW (lower, <500, is easier absorbed)
2. pKa
3. Solubility
4. Dosage form (liquid faster than tablet)
5. Anatomy and physiology of gut |
|
|
Term
|
Definition
| Various transport processes that take the drug from the site of absorption to general circulation |
|
|
Term
| What is the medium through which the drug distributes? |
|
Definition
|
|
Term
| List some factors that affect drug distribution |
|
Definition
| Body tissue characteristics, disease state, lipid solubility, regional pH differences, extend of drug protein binding |
|
|
Term
| What are some organs highly perfused with blood? What are some areas poorly perfused? |
|
Definition
High- heart, liver, lungs, kidneys
Medium- skeletal muscle
Low- fat tissue, brain, bone |
|
|
Term
| How would disease state affect drug distribution? |
|
Definition
| If there is a disease that affects blood perfusion, such as heart failure, drugs are less/slower distributed |
|
|
Term
| What form of a drug is more lipid/membrane soluble? |
|
Definition
|
|
Term
| What drug form is less fat soluble? |
|
Definition
Polar, hydrophyllic, ionized
Ex. Aminoglycosides |
|
|
Term
| Give an example of how regional differences in pH can trap a drug in a tissue |
|
Definition
Some drugs are unionized at 7.4 and pass into breast tissue. Once inside, they ionize due to acidic pH and become trapped.
Another example- urine |
|
|
Term
| List some common binding proteins found in the blood. How do they affect drug distribution? |
|
Definition
Albumin, α-acid glycoprotein, and lipoprotein
Bound drugs don't pass through membranes |
|
|
Term
| What is another term for metabolism? |
|
Definition
|
|
Term
|
Definition
| When drugs are acted on by liver enzymes and converted to metabolites (therapeutically inactive products) |
|
|
Term
| What is phase I of metabolic processes? |
|
Definition
| Oxidation, reduction, and hydrolysis |
|
|
Term
| What is phase II of metabolic processes? |
|
Definition
Conjugation (something added to the drug, often gluconic acid) to increase polarity
aka synthetic reactions |
|
|
Term
| What is the overall goal of metabolism? |
|
Definition
| To render a drug inactive and to make it more hydrophillic (polar) to be excreted in the urine |
|
|
Term
|
Definition
| The sum of metabolic and excretion processes in the body |
|
|
Term
| Renal excretion is the sum of what three kidney mechanisms? |
|
Definition
1. Glomerular filtration
2. Tubular secretion
3. Tubular reabsorption |
|
|
Term
| What is the most common mode of drug administration? |
|
Definition
|
|
Term
| What are downsides to oral drug administration? |
|
Definition
| Some is lost in degradation, drug absorbed in an unpredictable manner, drugs can't be given to patients with nausea, GI intolerance, or unconsciousness |
|
|
Term
| Other than urine, what ways can drugs be excreted? |
|
Definition
|
|
Term
|
Definition
Any route other than the GI tract (usually means injection)
para=outside enteron=intestine |
|
|
Term
| What is a requirement for parenteral drug formulations? |
|
Definition
|
|
Term
| List the parenteral needle routes from shortest needle to longest needle |
|
Definition
| Intradermal, subcutaneous, intravenous, intramuscular |
|
|
Term
|
Definition
| Intravenous and (less commonly) intratria, introduction of drug directly into vasculature |
|
|
Term
| What are benefits to intravascular administration? |
|
Definition
| Bypasses absorption, rapid and complete drug availability in systemic circulation, good for emergencies |
|
|
Term
| What are downsides to intravascular administration? |
|
Definition
| Painful, infection risk, requires skill and training to administer |
|
|
Term
|
Definition
| Administration into muscle tissue |
|
|
Term
| Where are the common sites of intramuscular injection? |
|
Definition
| Deltoid, vastus lateralis, gluteus |
|
|
Term
| When would intramuscular administration be used? |
|
Definition
| When a predictable and uniform absorption is desired over immediate effect |
|
|
Term
| What are downsides to intramuscular administration? |
|
Definition
| Slower, irritation around injection site, painful, requires skill/training to administer |
|
|
Term
| Define subcutaneous administration |
|
Definition
| Drug is injected into the connective tissue below the skin |
|
|
Term
| Why would subcutaneous injection be chosen? |
|
Definition
| If a slower rate of absorption is desired; to avoid an intense, short, frequent dosage |
|
|
Term
| What are classic examples of subcutaneous injections? |
|
Definition
| Insulin, sodium heparin (can't be oral and need to be absorbed slowly over hours) |
|
|
Term
| What is a benefit of subcutaneous over iv or im? |
|
Definition
| Subcutaneous doesn't require medical supervision and can be self administered |
|
|
Term
|
Definition
| Drug is injected into a skin layer, uncommon |
|
|
Term
| When would intradermal be used? |
|
Definition
| Usually for diagnostic and test procedures, such as allergy testing or PPD testing |
|
|
Term
| Define intrathecal administration |
|
Definition
| Drug is injected into spinal canal |
|
|
Term
| When is intrathecal administration used? |
|
Definition
| Spinal anesthesia, chemotherapy, or pain management |
|
|
Term
| Define intraperitoneal administration |
|
Definition
| Drug is injected into the peritoneum (aka paritoneal cavity), a serous membrane which forms the lining of abdominal cavity |
|
|
Term
| When would intraperitoneal administration be used? |
|
Definition
| When large amounts of blood replacement fluids or needed; when low blood pressure prevents use of suitable iv |
|
|
Term
| When would topical drug administration be used? |
|
Definition
| When localized effects are required |
|
|
Term
| What are the three categories of drug administration? |
|
Definition
| Oral, parenteral, topical |
|
|
Term
| Define inhalation administration |
|
Definition
| Nose/lung delivery system |
|
|
Term
| When would a nose inhalation administration be used? |
|
Definition
| If the drug is a decongestant |
|
|
Term
| When would a lung inhalation administration be used? |
|
Definition
Anti-asthmatic or to manage COPDs with bronchiodialators, corticosteroids
(Side note- Nebulizers are used if the patient cannot take a deep enough breath for a metered dose inhaler) |
|
|
Term
| Define dermal drug administration |
|
Definition
Drug is applied directly on the intended region to treat skin disorders
Also, transdermal administration is when drug is introduced into circulation after application to the skin |
|
|
Term
| Give an example of a disease requiring dermal topical administered drug |
|
Definition
|
|
Term
| Give an example of a transdermal topical administered drug |
|
Definition
| Scoplamine patch for motion sickness |
|
|
Term
| Define oral mucosal administration |
|
Definition
| Drug is administered in the form of gel or paste in the mouth for localized effect |
|
|
Term
| Give an example of a complaint requiring oral mucosal topical administered drug |
|
Definition
|
|
Term
| What form are rectal/vaginal administered drugs in? |
|
Definition
| Suppositories, ointments, or creams |
|
|
Term
| What sorts of diseases would require rectal/vaginal drug administration |
|
Definition
(I'm sure we all just got some lovely mental images)
Localized infection, hemorrhoids, inflammation |
|
|
Term
|
Definition
| Topical drug administration in the form of solution to treat various eye infections or to manage post operative eye |
|
|
Term
|
Definition
| Injection into the vitreous of the eye |
|
|
Term
|
Definition
| Injection directly into the heart. Rare. example: epinephrine in cardiac arrest |
|
|
Term
|
Definition
| Penile injection, often used to treat erectile dysfunction (phenylephrine) |
|
|
Term
|
Definition
| A homogenous molecular dispersion of two or more components |
|
|
Term
|
Definition
| The concentration of solute dissolved in a unit of solvent in equilibrium at a certain temperature |
|
|
Term
| How is solublilization related to precipitation? |
|
Definition
| They are in equilibrium and can shift to either side |
|
|
Term
| Define solubility constant Ksolubility |
|
Definition
| Ksolubility= solubilization rate/precipitation rate |
|
|
Term
| What are the three work-requiring steps of dissolution? |
|
Definition
1. Molecular breakdown of solute
2. Creation of molecular space for solute molecules
3. Integration of solute molecules |
|
|
Term
| Define heat of solution (ΔHsolution) |
|
Definition
| The heat absorbed per mole when a small quantity of solute is added to a large quantity of solution |
|
|
Term
| Give the formula for heat of solution (ΔHsolution) |
|
Definition
| ΔHsolution = ΔH sublimation + ΔH hydration |
|
|
Term
|
Definition
| Energy required to separate 1 mole of solute into its ions in gaseous states |
|
|
Term
|
Definition
| Heat liberation when one mole of gaseous ions are hydrated |
|
|
Term
| How are ΔH solution and solubility related? |
|
Definition
| The lower the ΔH solution, the more soluble (inversely related) |
|
|
Term
| Define solubility product |
|
Definition
A property of only slightly soluble electrolytes
AaBb ↔ aA+ + bB- |
|
|
Term
|
Definition
K'sp= [A+]a[B-]b
Make sure you know how to solve. For example, moles need to be doubled if 2 are produced in solution, then squared as indicated by the ^a and ^b above
Has the ' because it is not ideal mathematically |
|
|
Term
| When will a solution precipitate (based on ion product and solubility product)? |
|
Definition
| Precipitation will occur if ionic product > solubility product |
|
|
Term
| What happens if a common ion is added to a solution? |
|
Definition
| It shifts the equilibrium to the left (reducing solubility) because it increases ionic product |
|
|
Term
| What happens if an indifferent ion is added to a solution? |
|
Definition
| Equilibrium is shifted towards the right (increasing solubility) |
|
|
Term
| Why does an indifferent electrolyte increase solubility? |
|
Definition
| From his notes: Because it increases ionic strength, which reduces the "activity coefficient" of the sparingly soluble salt
From what I understand: Because the indifferent ions will bind to the solute ions, reducing common ion availability and forming more soluble products |
|
|
Term
| Define activity coefficient |
|
Definition
A function of the work of solubilization and the volumes of solute and solvent
Xideal x γ = X real
Relates real and ideal work of solubilization |
|
|
Term
| How does addition of an indifferent electrolyte decrease γ ? |
|
Definition
Ideal Ksp = γAB x [A+][B-]
So Ideal Ksp = γAB x Apparent Ksp
Apparent Ksp = Ideal Ksp / γAB
(γAB and Apparent Ksp are inversely related) |
|
|
Term
| Give an example of a clinical discovery where an indifferent ion was added into a solution |
|
Definition
Oral or iv administration of phosphate salts lowers serum calcium concentration in hypercalemic human subjects.
Once calcium was precipitated as CaHPO4, it could be eliminated |
|
|
Term
| Why does heating enhance solubility in liquids (most of the time)? |
|
Definition
| Because of LeChatlier's principle. Solubilization is usually endothermic, by adding heat the reaction can shift to lead to more solubilization |
|
|
Term
| How do cosolvents aid solubility? |
|
Definition
| Cosolvents aid in dissolving unionized molecules, especially if the solute is nonpolar |
|
|
Term
| When do cosolvents decrease solubility? |
|
Definition
If the solute is polar
(water is already polar so adding a nonpolar cosolvent would decrease solubility) |
|
|
Term
| List some common co-solvents |
|
Definition
| Glycerin, ethyl alcohol, propylene glycol, polyethylene glycol |
|
|
Term
| How does pH assist solubility? |
|
Definition
| Adding an acid or base promotes ionization, ionized solutes have strong ion-dipole interactions with water |
|
|
Term
| What is another way to represent HA ↔ H+ + A- ? |
|
Definition
S= So + Si
So is unionized
Si is ionized |
|
|
Term
| Give the Henderson-Hasselbach equation for solubility |
|
Definition
ph= pKa + log (S-So/So)
For weak acid
ph= 14- pKa + log (So/S-So)
For weak base |
|
|
Term
| What happens when alcohol is added to an aqueous solution of weak electrolytes? |
|
Definition
Increases the solubility of un-ionized species
Decreases solubility by raising pKa |
|
|
Term
| How do surfactants influence solubility? |
|
Definition
Increases:
Ionized drug remains in the water phase, unionized are allowed to reside in the hydrophobic core of micelles |
|
|
Term
|
Definition
| Enhances solubility to a maximum level before saturation; works through relatively weak forces such as hiding hydrophobicity |
|
|
Term
| Give some examples of complexing agents |
|
Definition
| Ammonia, caffeine, phenols, EDTA (chelation), cyclodextrins, molecular complexes PEG, PVP, methyl cellulose |
|
|
Term
|
Definition
| Cycles of glucose (with a cavity) that increase solubility of hydrophobic drugs through complexation (hiding hydrophobic groups in core) |
|
|
Term
|
Definition
| Modifying a drug so it is more soluble for transport across the membrane. After transport, metabolism turns it back into the active drug. |
|
|
Term
| Give an example of prodrug strategy |
|
Definition
| Methyldopa (active drug) is converted to methyldopate ester (prodrug) and solublized as hydrochloric salt for preparation of iv injection |
|
|
Term
| How does mitrometrics influence solubility |
|
Definition
| All he wants us to know is that decreasing particle size or asymmetry increases solubility |
|
|
Term
| List the steps of phase-solubility analysis |
|
Definition
1. Mix in increasing amount of solvent at constant temp and pressure
2. Separate undissolved solution and estimate dissolved solute
3. Plot solution concentration vs system concentration |
|
|
Term
| What is Gibb's phase rule |
|
Definition
F=C-P+2
Degrees of freedom= #components - #phases + 2 |
|
|
Term
| When calculating degrees of freedom, what are the degrees used? |
|
Definition
1. Concentration
2. Temperature
3. Pressure
Subtract them if they are constant! |
|
|
Term
| What do miscibility of liquids depend on? |
|
Definition
| Internal pressures (ex. polarity is a high internal pressure) |
|
|
Term
| Define complete miscibility |
|
Definition
| Solvents are miscible in any proportion |
|
|
Term
| If a solute is added to a binary liquid-liquid system, what happens? |
|
Definition
It is now a ternary system
A) If solute is only soluble in liquid, miscibility is decreased
B) If solute is equally soluble in both liquids, miscibility is increased (blending) |
|
|
Term
|
Definition
| Increased miscibility in a liquid-liquid system due to addition of a solute that is equally soluble in both liquids |
|
|
Term
| What happens when a solute is added to immiscible solvents? |
|
Definition
| The solute distributes itself between two layers in a definite ratio, K (distribution/partition coefficient)
K= C1(oil)/C2(water)
or
K= C1(water)/C2(alcohol) |
|
|
Term
| If a solute is ionizing in one of the solvents, what happens to the distribution coefficient? |
|
Definition
| It is now K' and you add the unionized form of the solute to the concentration where it is dissociating |
|
|
Term
| *I just want to include a note here that I did not attempt to make flashcards for the equation manipulations for the "distribution" notes. It is math rearrangement that does not translate well to flashcards. |
|
Definition
|
|
Term
| What is required for preservatives to work? |
|
Definition
They need to partition into microbes to work
ex. Benzoic acid needs to be in [HA], water phase |
|
|
Term
| Define octanol-water partician coefficient |
|
Definition
| An indication of lipophilicity or hydrophilicity of a drug. A drug with higher coefficient is stronger and longer lasting |
|
|
Term
| What is the octanol/water coefficient required for oral administration? |
|
Definition
| Log of the partition coefficient must be <5 |
|
|
Term
| What are Lipinski's rule for oral administration? |
|
Definition
An orally active drug has no more than one violation of the following criteria:
1. Not more than 5 hydrogen bond donors (nitrogen or oxygen atoms with one or more hydrogen atoms)
2. Not more than 10 hydrogen bond acceptors (nitrogen or oxygen atoms)
3. A molecular mass not greater than 500 daltons
4. An octanol-water partition coefficient[3] log P not greater than 5
Notice all the rules have multiples of 5 in them! |
|
|
Term
| What are benefits to oral solutions over oral tablets/capsules? |
|
Definition
-Better for infants, pediatrics, geriatic, psychiatric
-Therapeutically effective and diverse
-Minimizes "cheeking" |
|
|
Term
| What are disadvantages to oral solutions over oral tablets/capsules? |
|
Definition
-Less stable
-Some drugs are not soluble
-Must mask taste
-Bulky, hard to transport
-Requires patient measurement |
|
|
Term
| What are the three phase types of solutions? |
|
Definition
| Solids in liquids, liquids in liquids, gases in liquids |
|
|
Term
| What solutes, other than the drug, are often added to solutions? |
|
Definition
| Color, flavor, sweetness, stability, buffering salts, preservatives |
|
|
Term
| What is a consideration when adding dye to solutions? |
|
Definition
| The pH needs to be watched because the dye might precipitate out |
|
|
Term
| Give two examples of official aqueous saturated solutions |
|
Definition
|
|
Term
| List three auxiliary solvents |
|
Definition
| Alcohol, glycerin, propylene glycol |
|
|
Term
| What is a recent concern of using propylene glycol as a solvent? |
|
Definition
The WHO recently established a maximum daily intake (though there is no known toxicity dose)
Concerns of lethargy, apnea, and metabolic acidosis in pediatrics |
|
|
Term
| What are the three ways to get purified water? |
|
Definition
| Distillation, ion exchange treatment, or reverse osmosis |
|
|
Term
| What is the definition of a purified water? |
|
Definition
| When evaporated, it must not yield more than 0.001% residue (100x more pure than tap water) |
|
|
Term
| What are four types of USP waters? |
|
Definition
1. Purified water
2.Water for injection (most widely used)
3. sterile water for injection (packaged in single dose containers)
4. Bacteriostatic water for injection (contains antimicrobial agents) |
|
|
Term
|
Definition
| Ethanol, ethyl alcohol 95-96% |
|
|
Term
| Describe dehydrated alcohol, USP |
|
Definition
No less than 99.5% ethanol
Used where a water-free alcohol is desired |
|
|
Term
| Describe diluted alcohol, USP |
|
Definition
Useful mix of alcohol and purified water
49% |
|
|
Term
|
Definition
70% ethyl alcohol with water, denaturants, color/purfume, stabilizer
Denaturants discourage consumption |
|
|
Term
| Describe isopropyl rubbing alcohol |
|
Definition
70% or 91% isopropyl alcohol
With water, color/purfume, stabilizers
Used for hypodermic injections and disinfecting skin |
|
|
Term
| What is the first step in making a drug solution? |
|
Definition
Check the solubility of the drug
Remington's or Merck Index |
|
|
Term
| What units are solubility given in |
|
Definition
| Grams of solute per mL of solvent |
|
|
Term
|
Definition
A way to test if a drug will still be soluble under storage at non-standard temperatures
Solutions are subject to temperature elevations in 10 degree Celsius |
|
|
Term
| When heating a solution to dissolve a drug, what is important to remember? |
|
Definition
| Do not use concentrations higher than the solubility at room temperature |
|
|
Term
| In liquids, which three solvent combinations are miscible? |
|
Definition
1. Alcohol and water
2. Glycerin and water
3. Glycerin and alcohol |
|
|
Term
| What is the main concern of stability of solutions? |
|
Definition
|
|
Term
|
Definition
| a pharmacological or immunological agent that modifies the effect of other agents, such as a drug or vaccine, while having few if any direct effects when given by itself |
|
|
Term
| Define dry mixtures for reconstitution |
|
Definition
| Include everything besides the solvent (usually distilled water) |
|
|
Term
| Describe rehydration solutions |
|
Definition
| Things like pedialyte with lots of electrolytes, liquid and powder, should not be mixed with electrolyte containing liquids |
|
|
Term
| Define oral colonic lavage solution |
|
Definition
An osmotic laxative, has electolytes with polyethylene glycol
240mL every 10 minutes until 4L consumed |
|
|
Term
| Define magnesium citrate oral solution |
|
Definition
| A saline cathartic with citric acid, lemon oil, syrup, and carbonation |
|
|
Term
| Define sodium citrate and citric acid oral solution |
|
Definition
| Used to alleviate gout or uric acid by being an alkalinizer |
|
|
Term
|
Definition
| Sugared vehicles (little or no alcohol), pH varies, must be preserved against bacteria unless sucrose is greater than 65%w/w or 85%w/v |
|
|
Term
| What are the three types of syrup |
|
Definition
| Simple, flavoring, and medicinal |
|
|
Term
|
Definition
850g sucrose and 450mL water/L
Concentrated, but not saturated. Must make sure it is stable at the temperature needed. |
|
|
Term
| Do syrups have a higher or lower solvent power than water? |
|
Definition
| Lower (they are worse solvents) because there is already bonding between syrup and water |
|
|
Term
| What can replace sugar in syrups? |
|
Definition
Methylcellulose or hydroxyethylcellulose (important for diabetic patients
Cellulose (to increase viscocity) and artificial sweetener |
|
|
Term
| List some antimicrobial preservatives |
|
Definition
| Benzoic acid, sodium benzoate, methylparaben, polyparaben, alcohol, sorbic acid |
|
|
Term
|
Definition
Must be water soluble, synthetic or naturally occurring
Ex. orange oil, vanillin |
|
|
Term
| What are the three ways to preserve syrups |
|
Definition
| Solution with heat, agitation without heat, percolation |
|
|
Term
| Define inversion (in a syrup) |
|
Definition
Under heat, sucrose is hydrolyzed into dextrose and fructose (sweeter and darker)
Overheating causes caramelization (more susceptible to decomposition) |
|
|
Term
|
Definition
Forming an extract of sucrose to prepare a syrup
Uncommon |
|
|
Term
|
Definition
Clear, sweetened hydroalcoholic solutions
Alcohol 5-40%
Less effective in masking taste than syrups
Glycerin is often added to enhance solvent and act as preservative |
|
|
Term
| What are some advantages and disadvantages of elixers? |
|
Definition
Advantage: flexibility and ease of dosing
Disadvantage: alcohol content |
|
|
Term
|
Definition
Alcoholic or hydroalcoholic solutions prepared from vegetable or chemical substances (Nonvolatile)
Alcohol from 15-80%
Can't be mixed in diverse liquids, precipitation is common
Poor taste |
|
|
Term
| If a patient is on metronidazole or chloropropamide, what should they not have? |
|
Definition
Alcohol-containing substances
Disulfurrin reaction, very bad |
|
|
Term
|
Definition
| Aqueous or aleaginous solutions in the form of course droplets or as finely divided solids to be applied topically |
|
|
Term
|
Definition
| The amount of NaCl that is osmotically equivalent to 1g of the drug |
|
|
Term
| Describe aluminum acetate topical solution |
|
Definition
| Applied topically as an astringent wash; used in various types of dermatologic lotions/creams/pastes |
|
|
Term
| What is another term for CaOH topical solution? |
|
Definition
|
|
Term
| Define Coal Tar topical solution? |
|
Definition
| An alcoholic solution containing 20% coal tar and 5% polysorbate 80 (a nonionic surfactant) |
|
|
Term
| Define hydrogen peroxide topical solution |
|
Definition
| Local anti-infective for use topically on the skin |
|
|
Term
| Can you use ear products in the eye? Can you use eye products in the ear? |
|
Definition
| You can use eye products in the ear, but not the other way around |
|
|
Term
| Define chlorhexidine gluconate solution |
|
Definition
| Broad spectrum antiseptic, used as a surgical scrub and skin cleanser |
|
|
Term
| Define thimerosal topical solution |
|
Definition
| Water-soluble mercurial antibacterial and mild antifungal agent, also used as a preservative |
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Term
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Definition
| Solutions administered rectally for local effects (hydrocortisone) or for systemic absorption (aminophylline) |
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Term
| What are two examples of topical tinctures |
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Definition
| Iodine tincture, compound benzoin tincture (prepared by maceration) |
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Term
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Definition
| "to soak", a properly comminuted drug is permitted to soak in the menstuum until the soluble constituents are dissolved |
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Term
| Define spirits (essences) |
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Definition
Alcoholic solutions (>60%) of volatile substances
Separate from water, used as a flavoring agent, may be taken orally, topically, or inhaled |
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Term
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Definition
| Alcoholic or oleaginous solutions or emulsions of various medicinal substances intended to be rubbed on the skin |
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Term
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Definition
Liquid preparations composed of pyroxylin dissolved in a solvent mixture
Usually composed of alcohol and ether with or without medicinal substances |
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