pharmaceutics exam 3 Flashcards
(197 cards)
what are solutions
what may solutions be
“Liquid preparations that contain one or more chemical substances dissolved in a suitable solvent or mixture of mutually miscible solvents”.
Solutions may be,
- Oral
- Otic
- Opthalmic
- Topical
What is the maximum concentration to which a solution can be prepared with that agent and solvent?
Attractive forces- what do they cause molecules to do
Repulsive forces- what does it cause molecules to do
Dipolar molecules-
Hydrogen bonding-
in solution, are there are attractive or repulsive forces
what do you want a balance of
what atoms of hydrogens move close to
what molecules also form hydrogen bonds
Solute must dissolve – attractive forces cause molecules to cohere and adhere to each other based on their attractiveness
Repulsive: prevents the molecules from interpenetrating each other
In a solution, there are both but if they are equal then the potential energy is minimal – do not have too many attractive or repellent forces and that’s when the solution is most stable and dissolved
Want a balance of both attractive and repulsive forces
Dipolar molecules align to each other based on negative and + end
Hydrogen atoms move in close to electronegative atoms (i.e., F, O, N)
Hydrogen bonds exist also with
Esters, Carboxylic acids, Aldehydes, Polypeptides
How to improve solubility conditions
What options are available to pharmacists?
what consists of 0.03% iodine
can use:
Different solubilizing agents
Different chemical salt form of medicinal agent
Alteration of the pH of a solution
Partial or whole substitution of a solvent
Example; 1g of iodine granules in 3,000 mL (0.03% iodine)
Alternative: dissolve in Potassium Iodide, Sodium Iodide
Iodine Topical Solution, USP (contains 2% iodine, 2.4% sodium iodide)
How do you make sure that solute gets into solution:
what do undissolved solutes need to do
in dissolved solution, what does the solvent have a higgher affinity for
How do you make sure that solute gets into solution: excipients – additives to improve solubility.
Example: pure water, can add some alcohol
Undissolved solute: water/solvent needs to overcome the balance of attractions between the solute molecules (so the affinity for one molecule for another); solvent needs to be able to overcome the solute-solute attraction to make a solute-solvent attraction
- (easier to do for monovalent molecules or molecules where at least ine atom is monovalent than a molecule that is multivalent).
- Need to overcome the attraction of the solute
In dissolved, the solvent has a higher affinity for the solute and was able to overcome the solute-solute attraction
Want a solute-solvent interaction.
The potential energy is a mimimum and you have a more stable solvent
When the exact solubility is not known (or has yet to be
determined), general expressions of relative solubility may be used.
what are they and how many are there
what is the unit
what do you need to do if you have more and more insoluble particles
Very Soluble <1
Freely Soluble 1-10
Soluble 10-30
Sparingly Soluble 30-100
Slightly Soluble 100-1000
Very Slightly Soluble 1,000-10,000
Practically Insoluble >10,000
or Insoluble
all in parts per whole
More and more insoluble: need more and more solvent
what Factors influence solubility
what is a positive heat of solution
what is a negative heat of solution
Temperature:
- “Positive heat of solution”
pH of the solution:
Weak acids or weak bases
Physical agitation:
Extent to which solvent passes over solute
Particle size:
Finer the powder, greater the surface area, the more rapid dissolving process
Most drugs have a positive heat of solution so they dissolve with heat. Some might have a negative heat of solution, and do not dissolve and this makes things worse
Solubility: Beneficial considerations
are salts more or less soluble in water
what are organic bases most soluble in
is alcohol more or less lipophlic
Salts of organic compounds are more soluble in water compared to their organic base counterparts.
Organic bases are more soluble in organic solvents
Like prefers like
For atropine 455.0 mL of water for 1 g of drug
For atropine sulfate 0.5 mL of water for 1 g of drug
Alcohol is more of a lipophilic environment so molecules might dissolve better.
- this is why for drugs that are not as soluble in water, alcohol is used as an alternative
“like dissolves like”
wha do solvents need in order to dissolve
what are organic molecules most soluble in and what is the exception
what are examples of polar groups
do halogens increase or decrease solubility and why
what happens in Cl or F is added
Solvents having chemical structures most similar to the solute will most likely dissolve it.
For i.e., organic compounds are more soluble in organic solvents compared to in water.
One exception is if organic compound has polar functional group.
Polar groups are:
OH, CHO, COH, CHOL, CH2OH, COOH,
NO2 and SO3H – dissolve well in water
In general, halogen atoms decrease solubility
–Because of an increase in MW without proportionate increase in polarity
If Cl or F is added, then there is more MW without the proportional increase in polarity which is why the single addition of a Cl or F does not improve solubility but actually decreases it
Inorganic MOLECULES
what does monovalent mean
If cation and anion of an ionic compound are monovalent, what is easily overcome
what is you have two ions
what happens in the catiion and anion are multivalent
how much solubility is there for this
are ammonium and quaternary ammonium salts water or lipid soluble
what kind of molecules are water insoluble
If cation and anion of an ionic compound are monovalent, solute-solute attractive forces are easily overcome by the solvent. Not very strong
(i.e., NaCl, LiBr, KI).
Same is true if one of the two ions in an ionic compound is monovalent (i.e., BaCl2, MgI2)
If both the cation and anion are multivalent, the solute-solute interaction may be too great to overcome (i.e., CaSO4, BaSO4) by the solvent
This results in POOR WATER SOLUBILITY
Ammonium and quaternary ammonium salts are water soluble
Phosphates, Carbonates, Silicates, Borates, and Hypochlorites are water insoluble (except for their alkali metal salts and ammonium salts).
organic MOLECULES
molecules what number of polar functional groups is sufficient to solubilize chain lengths with how many carbons
what is more soluble: branched or straight chains
how does MW affect water solubility
what is can increase in structural similarity between solutes result in
Molecules having one polar functional group is sufficient to solubilize chain lengths consisting of 5 carbons
Molecules having branched chains are more soluble than corresponding straight-chain compounds
Water solubility decreases with increase in molecular weight (like with adding F, increase in MW without proportional increase in solubility)
Increased structural similarity between solute and solvent = increased solubility (remember: “like dissolves like”)
Solvents for liquid preparations
Alcohol, USP: Ethyl alcohol, ethanol, C2H5OH
A primary solvent for many organic compounds
When mixed with water = hydroalcoholic mixture
Alcohol USP is 94.9% to 96.0% C2H5OH by volume, when determined at 15.56 °C
15.56 °C (U.S. government standard temp. for alcohol determinations).
Dehydrated Alcohol, USP contains not less than 99.5% C2H5OH.
Want to promote solute, solvent interactions
add ethyl alcohol to be a part of solution
Dehydrated: less water
for drugs not soluble in water, what is a suitable alternative and why
what are examples of insoluble agent
when alcohol is too much, what can be used
are the limits of alcohol content for For children < 6 years, 6-12 and 12+
For drugs not soluble in water, alcohol is preferred as a suitable alternative due to its miscibility in water and ability to dissolve many water insoluble agents.
For e.g., Drug agents, flavorants, antimicrobial preservatives.
When alcohol content is too much, glycerin and glycols can be used to reduce total amount of alcohol needed.
FDA proposed for manufacturers of OTC oral drug products
For children < 6 years of age alcohol limit is 0.5%
For children 6 to 12 years of age, limit is 5%
For children over 12 years of age & adults limit is 10%
Diluted Alcohol, NF
how is it prepared
since liquids tend to contract, what is the final volume
what is diluted alcohol useful for
Prepared by mixing equal parts of alcohol USP with purified water
Since liquids tend to contract during mixing the final volume is generally 3% less than what otherwise should be expected.
For example, if 50 mL of each component is combined the result is 97 mL.
Dilute alcohol is a useful hydroalcoholic solvent in various pharmaceutical processes and preparations
Rubbing Alcohol
how much ethyl alcohol does it have
To discourage oral ingestion each, how much of a certain solution is added to each ____mL of solution – how does it taste
what is the denaturant that is employed called
what is it made of
Rubbing alcohol contains about 70% ethyl alcohol by volume, remaining is water, denaturants (with or without color additives and perfume oils and stabilizers).
To discourage oral ingestion each 100 mL must contain not less than 355mg of sucrose octa-acetate (or 1.4 mg of denatonium benzoate) which has a bitter taste and discourages internal use.
Internal Revenue Service- U.S. Treasury Department, the denaturant employed is called Formula 23-H
8 Parts (by volume) of acetone
1.5 Parts (by volume) of methyl isobutyl ketone
100 parts (by volume) of ethyl alcohol
Glycerin, USP (Glycerol)
A clear syrupy liquid with a sweet taste
Miscible in water and in alcohol
Glycerin is naturally viscous, but can be made less viscous by heating
Can be used as a preservative or stabilizer
Can also be used for internal applications in addition to external use
Isopropyl rubbing alcohol
how much isopropyl alcohol does it have
where is it used
how much of it is used to prepare diabetc needles and syringes
what is a rubefacient and what is its mechanism
Isopropyl rubbing alcohol, ~70% isopropyl alcohol.
Remaining components are water (with or without colorants), stabilizers and perfumes.
Used externally as *rubefacient and soothing rub vehicle for topical purposes.
To prepare diabetic needles and syringes for hypodermic injections of insulin, a commercially available ~91% isopropyl rubbing alcohol is used also.
- “A rubefacient is a substance for topical application that produces redness of the skin e.g. by causing dilation of the capillaries and an increase in blood circulation”
Propylene glycol, USP
Viscous liquid, miscible in alcohol and water
Relatively nontoxic liquid that is practically colorless, odorless, and tasteless.
Used as a solvent for flavors, extracts, drugs, food antioxidants as well as a heat transfer medium
Can substitute for glycerin in pharmaceutical formulations
Purified Water, USP, H20
Must meet U.S. Public Health Service regulations with respect to bacteriologic purity.
Drinking water should be,
Clear, colorless, odorless, neutral or slightly acidic or alkaline.
Tap water not acceptable for manufacturing or extemporaneous compounding
Contains 0.1% of solids per 100 mL of evaporated H2O
Possible chemical incompatibilities between solids and drug agent could result.
Signs that chemical incompatibilities have occurred
Precipitation, discoloration, effervescence
Preparation of solutions
usually, which is greater amount of solute or solvent
how are pharmaceutical preparations expressed
what are
W/V
V/V
W/W
what are the unfavorable interactions
usually, the amount of solute is far less than the amount of solvent
pharmaceutical preparations are expressed in percent strength
W/V:
percent weight in volume
- solids in liquids
V/V:
percent volume in volume
liquids in liquids
W/W: percent weight in weight
- solids in semisolids
unfavorable interactions to know:
- Liquid pharmaceuticals for oral administration to patient usual dose = 5 (one teaspoonful), 10, 15 mL (one tablespoon).
Purified Water, USP, H20
how is it obtained/what kinds are there
how many impurities does it have in comparison to drinking water
when evaporated how much is in solid form
what is it used for
Distillation, Ion exchange treatment, reverse osmosis
As a result, fewer impurities than drinking water
When evaporated no more than 0.001% total solid (1 mg of solids per 100 mL of water)
Used in the preparation of aqueous dosage forms (except for IV administered drug substances)
Considerations for pharmacists
some chemical agents do what
what can you do
Some chemical agents take longer to dissolve.
what you can do to help with this
- Apply heat
- Reduce particle size of the solute
- Use a solubilizing agent
- Apply vigorous agitation
Which of the following would suggest that your newly prepared solution contains chemical incompatibilities?
A) Effervescence
B) Discoloration
C) Precipitation
D) A and B only
E) A, B and C
All of them!
Signs that chemical incompatibilities have occurred
Precipitation, discoloration, effervescence
From slide 21 :)
Dry Mixtures for Solution
it contains everything for formulation except what
after reconstitution, where should it be placed, and for how long
with any remaining amounts, what should the pharmacist tell the patient?
what are examples of this
what needs to be done for oral powders
Dry mixtures for solution contain all of the required components of the formulation (i.e, colorants) EXCEPT the solvent.
Following reconstitution using required volume of liquid solution, it should be stored in the refrigerator for a period not to exceed what’s written on label.
Typically 7 to 14 days
Pharmacist to instruct patient to discard remaining
Examples are,
Cloxacillin Sodium for Oral Solution, USP- an anti-infective antibiotic
Penicillin V Potassium for Oral Solution, USP- an anti-infective antibiotics
Potassium Chloride for Oral Solution, USP- a potassium supplement
For oral: powder that needs to be reconstituted
Oral Solutions
When will a pharmacist be required to dispense a commercially prepared oral solution?
- commercial
- pediatric
- bulk
When will a pharmacist be required to dispense a commercially prepared oral solution?
When necessary to dilute a commercial preparation
When necessary to prepare a pediatric solution by reconstitution of a dry powder
When necessary to extemporaneously compound an oral solution from bulk components