Surfactants Flashcards
What is a surface? What is an interface? What are the types of interfaces?
surface
- outer boundary of a material
interface
- each surface is an interface
- molecules at the interface have different properties compared to molecules in the bulk of the phases on both sides
gas-liquid = solution gas-solid = tablet liquid-liquid = emulsion liquid-solid = suspension solid-solid = layered tablets
What is surface tension?
surface tension
- unbalanced forces on liquid surface which result in a state of tension
- force that must be applied parallel to the surface so as to counterbalance the net inward pull
What are surfactants?
surface active agents
- surfactants are compounds of amphiphilic nature, i.e. their chemical structure displays two distinct regions = hydrophobic non-polar regions and hydrophilic polar regions
What are the types of surfactants?
anionic surfactants
cationic surfactant
non-ionic surfactant
amphoteric surfactants = both positive and negative charge
How do surfactants work?
surfactants adsorb at the interface
the hydrophilic region (head) is dissolves well in the water
- remains in contact with aqueous solution
the hydrophobic region is not soluble in the hostile aqueous medium
- ‘escapes’ from the hostile aqueous environment and expands/dissolves in the air/oil
adsorbed surfactant molecule replace water molecules at the surface
- net inward pulling force (water become concave to try to reduce SA and minimise surface tension) reduces which reduces surface tension
- surface tension become stable when the interface is saturated with surfactants
When do micelles form?
micelles form when the interface is saturated with surfactants
- surfactants are forced to submerge in water due to saturation
micelles form at critical micelle concentration
- when increasing surfactant has not effect on surface tension
- consists of 50 monomers of surfactants
What can micelles be used for?
micelles can be used to increase the solubility of hydrophobic drugs
- micelle centre resembles a separate organic phase
- drug can be held in the centre of a reverse micelle = increases solubility as the hydrophobic tails are facing outward. these can pass through the lipid bilayer
reverse micelles
- hydrophilic heads face inwards
- hydrophobic tails face outwards
what are emulsions?
an emulsion is a disperse system in which an insoluble (immiscible) liquid phase is dispersed in a second liquid phase
- oil in water
- water in oil
What are the types of emulsions? What are their properties?
depends on droplet size
- coarse emulsion = 10 micrometers to 100 micrometers
- fine emusions - 0. 1 to 5 micrometers
- microemulsions (colloidal) = 10 nanometers - 100 nanometers
What are the advantages of emulsions?
deliver poorly soluble drugs
mask the taste of therapeutic drugs
oral administration of therapeutic drugs
reduce drug irritancy of topical application
emulsions for total parenteral nutrition
What are the disadvantages of emulsions?
poor physical stability
- difficult to disperse immiscible liquids
- separate easily
- coalesce at the top
What is the required HLB?
rHLB is the HLB value required to most effectively form an emulsion for a given oil
How do surfactants increase the stability of emulsions?
when a hydrophilic and hydrophobic surfactants are both employed, they interact on the interface
this interaction results in a mechanically robust interfacial film
- prevents disruption and coalescence of droplets and gives greater lowering of the interfacial tension.
hydrophilic colloidal polymers
- starch, cellulose
Why are emulsions unstable? How can it be stabilised?
they have a high gibbs free energy = unstable
- internal area cannot be reduced = droplets would coalesce
- surface tension must be reduced = surfactant
natural tendency is to separate to revert to state of lowest energy
- not suitable as emulsion will not be dispersed
What are the factors affecting stability of emulsions?
flocculation - reversible - droplets aggregate towards each other creaming - droplets combine and rise to the top coalescence and breaking - irreversible - droplets joining to form bigger droplets and a layer at the top miscellaneous physical and chemical changes phase inversion