1. Interfacial phenomena are important in pharmacy for drug adsorption, penetration through membranes, emulsion formation and stability, and suspension of insoluble particles. 2. Surface tension is the inward force at the liquid interface, while interfacial tension exists between immiscible liquids. Temperature, additives, and molecular interactions influence surface/interfacial tensions. 3. Several methods measure these tensions, including the capillary rise, Du Nouy ring, and drop weight methods. Surface-active agents are amphiphilic molecules that adsorb at interfaces and are used as wetting, solubilizing, and emulsifying agents in pharmaceutical formulations.

1. Prepared by:
Rohit Kamboj
Assistant Professor
GGS College of Pharmacy

2. Introduction
 Interface is the boundary between two or more phases exist
together
 Several types of interface can exist depending on whether the two
adjacent phases are in solid, liquid or gaseous state.
 Importance of Interfacial phenomena in pharmacy:
 Adsorption of drugs into solid adjuncts in dosage forms
 Penetration of molecules through biological membranes
 Emulsion formation and stability
 The dispersion of insoluble particles in liquid media for suspensions.

3. Surface and Interfacial Tensions
• In the liquid state, the cohesive forces between adjacent
molecules are well developed.
For the molecules in the bulk of a liquid
• They are surrounded in all directions by other molecules
for which they have an equal attraction.
For the molecules at the surface (at the liquid/air interface)
 Only attractive cohesive forces with other liquid molecules
which are situated below and adjacent to them.
 They can develop adhesive forces of attraction with the
molecules of the other phase in the interface.
Liquid Interface

4. Surface Tension
 Thus SURFACE TENSION [γ ]
is the force per unit length that
must be applied parallel to the
surface so as to counterbalance
the net inward pull and has the
units of dyne/cm.
 INTERFACIAL TENSION is the force
per unit length existing at the interface
between two immiscible liquid phases and
has the units of dyne/cm.
 If two liquids are completely miscible, no
interfacial tension exists between them.

5. • Internal Factors : The surface tension is observed in liquids
due to Intermolecular attractive forces.
• External Factors : When substances are added to liquids, these
alter the surface and interface tension. Example are Surface
active agents decreases Surface tension
• Effect of Temperature: As temp increases the Surface tension
of liquids decreases due to enhance kinetic energy that weakens
cohesive force. At critical temp Surface tension is 0.
Factors influencing Surface
and Interfacial tension

6.  Methods for measuring surface and interfacial tension
1- Capillary rise method
2- Ring (Du Nouy) tensiometer
3- Drop weight method (Stalagmometer)
4- Drop Count Method
 The choice of the method for measuring surface and
interfacial tension depend on:
 Whether surface or interfacial tension is to be determined.
 The accuracy desired
 The size of sample.

7. 7
Capillary Rise Method
When a capillary tube is placed in a liquid, it rises up the
tube a certain distance. By measuring this rise, it is possible
to determine the surface tension of the liquid. It is not
possible, to obtain interfacial tensions using the capillary
rise method.
 Cohesive force is the force existing between like mole-
cules in the surface of a liquid
Adhesive force is the force existing between unlike
molecules, such as that between a liquid and the wall of a
glass capillary tube
 When the force of Adhesion is greater than the cohesion,
the liquid is said to wet the capillary wall, spreading over it,
and rising in the tube.
The Principle

8. 8
The upward component of the force resulting from
the surface tension of the liquid at any point on the
circumference is given by:
Thus the total upward force around the inside
circumference of the tube is
Where
Ө = the contact angle between the surface of the
liquid and the capillary wall
2 π r = the inside circumference of the capillary.
For water the angle Ө is insignificant, i.e. the liquid wets
the capillary wall so that cos Ө = unity
Cont. angle
water and glass
a = γ cos Ө
a = 2 π r γ cos Ө

9. 9
The downward force of gravity
Downward component b = (mass x acceleration)
b = (mass x acceleration + w)
= Volume x density x acceleration
= cross-sectional area x height x density x acceleration
At Maximum height, the opposing forces are in equilibrium
i.e. a=b
Where:
h = the height of the liquid column to the lowest point of the meniscus
p = density of the liquid
g = the acceleration of gravity
w = the weight of the upper part of the meniscus.
2 π r γ = π r 2 h p g
γ = 1/2 r h p g
π r 2 x h x p x g

10. Ring (Du Nouy) Tensiometer
 the principle of the instrument depends on the fact that:
the force necessary to detach a platinum-iridium ring
immersed at the surface or interface is proportional to the
surface or interfacial tension.
 The force of detachment is recorded in dynes
on a calibrated dial
 The surface tension is given by:
Where:
F = the detachment force
R1 and R 2= the inner and outer radii of the ring.
γ = F / 2 π (R1 + R2)
 For measuring surface and interfacial tensions.
The principle

11. 11
If the volume or weight of a drop as it is detached from a tip of
known radius is determined, the surface and interfacial tension can
be calculated from
Where m = the mass of the drop
V = the volume of the drop
p = the density of the liquid
r = the radius of the tip
g = the acceleration due to gravity
 The tip must be wetted by the liquid so as
the drop doesn’t climb the outside of the tube.
γ1 = vρ1g
2 π rn¹
Drop Weight and Drop volume method
γ2 = vρ2g
2 π rn2
Drop Count
γ1/γ2 = ρ1n2/ρ2n1
Drop Weight
γ1/γ2 = W1/W2

12. 12
When a liquid such as oleic acid is placed on the surface of other liquid
like water, it will spread as a film if the adhesion force is greater than the
cohesive forces.
The term film applies to a duplex film as opposed to monomolecular
film.
Duplex films are sufficiently thick so that surface and interface are
independent of one another.
Spreading coefficient
γ L
γ S
γ Ls

13. 13
As surface or interfacial work is equal to surface tension multiplied by the
area increment.
The work of cohesion, which is the energy required to separate the
molecules of the spreading liquid so as it can flow over the sub-layer=
Where 2 surfaces each with a surface tension = γ L
The work of adhesion, which is the energy required to break the attraction
between the unlike molecules =
Where: γ L =the surface tension of the spreading liquid
γ S =the surface tension of the sublayer liquid
γ LS =the interfacial tension between the two liquids.
Spreading occurs if the work of adhesion is greater than the work of
cohesion, i.e. Wa > Wc or Wa - Wc > 0
Wc = 2 γ L
Wa = γ L + γ S - γ LS

14. Wc = 2 γ L
Wc = γLΔA + γLΔA
S= WA-
Wc
Wc = 2 γLΔA
ΔA=1cm
Work of Cohesion
Wc = 2γL-----1
γ L
γ L
Wa = γ L ΔA + γ S ΔA - γ LSΔA
Work of Adhesion
Wa = γ L + γ S - γ LS ------2
γ L
γ S

15. 15
Spreading Coefficient is The difference between
the work of adhesion and the work of cohesion
S = Wa - Wc = (γ L + γ S - γ LS ) - 2 γ L
S = γ S - γ L - γ LS
S = γ S – (γ L + γ LS )
Spreading occurs (S is positive) when the surface tension of the sub-layer
liquid is greater than the sum of the surface tension of the spreading liquid
and the interfacial tension between the sub-layer and the spreading liquid.
If (γ L + γ LS ) is larger than YS , (S is negative) the substance forms globules
or a floating lens and fails to spread over the surface.

16. 16
Application of Spreading coefficient in pharmacy
 The requirement of film coats to be spreaded over the
tablet surfaces.
 The requirement of lotions with mineral oils to spread on
the skin by the addition of surfactants.

17. 17

18. ADSORPTION:
 It is surface effect.
 E.g. concentration of alkaloid molecule on the surface
of clay.
ABSORPTION:
 Gas or liq penetrates in to the capillary spaces of
absorbing medium.
 The taking up of water by a sponge is absorption.
18

19.  Positive adsorption:
The concentration of dissolved material on the interface
is higher than that of solution internal.
 Negative adsorption:
The concentration of dissolved material on the interface
is less than that of solution internal.
19

20. 20
 Molecules and ions that are adsorbed at interfaces are termed
surface active agents, surfactants or amphiphile
 The molecule or ion has a certain affinity for both polar and
nonpolar solvents.
 Depending on the number and nature of the polar and nonpolar
groups present, the amphiphile may be hydrophilic, lipophilic or be
reasonably well-balanced between these two extremes.
 It is the amphiphilic nature of surface active agents which causes
them to be adsorbed at interfaces, whether these be liquid/gas or
liquid/liquid.

21. Surface active agent

22. 22
Functional Classification
According to their pharmaceutical use, surfactants can be
divided into the following groups:
 Wetting agents
 Solubilizing agents
 Emulsifying agents
 Dispersing, Suspending and Defloculating agents
 Foaming and antifoaming agents
 Detergents

23. 23
A scale showing classification of
surfactant function on the basis of
HLB values of surfactants.
The higher the HLB of a surfactant
the more hydrophilic it is.
Example: Spans with low HLB are
lipophilic. Tweens with high HLB are
hydrophilic.

24. Adsorption at Solid interface
 A gas or liquid is adsorbed on solid surface.
 The material used to adsorb gas or liquid (solid) is
known as adsorbent.
 The substance that is attached to the surface of the
solid is called adsorbate.
 The degree of adsorption of gas by a solid depends on
1. Nature of adsorbent and its surface area.
2. Nature of adsorbate and the partial pressure of gas.
3. Temp.
24

25. Type of adsorption.
Physical adsorption Chemical adsorption
Reversible Irreversible
Weak van der Waals forces Strong chemical bond
Non-specific More specific
Common at low temp Occurs at high temp
Heat of adsorption is low (20 to 40
kj/mole)
Heat of adsorption is high (40 to 400
kj/mole)
e.g. adsorption of gases on charcoal e.g. adsorption of oxygen on silver or
gold.
25
Combination of both type of adsorption is known as sorption.
Desorption : adsorbed molecules or ions are removed from the
solid surface.

26. Adsorption at solid/gas interface
 Adsorption of gas is important in following area
1. Removal of objectionable odors from the room.
2. Prevention of obnoxious gases entering in to the
body (gas masks)
3. Estimation of surface area and particle size of
powders.
 The amount of gas adsorbed per unit area or unit
mass of solid is measured at diff pressure of the gas
at constant temp.
 The graph of amt of gas ad./unit A or m of solid Vs
pressure is known as adsorption isotherm.
26

27. Freundlich isotherm
 The relationship between pressure of the gas and amt
adsorbed at constant temp has been expressed by
freundlich isotherm eqn:
 Where x = wt of gas adsorbed per unit wt of adsorbent,m
 P= equilibrium pressure, k and n = constant.
 This eqn gives curvilinear graph when (x/m) is plotted
against pressure p.
 The constant k and n are evaluated from the exp and they
depends on temp and nature of the adsorbent and
adsorbate.
27
n
kP
m
x
y /1


28. Freundlich isotherm
28
x/m
p Log
(x/m) Log p
Slope =
1/n
Intercept =
k

29. Langmuir Adsorption
 The following assumptions are made for this:
1. The surface of solid posses fixed number of active
sites for the adsorption of gases.
2. At max adsorption, the gas layer that is found
around the solid is of only one molecule thick.
3. The rate of adsorption (condensation) is
proportional to number of sites unoccupied.
4. The rate of evaporation (desorption) is proportional
to the number of occupied sites.
29

30. Langmuir Adsorption
 The adsorption of gas on the solid surface depends on
the pressure of the gas in the experimental conditions.
 At a particular pressure, p,
 Fraction of site occupied : Ө
 Fraction of sites unoccupied: (1-Ө)
 Rate of adsorption: r1 = k1(1-Ө)P,
 Rate of desorption: r2 = k2Ө,
 Where k1 and k2 are proportionality constants for the
process of adsorption and desorption.
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31.  At equilibrium : r1 = r2
 If we consider,
 y= mass of gas adsorbed/g of adsorbrnt
 ym= mass of gas that 1 g of adsorbent can take up when a
monolayer is complete.
31
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