surface tension part 1

Khalifa M.Asif Yunus
M.Pharm (Pharmaceutics)
J I I U ’ S
Ali-Allana College of Pharmacy Akkalkuwa
NBAAccredited
Asst. Prof.
Pharmaceutics Department
Ali-Allana college of pharmacy Akkalkuwa
E-mail: khalifa4517@gmail.com Mob. No. +91 9925064346

Watch this video for better understanding
https://www.youtube.com/watch?v=XvxZ4XLDkR8&t=162s
Introduction of Surface tension

 The boundary between two phases is generally described as an
interface
 When one of the phase is a gas or a vapor, the term surface is
frequently used.
 These terms surface and interface can be used interchangeably
in some cases.

By: Khalifa M Asif Y Asst. Professor Pharmaceutics Dept. AACOP Akkalkuwa
Solid Phase
Gas Phase (air)
Solid Surface

Liquid Surface
Liquid Phase
Gas Phase

Liquid Phase
Solid Phase
Solid-Liquid
interface

Liquid-Liquid
interface
Liquid Phase
Liquid Phase

Surface Tension
The surface tension (γ) is defined as : The force in dynes acting along
the surface of a liquid at right angle to any line 1 cm in length.
Units of Surface Tension
 In CGS system is dynes per centimeter (dyne cm–1).
 In SI system, the unit is Newton per meter (Nm–1).

Surface molecules pulled
inward
Interior molecules pulled
equally in all direction

Surface tension is caused by the net inward pull on the surface
molecules.
At the bulk of the liquid;
 Molecules in the interior experience an attractive force from
neighboring molecules which surround on all sides
At the liquid surface:
 Molecules on the surface have neighboring molecules only
on one side and thus experience an attractive force which
tends to pull them into the interior

 The net effect is that the molecules at the surface of the liquid
experience an inward force toward the bulk of the liquid.
 Such force results in what is called Surface Tension.
 Due to this unbalanced forces, the surface of the liquid
behaves like a stretched elastic membrane containing the
molecules of the liquid inside.

 since the liquid tends to contract to a minimum area, the surface
of the liquid appears to be in a state of tension, so in order to
increase the area of the surface it is necessary to do work to bring
the molecules from the bulk of the liquid to the surface against
the inward attractive force.

Due to these unbalanced forces the liquid tends to adjust itself to
give a minimum surface area, which takes the form of a sphere and
for this reason
 Liquid rises in capillary tubes
 Droplets acquire spherical shape

1.Formation of spherical globules in emulsions.
The phenomenon of surface tension is responsible for following
processes. (Significance)

2. Formation of nearly spherical shape of falling water droplets.

3. Formation of spherical shape of mercury
particle on flat surface.

4. Rise of liquid in capillary tube.

5. Formation of hemispherical surface i.e.
lower meniscus.

Adhesional and Cohesional forces
Adhesional forces : Are forces which act between molecules of
different phases.
Cohesional forces : Are forces which act between molecules of the
same phase.
 Cohesional force tend to keep the phases separate while
adhesional forces tend to increase the affinity of two phases
 If adhesive force > cohesive force results;
• Wetting • Spreading • Rising in the tube

Interfacial Tension
“The tension existing at the interface between two immiscible
liquids. “
“The force per unit length existing at the interface between two
immiscible liquid.”
 When two liquid are completely miscible, the interface can not
be observed and hence, do not possess interfacial tension. E.g.
water & alcohol.

Factors influencing Surface and Interfacial tension
Internal
Factors
External
Factors
As temp increases the S.T of liquids
decreases due to enhance kinetic
energy that weakens cohesive force.
Water : 72.8
Benzene : 28.9
CCl4 : 26.7
Electrolyte increase S.T
S.A. Agents decreases S.T
Intermolecular
attractive forces

surface tension part 1

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surface tension part 1