2. .

3. 3
Upon completion of this course, the students should able to:
 Demonstrate basic knowledge of basic concepts of physical
pharmaceutical principles essential for their pharmacy study in
the next years.
 Demonstrate basic knowledge of important pharmacy-related
physical principles in areas such as states of matter, phase
equilibrium and phase rule, solutions of non-electrolytes,
adsorption, solubility, buffers and isotonic solutions and
rheology. The course also presents basic understanding of types
of disperse systems and methods of their preparation and
assessment.

5. STATES OF MATTER
•The Four States of Matter
• Four States
• Solid
• Liquid
• Gas
• Plasma

6. STATES OF MATTER
Based upon particle arrangement
Based upon energy of particles
Based upon distance between particles

7. STATES OF MATTER
SOLIDS
•Particles of solids are
tightly packed, vibrating
about a fixed position.
•Solids have a definite
shape and a definite
volume.

8. The molecules of solid are locked in a rigid
structure and can only vibrate. (Add thermal
energy and the vibrations increase.)
Some solids are crystalline, like table salt, in
which the atoms are arranged in a repeating
pattern. Some solids are amorphous, like
glass, in which the atoms have no orderly
arrangement. Either way, a solid has definite
volume and shape.
SOLIDS

9. STATES OF MATTER
LIQUID
 Particles of liquids are
tightly packed, but are far
enough apart to slide over
one another.
 Liquids have an indefinite
shape and a definite
volume.

10. A liquid is virtually
incompressible and has
definite volume but no
definite shape, if you pour a
liter of juice into several
glasses, the shape of the
juice has changed but the
total volume hasn’t.
LIQUID

11. STATES OF MATTER
GAS
 Particles of gases are very far
apart and move freely.
 Gases have an indefinite shape
and an indefinite volume.
 If a container of CO2 is opened,
it will diffuse throughout the
room.

12. PHASE CHANGES
Description of
Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Solid to
liquid
Melting
Heat goes into the
solid as it melts.
Liquid to
solid
Freezing
Heat leaves the liquid
as it freezes.

13. PHASE CHANGES
Description of
Phase Change
Term for Phase
Change
Heat Movement During
Phase Change
Liquid to gas Vaporization,
Heat goes into the
liquid as it vaporizes.
Gas to liquid Condensation
Heat leaves the gas as
it condenses.
Solid to gas Sublimation
Heat goes into the solid
as it sublimates.

15. But what happens if you raise the
temperature to super-high levels…
between
1000°C and 1,000,000,000°C ?
Will everything
just be a gas?

16. STATES OF MATTER
PLASMA
 A plasma is an ionized gas.
 A plasma is a very good conductor of
electricity and is affected by magnetic
fields.
 Plasmas, like gases have an indefinite
shape and an indefinite volume.
• Plasma is the common state of matter in
the universe, since the insides of stars
are plasmas.

17. STATES OF MATTER
SOLID
LIQUID GAS PLASMA
Tightly packed, in
a regular pattern
Vibrate, but do
not move from
place to place
Close together with
no regular
arrangement.
Vibrate, move
about, and slide
Well separated with
no regular
arrangement.
Vibrate and move
freely at high
Has no definite
volume or shape
and is composed
of electrical
charged particles

18. The term fluid refers to gases and liquids.
Gases and liquids have more in common with
each other than they do with solids, since gases
and liquids both have particles that are free to
move around. They are not locked in place as
they are in a solid.
The hotter the fluid, the faster its molecules
move, and the more space the fluid will occupy.
Also, unlike solids, fluids can flow.
Fluids

19. Does Heat Affect Matter?

20. Fast Facts about Heat
The boiling point: is the temperature at
which a substance changes from a liquid
to a gas.
How does the movement of the particles
change as it nears the boiling point?
The particle move faster and faster until
they escape from the liquid.

21. Fast Facts about Heat
The freezing point: is the temperature at
which a substance changes from a liquid to
a solid.
How does this happen?
The particles move slower until they are
closer together.

22. Pressure & Freezing
For most liquids the freezing point increases if its
pressure is increased, i.e., it’s easier to freeze most
liquids if they’re subjected to high pressures. In order
to turn a liquids into a solid, the molecules typically
must get close enough together to form a crystal.
Low temps mean slow moving molecules that are
closer together, but high pressure can squeeze the
molecules closer together, even if they’re not moving
very slowly.

23. Water is an exception to this because,
due to its molecular shape, it expands
upon freezing. So, squeezing water
makes freezing it harder. The pressure
on ice due to a passing skater can
actually melt a small amount of the ice.
Pressure & Freezing

24. Pressure & Boiling
The lower the pressure on a liquid, the easier
it is to make it boil, i.e., as pressure
increases, so does the boiling pt.
This is because in order for a liquid to boil,
molecules need enough kinetic energy to
break free from the attraction of the
molecules around it. It’s harder for a liquid to
vaporize when subjected to high pressure,
since gases take up more space than liquids.

25. Water, for example, boils at temps below 100 ºC up
in the mountains where the air pressure is lower. It
takes longer to cook food in boiling water at high
altitudes because the boiling water isn’t as hot. In a
vacuum water will boil at any temp, since there is
no pressure at the surface to prevent the water from
vaporizing. At high pressure water boils at a high
temp. In a pressure cooker water can remain liquid
up to 120 ºC, and the hotter water can cook food
faster.
Pressure & Boiling

26. Freezing of Solutions
The freezing point of a solution, such as salt
water, is lower than the freezing point for the
solvent by itself, e.g., pure water. The higher the
concentration of the solute, e.g. salt, the more the
freezing point is lowered.
The reason it is more difficult to freeze a liquid
when a substance is dissolved in it is because the
“foreign” molecules or atoms of a solute interfere
with the molecules of the solvent as they’re trying
to form a crystalline structure.

27. Boiling and Evaporation
Evaporation takes place only
at the surface of a liquid or
solid, while boiling takes
place throughout the body of
a liquid.
Boiling occurs at the boiling
temperature.
Particles that have “higher
kinetic energy” escape and
become vapor (gas).

28. Factors affecting the rate of evaporation: