1. SOLUTION AND COLLOID SPECIFIC LEARNING OBJECTIVE
At the end of the session the student should be able to explain:
Definitions of Solution and Colloids
System of Solutions and Colloids
Type of Solutions and Colloids

2. INTRODUCTION Types of solution Concentration SOLUTION
No.1
INTRODUCTION
Types of solution
No.2
Concentration
No.3
SOLUTION
Solution properties
No.4
Dialysis
No.5

3. SOLUTION INTRODUCTION MATTER Definition Classification Mixture
No. 1
MATTER
Definition
Classification
State of matter
Mixture
Pure substance

4. THE STATE OF MATTER
Matter
Solid
Liquid
Gas

5. CLASSIFICATION OF MATTER
Mixture
Pure substance
Homogeneous mixture
Heterogeneous mixture
Element
Compound

6. HOMOGENEOUS MIXTURE Homogenous mixtures called solutions And
Their distant relatives, colloidal suspensions

7. Solutions
Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms, molecules, or ions
These uniformly distributed particles are too small to reflect light, and as a result solutions are transparent (clear) – light passes through them

8. SUBSTANCES OF SOLUTIONS
Solute
Solvent
The most abundant substance in a solution is called solvent
The substance is dissolved in a solvent is called solute

9. SOLUTE Solute Electrolyte Nonelectrolyte
A solute that when dissolved in water forms a solution that conducts electricity.
Nonelectrolyte
A solute that when dissolved in water forms a solution that does not conduct electricity.

10. HEATS OF SOLUTION Heat is usually absorbed or released when a
solute dissolves in a solvent.
The process is endothermic, if heat is absorbed, and solution becomes cooler.
The process is exothermic, if heat is released, and solution temperature increases.
Endothermic : Solute + Solvent + Heat
Solution (NH4NO3 in water)
Exothermic : Solute + Solvent
Solution + Heat (NaOH in water)

11. INTRODUCTION Types of solution Concentration SOLUTION
No.1
INTRODUCTION
Types of solution
No.2
Concentration
No.3
SOLUTION
Solution properties
No.4
Dialysis
No.5

12. SOLUTION Types of solution Chemical term Medical term
No. 2
Chemical term
Medical term
Unsaturated
Saturated
Super saturated
Hypotonic
Isotonic
Hypertonic

13. Classification of Solubility
Chemical term
SOLUBILITY
Classification of Solubility
Three classify of solubility of a compound
1. Soluble
2. slightly soluble
3. insoluble

14. Soluble substances dissolve completely in the solvent and form solution
Insoluble substances do not dissolve in the solvent
The term immiscible is used to describe a liquid solute that does not dissolve in a liquid solvent

15. SOLUBILITY 1. Soluble 2. slightly soluble 3. insoluble
Depend on the Polarity
1. Soluble
2. slightly soluble
3. insoluble
Three type of polarity of a compound :
1. Polar
2. Semipolar
3. Nonpolar

16. UNSATURATED, SATURATED AND SUPERSATURATED SOLUTIONS
SOLUBILITY
Saturated solution, is a solution that contains the maximum amount of a solute in a given solvent, at a specific temperature.
Unsaturated solution, is a solution that contains less solute that it has the capacity to dissolve.
Supersaturated solution, contains more solute than is present in a saturated solution

17. SUPERSATURATED SOLUTIONS
Supersaturated solutions are usually prepared by forming a nearly saturated solution at a high temperature and then slowly cooling the solution to a lower temperature at which the solubility is lower. Such solutions are not stable. The addition of small amount of solid solute (or even a dust particle) will usually cause the excess solute to crystallize out of solution until the solution becomes saturated.

18. CRYSTALLIZATION CONVERTS A SUPERSATURATED SOLUTION TO A SATURATED SOLUTION
A supersaturated Seed crystal is added After excess solute is
solution and induces rapid crystallized, the
crystallization remaining solution is
saturated

19. SOLUTION Types of solution Chemical term Medical term
No. 2
Chemical term
Medical term
Unsaturated
Saturated
Super saturated
Hypotonic
Isotonic
Hypertonic

20. Hypotonic, Isotonic and Hypertonic solutions
Medical term
Hypotonic, Isotonic and Hypertonic solutions
Hypotonic solutions : the solution with the lower concentration of solute
If the concentration of water in the medium surrounding a cell is greater than that of the cytosol. Water enters the cell by osmosis
Isotonic solutions : the solution being compared have equal concentration of solutes.
When red blood cells are placed in a 0.9% salt solution, they neither gain nor lose water by osmosis
Hypertonic solutions : The solution with the higher concentration of solutes.
If red cells are placed in sea water (about 3% salt), they lose water by osmosis and the cells shrivel up.

21. Red blood cells in the Hypotonic, Isotonic and Hypertonic solutions
with hypotonic
solution
Red blood cells
with isotonic
solution
Red blood cells
with hypertonic
solution

22. INTRODUCTION Types of solution Concentration SOLUTION
No.1
INTRODUCTION
Types of solution
No.2
Concentration
No.3
SOLUTION
Solution properties
No.4
Dialysis
No.5

23. continued to next slide
SOLUTION
Concentration
No. 3
Molarity (M)
Percent (%)
Molarity (M) :
a solution concentration that is expressed in term of the number of moles of solute contained in a liter of solution.
Percent : a solution concentration that expresses the amount of solute in 100 parts of solution.
continued to next slide

24. continued to next slide
SOLUTION
Concentration
No. 3
Molality (m)
Normality (N)
Molality (m) :
a solution concentration that is expressed in term of the number of moles of solute contained in a kilogram of solvent.
Normality (N) : a solution concentration that is expresses in term of the number of gram equivalent of solute contained in a liter of solvent.
continued to next slide

25. Continuation :
Weight/weight percent : a concentration that expresses the mass of solute contained in 100 mass units of solution.
Weight/volume percent : a concentration that expresses the grams of solute contained in 100 ml of solution.
Volume/volume percent : a concentration that expresses the volume of liquid solute contained in 100 volume of solution.

26. DILUTION The volumetric scales of concentration are
those, like molar concentration and normality,
in which the concentration is expressed on a
volumetric scale, the amount of solute per
fixed volume of solution, when the
concentration is expressed on a volumetric
scale, the amount of solute contained in a
given volume of solution is equal to the
product of the volume and the concentration:
Amount of solute = volume x concentration
continued

27. If a solution is diluted, the volume is increased
and the concentration is decreased, but the
total amount of solute is constant. Hence, two
solutions of different concentrations but
containing the same amounts of solute will be
related to each other as follows:
Volume1 x concentration1 = Volume2 x concentration2
continued

28. If any three terms in the above equation are
continued
If any three terms in the above equation are
known, the fourth can be calculated. The
quantities on both sides of the equation must
be expressed in the same units

29. INTRODUCTION Types of solution Concentration SOLUTION
No.1
INTRODUCTION
Types of solution
No.2
Concentration
No.3
SOLUTION
Solution properties
No.4
Dialysis
No.5

30. SOLUTION Colligative properties (continued to next slide)
SOLUTION PROPERTIES
No. 4
Electrical conductivity and
colligative properties
Colligative properties (continued to next slide)

31. COLLIGATIVE PROPERTIES
The properties that depend only on the concentration of solute particles present and not on the actual identity of the solute.
Three closely related colligative properties are
1. Vapor pressure
2. Boiling point
3. Freezing point
4. Osmotic pressure

32. The equation for calculated the boiling point or freezing point difference between pure solvent and solution
Δ tb = nKbm
Δ tf = nKfm
Δ t is the boiling point or freezing point difference between pure solvent and solution.
Kb and Kf are constants characteristic of the solvent used in the solution.

33. for example : Calculate the boiling and freezing points of the following solutions
171.0 g of sugar (C12H22O11) is dissolved in 1.00 kg of water, Kb = C/m and Kf = C/m
Answer :
a. To fine the boiling point, calculate solution
molality :
171.0 g (C12H22O11) mol C12H22O =
342.0 g C12H22O11
= mol C12H22O11
m = moles of solute/1 kg of solvent = 0.50 mol/1.0 kg
= 0.50 mol/kg continued to next slide x

34. Continuation:
b. Determine n : because sugar does not
dissociate upon dissolving, n = 1.
c. Δ tb = nKbm = (1)(0.52 0C/m)(0.50m)
= 0,26 0C
d. Δ tf = nKfm = (1)(1.86 0C/m)(0.50m)
= 0,93 0C

35. OSMOTIC PRESSURE
Is the hydrostatic pressure required to prevent the net flow of solvent through a semipermeable membrane into a solution.
Osmotic pressure ()
 = nMRT (van’t Hoff equation)
T = temperature in Kelvins
R = the ideal gas constant
(0.82 L-atmosphere/degree.mole)
M = the solution molarity

36. OSMOSIS
The process in which solvent flows through a semipermeable membrane into a solution.

37. INTRODUCTION Types of solution Concentration SOLUTION
No.1
INTRODUCTION
Types of solution
No.2
Concentration
No.3
SOLUTION
Solution properties
No.4
Dialysis
No.5

38. SOLUTION
Dialysis
No. 5
Earlier we discussed semipermeable membranes that selectively allow solvent to pass but retain dissolved solutes during osmosis.
Dialysis, another membrane process, is also important in living organisms.

39. Continuation
Dialyzing membranes :
A semipermeable membranes with pores large enough to allow solvent molecules, other small molecules, and hydrat ions to pass through (are semipermeable membranes with larger pores than osmotic membranes).

40. Continuation
Dialysis : A process in which solvent molecules, other small molecules, and hydrat ions pass from a solution through a membrane (is the passage of ions and small molecules through such membranes).

41. DIALYSIS. This is one method of dialysis used to purify proteins

43. Application of Dialysis
Dialysate + waste product
Dialysis tubing
Fresh dialysate
Scheme of dialysis process

44. A similar technique is used to clean the blood of people suffering kidney mal function
The blood is pumped through tubing made of a dialyzing membrane.
The tubing passes through a bath in which impurities collect after passing out of the blood.
Blood proteins and other important large molecules remain in the blood.

45. Scheme of hemodialysis process
blood
dialysat
dialysat
blood
Scheme of hemodialysis process

46. Continuation
Dialysis is most commonly used to remove salts and other small molecules from solutions of macromolecules. During the separation and purification of biomolecules, small molecules are added to selectively precipitate or dissolve the desire molecule.

47. Continuation
Dialysis is also useful for removing small ions and molecules that are weakly bound to biomolecules. Protein cofactors such as NAD, FAD, and metal ions can be dissociated by dialysis. The removal of metal ions is facilitated by the addition of a chelating agent (EDTA) to the dialysate.
Minerals are bound by EDTA, these are: Ca, Fe, etc.

48. EDTA : Ethylenediaminetetra-acetic acid

49. EDTA with Metal
Ca, Fe, etc

50. INTRODUCTION Types of colloid COLLOID Colloid properties
No.1
INTRODUCTION
No.2
Types of colloid
COLLOID
No.3
Colloid properties

51. INTRODUCTION : ° Definition ° Diameter of colloid particle
No. 1
INTRODUCTION : ° Definition ° Diameter of colloid particle

52. Definition
colloids (or colloidal suspensions) are homogeneous mixture of two or more components in which there is more of one component than of the others.
In solutions the terms solvent and solute are used for the components, but in colloids the terms dispersing medium (for solvent) and dispersed phase (for solute) are used.

53. DIAMETERS OF THE DISPERSED PHASE
The dispersed phase of colloids is made up of much larger particles (very large molecules or small pieces of matter) with diameters:
10ˉ7 to 10 ˉ5 cm (10 – 1000 A˚)

54. INTRODUCTION Types of colloid COLLOID Colloid properties
No.1
INTRODUCTION
Types of colloid
No.2
COLLOID
No.3
Colloid properties

55. COLLOID Types of colloid
No.2
Types of colloid

56. TYPES OF COLLOID Type Name Examples Aerosol Foam Emulsion Sol
Solid foam
Fog, aerosol sprays, some air pollutants
Smoke, some air pollutants
Whipped cream, shaving cream
Milk, mayonnaise
Paint, ink, gelatin dessert
Marshmallow, pumice stone, foam rubber
Butter, cheese
Pearls, opals, colored glass, some metal alloys
Dispersing medium
Dispersed phase
Gas
Liquid
Solid

57. LYOPHOBIC AND LYOPHILIC SYSTEM
Colloidal solutions with a liquid as
Dispersion medium can be divided
roughly into two Categories :
Lyophilic Sols
Lyophobic Sols

58. DIFFERENCES BETWEEN THE TWO TYPES
SURFACE TENSION SIMILAR TO THAT OF DISPERSION MEDIUM.
VISCOSITY SIMILAR TO THAT OF MEDIUM.
SMALL QUANTITIES OF ELECTROLYTES CAUSE PRECIPITATION.
THE PARTICLES ARE EASILY DETECTED IN THE ULTRAMICROSCOPE.
THE PARTICLES MIGRATE
IN ONE DIRECTION IN AN ELECTRIC FIELD.
SURFACE TENSION OFTEN LOWER THAN THAT OF DISPERSION MEDIUM.
VISCOSITY MUCH HIGHER THAN THAT OF MEDIUM.
SMALL QUANTITIES OF ELECTROLYTES HAVE LITTLE EFFECT, BUT LARGE AMOUNTS MAY CAUSE SALTING OUT.
THE PARTICLES CANNOT BE READILY DETECTED IN THE ULTRAMICROSCOPE.
THE PARTICLES MAY MIGRATE IN EITHER DIRECTION OR NOT AT ALL IN ELECTRICAL FIELD.

59. INTRODUCTION Types of colloid COLLOID Colloid properties
No.1
INTRODUCTION
No.2
Types of colloid
COLLOID
No.3
Colloid properties

60. EMULSIFYING AGENTS OR STABILIZING AGENTS
COLLOID
No.3
Colloid properties
TYNDALL EFFECT
BROWNIAN MOVEMENT
COLLOID FORMATION
COLLOID DESTRUCTION
EMULSIFYING AGENTS OR STABILIZING AGENTS

61. TYNDALL EFFECT
When a beam of light passes through them, they will be scattered the light, and the path of the light becomes visible.
And hence it is generally called the Tyndall effect.

62. source colloid CuSO4 Fe(OH)3
The light beam passes from left to right through a purple gold sol (a colloid), a blue copper sulfate solution, and colloidal iron (III) hydroxide. The light path can be seen in both colloids, but not in the copper sulfate solution.

63. BROWNIAN MOVEMENT
As is to be expected, because of their small size, colloidal particles are seen in the ultramicroscope to display vigorous Brownian movement.

64. COLLOID FORMATION AND DESTRUCTION
Much of the interest in colloids is related to their formation or destruction.
Colloid particles tend to attract and absorb ions that are present in the dispersing medium.
The charge (+ or -) of the adsorbed ions depends on the nature of the colloid, but all colloid particles within a particular system will attract only one charge or the other.
This repulsion help prevent the particles from coalescing into aggregates large enough to settle out.

65. EMULSIFYING AGENTS OR STABILIZING AGENTS
Emulsifying agents is substances that stabilize the colloids (prevented from coalescing)
For examples :
1. Egg : the compound in the egg
yolk acting as the emulsifying
agents
2. Soaps and detergents
3. Etc (CMC = carboxyl methyl cellulose )

66. Summary Reference:
Mushtaq Ahmad, Essentials of Medical Biochemistry 6th Edition, Vol.1-2, Merit Publisher, Multan, 1999