1. SOLUTIONS –
• homogeneous dispersion of two or more
substances in an ionic or molecular scale
Na
+
OH
H
Cl
- H O
H
CHO
CH OH
CH2OH
O H
H
Very small particles, too small to be seen
By the unaided eye

2. Kinds of Mixture Particle Size
suspension
colloid
solution
10-4 cm. in diameter
10-5 – 10-6 cm. in diameter
10-7 cm. in diameter
Always suspended in the
medium (too small to be
pulled down by gravity)
Shows Tyndall Effect :
reflect light to produce a
visible beam of light
Always suspended in the
medium ( too small to
be pulled down by
gravity)
Settles upon standing

3. Kinds of Solutions
Solid state Alloys ( Coin, brass)
Liquid state Sea water, alcohol in water
Dissolved Oxygen (DO)
Gaseous state Air

4. Parts of a Solution
solution
solute
solvent
Dissolved substance
Dissolving medium
is
is

5. Parts of a solution
Physical state amount
Solute Dissolved
substance
Solid, gas Less
Solvent Dissolving
medium
liquid more

6. Nature of Dissolving Process:
Na
+
Na
+
Na
+
Na
+
Cl
-
Cl
-
Cl
-
Cl
-
H O
H Cl
-
H2O
H2O
H2O
H2O
solvated iondissolving rate
crystallizing rate
salt

7. Nature of the Dissolving Process
Na+1
Na+1 Na+1
Cl-1
Na+1
Cl-1
Cl-1Cl-1
Cl-1 Na+1
H2O
H2O
H2O
H2O
Dissolving rate
Crystallizing rate
salt
Solvated ion

8. Nature of Dissolving Process:
• The nature of the dissolving process is
• a 2 way process
1. Process of dissolution
2. Process of crystallization

9. Which, at one point in time the 2 processes
will attain equilibrium
• At equilibrium
• Rate of dissolution == rate of crystallization
• Solution is called saturated solution
• Concentration of the solution is constant
• corresponds to the solubility of the solute in question .
•

10. Solubility –
• maximum amount of solute that will be
dissolved by a given amount of solvent
producing a stable system, under a specified
temperature

11. Factors affecting Solubility
Nature of solute and solvent :
• Like Dissolves Like
IMFA
solute &solvent
IMFA
solute
IMFA
solvent

12. Temperature
Heat of solution
Solid in liquid
Gas in liquid
T increases solubility
increases
Endothermic
T increases solubility
decreases
exothermic
exothermic
T increases solubility
decreases

13. Pressure
• Pressure –has little or no effect on the
solubility of solid in liquid, liquid in liquid
• Gas in liquid : Pressure increases, solubility
increases

14. When can a gas become soluble in water ?
gas
liquid
For the gas to become soluble in the liquid , it must come
into contact with the liquid: IMFA forming ( exothermic heat
flow )
Applied Pressure: Pressure increases, solubility of gas in
water increases
And this will be effectedby applying pressure
to the gas so that IMFA is formed between the
gas and water.
A process which involves
IMFA forming results for heat
To flow out to the sorrounding.

15. Factors affecting Rate of Dissolution
1. Temperature : As temperature increases, rate
of dissolving increases.
2. Stirring increases rate of dissolving
3. Surface area – As surface area increases, rate
of dissolving increases

16. Concentration = is the amount of solute present in a
given amount of solvent producing a solution
Described
qualitatively quantitatively
dilute concentrated
saturated
unsaturated supersaturated
% Molarity (M)
Normality (N)
Molality (m) Mole fraction (X)

17. 1. Dilute- contains a relatively low amount of solute
2. Concentrated – contains a relatively high amount of
solute
3. Saturated – contains the maximum amount of solute
that can be dissolved by a measured amount of
solvent (solubility equivalent )
4. Unsaturated – one which contains solute
concentration lower than the concentration in the
saturated solution.
5. Supersaturated – one which contain solute
concentration higher than the concentration in the
saturated Solution.

18. Dilute concentrated

19. 46.5 g NaAc/100 g H2O
25 C
solubility
80 g NaAC/
100 g H20 50 C
all 80 g solute
dissolves cool to
25 C
all 80 g NaAc is in
water as a solution
indefinitely
called
supersaturated
solution
which can
be destroyed by
seeding agitation
Saturated supersaturated
If amount of NaAc is < 46.5 g in 100 g H2O
At 25 oC
Unsaturated solution
Saturated solution
With undissolved
solute

20. A B C
At the start of Dissolving
Solute amount in
Solvent is zero
During dissolving
Solute amount in solvent
Has increased, but still less
Than the dissolving rate
After dissolving
Solute amount in solvent
Has increased so that
dissolving
Rate is equal to the
crystallizing rate
At what point during the dissolving rate is the saturated solution ?
C
Not a solution Unsaturated solution Saturated solution

21. QUANTITATIVE METHODS OF EXPRESSING CONCENTRATION OF
SOLUTION
SOLUTION
SOLUTE
SOLVENT/WATER
%
Molarity
Normality
molality
Mole fraction

22. PerCent = Part Quantity/Total Quantity X 100
1. Percent by mass = grams ofsolute/grams of solution X 100
2. Percent by volume = volume of solute/volume of solution X 100
3. Percent by mass-volume = grams of solute/volume of solution X 100

23. A 0.50 liter bottle
of wine contains
60 ml ethanol.
What is the % v/v
ethanol in the
solution ?
SOLUTION
SOLUTE SOLVENT
0.50 liter
60 ml
volume solute
% = ------------------- X 100
volume solution

24. How many grams
of KCl are required
to prepare 250
grams of an
aqueous solution
that is 10.0 % KCl
by mass
SOLUTION
SOLUTE SOLVENT
?
250 grams
means
10 g KCl = 100 g solution
Conversion factor

25. Molarity (M)
SOLUTION
SOLUTE
SOLVENT/WATER
MOLE
Wt./MW
LITER
OR

26. What is the M
of a 10 % HCl
solution of a
density of
1.2 g /ml
SOLUTION
SOLUTE SOLVENT
10 g HCl = 100 g solution
10g HCl = 100 g soluton
means
M = wt/mwt/liter

27. NORMALITY (N)
SOLUTION
SOLUTE
SOLVENT/WATER
Number of equivalents
( (wt/MW ) X F )
Number of milliequivalents
( (wt/MW) X F X 1000)
LITER
milliliter

28. Mole fraction (X)
SOLUTION
SOLUTE
SOLVENT/WATER
mole MoleAdd to
Mole total
Mole solute/mole total

29. Molality (m)
SOLUTION
SOLUTE
SOLVENT/WATER
MOLE
Wt./MW
OR KG

30. Calculate the
molality of a
solution of 2.34 g
acetic acid,
HC2H3O2 in 35.0 g
water
SOLUTION
SOLUTE SOLVENT
2.34 g
HC2H3O2
35.0 g
MWT = 60.0 g/mole
wt/ MWT solute
m = -------------------
Kg solvent

31. DILUTION
• = process of adding water to a solution of known
concentration to obtain a new solution of different
concentration

32. 6MHCl
300mL.
+300mlwater
3MHCl
600mL

33. solute solute
add water
What happens to the amount of solute upon dilution ?

34. 1.8 moles 1.8 moles
6M HCl
300 mL.
+ 300 ml water
3M HCl
600 mL

35. IN DILUTION
• :
• Amount of solute in original solution = amount of solute in the prepared solution
•

36. Calculate the M of
55.0 g NaCl in
125 ml of solution
SOLUTIONso
SOLUTE SOLVENT
55.0 g
125 ml
M = wt/mwt/liter

37. Theory Acid Base
Arrhenius
One which contains a
hydrogen which will be
yielded as a H+1 in water
One which contains a
hydroxide which will
be yielded as OH-! In
water
Bronstead Lowry Proton donor Proton acceptor
Lewis E’ pair acceptor
E’ pair donor

38. H Cl H
+1
+ Cl
It has H +1: has a potential to donate
Proton donor
Bronsted acid
H
+1
E pair acceptor
Lewis acid
Arrhenius acid
+ 2e' H

39. Na OH OH
-1
Na
+1
+
it has OH w/c is
negative; potential
proton acceptor
Bronsted base
OH
-1
Na
+1
+
Has several e’
pairs; potential e’
pair donor
Lewis base
Arrhenius base

40. HCl
H2O
H
+
Cl
-
+
Acid
Conjugate base
What had become of the
acid after donating a
proton

41. NH3 NH4
+
H2O
OH
-
BASE CONJUGATE ACID
What had become of
the base after
donating
2 electrons

42. HCl
H2O
H
+
Cl
-
+
acid Conjugate base
base Conjugate acid
A strong acid has a weak conjugate base
SA
Weak
SB
At equilibrium weak are favored

43. solute Solvent (water)
solution
electrolytes
Strong :
HCl H
+
Cl
-
+
NaOH Na
+
OH
-
+
Weak
HC2H3O2 H
+
C2H3O2
-
+
Mg(O H) 2 Mg
+2
2 OH
-
+
Aside as being a solvent ,
something important is
happening to water
Acid, base, salt

44. H2O dissociates (into ions) to an extremely small but very important degree.
Kw = 1 X 10 -14 (0.00000000000001)
T= 250 C
H2O H
+
OH
-
+
Arithmetically of the value
1x10 -7 M 1x10 -7 M
WATER IS A NON ELECTROLYTE
Ion product constant :
Kw = (H+) (OH-)
Called
acidity
basicity
neutral

45. solution
• solute • Solvent (water)
electrolyte Non electrolyte
HCl H
+1
Cl +
NaOH OH
-
Na
+1
+
acid
base
HOHH
+
OH
-
+
Interplay of these ions is
ACIDITY AND OR BASICITY

46. Possible interplays are
H
+
OH
-
H
+
OH
-
H
+
OH
-
<
>
=
Acidic
basic
neutral

47. When an acid is added to water , the H+ concentration of the
resulting solution is determined solely by the acid
base OH-
base
HCl Cl
-
H
+
0.01 M
H2O H
+
OH
-
H
+
solution
=
0.01
0.01
NaOH Na
+
OH
-
+
0.02 M
H2O H
+
OH
-
+
OH-
solution
=
0.02 M
0.02 M
Small amount
acidic
Small amount
basic

48. Colligative Properties- dependent only on the ratio of the number of
solute particle to the number of solvent particles and not on the
nature of the solute.
• Vapor pressure lowering
• Boiling point elevation
• Freezinf point Depression
• Osmotic Pressure
Does not matter wether
solute is an acid or base or
salt

49. Vapor pressure
P air
Temperature : Boiling point
solvent

50. Vapor pressure
P air
Solute occupies some areas of the liquid and interfers with the evaporation
less

51. Vapor pressure
P air
TBoiling point Elevation
more