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1. ClassXII

2. Chapter name – Solution and colligative property
Subject- Chemistry
Teacher- Azeem khan
Marks- 6
State- Maharashtra Board

8. Factor affecting Solvation
Nature of Solute- solute may be crystalline,
amorphous, ionic or covalent.
Nature of Solvent- solvent classified as polar and non
polar.
Amount of Solvent- more amount of a solvent, will
dissolve more quantity of the solute.
Temperature- solubility depend upon temperature.
Pressure- only for solutions which involve gases solute.

9. Classification of
Solution

12. Pumic stone

13. Benezene in
toluene
CO2 dissovled
in water
salt in
water
Smoke
Moister
sodalime

14. Concentration of solution of solids
in liquid molarity

15. Which solution
will be more
salty?
More
Quantity

16. More amount of solute.

29. Percent mass
by volume

31. Molality

33. Depend upon Density of solution

34. Percent by
mass

37. Formula

40. Parts per
million

42. Relation between
concentration

51. 6

60. Solvant

64. Endothermic.

66. Solubility of gas in liquid

70. William Henry
Increase in pressure
increase solubility.
Effect on change of pressure on solubility
Gas being compressed, their
solubility in liquid is greatly
influenced by external
pressure.
Henry’s law constant
increase and solubility of
gas in liquid decreases.

73. Applications of Henry Law

74. Increase in the
solubility of CO2
in soda water
and soda drinks
is due to high
pressure of gas.
These bottles
are sealed under
high pressure.

75. This leads to lower concentration of oxygen in blood and
tissues of mountain climbers as well as people living at
higher altitudes. They become weak and unable to think
properly due to lower pressure of oxygen. These symptoms
are called anoxia
At higher altitudes
the partial pressure
of oxygen is less then
that of Ground level.

76. Deep sea diners will suffer with higher dissolution of
atmospheric gases under water, at high pressure. To avoid
toxic effects of higher concentration of nitrogen, the
respiration tanks of air are diluted with helium (56% N2,
32%O2, and 12%He).

78. Solid solution

84. alloy

88. Vapour Pressure

89. Intermolecular forces are
relatively strong
Slight Volatile
Lubricating oils

98. Surface of solid or
liquid.

99. François-Marie Raoult

101. Pº
1
Pº
2
Ps

105. P =KH X
William Henry Law-

106. According to Le Chateliers principle on increasing pressure,
equilibrium shifts in the direction of lesser no. of gas moles.
On decreasing temperature, equilibrium shifts in forward
direction for an exothermic change.
In general, solubility of gases increase with increasing
pressure and decreases with increasing temperature.

107. Where KH is Henry’s
law constant is
shown in fig. The
slope of the straight
line is KH Different
gases have different
KH values at the
same temperature.

108. This condition is
valid only in case
of dilure solution.
P = PºX is
Raoult's Law
Henry's Law is
closely related to
Raoult's Law.

111. Therefore, solvent behaves like an ideal solution.
Hence Raoult's Law is applicable for solvent and not
solute.
and Henry's law is applicable for Solute and not Solvent.

120. Acc. to Dalton’s law of partial pressures,
total P will be the sum of the partial P of
the components of solution

124. Ideal
solution

126. Interaction A and B

135. Energy will be
relaeased after
formation of AB
solution.
∆H = -ve

136. intermolecular space
will decreases
becouse of more
interaction.
Hence, Volume of
solution after mixing
will decreases.

137. Dot line
reperesent
ideal solution
and line
reperesent
negative
deviation.

148. Some liquids on mixing, form azeotropes
which are binary mixtures having the same
composition in liquid and vapour phase and boil at a
constant temperature.
In such cases, it is not possible to separate the
components by fractional distillation

149. 3beakercontaindifferentcomposition(amount)waterbutB.P100ºC.
10gNaCl
200ml 500ml 1litre
10gNaCl 10gNaCl
B.Pchanges
B.P=109ºC. B.P=104ºC. B.P=102ºC.
B.P of pure Substance is constant.
B.PofSolutionisnotconstantbecouseBoilingcompositionofsolutionis
change.
Example

150. Minimum boiling azeotrope Maximum boiling azeotrope
Soln Show Large
Negative deviation from
roults law.
Soln Show Large
Positive deviation from
Roults law.
Show Low B.P Show High B.P
high V.P low V.P
Low escaping
tendancy
High escaping
tendancy
Types of Azeotrope-
eg,For example, ethanol (95.5%) +
water (4.5%) mixture boils at 351.5
K.
(B.P. of ethanol = 78.1° C, B.P. of
E.g., HNO3 (68%) + water
(32%) mixture boils at 393.5 K.
(B.P. of HNO3 = 83° C, B.P. of
water = 100° C)

153. Colligative property

155. LOWERING
DEPRESSION
INCREASES
ELEVATION

156. LOWERING
DEPRESSION
INCREASES
ELEVATION

158. Equal to

159. Lowering of
Vapour pressure

163. Raoult’s law for
a solution of
non- volatile
solute

172. Relation between Molar
mass of solute and
relative lowering of
Vapour Pressure

182. Relation between
molar mass of
solute and elevation
of Boiling point

184. Freezing Point
Depression of Freezing point

189. Depression of freezing point
&
its relation with molar mass of
solute

194. Osmosis
Osomotic pressure
Reverse osmosis

206. Abbe Nollet Experiment for osmosis

207. Osmosis
occur
Osmotic
occur

208. • The experimental set up must have the arrangement for
applying an external mechanical pressure on the solution
so that there is no flow of solvent and concentration
remains unchanged.
• The external pressure applied to stop osmosis is a
measure of osmotic pressure.
• The entry of the solvent into the solution causes
its dilution and concentration changes.
Drawbacks of Abbe Nollet Experiment:
Remedy for Abbe Nollet Experiment:

210. Hypertonic solutions, Hyptonic
solutions
and
Isotonic solutions

217. Laws of osmotic pressure
vant Hoff general solution equation
Relation between osmotic pressure
and molar mass of solute

223. Gay-Lussac Law

228. Deviation in Colligative properties
Vant-Hoff factor

238. Abnormal molar mass and
Calculation of i

240. Dimer 120

246. Determination of i

250. This method is used to
measure the RLVP of a
solution.
Ostwald-Walker process

251. This method is used
to measure the RLVP
of a solution.
Ostwald-Walker process
 When dry air passes abouve the solution it gets saturated with vapors of the
solution.
 Weight of dry air increases due to absorbed vapors.
 Solution bulb lose mass to air.
loss in weight α P