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Summary Chemistry : Textbook For Class Xii, ISBN: 9788174506481 Chemistry,
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Solutions2.1 Types of Solutions 2.5 Ideal and Non-ideal Solu
2.2 Expressing Concentration of Solutions 2.6 Colligative Properties an
2.3 Solubility of Molar Mass
2.4 Vapour Pressure of Liquid Solutions 2.7 Abnormal Molar Masses
Topicwise Analysis of Last 10 Years’ CBSE Board Questions (
24
20
→
16
Number of questions
12
8
4
0
2.1 2.2 2.3 2.4 2.5 2.6 2.7
Topic →
8 Maximum total weightage is of Colligative 8 Maximum SA type questi
Properties and Determination of Molar Mass. Ideal and Non-Ideal Solu
Properties and Determinat
8 Maximum VSA type questions were asked
8 Maximum LA I type qu
from Colligative Properties and Determination of from Colligative Propertie
Molar Mass. of Molar Mass.
QUICK RECAP
,8 Solvent : The component which is present in Mass by volume w
larger amount and determines the physical percentage % =
V Vsolu
state of the solution is called solvent.
8 Types of solution : Depending upon the Mass fraction w1
nature of solute and solvent, solutions are x1 =
w1 + w2
classified as follows :
X Gaseous solutions : Solutions in which Strength w2 (in g)
gas acts as solvent. (g L–1) Vsolution (in m
Solute Solvent Examples
Parts per million w2
Solid Gas Iodine vapours in ×1
(ppm) (w1 + w2 )
air, dust or smoke
particles in air Molarity, (M) w2 × 1
Liquid Gas Water vapours in (mol L–1)
M2 × Vsolutio
air (humidity)
Gas Gas Air Molality, (m) w2 × 1000
(mol kg–1)
X Liquid solutions : Solutions in which M2 × w1 (in g
liquids are present in larger amount. Mole fraction, n1
(x) x1 =
Solute Solvent Examples n1 + n2
Solid Liquid Salt/sugar in water (x1 + x2 = 1)
In case of gase
Liquid Liquid Alcohol in water
p1
Gas Liquid Aerated drinks, O2 y1 =
p1 + p2
in water
X Solid solutions : Solutions in which
8 Solubility : Maximum am
solids are present in larger amount.
that can be dissolved in a sp
Solute Solvent Examples solvent at a specified tempe
Solid Solid Alloys solubility.
Liquid Solid Hg in Ag, Hg in Zn 8 Factors affecting solubili
(Amalgam) liquid :
X Nature of solute and
Gas Solid Solution of hydrogen solutes dissolve in po
in palladium. non‑polar solutes diss
solvents. (i.e., like disso
8 Different methods for expressing X Effect of temperature
concentration of solution : – If the dissoluti
Method of endothermic (DsolH
Formula increases with rise
expressing
– If dissolution proc
Mass percentage w w2 (DsolH < 0), the so
% = × 100
, 8 Factors affecting solubility of a gas in a liquid : and p°2 are vapour p
X Effect of pressure : Henry’s law states components 1 and 2 resp
that “the partial pressure of the gas in temperature.
vapour phase (p) is proportional to
8 Dalton’s law of partial pr
the mole fraction of the gas (x) in the
solution” Ptotal = p1 + p2 = x1 p1° + x
p = KH x where, KH is the Henry’s law = (1 – x2)p1° + x2 p2
constant and is different for different x2
gases at a particular temperature.
Higher the value of KH at a given pressure, 8 If y1 and y2 are the mo
the lower is the solubility of the gas in the components 1 and 2 respe
liquid. phase then, p1 = y1 Ptotal
X Effect of temperature : As dissolution is
8 Raoult’s law for solid-
an exothermic process, then according to It states that relative lo
Le Chatelier’s principle, the solubility
pressure of a solution
should decrease with increase of
volatile solute is equal to t
temperature.
the solute.
8 Raoult’s law : It states that for a solution of
p° − ps
volatile liquids, the partial vapour pressure = x2
of each component of the solution is directly p°
proportional to its mole fraction present in where, p° = vapour press
solution. p1 = p°1 x1 and p2 = p°2 x2 ; where p°1 ps = vapour pressu
x2 = mole fraction
8 Ideal and non-ideal solutions :
Ideal solutions Non-ideal solutions
Negative d
Positive deviation from Raoult’s law
Rao
Vapour pressure Vap
of solution o
+ p B p° p°A p°A
Vapour pressure
Vapour pressure
Vapour pressure
tal
= p A B pA p°B
Pto
p°A pB pA
pB pA
xA = 1 xA = 0 xA = 1 xA = 0 xA = 1
xB = 0 xB = 1 xB = 0 xB = 1 xB = 0
Mole fraction Mole fraction Mole
xB xB x
A – B interactions ≈ A – A A – B interactions << A – A and B – B A – B interact
and B – B interactions interactions
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