revision notes of class 12 chemistry

1. Solution in
30 mins
By-Bharat Panchal

2. ·
Types of
solutions
·
Expressing
concentration of solutes
·
solubility
·
Vapour Pressure of liquid solutions
·
Ideal & Non-Ideal Solutions
·
Colligative Properties
and Determination o
Molar Mass
· Abnormal Molaw Mass

3. One shot
+ Notes
Pox.O + Exemplar
MCO

4. SOLUTIONS
It is a homogeneous mixture of two or
more pure substance
5)
ule-Dissolved in sent- Dissolved in
smaller Quantity. larger quantity.
eg sugar, salt
e.g water, Milk.
-solution exit in single phase
- >
particle size in solution is less than I am
Dilute Solution: Large amount of Solvent
concentrated Solution:Small amount of Solver
Aqueous Solution solvent is water
Non-Aqueous Solution: solvent is other
than water

5. Mass Percentage (t) =
osolut
in soll
1100
Man of solution
Volume Percentage (F):me
Solute in soll
(100
volume of Solution
Mass by volume
(w) : Mass of solute insole
percentage Volume of Soln
*
100
Parts per million Copan):
of
componentx106
all component of solu
Mass Fraction (x) =
asolutepation xX
Mole fraction (K) =
UN:
AUB x(p =
Us
Unitless
xA
+xb =
1, more fraction is a
quantity.

6. Molarity(M) Number of moles of solute
per litre of solution.
M.gmoles
ofsolereal - wiXo
mL
m=
ox
i
Unit: molt or M or Mola
Molality (m): Number of moles of solute
per kg may of solvent
m =
waxing
m =
oeroles
of
solute
an ox rig
Relation ship blw Molarity and Molality:
M- Molarity
memolality
M:
sMiscikg),MBeMolar,
Man

7. SOLUBILITY: Maximum amount that can
be dissolved in a specific
amount of solvent at a specific temperature
Factors Affecting SinL
Nature of Solute and Solvent - Polar
solute dissolve in polar solvents and non
polar solutes dissolve in Non-polar
solventsi.e like dissolve like
effect of temperature
Exothermic AH:-ve Endotheomic Astr
solubility decreases solubility increases
with increase in with increase in
temperature temperature

8. essure No significant effect
HENRY'S LAW the partial pressure
of the gas in vapour phase is proportional
to the more fraction of gas
in solution.
p=KHCC kn Henry's Constant
·value of kn increases with increase in temp.
·
solubility decrease with increase in kH.
Effect of temperature:
As dissolution is an
exothermic process i.e solubility of
Gases in liquid decrease with increase
in temperature.
I

9. Vapour Pressure: The pressure exerted
&
by the vapour m
equilibrium with the
liquid/solution at
a particular temperature
factor. Weaker intermolecular forces greater
*
the vapour pressure.
temperature 4, NP also increases
* Molarity depends upon temperature but
molality doesn't
Application of Henups Laco
·
scuba divers suffer from bends
·
climbers suffer from anoxia.

10. RAOULT'S LAW:
The partial vapour
pressure of a component is equal volatile
to the vapour pressure of that
Solution: solute+ Solv
component in pure state multiplied
by the more fraction of that component. P
= Pr + OA
PA =
PAXCA OB =
b3XCIB
Non-volatile solute
for Volatile solute For Non-Volatile Solut
PT =
PA +PB Pp: PA solution: soletesolve
8
F: PAAXCIA
De =
PA
-
PXIA

11. Weaker interaction stronger interaction
PALPEXDA PACPANICA
&n = the NU = -
Y
AV = t AV: -
L
F
Pe=PA+Dr
-
03
O
p
ICA:1
x
A=
0
xy =
0 x5=
1

12. Azeotrope: These are liquid mixture
which distil over without change
i composition
the deviation are known as min.
poiling azeotropes e.g. CattsOH+HO
-
ve deviation are known as max.
boiling azeotobes e.g HNOs +HO

13. COLLIGATIVE PROPERTIES
Depends upon number of moles of solute.
GB
CI
Relative lowering of Yabour Dressure Relative
lowering of labour pressure is equal to
the more
fraction of solute in the solution.
=Cz =
kB
x
-
Lowering of X.P b not a colligative broberty
-
RLUP is a colligative Property
pi-x.p of pure solvent wa-mass of solute
0.-x.p g Solution M. -
Molar Mass of Solvent
wi-Mass & Solvent Mc-Molar Mass & solute

14. Elevation in Boiling Point =
B.Ot o Solution
containing a non-volatile solute is
always higher than
boiling point g
pure solvent and this difference in
boiling point is called elevation
in boiling point Atb =
ex-T'y
A
T
o=Kom
H m =
1
AT = kD
kn= K Kg molt

15. ATb =
kym
Fen:laoMoeYOOg
yeB.osorro
solvent
Kb-molal
elevation
constant
Ow
ebullioscopic
constant
me
morality
Note evalue
of Ky
depends
upon
nature of
solvent

16. Depression in freezing Point (ATS) rpt of
a solution
containing a non-volatile solute is always
lower than pot of pure solvent and
this difference in freezing point is
called depression in
freezing point.
A
T7 =
kwm=
1
i]
1
T =
kj
used to calcul-
-ale Me for
normal
molecules
*
f+motal depression or
Cryoscobic
constant
constant

17. AT =
Tj-Tf
71: freezing point of pure solvent
T7 =
freezing point of solution
ATH = kfXM
my-fYWYr
ortho
#
EEE
E
OSMOTIC PRESSURE: Soleut
External pressure used to stop
(nighconc) blowconc)
osmosis
M =
RT ↑= EX**T
7/
MB =
RXT

18. #= Osmotic pressure T: Temperature
v =
volume R: 900 constant
used to calculate Me for macromolecules
I
SOTONIC SOLUTION:
Two solution have same
osmotic bressure (T)
eg Saline solution (0.9%) and Blood.
TAT MB
El ↳
Hypotonic Solution
Hypertonic Soly
have osmotic Have low osmotic
High
bressure pressure
Reverse Osmosis
when a pressure more than
the osmotic pressure is applied to the
solution, the solvent may pass from
solution, into the solvent through
the semi-permeable membrane
e.
desalination of sea water.

19. ABNORMAL MOLECULAR MASS
In some cases,
observed colligative properties deviate from their normal
calculated values due to association or dissociation of
molecules.
solligative property c
MB
Higher values observed in case of association
of benzene
-
Norene Mossa
resea
Lower values observed in case
of dissociation
e.g KCS
·
YAN'T HOFF FACTOR (iT
ratio of observed value of
colligative property to the calculated value of colligative
property.
ioored
ColligativeProbe
interly
or i = normal molecular mass
observed molecular mass
or
i =
no.8 particles after association or dissociation
number of particles initially

20. Colligative Property and Van't Host factor
AT =
ikom I for strong electrolyte like
AT
= 1K+M kx =
1, NaU =
2, MgSOn
=
2
#= CRT KeSOn =
3, A(SOuly =S
ops - is
Degree of Dissociation (c) and Van't Holf factor(i)
if one molecule of a substance gets dissociated into
I particles and x is the degree of dissociation then
A
-
up
initially 1 mol D
↳
i =
th
At 29, 1-9 na
Total no.Imoles at a =
t
equilibrium: 1-xth<

21. o f
Association (x) and can't Host factor is
If a molecules
of a substance A associate to form An
and a is the degree of association, then
HA-An
initially 1 mot O
3
i =
1c+ Cdiss:
At equilibrium 1-x
I
Total no.
I moles at equili x =
1 Cass-the
re
=
1-x+f A
i = 1 no association or dissociation
is particles undergoes dissociation
ice particles undergoes association

22. Thank
You...