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Ionic equilibrium
Arrhenius concept of electrolyte and non-electrolyte
Electrolyte: those compounds whose aqueous solution is a conductor
of electricity.
Eg. Sodium chloride, hydro cleric acid, etc
Non electrolyte: those compounds whose aqueous solution is not a
conductor of electricity.
Eg methane, urea, etc
Classification of electrolytes
Strong electrolyte: those electrolytes which are completely dissociated
into their constituent ions. HCl H2SOy NaOH Nall NacSOy
, , , ,
Na(l(aq) Natags+ C1 Tags
X Number of moles dissociated
Number of moles initially taken
Weak electrolyte: those electrolytes which are not completely
dissociated into their constituent ions.
+
CHICOOH CH3COO + H
-
X Number of moles dissociated
Number of moles initially taken
Note: All organic acids are leak electrolytes (generally)
, Ost wald dilution law for weak electrolyte
+
CH3COOH CH3COO + H
-
to C
-
~
C-CX CX CX
teq
at K [CH3100] SM +
]
.
eg
:
[CH3COOM]
acid Ka =
CX .
CX
c -
CX
Ka =
CX2
1 -
Xo
I X
Ka = (x2
X I Ka
C
At As the concentration decreases or dilution increase, the X of weak
electrolyte increases and results in the increase of dissociated ions
Factors effecting degree of dissociation
Nature of electrolyte
Polarity of solvent Xx Polarity of solvent or
dielectric constant
Polarity of solvent &
dielectric constant
Effect of dilution
X = Ka Degree of dissociation L Dilution
C
(Addition of solvent)
, Effect of temperature
+
CH3COOH CH3CO0 H
-
+
H = + Ve endothermic
TX reaction
X Number of moles dissociated
Number of moles initially taken
As the temperature increases, the degree o dissociation of weak
electrolyte increases.
Effect of presence of common ion
-
-
HF
-
CHE COOH CHOCOO- + + HU
-
-
-
Xi -
-
X X 2
+
CHSCOOH CH3COO- + H
Xz
+
HCI H + 4-
In presence of common ion coming from another electrolyte, the
degree of dissociation f week electrolyte decreases.
, Arrhenius concept of acid and bases
Acid: those compounds which give in the aqueous solution
+
HCI H + C-
-
2
+
H2SO4 2H +
SOy
Base: those compounds which give in its aqueous solution
NaOH - Nat + OH-
+
KOH -
K + OH-
NHnOH - NHnT + OH-
According to Arrhenius water is an amphoteric compound in nature.
Amphoteric compound: those compounds which can act as acids as
well as bases.
acid
I
,
↑
H20 + OH-
base
Neutralisation reaction: the reaction bet ween aid and base. in
this reaction and and base form salt and water.
HCI '
NaOH -
Nall - H20
acid base salt water
Note: this reaction is always an exothermic process.
Limitations of Arrhenius concept of acid and bases
Does not explain the acid & basic nature in solid or gaseous state
Does not explain the basic nature of NH3 PH3 C S-2 , , ,
and does not explain the acidic nature of CO2 500 P2Os BF3 , , , ,
BUz
t
Does not explain the existence of ion as 3 ion
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