electrochemistry physical chemistry b.sc first year second semester
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ELECTROCHEMISTRYPHYSICAL CHEMISTRY
B.Sc FIRST YEARSECOND SEMESTER
DEBYE-HUCKEL THEORY
• The first successful attempts to explain the variation of equivalent conductance of strong electrolytes with dilution was made by Debye and Huckel(1923).
• The fundamental idea underlying their work is that because of electrical attraction among the oppositely charged ions.
INTERIONIC EFFECTS
• The electrical attractions among the oppositely charged ions which affect the speed of an ion in the electric field are called “interionic effects”.
There are two such effects :- Relaxation effect or Asymmetry effectElectrophoretic effect
RELAXATION EFFECTS OR ASYMMETRY EFFECTS
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-- -
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-+
+
(a) (b)
Symmetrical ionic atmosphere around a positive ion
Ionic atmosphere becoming asymmetrical when central ion moves FIG:1
ELECTROPHORETIC EFFECT
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_ _
_+
FIG:2
DEBYE-HUCKEL-ONSAGER EQUATION Debye and huckel (1923)derived a mathematical
expression for the variation of equivalent conductance with concentration. This equation was further improved by Onsager(1926-1927) and is known as Debye-Huckel-Onsager equation.
Λc = Λ0-[82.4/(DT)1/2 ή +8.20X105/(DT)3/2 λ0]√CWhere Λc =Equivalent conductance at concentration c. Λ0 =Equivalent conductance at infinite dilution. D = Diectric constant of the medium. ή =Coefficient of viscosity of the medium. T =Temperature of the solution in degree absolute. c = Concentration of the solution in moles/litre.As D and ή are constant for a particular solvent.Therefore,at constant temperature, the above equation can be written in the form: Λc= Λ0-(A+BΛ0)√c where A and B are constants for a particular solvent
VERIFICATION OF THE ONSAGER EQUATION
Two tests can be readily performed to verify the onsager equation.These are:- The plot of Λc vs √c should be linear.The slope of the line should be equal to A+B Λ0, calculated by substituting the value of various constants directly.
Equ
ival
ent
cond
ucta
nce
√concentration c
HCI ACID
KCl
AgNO3
NaCl
FIG:3 TESTS OF ONSAGER EQUATION
MIGRATION OF IONS AND TRANSPORT NO
The movement of ions towards the oppositely charged electrode is called migration of ions.
KNO3 SOLUTION
KNO3 SOLUTION IN JELLY
CHARCOAL POWDER
CuCr2O7
SOLUTION IN JELLY (GREEN)
Cu2+ (Blue) Cr2O72- (YELLOW)
FIG:4 DEMONSTRATION OF THE MIGRATION OF IONS
HITTORF’S THEORETICAL DEVICE
According to faraday’s second law of electrolysis, when the same quantity of electricity is passed through solution of different electrolytes, the ions are always liberated in equivalent amounts.
To explain this ,consider a cell containing the solution and provided with the anode A and the cathode C.Let the solution lying between the electrodes A and C be divided into three compartment. Before electrolysis suppose there are 13 pairs of ions.
WHEN ELECTRODES ARE NOT ATTACKED:- The following different cases may be considered Case 1:When only anion moves.Case 2: When cations and anions move at the same rate.Case 3: when cations move at double the speed of the anions
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----A C
a b
I
II
III
IV
ANODIC COMPARTMENT
CENTRAL COMPARTMENT
CATHODIC COMPARTMENT
+ + + + + + + + + + + + + _ _ _ _ _ _ _ _ _ _ _ _ _ + + + + + + + + + + + + +_ _ _ _ _ _ _ _ _ _ _ _ _ _ _
+ + + + + + + + + + + + +_ _ _ _ _ _ _ _ _ _ _ _ _ 2
+ + + + + + + + + + + + + _ _ _ _ _ _ _ _ _ _ _ _ _
2
2
2
1
FIG: 5 MIGRATION VELOCITY OF IONS AND CHANGE IN CONCENTRATION WHEN ELECTRODES ARE NOT ATTACKED
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CONCLUSION
Fall in concentration around any electrode is directly proportional to the speed of the ions moving away from it. It means:
Fall in con. around anode =Speed of cation
No. of ions liberated on both the electrodes is equal.
CASE IV:- WHEN ELECTRODES ARE ATTACKABLE
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----A C
a b
I
II
III
IV
ANODIC COMPARTMENT
CENTRAL COMPARTMENT
CATHODIC COMPARTMENT
+ + + + + + + + + + + + + _ _ _ _ _ _ _ _ _ _ _ _ _ + + + + + + + + + + + + + +_ _ _ _ _ _ _ _ _ _ _ _
+ + + + + + + + + + + + + + + + +_ _ _ _ _ _ _ _ _ _ _ _ _ 2
+ + + + + + + + + + + + + + + + _ _ _ _ _ _ _ _ _ _ _ _ _
2
2
2
1
FIG: 6 MIGRATION VELOCITY OF IONS AND CHANGE IN CONCENTRATION WHEN ELECTRODES ARE ATTACKED
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CONCLUSION
Fall in conc. In the anodic compartment due to migration of Ag+ ions=(x-y)gram equivalents
Fall in conc. around cathode=Increase in conc. Around anode=y gram equivalents
Thus, the speed ratio will be given by: Speed of Ag+ ions/Speed of Nitrate ion=x-y/y
TRANSPORT NUMBER
The fraction of the total current carried by an ion is called its transport number or Hittorf’s number.
Transport number of anion na= ua
ua+uc
Transport number of cation nC= uC
ua+uc
DETERMINATION OF TRANSPORT NUMBERS BY HITTORF’S METHOD
Hittorf’s method:- Principle:- The method is based upon the
principle that the fall in concentration around an electrode is proportional to the speed of the ion moving away from it.
nc=Number of gram equivalent lost from the anodic compartment
Number of gram equivalent deposited in the voltameter
APPARATUS FOR THE DETERMINATION OF TRANSPORT NUMBER
VARIABLE RESISTENCE+
EXPERIMENTAL SOLUTION
MILLI-AMMETER
+ _
+ _
VOLTAMETER OF COULOMETER
FIG:7
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• (ii) Strong Acid with a Weak Base• The titration of a strong acid with a weak base may be illustrated by the
neutralization of dilute• HCl by dilute NH4OH.• H+Cl- + NH4OH NH4• + + Cl- + H2O
(i) Strong Acid with a Strong BaseWhen a strong alkali, e.g., sodium hydroxide is added to a solution of a strong acid, e.g.,hydrochloric acid, the following reaction occurs:(H+ + Cl-) + (Na+ + OH-) = Na+ + Cl- + H2O
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