Jas Ion Transport in Solution Part1
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Transcript of Jas Ion Transport in Solution Part1
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TRANSPORT OF IONS IN SOLUTION
Jaslin Ikhsan, Ph.D.Chemistry Ed. Department
State University of Yogyakarta
Conductivity of electrolyte solutionsStrong and weak electrolyte
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Mahasiswa dapat menjelaskan pengertian
konduktansi dan konduktivitas
Mahasiswa dapat menghitung konduktivitas
molar larutan
Mahasiswa dapat menjelaskan hukum
pengenceran Ostwald
Mahasiswa dapat menentukan pKa dengan
menggunakan hasil pengukuran konduktivitas
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Conductivity of Electrolyte Solution
Ions in solution can be set in motion by applying a
potential difference between two electrodes. The conductance (G) of a solution is defined as the
inverse of the resistance (R):
For parallel plate electrodes with areaA, itfollows:
GR
in units of 1 1,
G A
L
Where,
:the conductivity,
L :the distance separating the plates
Units:
GS (siemens)
R
S m-1
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Conductivity of Electrolyte Solution
The conductivity of a solution depends on the number of ions
present. Consequently, the molar conductivitymis used
C is molar concentration of electrolyte and
unit of mis S m2mol-1
mC
In real solutions,mdepends on the concentration
of the electrolyte. This could be due to:
Ion-ion interactions1
The concentration dependence of conductance
indicates that there are 2 classes of electrolyte Strong electrolyte: molar conductivity dependsslightly on the molar concentration
Weak electrolyte: molar concentration falls
sharply as the concentration increases
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Strong Electrolyte
Fully ionized in solution
Kohlrauschs law
0m is the limiting molar conductivity
K is a constant which typically depends on the
stoichiometry of the electrolyte
C1/2arises from ion-ion interactions as estimated by the
Debye-Hckel theory.
m m KC 0 1 2/
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Strong Electrolyte
Law of the independent migration of ions: limiting molar
conductivity can be expressed as a sum of ions contribution
ions migrate independently in
the zero concentration limit
0m
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Weak Electrolyte
Not fully ionized in solution
HA aq H O l H O aq A aq
c c c
( ) ( ) ( ) ( )
( )
2 3
1
K c
a
2
1
,
2
2
2
2
0
4
2
2
4
2
c K K
c K K
K K K c
c
K
c
K K c
c
a a
a a
a a a
a a a
K
c
K
c
c
K
K
c
c
K
a a
a
a
a
2 21
4
21
41
1 2
1 2
/
/
11
c
Ka is degree of ionisation
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Weak Electrolyte
The molar Conductivity (at
higher concentrations) can
be expressed as:
At infinite dilution, theweak acid is fully
dissociated (= 100%)
It can be proven by the
Ostwald dilution law whichallows estimating limiting
molar conductance:
m m 0
m m
m m
m m
m m a
m m a m
m
m
x
x c
K
c
Kx
0
0
0
0
0 0 0
1 1
1 1 1
1 11
1 1
1 10 0 2
m m
m
a m
c
K
( )
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Weak Electrolyte
The limiting molar conductance:
1 10 0 2
m m
m
a m
c
K
( )
Graph to determine the limitingvalue of the molar conductivity of
a solution by extrapolation to zero
concentration
Hukum Pengenceran
Ostwald
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Diskusi:
1. Konduktivitas molar larutan elektrolit pada 250C adalah 135,5 S
cm2 mol-1dan konsentrasinya adalah 5,35 x 10-2M. Hitunglah
konduktivitas larutan! (20)2. Sel konduktivitas mempunyai elektrode bidang yang sejajar,
masing-masing luasnya 2,2 cm x 2,2 cm, dan terpisah sejauh
2,75 cm. Jika sel diisi dengan larutan elektrolit, tahanannya
adalah 351 ohm. Berapakah konduktivitas larutan? (25)
3. Pada 250C konduktivitas larutan elektrolit kuat dalam air adalah109,9 S cm2 mol-1untuk konsentrasi 6,2 x 10-3M dan 106,1 S
cm2 mol-1untuk konsentrasi 1,50 x 10-2M. Berapakah
konduktivitas molar pembatas elektrolit tersebut? (30)
4. Konduktivitas molar 0,1000 M KCl (aq) adalah 129 S cm2
mol-1
dan tahanan terukur dalam sel konduktivitas adalah 28,44 ohm.
Tahanan itu besarnya 28,50 ohm jika sel yang sama berisi 0,1000
M NH4Cl (aq). Hitunglah konduktivitas molar NH4Cl (aq) pada
konsentrasi ini! (25)
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Thank You