12
A d s o r p t i o n - D e s o r p t i o n Kinetics at the M e t a l - O x i d e - S o l u t i o n Interface
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Studied by R e l a x a t i o n M e t h o d s 1
2
Tatsuya Yasunaga and Tetsuya Ikeda 1
Institute of Science and Technology, Kinki University, Higashi-Osaka 577, Japan department of Chemistry, Faculty of Science, Hiroshima University, Hiroshima 730, Japan Chemical relaxation methods can be used to determine mechanisms of reactions of ions at the mineral/water interface. In this paper, a review of chemical relaxation studies of adsorption/desorption kinetics of inorganic ions at the metal oxide/aqueous interface is presented. Plausible mechanisms based on the triple layer surface complexation model are discussed. Relaxation kinetic studies of the intercalation/ deintercalation of organic and inorganic ions in layered, cage-structured, and channel-structured minerals are also reviewed. In the intercalation studies, plausible mechanisms based on ion-exchange and adsorption/desorption reactions are presented; steric and chemical properties of the solute and interlayered compounds are shown to influence the reaction rates. We also discuss the elementary reaction steps which are important in the stereoselective and reactive properties of interlayered compounds. The fast reactions of ions between aqueous and mineral phases have been studied extensively in a variety of fields including colloidal chemistry, geochemistry, environmental engineering, soil science, and catalysis (1-6). Various experimental approaches and techniques have been utilized to address the questions of interest in any given field as this volume exemplifies. Recently, chemical relaxation techniques have been applied to study the kinetics of interaction of ions with minerals in aqueous suspension (7). These methods allow mechanistic information to be obtained for elementary processes which occur rapidly, e.g., for processes which occur within seconds to as fast as nanoseconds (8). Many important phenomena can be studied including adsorption/desorption reactions of ions at electri fied interfaces and intercalation/deintercalation of ions with minerals having unique interlayer structure. In this paper, a review of the mechanistic information that has been obtained in chemical relaxation studies of reactions of ions with metal oxide minerals in aqueous suspensions is discussed. The 0097-6156/ 86/ 0323-0230507.00/ 0 © 1986 American Chemical Society In Geochemical Processes at Mineral Surfaces; Davis, J., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 1987.
12.
YASUNAGA AND IKEDA
review
is
devided
Relaxation
Reaction
Summary
and
Chemical
of
ture,
the
The
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methods
and
3T
the
librium ter
P
;
RT _
_
RT
Δν,
P,T
and
ΔΜ a r e
of
constant
detection
tivity
of
milliseconds
In
electric
can be
conductivity and
to
at
the
been a
described
is
much f a s t e r 20 k V / c m .
this
of
apparatus
of
by
7 atm. The
means (b)
of
operating
ζ-potential the
Fe30it,
compounds
used
and
an
the the
time of
of the
Sample
}
;
and
parame remeans
were a -
and
compound
(7).
200
with It
The
the
conduc
has
a
time
conductivity
occuring
ys.
of
of
atm.
electric time
as
(10).
of
on
the
the
the
by
changing
order
applied
strength
of
of
the
electric-field-jump
that
For
solenoid apparatus
of
this
the
under
15
detection
pressure-jump aqueous
suspension
particles
method
external The
system,
valve is
an
method.
metal-oxide
metal-oxide
are
mixed
nitrogen
gas
measured
by
ms. was
(11).
The m e t a l
silica-alumina,
oxides
used
andy-Al203.
γ-zirconium phosphates (HT),
conductivity order
measurement
stopped-flow
Preparation.
T1O2,
the
(9).
aqueous this
on
rise
0.1
same
electric
α-FeOOH,
hydrotalcite-like
J
equi
The
suitable
apparatus
of
details
micro-electrophoresis
Materials
Fe2Û3,
dead
an
the
external
electric
elsewhere
perturbed
previously and
the
reactions
than
be
by is
of
The
elsewhere
apparatus
solution The
to
The
cannot
detected
described
electrolyte rapidly
found
±
1).
with
method w i t h
microseconds.
which
an some
occuring
pressure
applied
is
system
tempera
volume,
methods,
strength).
by
pressure-jump
field
may b e
(Figure
details
bursting
can be
field
relaxation
field
parameter
equilib
by
standard
altering
observed
reactions
The
using
have
can be
of Κ on
Materials
electric
Reactions
given
enthalpy,
rapidly
electric apparatus
constant
jump-relaxation
or
to
perturbations
are
by
signals
system
field
standard
electric-field-jump
detecting
small
equilibrium
changed
as
80 y s
Methods
pressure,
milliseconds.
of
The
the
applied
detection
constant
(5)
U
Pressure-jump
can be
relaxation
(3)
and
K
relaxation
such
the
reaction.
is
or
Apparatus. to
Kinetics,
ΔΗ
BE
(temperature,
seconds
Chemical
K
^
E x p e r i m e n t a l Methods (a)
of
and M a t e r i a l s ,
2
RT
;
involve
electric
3 P }T
moment
detection
Principles
Intercalation
of
^
equilibration of
231
ΔΗ
=
jHnK
ΔΗ,
(1)
Methods
Chemical Relaxation
31nK V
electric
(4)
dependences
pressure,
where
sections:
Experimental
Kinetics,
relaxation
(8).
five
(2)
Kinetics
Conclusions.
Principles
rium
into
Method,
Surface
A dsorption-Desorption
montmorillonite
(α-,
were
Layered
γ-ZrP),
(Mont),
zeolite
In Geochemical Processes at Mineral Surfaces; Davis, J., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 1987.
T1S2, 4A
GEOCHEMICAL PROCESSES AT MINERAL SURFACES
232
(Z-4A),
and z e o l i t e
intercalation interlayer
space
of
three-dimensional were
no s i g n
the
equilibrium were
was c o n t r o l l e d
Surface In ion
Reaction
aqueous
(4).
concentration
equilibrated
to
(10-22).
preparation.
of
obtain A l l
The tem
a t 25 ° C .
Kinetics
suspensions,
metal
One c a n d e s c r i b e on surface
stable
course
used
elsewhere
The
particles
very
the time
techniques
h after
by the
by the
of
formed
over
are described
f o r 24-72
diameters
particles
The a n a l y t i c a l
varied
patterns.
i s separated
T h e mean
small
of sedimentation
k i n e t i c measurements.
perature
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with
Such
distance
diffraction
zeolite
structures.
1 ym.
the
samples
The i n t e r l a y e r from X - r a y
the crystalline
cage
approximately
suspensions
H-ZSM-5.
was d e t e r m i n e d
oxides
have
amphoteric
the adsorption/desorption
hydroxyl
groups
(SOH) u s i n g
of H
properties and counter
+
the following
mass
action
equations : in
t h e pH r a n g e
below
the
p H
z
p
c
ki S0H£
SOH k
S0H+
+
t h e pH r a n g e
H+
above k
(I)
2
A" ^
SOHt k_
in
+
the
A"
(II)
2
p H
z
p
c
3
SOH
a*-
SO"
+
H+
(III)
k-3 ki* SO"
where the 2,
p H
z
p
metal 3 , 4)
c
,
+
B+
^
A ~ , and B
oxide,
stand
+
an anion,
are the rate
equilibrium
SO"
are given
[S0H][H+] Κι
=
εψ -
a
n
ion
-
=
εψ
[SOH]
K
cation
"
K l
n
— [S0~][B ] +
)
=
4 n i o n
(4)
e
B
=
K*
n
t
ψ
P(~ > k T
&
5
β
— = k T
0
exp(
T
θ
x
f i
βψ
«p r
o > r "Ό 70 O n m m m m
O m O o x m
In Geochemical Processes at Mineral Surfaces; Davis, J., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 1987.
+
Mont
2
d
d
NH+/H (80)
^
When
^
the
dash
2
2
constants
3
Aperture
or
k
these
2
3
2
x
k 3
are
3
made,
an
2
+k 3
);
rate
S(A)M
modified
intrinsic
/(k_
should
+k- k ) .
-*k
systems
+k-ik-
ratio.
for
2
distance.
Silica-alumina
Rate
2
3
+k_i),
k-3 - > k _ i k - k - / ( k k
k-x + k - i k _ / ( k
constants
approximation
rate
be
S(M)A;
appears
x
2
S(A)M
3
or
in
this
2
3
2
+k_i
2
column and 2
3
+k ),
+k_i),
the
S (M) A
and
S (A) M
ki+ kik /(k +k_!k-
S(M)A; ki +k k k /(k k
follows:
constants.
and
as
intermediate
6 . 5
1800
700
has
e
6 . 5
the
e
e
e
6 . 5
380
15
800
been
220
650
represents
for
200
applicable.
580
440
85000
4 . 5 e
e
0.73
2100
0.48
4 . 5
1.8
e
4 . 5
1.3 0.28
1.3
e
0.42
4.5 4 . 5
1600
3.7
2800
3.7 2.3
28 1.8
12000
not
(continued)
18000
V
steady-state
d
expression
The
a
+
NH+/H (160)
+
NHt/H+(40)
H-ZSM-5
L-arg
3
+
+
(CH ) NHI/Na
7
+
5
3
n-C H NHT/Na
2
C H NHt/Na
3
CH NHt/Na
+
Z-4A
NH|/Na
Table
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GEOCHEMICAL PROCESSES AT MINERAL SURFACES
250
is
apparent
calate seen
from
more
that
steric
the trend
factors
step)
rate
step)
effects.
constants
properties
of
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for
the L
(levorotatory)
minerals.
To test
intercalation
in
interlayer Table
V.
suggests with (b)
that
is
a topic
volume
spacing
of
(see,
based
interest
Voudrias
to L-ornithine
However,
this
of
a
reaction
catalyst.
determined
k
The
rate
kinetic
constants
responsible product ated
with study
from
show t h a t step
this
(step
the observed suggests
study
of Acidic
3),
play
activities
interlayer
turn
depend
obtained H
+
(22) as
is
slowly
from
the relaxation
a r e summarized
Lknown.
i n the absence
reaction
i n the
technique
was
3
^
i n Table
(steps hours
the rate
Urea
The
1 a n d 2)
hydrolysis. over
V.
(XIII)
are
T h e much and not
limiting
slower
associ-
step. size
the c a t a l y t i c
potential
role
on I n t e r c a l a t i o n protons
V.
bound
in their and a c i d i c
kinetic
different
i n Table
S(Na)
i n determining
The c a t a l y t i c
at three
of
is well
and molecular
on t h e s i l i c a - a l u m i n a r a t i o
i n H-ZSM-5
this
spacing
zoelite,
an important
(23).
steps
occuring
Properties
of t h e H-ZSM-5
framework
by arginase,
are given
catalyzed
i n the environment.
Effect
in
Orn or
of
minerals
mineral
contaminants
elsewhere
k
relaxations,
that
nature.
The h y d r o l y s i s
S(Na-Orn*Urea) ^
may b e i m p o r t a n t
(c)
of
of organic
2
contaminant
channels
in
the pressure-jump
intercalation
f o r the observed
release
This
associated
acids
2
data
summarized
L-histidine
H 0
+
using constants
are
for
for the hydrolysis
^s(Na)Arg+-"^
Arg ~
rate
very
isomer
layered
(19):
ki S ( N a ) ^
of
The r a t e
and d i s c u s s e d
systems
optical
The a b i l i t y
only
alkyl-
of L - and D - h i s t i d i n e
amino
reactions
using
follows
living
r e a c t i v i t y may b e
place
The mechanism
t o be as
of
properties
and urea, catalyzed
of montmorillonite
the
the chemical
investigation
of
steric
important.
and Reinhard).
takes
of
that
(21).
Phenomena.
hydrolysis
arginine
presence
be
enhanced
the L-form
The
step
(deintercalation
value
a
the rates
on t h i s
chemical of
ion.
compound was i n v e s t i g a t e d
the s l i g h t l y
current e.g.,
the p K
technique
is
both
reflecting
k_i
13, suggesting
hypothesis,
Intercalation
to catalyze
constant
the D (dextrorotatory)
relaxation
selection
Catalytic
with
of
and the subsequent i o n -
the stereoselective
relative
natural
surfaces
over
this
A s shown
site
for the preference
i n t o HT l a y e r e d
pressure-jump
and
with
the exchanging
i o n may a l s o
explanation
may b e a s s o c i a t e d
the
better
i n Figure
inter12 i t
(the i n t e r c a l a t i o n
2
the rate
the exchanging
A possible
of
to
i s a function
the c a t i o n volume,
hand,
to correlate
ammonium i o n a s shown
are able
From F i g u r e
reaction
k i and k
with
ions
phase.
to an adsorption
correlate
On t h e o t h e r
seems
the smaller
the solid
i n the overall
the aperture
exchange
data, into
and chemical p r o p e r t i e s
intercalation through
these
favorably
Phenomena.
and a c i d i c
properties
studies
o f H-ZSM-5
The rate ratios
The mechanism t h a t
in
constants
of exchange
silica-alumina
In the
on t h e a l u m i n o s i l i c a t e
catalytic
(23).
of
o f NH"J" f o r
(40,
8 0 , 160)
was p r o p o s e d
follows:
In Geochemical Processes at Mineral Surfaces; Davis, J., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 1987.
is
Adsorption-Desorption
Kinetics
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YASUNAGA AND IKEDA
In Geochemical Processes at Mineral Surfaces; Davis, J., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 1987.
GEOCHEMICAL PROCESSES AT MINERAL SURFACES
252
S (H)
where of
+
^
the intermediates
S(NH\)
in
this
of
the ion-exchange
study,
the
were
trend
reaction.
t h e same
acidity
values
silica)
This
i o n i s not appreciably properties
reactivity
and Conclusions
In
r e v i e w we h a v e
this
successfully
mineral/water
charged, theory
and
shown
reaction
cations
have
have
ions
also
been
illustrated have
been
steric
hence
to the
silica-alumina where
play
of the
the inter
(e.g.,
NR*t) t h e
an important
role
ions double
of
studies
properties
anions of
of inorganic and interlayer
information
on the rates
catalytic
layer
obtain
adsorbing
kinetic
predominately
and chemical
of influence
to
with
adsorption/desorption
and s p e c i f i c a l l y Relaxation
canbe
occuring at
electrical
c a n be combined
The mechanistic
methods
of inorganic
oxides,
and ion-exchange
having
stereoselective,
relaxation
of reactions
Mechanisms
discussed.
minerals
degrees
with
data
counterion,
reviewed.
that
varying
Minerals have
with
chemical
metal
and rate
intercalation/deintercalation organic
a
hindered
For reactions
mechanisms.
been
result
studied;
to the acidity
site
t h e dynamics
nonporous
electrolyte
ratios
i n systems
sterically
that
to study
and equilibrium
proton,
that
t o be
V, the interlayer
corresponds
3
scheme
results
of the minerals.
interface.
essentially
plausible of
applied
was found
from
related
of the ion-exchange
Summary
the
i n going
implies
chemical
the relative
the kinetic
i n Table
of k i and k _
calating in
i n the reaction
+
for a l l silica-alumina
(more
site.
(XIV)
observed
A s shown
o f 40 t o 1 6 0 , and i s d i r e c t l y
ion-exchange
H+
to interpret
i . e . , the relaxation
of increasing
increasing ratio
+
S(H)NH"t a n d S ( N H O H
Equation XII are not required
spacings
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N H l ^
of ions of
surface
obtained has and minerals
reaction.
and i o n - s i e v e
properties
discussed.
Acknowledgments The
authors
critical
are grateful
reading
t o Kim F . Hayes a t
of the manuscript
Stanford
and f o r helpful
University for
discussion.
Literature Cited 1.
Allen, L. H.; Matijevic, E . ; Meites, L. J. Inorg. Nucl. Chem. 1971, 33, 1293-1299. 2. Huang, C. P.; Stumm, W. J . J. Colloid Interface Sci. 1973, 43, 409-420. 3. James, R. O.; Healy, T. W. J. Colloid Interface Sci. 1972, 40, 42-52, 53-64, 65-81. 4. Davis, J . Α.; Leckie, J . O. J . Colloid Interface Sci. 1978, 67, 90-107. 5. Davis, J . Α.; Leckie, J . O. J. Colloid Interface Sci. 1980, 74, 32-43.
In Geochemical Processes at Mineral Surfaces; Davis, J., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 1987.
12.
YASUNAGA AND IKEDA
6. 7. 8. 9. 10.
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11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23.
Adsorption-Desorption Kinetics
253
Whittinham, M. S.; Jacobson, A. J., Eds., "Intercalation Chemistry"; Academic Press: New York, 1982. Hachiya, K.; Ashida, M.; Sasaki, M.; Kan, H.; Inoue, T.; Yasunaga, T. J. Phys. Chem. 1979, 83, 1866-1871. Bernasconi, C. F. "Relaxation Kinetics"; Academic Press: New York, 1976. Tsuji, T.; Yasunaga, T.; Sano, T.; Ushio, H. J. Am. Chem. Soc. 1976, 98, 813-818. Ikeda, T.; Nakahara, J.; Sasaki, M.; Yasunaga, T. J . Colloid Interface Sci. 1984, 97, 278-283. Dolzhenkova, A. N.; Gevorkyan, Β. Α.; Vishnyakova, G. V. Obogasch. Rud. (Leningrad), 1973, 18, 31. Astumian, R. D.; Sasaki, M.; Yasunaga, T.; Schelly, Z. A. J. Phys. Chem. 1981, 85, 3832-3835. Astumian, R. D.; Schelly, Z. A. J. Am. Chem. Soc. 1984, 106, 304-308. Sasaki, M.; Moriya M.; Yasunaga, T.; Astumian, R. D. J. Phys. Chem. 1983, 87, 1449-1453. Mikami, N.; Sasaki, M.; Hachiya, K.; Astumian R. D.; Ikeda, T.; Yasunaga, T. J . Phys. Chem. 1983, 87, 1454-1458. Hachiya, K.; Sasaki, M.; Saruta, Y.; Mikami, N.; Yasunaga, T. J. Phys. Chem. 1984, 88, 23-27. Hachiya, K.; Sasaki, M.; Ikeda, T.; Mikami, N.; Yasunaga, T. J. Phys. Chem. 1984, 88, 27-31. Ikeda, T.; Sasaki, M.; Yasunaga, T. J . Phys. Chem. 1983, 87, 745-749. Ikeda, T.; Yasunaga, T. J . Phys. Chem. 1984, 88, 1253-1257. Mikami, N.; Sasaki, M.; Yasunaga, T.; Hayes, K. F. J. Phys. Chem. 1984, 88, 3229-3233. Ikeda, T.; Amoh, H.; Yasunaga, T. J . Am. Chem. Sco. 1984, 106, 5772-5775. Ikeda, T.; Yasunaga, T. J. Colloid Interface Sci. 1984, 99, 183-186. Kokotailo, G. T.; Lowton, S. L . ; Olson, D. H.; Meier, W. M. Nature (London), 1978, 272, 437-438.
RECEIVED June
18, 1986
In Geochemical Processes at Mineral Surfaces; Davis, J., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 1987.