HAL Id: hal-02350935
https://hal.archives-ouvertes.fr/hal-02350935
Submitted on 6 Nov 2019
HAL is a multi-disciplinary open access archive for the deposit and dissemination of sci- entific research documents, whether they are pub- lished or not. The documents may come from teaching and research institutions in France or abroad, or from public or private research centers.
L’archive ouverte pluridisciplinaire HAL, est destinée au dépôt et à la diffusion de documents scientifiques de niveau recherche, publiés ou non, émanant des établissements d’enseignement et de recherche français ou étrangers, des laboratoires publics ou privés.
The Role of pH, Temperature, and NH4+ during Mica Weathering
Daniel Lamarca-Irisarri, Alexander van Driessche, Guntram Jordan, Chiara Cappelli, F. Javier Huertas
To cite this version:
Daniel Lamarca-Irisarri, Alexander van Driessche, Guntram Jordan, Chiara Cappelli, F. Javier Huer-
tas. The Role of pH, Temperature, and NH4+ during Mica Weathering. ACS Earth and Space
Chemistry, ACS, In press, �10.1021/acsearthspacechem.9b00219�. �hal-02350935�
HAL Id: hal-02350935
https://hal.archives-ouvertes.fr/hal-02350935
Submitted on 6 Nov 2019
HAL is a multi-disciplinary open access archive for the deposit and dissemination of sci- entific research documents, whether they are pub- lished or not. The documents may come from teaching and research institutions in France or abroad, or from public or private research centers.
L’archive ouverte pluridisciplinaire HAL, est destinée au dépôt et à la diffusion de documents scientifiques de niveau recherche, publiés ou non, émanant des établissements d’enseignement et de recherche français ou étrangers, des laboratoires publics ou privés.
The Role of pH, Temperature, and NH4+ during Mica Weathering
Daniel Lamarca-Irisarri, Alexander van Driessche, Guntram Jordan, Chiara Cappelli, F. Javier Huertas
To cite this version:
Daniel Lamarca-Irisarri, Alexander van Driessche, Guntram Jordan, Chiara Cappelli, F. Javier Huer-
tas. The Role of pH, Temperature, and NH4+ during Mica Weathering. ACS Earth and Space
Chemistry, ACS, 2019, �10.1021/acsearthspacechem.9b00219�. �hal-02350935�
1
The Role of pH, Temperature, and NH 4 + during Mica Weathering
2
Daniel Lamarca-Irisarri,
†Alexander E. S. Van Driessche,*
,‡Guntram Jordan,
§Chiara Cappelli,
∥3
and F. Javier Huertas
†4†
Instituto Andaluz de Ciencias de la Tierra (CSIC-University of Granada), Avda. de las Palmeras 4, 18100 Armilla, Granada, Spain
5‡
Universite ́ Grenoble Alpes, Universite ́ Savoie Mont Blanc, CNRS, IRD, IFSTTAR, ISTerre, F-38000 Grenoble, France
6§
Department fu ̈ r Geo- und Umweltwissenschaften, Ludwig-Maximilians-Universita ̈ t Mu ̈ nchen, Theresienstr. 41, 80333 Mu ̈ nchen,
7
Germany
8∥
Department of Geological Sciences, The University of Alabama, 201 Seventh Avenue, 2003 Bevill Building, 35487 Tuscaloosa,
9
Alabama, United States
10
*
S Supporting Information11
ABSTRACT: Phyllosilicates are abundant materials both on Earth and Mars,
12
and the weathering of these minerals is an essential part of a wide variety of
13
geochemical cycles. Alteration mainly takes place at the solution − mineral
14
interface and needs to be fully understood in order to correctly model global
15
water − rock interactions. To directly link the physicochemical solution
16
properties to the dominant surface processes controlling phyllosilicate
17
alteration, we used a custom-built hydrothermal atomic force microscope to
18
study in situ the surface reactivity of biotite, phlogopite, and muscovite in
19
contact with aqueous solutions for a broad range of temperatures and pH
20
values. On the basis of our microscopic observations correlated with
21
previously obtained macroscopic dissolution rates, we have constructed a
22
tentative weathering diagram for mica minerals connecting the dominant
23
surface mechanisms and bulk dissolution behavior to the physicochemical
24
solution properties (pH, T, and speciation). The resulting diagram can be
25
divided into two main areas: low-grade weathering occurring at low temperatures and mildly acidic to neutral pH and high-
26
grade weathering taking place at high temperatures and low pH, separated by a transition zone. Each of these areas is
27
characterized by a series of chemical and physical surface processes, which can be related directly or indirectly to incongruent
28
and congruent bulk dissolution. The transition temperatures and pH values depend on the type of mica, with biotite being the
29
most reactive one and muscovite the least reactive one. It is noteworthy that for close to neutral pH conditions the presence of
30
NH
4+shifts the transitions from low- to high-grade weathering to a signi fi cantly lower temperature.
31
KEYWORDS: hydration, dissolution, (re)precipitation, biotite, muscovite, phlogopite, in situ observation, weathering diagram
1. INTRODUCTION
32
The weathering of phyllosilicates, e.g., clay minerals and micas,
33
is a ubiquitous process on the (sub)surface of Earth
1,2and
34
Mars.
3In the latter case, the presence of phyllosilicates is used
35
as an important indicator of past climate.
4,5On Earth, clay
36
minerals (partially) determine many physicochemical proper-
37
ties such as porosity, ion exchange, and adsorption of
38
sediments and soils that in turn control the circulation of
39
fl uids and availability of nutrients and contaminants.
6,7Clay
40
minerals are also important in engineered environments, where
41
they are routinely used as binders for molding sands in
42
foundries,
8,9sealing liners in land fi lls and water dams,
10or as
43
barriers in geological long-term nuclear waste disposal
44
facilities,
11to name just a few. Accordingly, the reactivity of
45
clay minerals has been studied in detail for a broad range of
46
conditions probing the in fl uence of pH, temperature, and
47
salinity, among others.
12−18Micas are important rock-forming
48
minerals, whose dissolution directly in fl uences soil and
groundwater chemistry. In soils, for example, the release of
49potassium from micas, such as biotite, is essential for plant
50growth.
19In deeper media the alteration of micas to
51expandable smectites and vermiculite leads to changes in the
52rock structure and sediment porosity.
20 53The reactivity of mica has been extensively studied using
54mainly macroscopic (i.e., bulk) and microscopic (i.e., nano-
55scale) approaches. Di ff erent mica minerals, such as biotite,
56phlogopite, muscovite, or other sheet silicates, such as
57apophyllite, have been investigated.
21−25Bulk studies have
58shown that a departure from neutral pH conditions always
59leads to faster dissolution.
22,23,26−28Also, at higher temper-
60atures the dissolution rate is higher.
27On the other hand,
61Received: August 7, 2019 Revised: October 18, 2019 Accepted: October 22, 2019 Published: October 22, 2019 A
62
single-crystal experiments unveiled that dissolution mainly
63
takes place at the crystal edges, while often the basal surface is
64
more resistant to dissolution showing for certain experimental
65
conditions hydration patterns, surface decomposition, and/or
66
etch pit formation.
29−32In situ and ex situ atomic force
67
microscopy (AFM) studies at elevated temperatures (>80 ° C)
68
have shown that the reactivity of the basal surface increases
69
signi fi cantly,
32,33although it was observed that at temperatures
70
above 120 ° C the formation of secondary phases (e.g.,
71
gibbsite/kaolinite) coats the surface, blocking reactive sites
72
and thus lowering the basal surface reactivity.
32However,
73
despite the insights gained from the previous studies, a general
74
correlation between the physiochemical solution properties
75
(e.g., pH, temperature, and salinities) and the nanoscale
76
patterns at the mineral − solution interface that result from the
77
various alteration processes (i.e., dissolution, hydration, ion
78
exchange, and (re)precipitation) has not yet been established.
79
Moreover, the link between surface processes and the
80
measured bulk dissolution rates also warrants further
81
clari fi cation.
82
Recently, it was reported that mica minerals could act as an
83
important carbon reservoir. Detailed AFM observations of
84
phlogophite and muscovite revealed that nanoprotusions, i.e.,
85
bulges, located at the basal surfaces trapped signi fi cant
86
quantities of hydrocarbons
34and supercritical CO
2,
3587
respectively. At present, it remains unclear if these inclusions
88
are primary, i.e. syngenetic with the rock formation, or
89
secondary, i.e. related to weathering phenomena, and how the
90
hydrocarbons/scCO
2entered the interlayer of these non-
91
swelling phyllosilicates. Only the reaction with wet-scCO
292
caused the formation of bulges, whereas scN
2, dry-scCO
2,
93
and scCO
2-saturated brine did not. This suggests that a scCO
2-
94
acidi fi ed water fi lm between bulk scCO
2and muscovite is
95
needed for CO
2molecules to enter the interlayers. These
96
observations further highlight the crucial role of surface
97
processes during phyllosilicate weathering.
98
To further our understanding of the complex interplay
99
between the physicochemical solution properties and the
100
process controlling mica alteration we directly observed the
101
surface reactivity of biotite, phlogopite, and muscovite in
102
contact with aqueous solutions for a broad range of pH values
103
(1−6.8) and temperatures (23−120 °C), making use of
104
hydrothermal atomic force microscopy (HAFM). These short-
105
term (up to ∼ 8 h) in situ experiments were complemented
106
with ex situ characterization of long-term (up to 50 days) and
107
high-temperature (up to 200 ° C) experiments conducted in
108
hydrothermal batch reactors. In ammonium-rich environments
109
(e.g., crustal rocks, diagenetic sediments), potassium of K-
110
bearing minerals is commonly substituted by ammonium
111
because of the similar charge and ionic radius.
36Despite this
112
abundant occurrence of mica with NH
4+fi xed in its interlayer,
113
and its capacity to act as a signi fi cant source of protons at
114
circumneutral pH, the potential in fl uence of this ion on
115
phyllosilicate weathering has been largely overlooked. There-
116
fore, in this study we have also conducted experiments at pH
117
6.8 using solutions containing 0.1 M NH
4+.
118
The obtained microscopic data were analyzed in detail and
119
correlated with previously obtained macroscopic dissolution
120
rates. On the basis of these insights we constructed a tentative
121
weathering diagram, linking the surface mechanism and bulk
122
dissolution behavior to the main physicochemical solution
123
properties.
2. MATERIALS AND METHODS
2.1. Natural Samples. The materials used in this study are
124(1) Bancroft biotite, (2) Templeton phlogopite, and (3)
125Madras muscovite. Their chemical bulk composition was
126determined by X-ray fl uorescence spectrometry (XRF), and an
127estimation of Fe
2+and Fe
3+was obtained based on literature
128data.
37,38 129(1) Biotite: K
0.97(Mg
1.40Fe
2+1.18Fe
3+0.11Al
0.04Ti
0.09Mn
0.09)-
130(Al
0.97Si
3.03)O
10(OH)
2 131(2) Phlogopite: K
0.93(Mg
2.63Fe
2+0.13Fe
3+0.02Al
0.16)(Al
1.03-
132Si
2.97)O
10(OH)
2 133(3) Muscovite: (K
0.9Na
0.08)(Mg
0.09Fe
2+0.17Fe
3+0.02Al
1.75-
134Ti
0.03)(Al
0.94Si
3.06)O
10(OH)
2 1352.2. In Situ Characterization. In situ observation of the
136mica-solution interface was carried out using a custom-built
137contact-mode hydrothermal atomic force microscope
39,40and
138uncoated Si-cantilevers with integrated tips (Nanosensors). A
139schematic drawing of this experimental setup can be found in
140ref 38. For the experiments, mica fl akes with an area of ∼ 25 −
14135 mm
2and thickness of ∼ 0.1 − 0.4 mm were exfoliated
142immediately before fi xing them with a titanium wire within the
143HAFM cell. Subsequently, the cell was fi lled with solution,
144sealed, and pressurized to reach the desired temperature (80,
145100, or 120 ° C). The cell has been connected to 3 reservoirs
146containing solutions with di ff erent compositions, which could
147be fl owed through the cell independently. The fl ow rates
148ranged from 3 to 5 mm
3· s
−1, allowing a rapid renewal of the
149fl uid within the cell (volume ≈ 500 μ L). Because of rapid fl uid
150renewal and a mineral surface area of only a few square
151millimeters, the chemical composition of the fl uid was
152negligibly a ff ected by mineral −fl uid reactions occurring in
153 154 t1the cell. All solutions (Table 1) were prepared by dissolving
reagent grade chemicals into deionized water (18 M Ω· cm).
155Using this setup, a total of over 60 experiments (Table S1)
156were performed of varying duration (3 − 10 h).
157Two di ff erent protocols were used for the in situ HAFM
158measurements: (I) variable pH experiments to test the pH
159e ff ect on the surface reactivity and (II) constant pH
160experiments to study the long-term e ff ect of each experimental
161solution on the alteration dynamics.
1622.3. Ex Situ Characterization. To extend the observation
163time ( ∼ 10 h max) of the HAFM experiments, batch reactors
164were set up for posterior ex situ characterization of the reacted
165surfaces. In each 45 mL reactor (Parr 4744), one mica fl ake of
166∼ 25 − 35 mm
2and ∼ 0.1 − 0.4 mm thickness was placed and 35
167mL of reacting solution was added (Table 1). The reactors
168were maintained in an oven at constant temperatures of 120
169Table 1. Overview of the Aqueous Solutions Used To React with the Mica Surfaces
solution pH remarks
0.1 M HCl 1.0 For the pH 2 and 4 solutions, the ionic strength was keep constant, with respect to the pH 1 solution, by adding a corresponding amount of KCl.
0.01 M HCl 2.0 0.001 M HCl 4.0
deionized water
5.8 Always used as initial solution during pressurization and heating of the HAFM system.
0.1 M ammonium acetate
6.8
B
170
and 200 ° C ( ± 3 ° C) for 1, 2, 3, and 50 days. Mica samples
171
were recovered from the reactors and washed three times with
172
deionized water. Then, the basal surface topography of the
173
reacted mica fl akes was immediately characterized using AFM.
174
Measurements were done at room temperature ( ∼ 23 ° C) in
175
contact mode using nonconductive silicon nitride uncoated
176
tips (Bruker). For chemical characterization of the altered
177
surfaces, reacted samples were imaged using a scanning
178
electron microscope equipped with an energy-dispersive X-
179
ray spectroscope (SEM, CIC - University of Granada).
3. RESULTS
180
3.1. Hydration Processes. With our experimental setup,
181
two main features of mica hydration were observed: (I)
182
swelling f ronts, i.e., the fronts of more or less uniformly swelled
183
layers spreading laterally on the surface; the increase of the
184
layer height ranged between ∼ 0.5 nm and a few nanometers
185
and a ff ected large areas of the basal surface.
41−43(II) bulges,
186
i.e., abrupt and laterally con fi ned swelling of the surface in a
187
round or an elongated and partially branched shape. Bulges can
188
migrate on the surface and most likely result from an excessive
189
but spatially con fi ned hydration.
28,39,40190
3.1.1. Bulge Formation. At pH 1 and T > 80 ° C, the
191
reactivity of biotite was too high for evaluable AFM
192
observations for a su ffi ciently long period of time. At pH 1
and 20 − 80 ° C, the formation of point-shaped bulges (up to 25
193 194 f1nm in height) was observed after ∼ 30 min (Figure 1A,B), which eventually broke open at the top. Similar observations
195were made at pH 2 in the temperature range of 80 − 100 ° C
196(data not shown). At pH 4 (80 and 100 ° C), the top of the
197bulges became more rounded and remained unbroken. It is
198worth noting that at pH 4 − 5.8, bulges still migrated across the
199surface (Figure 1C − F). In NH
4+-solutions (pH 6.8), bulges
200were less abundant but were also round-shaped and did not
201break open.
202203 f2
At pH 4 − 6.8 and all temperatures, bulges branched (Figure
204 f2
2A) following directions that roughly corresponded to the main PBC directions ⟨ 110 ⟩ , ⟨ 11 ̅ 0 ⟩ , and ⟨ 100 ⟩ .
44This indicates
205a certain degree of structural control over the formation and
206migration of bulges. Occasionally, bulges showed an open side
207at steps (Figure 2B) and allowed comparison of the spacing
208between the swelled and nonswelled layers revealing a roughly
209doubled spacing of the altered layer (Figure 2C) at pH ≥ 4
210and an expansion of 28 − 30 nm/layer at pH ≤ 2 (Figure S1),
211due to complete disruption of the mica layered structure.
212Within the pH range tested here, no bulge formation was
213observed on muscovite and phlogopite. Previous studies of
214cation exchange in phlogopite (using octylammonium and
215NaCl solutions), however, did report the formation and
216migration of bulges.
42,43Recently, bulges (referred to as
217Figure 1.In situ HAFM images of initial surface patterns formed on biotite basal faces in contact with acidic solutions. (A) Typical bulges observed after 35 min at pH 1 and 80°C. (B) Cross sections of the bulge structures observed in image A, showing sharp profiles, indicating the initial stage of fracturing. (C) Cross sections and (D−F) time-lapse images of bulge formation and migration at pH 4 and 100°C. After 5 h and 20 min bulges of 30 nm developed. These structures moved at a rate of∼0.85μm/min toward the upper right corner of the image, leaving behind two elongated relict areas.
Figure 2.(A) Optical microscope image of a (001) surface of biotite reacted for 16 days at 50°C and pH 6.8, showing the regular alignment of the bulges, and (B) AFM deflection image of (001) face of biotite reacted for 3 days at 200°C and pH 6.8, (C) showing a∼200 nm high broken bulge (1) and a∼100 nm high nonswelled area (2). This points to a ratio of about 2 nm/layer (1 nm of swelling).
Article
C
218
nanoprotrusions) containing hydrocarbons were detected on
219
phlogopite from Ugandan kamafugite rock samples.
34220
Furthermore, bulges (referred to as blistering) were observed
221
on muscovite exposed to water-saturated scCO
2at 12 MPa and
222
90 ° C.
35223
3.1.2. Swelling Front Formation and Collapse Structures.
224
The second hydration process frequently observed during the
225
initial stages of biotite alteration is the development of swelling
226
fronts. At pH 1 − 2, the swelling fronts appeared static (by the
227
time AFM imaging started). However, at pH 4 − 5.8 and T =
f3 228
25 − 120 ° C, swelling fronts were moving still (Figure 3).
229
To further unravel the in fl uence of pH on the hydration
230
patterns, experiments were carried out with several sequential
231
in situ changes of solution pH. Three di ff erent solution
232
sequences were tested: (I) pH 5.8 → 6.8, (II) pH 5.8 → 6.8 →
233
2.0 → 5.8 → 6.8, and (III) pH 4.0 → 6.8. The most noticeable
234
surface process during these runs was the collapse of previously
235
formed swelled layers when an ammonium solution (pH 6.8)
236
was introduced (Figures 3D and S2). Experiments using
237
sequence I repeatedly allowed observation of the swelling and
238
fl attening of the surface (Figure S3). As a consequence of this
239
repeated sequence, swelling and collapse networks resulted on
240
the surface (Figure S4). A common structure associated with
241
the collapse of swelling fronts and bulges is the formation of
242
relict areas (circles in Figure 3D). Relict areas (also termed
243
engulfed areas
43) are small swelled remnants of previously
244
large swelled or bulged surface areas. Thus, the relict areas
245
likely represent isolated vertically expanded areas on the
246
surface in which water molecules from a previous large-scale
247
hydration event are trapped.
3.2. Dissolution Patterns. Given the dissolution dynamics
248and the overall observed surface roughness, we have differ-
249entiated two levels of surface alteration occurring during the
250reaction of aqueous solutions with mica minerals: (I) low-
251grade decomposition (LGD), which is characterized by
252roughening (<1 nm height fl uctuations) and weakening of
253the given surface layers (which decompose by the mechanical
254impact of the AFM-tip), rather than by mono or multilayer
255etch pit formation and subsequent step retreat, and (II) high-
256grade decomposition (HGD), which is characterized by a
257roughening of the surface due to the formation of a high
258mono- or multilayer step density (via a high etch pit nucleation
259rate).
260Dissolution (ss) usually initiated after the above-described
261hydration processes. With decreasing pH and increasing
262temperature, however, delay of dissolution decreased and
263both processes occurred increasingly contemporaneous. At pH
2641 the surface reactivity is high and was best observed at room
265temperature (23 ° C). For these conditions, dissolution is
266dominated by step retreat ( ∼ 0.01 μ m/min), which often
267advanced more rapidly in a speci fi c direction as a consequence
268of coalescensing pits concentrated along that direction and
269 270 f4eventually created dissolution channels (Figure 4 A,B). Also the nucleation of monolayer ( ∼ 1 nm) etch pits was frequently
271observed (data not shown). At higher temperatures (80 ° C),
272the formation of etch pits was very abundant and rapidly led to
273a rough surface, i.e., HGD (Figure 4 C,D). At pH 2 and 100
274° C, the surface reactivity was lower compared to pH 1 and
275dominated by step retreat. This corresponds well with previous
276in situ confocal microscopy observations of biotite flakes
277reacting with nitric acid solutions at pH 1.
45We also detected
278the development of fusiform-shaped swelled areas (see
279previous section), which in some cases cracked open and
280collapsed. Cracking of the swelled layers resulted in steps with
281subsequent retreat (Figure S5). Starting from 120 ° C etch pit
282formation became the dominant dissolution process (Figure
2834G,H). Thus, at low pH, etch pit formation and step retreat are
284the most common dissolution processes taking place on the
285(001) surface of biotite, with temperature being the parameter
286controlling which process will be dominant.
287At pH 4, the reactivity of biotite is dominated by partial and
288unordered destruction of the top TOT-layer (characterized by
289<1 nm height fl uctuations of the surface layer), which
290weakened the surface, and which we define as low-grade
291surface weathering. Importantly, for these solution conditions
292 293 f5heterogeneous surface reactivity was observed. Figure 5 shows how certain areas of a layer were dissolved because of etch pit
294nucleation, while other areas of the same layer were less
295reactive, remaining virtually unaltered for the duration of the
296observation. These more reactive areas were previously
297affected by bulging that did not fully collapse afterward. This
298suggests that not fully collapsed layers are more prone to
299dissolve, i.e. the bulging process weakened the structure of the
300top layers.
301Because of the low surface reactivity at pH 5.8, dissolution
302patterns could not be observed during HAFM experiments. To
303obtain information about the surface reactivity for these
304solutions, mineral alteration was carried out in batch reactors
305at 200 ° C and characterized ex situ. After 3 days of reaction,
306mainly low-grade surface weathering was observed but no etch
307pits could be detected.
308In the solutions containing NH
4+(pH 6.8) at T ≤ 120 ° C,
309hydration, dissolution, and precipitation processes occurred
310Figure 3.In situ HAFM observation (6.3 h) of the interaction of a pH 4 solution at 100°C with a biotite surface: (A) initial biotite surface topography after reaching 100 °C and (B) formation of swelling fronts (white arrows) of 5 nm in height after 340 min. (C) Subsequently, bulges evolved during the following 25 min (white arrows). This bulging network was approximately 60 nm in height.
(D) General collapse after 10 min of ammonium solution treatment.
Several relict areas remained on the surface (white circles), and overall increase of the surface roughness is observed.
D
311
simultaneously with comparable intensity and obscured
312
observation of individual etch pits and/or retreating steps. At
T > 120 ° C, etch pits formed, although with a lower density
313than in acidic solutions. The fact that at pH 5.8 and T > 120
314°C no etch pits were observed (see above) points to a
315remarkable promotion of the reactivity of biotite basal surface
316by NH
4+.
317Samples reacted with NH
4+solutions for longer times at
318di ff erent temperatures (50 and 120 ° C) were analyzed ex situ
319by SEM. This revealed the presence of Si-enriched layers
320(Figure S6). Such layers were much more extensive for the
321samples reacted at 50 ° C than those at 120 ° C, where Si-
322enrichment was detected only at step edges. The long-term
323experiments (50 days) at 200 ° C revealed intense pit
324formation, reaching a depth of up to 10 nm (Figure S7).
325The angles between intersecting edges of these pits correspond
326with those of the structure of the basal surface, which indicates
327that dissolution morphology is eventually controlled by
328structural factors.
44−46 3293.3. Precipitates. At pH 1 − 5.8 and T < 100 ° C, no
330precipitates were formed within approximately 5 h of HAFM
331imaging. In contrast, in NH
4+solutions (pH 6.8), extensive
332formation of a secondary phase(s) was observed during in situ
333HAFM imaging of biotite and muscovite but never in the case
334of phlogopite. Isolated particles of ∼ 1 nm height appeared on
335biotite and muscovite after 140 min at 120 ° C and 5 h at 100
336° C, respectively (Figure S8). In both cases, the individual
337particles formed randomly, expanded laterally, merged, and
338covered the entire surface while the height remained constant.
339When a pH 2 solution was injected into the HAFM liquid cell,
340the coating rapidly dissolved, exposing the pristine mica
341surface. The persistence of the underlying mica surface clearly
342shows that no surface amorphization took place under these
343conditions (which would have led to fast and instantaneous
344dissolution in the presence of an acidic solution).
345Batch experiments on biotite reacted for 3 days at pH 6.8
346and T = 120 ° C showed the presence of precipitates forming a
347coating ( ∼ 1 nm) on the surface and areas depleted in
348octahedral cations/enriched in Si (Figure S9). At pH 6.8 and T
349= 200 ° C, the surface was partially coated with dendritic
350 351 f6shaped precipitates after 1 day (Figure 6A). These precipitates had a height of ∼ 1.2 nm. After 2 days of reaction at 200 ° C,
352the precipitates coated the surface while their height remained
353unchanged. After 50 days at 200 ° C, large precipitates were
354observed mainly composed of Fe and Al and some containing
355Ti (Figure 6B).
356Figure 4.In situ (H)AFM observation of biotite dissolution at low pH. (A and B) At pH 1 and 23°C, surface dissolution is dominated by step retreat and etch pit development (black arrows); (C and D) pH 1 and 80°C. Abundant surface swelling was observed 38 min after the onset of the experiment, and after 51 min, the roughness increased because of the formation of numerous small etch pits (inset E (deflection channel) and F (height channel) indicated by a black arrow), (G and H) pH 2 and 120 °C. After 47 min of reaction, abundant etch pits have developed (black arrow) and step retreat has occurred.
Figure 5.In situ HAFM images of the biotite surface reactivity at pH 4 and 120°C, which shows the link between hydration and dissolution dynamics. (A and B) Migration of bulges (b) and swelling fronts (s) on the (001) face of biotite. Once the bulges disappeared (C), the remaining layer was“weakened”in areas that are not completely collapsed and dissolved more readily than the rest of the surface; (D) a zoomed-in view of the dotted rectangular area of images A−C. Abundant etch pits (1−3 nm deep) developed in the area that was previously affected by two bulges.
The area unaffected by bulges, or affected by bulges that totally collapsed in a second step, shows only <1 nm heightfluctuations of the surface layer (no≥1 nm etch pits are observed).
Article
E
4. DISCUSSION
357
4.1. Hydration. During the initial stages of the mica surface
358
alteration, both bulges and swelling fronts were the most
359
common surface features. Crystalline swelling (intercalation
360
between individual 2:1 layers) is a process controlled by a
361
balance between attractive forces (i.e., Coulombic attraction
362
between the negative TOT-layers and the interlayer cations
363
and van der Waals interactions between adjacent layers) and
364
repulsive forces (mainly due to the hydration potential energy
365
of the interlayer cations
47). At acidic pH, a rapid K
+− H
3O
+ion
366
exchange likely takes place and an increase of interlayer space
367
occurs because of the readjustment between attraction and
368
repulsion forces and the entrance of water molecules (e.g., 41).
369
When ammonium is added to the solution, a general collapse
370
of the swelled layers occurred, most likely because strong
371
hydrogen bonds form among NH
4+, H
2O, and the negatively
372
charged mineral surface recreating a tight interlayer structure.
47373
In the case of bulges (i.e., nanoprotrusions or blistering), the
374
precise formation mechanism is still unclear, but it seems to be
375
related to the excess water uptake due to local variations of the
376
layer charge.
31Indeed, the local decrease of negative layer
377
charge leads to a decrease of the Coulombic attraction between
378
the interlayer cations and the surface charge sites
47likely
379
causing a higher cation hydration. Bulges also have the capacity
380
to migrate across the surface until they reach a location where
381
the negative charge is high enough to stop them from moving
382
(Figures 3 and S2). However, this behavior has been observed
383
only between pH 4 and 5.8. At lower pH values, the
384
hydronium concentration is high enough to favor the exchange
385
between interlayer cations and hydronium (K
+− H
3O
+) and the
386
mica structure alteration by reactive sites protonation (proton-
387
promoted dissolution). Our observations during both fi xed and
variable pH experiments showed that the development of
388bulges is mainly linked to previous mineral features such as
389swelling fronts (e.g., Figures S2 and S3), cracks or layer edges
390where charge imbalance and bond strain could exist.
391Importantly, our observations also show that bulges play a
392key role in the development of softened areas, which show
393increased dissolution dynamics (see e.g. Figure 5).
394The morphology of bulges changes as a function of pH, i.e.
395at acidic pH they have a sharp pro fi le and are usually cracked
396open along their axial plain, while the profile of bulges formed
397in near neutral conditions tends to be rounded. This might be
398the result of the higher capacity of hydronium to attack the Si −
399O − Si and Si − O − Al groups of the tetrahedral sheet than water
400molecules. This agrees with our measurements of the surface
401topography of bulges; these expanded ∼ 2 nm per layer
402between pH 4 and 6.8 and ∼ 16 nm per layer in acidic media
403(pH < 4). The 2 nm per layer ratio can be linked to the
404expansion capacity of phyllosilicates of low charge while the
405much higher ratio in acidic media points to a generalized
406destabilization of the crystalline structure, which eventually
407leads to its disruption, e.g., cracking of the surface layers. Also
408important to consider is the role of Fe
2+oxidation in the
409expansion of mica layers. During mica dissolution, Fe
2+will
410oxidize (even in very acidic HCl solutions), which should
411reduce the TOT-layer charge and favor the release of interlayer
412cations, making the structure unstable and favoring volume
413expansion and cracking of the top layers. This process has been
414observed in fi eld studies, where during the weathering of
415quartz diorites Fe(II) oxidation in biotite led to volume
416expansion and produced fractures which accelerated further
417reactions.
48 418Figure 6.(A) Ex situ AFM characterization of a biotite surface reacted with a pH 6.8 solution for 1 day at 200°C. Dendritic-shaped precipitates with a thickness of∼1.2 nm covered the basal surface of biotite. Height profile at the right side is that of the white dotted line shown in the 3D AFM image representing the black dotted square area in the 2D image. (B) AFM and SEM images of basal biotite surface reacted for 50 days at 200
°C and pH 6.8, showing (upper) plate-shaped precipitates composed of Fe−Al oxy-hydroxides and (lower) pseudohexagonal to rounded precipitates composed of a Fe−Al rich planar base and a Ti-rich core. Chemical analysis of the different points are (1) 39.3% Al; (2) 1.9% Al and 58.4% Fe; (3) 2.4% Al and 59.5 Fe; and (4) 4.7% Al, 17.1% Fe, and 38.4 Ti.
F
419
Bulges and swelling fronts were observed only for biotite and
420
phlogopite but not for muscovite. This is likely related to the
421
more stable octahedral aluminum in muscovite with respect to
422
iron and magnesium in biotite or phlogopite. Moreover, the
423
diversity of the crystal structure of micas (hydroxyl orientation
424
and tetrahedral twisting and tilting degree), together with their
425
difference in composition, explains the stronger interlayer K
+426
retention and thus the higher stability of muscovite
427
structure.
24,32,49Notwithstanding, a recent study observed
428
abundant formation of bulges on muscovite when reacting at
429
high pressure (12 MPa) and 90 ° C with water saturated in
430
scCO2
35which may lead to the assumption that pressure
431
promotes bulge formation in the case of muscovite.
432
4.2. Dissolution. Our results show that the dissolution
433
dynamics are strongly influenced by both pH and temperature,
434
allowing distinction of two main regimes: (i) At moderate to
435
neutral pH and temperatures up to 100 ° C, low-grade
436
weathering of the mica was observed. This was characterized
437
by the development of shallow roughening ( ∼ 0.2 − 0.5 nm)
438
and weakening of the surface layers (the AFM cantilever tip
439
could easily disrupt the top layer of the basal surface). This is
440
probably the result of unordered destruction of bonds within
441
the TOT layer and incongruent release of material resulting in
442
a certain waviness and undulation of the top surface layer.
443
Hence, these alteration features can be linked to incongruent
444
dissolution previously reported for fl ow-through experi-
445
ments.
22,26,29,50(ii) When the alteration reaction is accelerated
446
by using more aggressive dissolution conditions, i.e. decreasing
447
the pH and/or increasing the temperature (pH 1 and >23 ° C,
448
pH 2 and ≥ 80 ° C, and circumneutral ammonium media at
449
>100 ° C), high-grade decomposition of the surface sets in
450
during the initial stages being characterized by the formation of
451
abundant mono- and multilayer etch pits and step retreat. This
dissolution regime can be linked to congruent dissolution.
24It
452is worth noting that formation of secondary phases on the
453surface may cause retention of material from the e ffl uent
454solution of the cell. A comparison of the chemical
455compositions of input and e ffl uent solution in fl ow-through
456experiments, therefore, might not be apt to reveal congruent
457dissolution in all cases.
458In addition, the results show that ammonium promotes the
459dissolution of micas at circumneutral pH conditions. This can
460be explained by the NH
4+capacity to dissociate into H
++ NH
3 461(e.g., up to 22% at 200 °C), increasing locally the
462concentration of protons in the medium,
51−54which are in
463turn responsible for the attack of Si − O − Si and Al − O − Si
464bonds.
4654.3. Precipitates. During mineral weathering, it is not
466uncommon to observe the formation of amorphous and/or
467crystalline secondary phases on the dissolving surface. This
468occurs because the ions that are released form the mineral can
469interact with each other, or with ions already in the solution,
470and precipitate as a new phase. This can even take place when
471the bulk solution is undersaturated with respect to the
472secondary phase, which is usually termed reprecipitation.
55 473The precipitation of secondary phases during mica alteration
474has been observed for a broad range of pH values and
475temperatures (25 − 200 ° C) using di ff erent experimental
476techniques.
32,56,57In this work, our goal was to constrain the
477physicochemical solution parameters that promote the
478formation of secondary phases; to observe the initial stages
479of this process; and if possible, to identify the precipitates.
480Only in neutral media containing NH
4+we observed the
481formation of secondary Al − Fe phases on the mica surface (in
482situ and ex situ). VP-SEM imaging combined with EDX
483analysis also showed that step edges are preferential sites for
484Figure 7. Schematic representation of the different processes detected for biotite weathering as a function of pH, temperature, and solution speciation. Two main areas, separated by a transition zone (gray), can be distinguished, i.e. high-grade (purple) and low-grade (pink) weathering.
Each area is characterized by a series of surface processes (CD, congruent dissolution; ID, incongruent dissolution). In the presence of NH4+, the enhancement of mica dissolution promotes the precipitation of secondary phases and formation of etch pits, and as such the high-grade weathering zone is shifted to lower temperatures.
Article
G
485
the deposition of Fe-, Al-, and Si-rich phases. Because these
486
components are present only in the mineral phase, the
487
precipitates must have formed through a dissolution − (re)-
488
precipitation process. Some studies have already pointed to the
489
e ff ect of ammonium in the precipitation of Al phases during
490
phyllosilicate alteration experiment due to competitive ion
491
exchange.
58These studies agree with our observations where
492
precipitates correspond to Al and Fe (oxy-)hydroxides, whose
493
formation is favored as solution pH shifts to neutral or alkaline
494
(due to reduced solubility of these phases).
495
In the case of Al-rich secondary phases, Johnsson and co-
496
workers
56proposed that the formation of these phases starts
497
with the exchange of the interlayer K
+by H
3O
+, which leads to
498
the protonation of basal sites where Al can be fi xated and thus
499
serve as a possible hotspot for the nucleation of Al (oxy-
500
)hydroxides. The exchange of K
+for H
3O
+also alters the
501
surface charge of the mica surface, which can promote the
502
polymerization of Al phases.
59Taking into account that
503
ammonium acts as a very weak acid, at higher NH
4+504
concentrations, more protons are available, and thus, more
505
secondary phases should be observed, which was the case in
506
our experiments. In the experiments with phlogopite no
507
precipitates were observed. This is a direct consequence of the
508
high solubility of Mg-phases for the entire range of tested pH
509
values.
5. CONCLUDING REMARKS
510
In this study, we have shown that during the interaction of
511
aqueous solutions with mica minerals several surface processes,
512
i.e., hydration, dissolution, and (re)-precipitation can occur
513
simultaneously. Temperature, pH, and the chemical composi-
514
tion of the mica surface and the solution determine which of
515
these processes are dominant. On the basis of our experimental
516
and previously reported data we have constructed for the fi rst
517
time a detailed weathering diagram for biotite, linking the
518
physicochemical solution properties with the prevailing surface
519
processes for a broad range of possible alteration conditions
f7 520
(Figure 7). Although the precise location of these boundaries
521
of this diagram will shift for phlogopite and muscovite, the
522
general trends are comparable.
523
Our nanoscale observations also allowed us to correlate
524
surface processes with the expected macroscopic outcome of
525
the alteration process, i.e., congruent or incongruent
526
dissolution. Low-grade weathering, representative of macro-
527
scopically observed incongruent dissolution, is favored under
528
less “ aggressive ” conditions (pH 4 − 6.8 and temperatures <100
529
° C), preferentially releasing interlayer and octahedral cations
530
over the tetrahedral compounds through the formation of
531
shallow etch pits. Under these conditions the tetrahedral
532
positions can be attacked, which will lead to congruent
533
dissolution, i.e., step retreat. Thus, macroscopically we will fi rst
534
detect incongruent dissolution, while during later stages
535
congruent dissolution will take over as already theorized by
536
Malmström and Banwart.
26At close to neutral pH in the
537
presence of NH
4+the high-grade weathering zone is shifted to
538
signi fi cantly lower temperatures.
539
Finally, the weathering diagram (Figure 7) also highlights
540
that during low-grade dissolution bulges are important features
541
on the basal surface. Hence, under these conditions it seems
542
more plausible that signi fi cant quantities of hydrocarbons
34543
and supercritical CO
235can be trapped.
■ ASSOCIATED CONTENT 544
*
S Supporting Information 545The Supporting Information is available free of charge on the
546ACS Publications website at DOI: 10.1021/acsearthspace-
547chem.9b00219.
548Supporting Table S1 and Figures S1 − S9 (PDF)
549■ AUTHOR INFORMATION 550
Corresponding Author 551
* E-mail: alexander.van-driessche@univ-grenoble-alpes.fr.
552ORCID 553
Alexander E. S. Van Driessche:
0000-0003-2528-3425 554Notes 555
The authors declare no competing fi nancial interest.
556■ ACKNOWLEDGMENTS 557
This study was supported by funding from the Spanish
558Government Contracts (MINECO CGL2011-22567 and
559CGL2014-55108-P, with contribution of EU-FEDER funds)
560and the PICS 2017 CNRS program (PICS07954). D.L.-I. was
561supported by an FPI fellowship (BES-2012-058890) and
562Grants (EEBB-I-16-11519 and EEBB-I-15-10043).
563■
(1)REFERENCES
Wilson, M. J. Weathering of the primary rock-forming minerals:564565processes, products and rates.Clay Miner.2004,39, 233−266. 566
(2)Churchman, G. J. The Alteration and Formation of Soil Minerals 567
by Weathering. InHandbook of Soil Science; Sumner, M. E., Ed.; CRC 568
Press: Boca Raton, FL, 2000. 569
(3) Altheide, T. S.; Chevrier, V. F.; Noe Dobrea, E. Mineralogical570
characterization of acid weathered phyllosilicates with implications for 571
secondary martian deposits.Geochim. Cosmochim. Acta2010,74(21),572
6232−6248. 573
(4) Ehlmann, B. L.; Mustard, J. F.; Murchie, S. L.; Bibring, J.-P.; 574
Meunier, A.; Fraeman, A. A.; Langevin, Y. Subsurface water and clay 575
mineral formation during the early history of Mars.Nature2011,479, 576
53−60. 577
(5) Carter, J.; Loizeau, D.; Mangold, N.; Poulet, F.; Bibring, J.-P. 578
Widespread surface weathering on early Mars: A case for a warmer 579
and wetter climate.Icarus2015,248, 373−382. 580
(6)Dixon, J. D. Roles of clays in soils.Appl. Clay Sci.1991,5, 489− 581
503. 582
(7)Churchman, G. J. Game Changer in Soil Science. Functional role 583
of clay minerals in soil.J. Plant Nutr. Soil Sci.2018,181, 99−103. 584
(8)Schiebel, K.; Jordan, G.; Kaestner, A.; Schillinger, B.; Georgii, R.; 585
Hess, K.-U.; Boehnke, S.; Schmahl, W. W. Effects of heat and cyclic 586
reuse on the properties of bentonite-bonded sand. Eur. J. Mineral.587
2018,30, 1115−1125. 588
(9)Schiebel, K.; Jordan, G.; Kaestner, A.; Schillinger, B.; Boehnke, 589
S.; Schmahl, W. W. Neutron radiographic study of the effect of heat- 590
driven water transport on the tensile strength of bentonite bonded 591
moulding sand.Transp. Porous Media2018,121, 369−387. 592
(10)Wolters, F.; Baille, W.; Emmerich, K.; Schmidt, E.; Wolters, C.;593
Königer, F.; Kunz, J.; Krase, V.; Schellhorn, M. High-density bimodal594
bentonite blends for hydraulic sealings at the ibbenbüren coalmine. 595
Clay Miner.2015,50(3), 391−403. 596
(11) Mukherjee, S. The Science of Clays: Applications in Industry, 597
Engineering, and Environment; Springer: Netherlands, 2013; p 335. 598
(12)Zysset, M.; Schindler, P. W. The proton promoted dissolution 599
kinetics of K-montmorillonite. Geochim. Cosmochim. Acta 1996,60 600
(6), 921−931. 601
(13)Furrer, G.; Zysset, M.; Schilndler, P. W. Weathering kinetics of 602
montmorillonite: investigations in batch and mixed flow reactors.603
Geochemistry of Clay-Pore Fluid Interactions, 1st ed.; Manning, D. A. 604 H