H CHARACTERIZATION OF IRON AND MANGANESE
2.4 Results and Discussion
2.4.3 Reductive dissolution experiments
2.4.3.1 Iron
The total Fe-oxide concentrations
(Felll(TiEDTA))
determinedby
the Ti-EDTA extraction are shown in
Figure
2-3b. Acomparison
withFigure
2-3a shows that ferric oxides account for the
major
fraction of iron(50-80%
of
Fetot)
in theanalyzed grain
size fractions. There isagain significantly
more
Felll(TiEDTA)
in thedeeper samples
than in the referencesample (4.0-5.0 m).
The distribution of the ferric oxides isstrongly grain
sizedependent.
Thelargest
difference between thebackground sample
andthe other
samples
is observed for the smallestgrain
sizefractions,
whereas in the 0.25-0.5 mm
fraction,
theFe(lll)-oxide
contents aresimilar in the
sample
from 4-5 m and in the lowersamples (30-35
Figure 2-5
Correlation between ferricoxideconcentrations
Fe(lll)(TiEDTA)
in the sieved samples and their respective specificsurface area, which wascalculated from the radius of the particles and adensity p = 2.6g/cm3.
Fe(lll) (Ti-EDTA) [umo^g]
150
100-
50-
0
4.0-5.0m
(Reference)
J
7.5-8.0 m o 11.3-11.8 m
"
12.5-13.0 m
*-
17.0-17.4 m
.-""
.--ST
°.-""'
oi
0
1x10'5 2x10"5 3x10'5 4x10"5 specific
surface area[m2/g]
Himol/g). Amorphous
ferricoxides,
determinedby
dissolution with ascorbicacid, Felll(AscA),
make up a very small fraction of the ferricoxides, slightly higher
in the referencesample (8-12%)
than in thedeeper samples (< 6%) (data
notshown).Figure
2-3c shows the concentration distribution of the difference betweenFetot
andFelll(TiEDTA).
Nolarge
difference is found for the variousgrain
sizefractions, demonstrating
that thepattern
ofFetot dependence
on thegrain
size in thesamples
below 5 m is dueto the ferric oxides. This is anevidence that most of the
Felll(TiEDTA)
fraction isproduced by
the insitutreatment. Ferrous
iron,
which was measured from the 5M HClextract,
does not accountentirely
for the non-reducible Fefraction,
additional forms of iron arepresent
which are not reducibleby
Ti-EDTA.The
striking pattern
of theFelll(TiEDTA)
distribution amonggrain
sizessuggests
thatprecipitation
of Fe-oxides is related to the availablesurface area. The
specific
surface area(SSA, m2/g)
islarger
for smallparticles
and can be calculated from their radius and thedensity
of theaquifer
sediment(2.6 g/cm3).
InFigure
2-5Felll(TiEDTA)
concentrationsare
plotted
versus the calculatedspecific
surface area and show agood
linearcorrelation. The
straight
line for thesamples
below the referencesample (< 5m)
have ahigher slope
than thestraight
line forthereference. The
origin
is aboutthe same for allsamples including
thereference and amounts to 21-28
umol/g.
In addition to the sieved
samples,
the stones P1 and P20 as well as thesamples
P22 and P24 were measured forFetot, Felll(TiEDTA)
andFelll(AscA).
Thesamples
P1 and P20 are enriched in ferricoxides; they
contain at leastten times more than the sieved
samples.
For P22 andP24,
the Fe-concentrations are similar to the concentrations in thesieved
samples,
but the ferric oxide fraction is moreimportant,
90-100%of the iron dissolved
by
5 M HCl is reducibleby
Ti-EDTA. Insamples P1, P20,
P22 andP24,
the Fe-oxides arecrystalline
to an extent ofover95%.Manganese
In the sieved
samples
reductivereagents
extractedonly
small amounts of manganese,inferring
that most of the manganese(Mntot, Figure 2-4)
is
present
asMn(ll).
Thesamples P1, P20,
P22 and P24 contained twoto three times more
Mntot
than the sievedsamples
and Mn wasmostly
reducible
by
Ti-EDTA(60
to 80% ofMntot).
These are theonly samples containing significant
Mn-oxideconcentrations,
which occurtogether
with the
largest crystalline
Fe-oxide fraction. Theoxygenation
ofmanganese(ll)
is much slower than theoxygenation
ofiron(ll) (Stumm
and
Morgan, 1996).
AtpH
7 and in the absence ofmicroorganisms
theoxygenation
ofMn(ll)
has a half-life time of in the order of years(Diem
and
Stumm, 1984),
and ferric oxides are known to enhance its oxidation(Davies
andMorgan, 1989). Therefore,
the association of Mn-oxides with Fe-oxides is notsurprising
andsuggests
a Fe-oxidecatalyzed
mechanism.
Additional information can be
gained
from sievedsamples by comparing
extraction results for the Mn
fractions, Mntot
andMn(lll,IV)(TiEDTA),
withand without
pretreatment
with acetic acid(for
selective calciteremoval),
in Table 2-1. No
significant
manganese concentrations were foundby
reductive dissolution
(Mn(lll,IV)(TiEDTA).
At least50% of the total manganese of the sievedsamples
is soluble in acetic acid solutionsTable 2-1
Selective chemical extractions with (HAc) and without(A) pretreatmentwith dilute acetic acid
Manganese [|imol/g]
0 HAc 0 HAc
samples Mntot Mnlll,IV(TiEDTA)
P20 19 6 ±2 8 8±1 15 8 ±0 2 7 7 ±0 4
Sieved
<0 063mm
4 0-5 0 3 8 ±0 1 2 5 ±0 1 0 4 ±0 6 0 6 ±0 0 11 3-11 8 6 7±0 1 1 6 ±0 1 0 6 ±0 7 0 9 ±0 2 17 0-17 5 9 2 ±0 2 1 8 ±0 1 0 5 ±0 4 1 1 ±0 0
(HAc).
Thus it islikely
that themostly
bivalent manganese isincorporated
in the calcite matrix or evenpresent
as manganouscarbonate
(rhodocrosite). Solubility
calculations indicate that thesystem
is saturated with
respect
toMnC03 (Kso
=2.5x10"11,
I =0.02,
T =15°C)
under the chemical conditions found in the
ground
water of LaNeuveville with a hardness of5mM
HC03~,
apH
of7.2 and 0 2mg/L Mn(ll).
Theseground
waterparameters
indicate aC02 partial
pressure, which is 50 timeshigher
than theatmospheric partial
pressure The air- saturatedground
water, which isinjected
back intotheaquifer,
has lostits excess of carbon dioxide, which leads to a
higher pH (calculated pH
=8.8)
Therefore itwill be oversaturated withrespect
tothe carbonateminerals
CaC03, MnC03
andFeC03. Hence,
from athermodynamic point
ofview,
rhodocrosite islikely
toprecipitate. Only
insample P20,
the amount of
Mntot remaining
afterpretreatment
with acetic acid isequivalent
to the reducible fraction(Mn(TiEDTA)), indicating
thepresence of