Bacterial contribution to manganese oxidation in a deep coastal sediment

Edenborn, Harry M.; Paquin, Y.; Chateauneuf, G.

doi:10.1016/0272-7714(85)90074-5

Cited by 27 publications

(8 citation statements)

References 22 publications

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“…Treatment of manganese-rich minewater is costly because multiple steps are required, incuding: (i) alkalization to pH >8.5; (ii) aeration to oxidize Mn(II) ions and precipitate MnO 2 ; and (iii) neutralization prior to discharge to the surface water environment. Mn(II) oxidation has been shown to be a primarily microbial process in lakes (Chapnick et al, 1982;Gregory and Staley, 1982;Tipping, 1984), in the suboxic zone of marine basins (Emerson et al, 1982;Tebo, 1991), in hydrothermal vents (Cowen et al, 1986;Mandernack et al, 1993), and in estuarine waters and sediments (Edenborn et al, 1985;Sunda et al, 1987). The accumulation of Mn in a variety of natural environments suggests that biological treatment is an option for the treatment of Mn-rich minewater.…”

Section: Introductionmentioning

confidence: 98%

Removal of Mn(II) ions from aqueous neutral media by manganese‐oxidizing fungus in the presence of carbon fiber

Sasaki

Konno

Endo

et al. 2004

Biotech & Bioengineering

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A manganese-oxidizing fungus was isolated from a hot spring in Japan. The fungus was increasingly effective at oxidizing Mn(II) ions as the concentration of organic carbon sources in the growth medium was decreased. The fungus oxidized 50 ppm of Mn(II) ions within 160 h in a pH 7.3 medium at 25jC. The presence of carbon fiber shortened the time to 80 h, and promoted steady oxidation. The oxidation products were identified by XPS and XRD to be poorly crystallized and amorphous MnO 2 , both with and without the fiber. These results suggest that the fiber participates in kinetically limited oxidation. The fungus was entangled with and clung to the fibers, and the oxidized Mn species accumulated on the fungus. Similarly shaped polyethylene telephthalate fiber did not enhance the oxidation, nor was adhesion of the fungus observed. Although the mechanism is still unknown, the present work shows that removal of Mn from solution through the precipitation and accumulation of Mn-oxides on the fungus in the presence of carbon fiber is a promising improvement for water treatment. B 2004 Wiley Periodicals, Inc.

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Section: Introductionmentioning

confidence: 98%

Removal of Mn(II) ions from aqueous neutral media by manganese‐oxidizing fungus in the presence of carbon fiber

Sasaki

Konno

Endo

et al. 2004

Biotech & Bioengineering

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“…This may explain why the first-order oxidation rate constant we measured is lower than most other first-order rate constants reported for coastal sediments. For example, Edenborn et al (1985), who conducted slurry experiments with sediments from the LSLE, found that the first-order oxidation rate constant for Mn(II) decreased from 50 h 21 to 2.74 h 21 between a sample taken from the top few millimeters of a core and one taken 3 cm below the core top. Concurrent with the lower rate measured at depth was a lower number of viable bacteria and lower concentrations of iron and manganese oxides (Edenborn et al 1985).…”

Section: Discussionmentioning

confidence: 99%

“…For example, Edenborn et al (1985), who conducted slurry experiments with sediments from the LSLE, found that the first-order oxidation rate constant for Mn(II) decreased from 50 h 21 to 2.74 h 21 between a sample taken from the top few millimeters of a core and one taken 3 cm below the core top. Concurrent with the lower rate measured at depth was a lower number of viable bacteria and lower concentrations of iron and manganese oxides (Edenborn et al 1985). The first-order oxidation rate constant we measured, 0.02 h 21 , is about two orders of magnitude smaller than the value (2.74 h 21 ) they obtained with sediment taken 3 cm below the sediment-water interface.…”

Section: Discussionmentioning

confidence: 99%

“…Several studies have examined the kinetics of manganese oxidation in sediments (Edenborn et al 1985;Canfield et al 1993;Thamdrup et al 1994a). Homogeneous oxidation of Mn(II) by O 2 is extremely slow (10 7 times slower than oxidation of Fe(II) at pH 8 and 25uC; Morgan 2000), but the presence of MnO 2 and other mineral surfaces in natural sediments, such as c-FeOOH, a-FeOOH, SiO 2 , Al 2 O 3 , or calcite catalyzes Mn(II) oxidation (Sung and Morgan 1981;Davies and Morgan 1989;A.…”

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confidence: 99%

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Kinetics of manganese adsorption, desorption, and oxidation in coastal marine sediments

Richard

Sundby

Mucci

2013

Limnology & Oceanography

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Ejection of excavated manganese (Mn)-laden particles from anoxic subsurface sediment onto an oxic sediment-water interface by infauna and by other physical disturbances triggers desorption and oxidation of reduced manganese species. These competing reactions determine whether adsorbed Mn(II) will be desorbed and escape into the water column or be oxidized to Mn(IV) and retained as an insoluble component of the sediment. Consequently, the net flux of Mn(II) to the water column depends on the relative rates of the two reactions. We determined the rates of Mn(II) adsorption, desorption, and oxidation by incubating slurries of natural anoxic sediment at 25uC and monitoring the concentration of manganese in the aqueous phase of the slurry. The kinetics of adsorption, desorption, and oxidation were fitted to first-order rate laws. The first-order rate constants for adsorption (k' ads 5 7.0 6 3.4 h 21 ) and desorption (k' des 5 12.7 6 3.3 h 21 ) are more than two orders of magnitude greater than the first-order rate constant for oxidation (k' ox 5 0.020 6 0.006 h 21 ). The combination of rapid desorption kinetics and slow oxidation kinetics allows dissolved manganese to be dispersed into the bottom water by turbulent diffusion and escape local reoxidation and retention at the sediment-water interface. Thus, advection of anoxic sediment to the sediment-water interface contributes to the overall flux of manganese from the sediment to the water column.

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“…Consequently, HgCl, can be added to seawater or pore waters from a concentrated stock solution (e.g. 0.1 M HgCl,) to inhibit bacterial activity in preserved samples (Edenborn et al 1985). The Hg2+ which would normally interfere with the titration is removed by the ion exchange resin.…”

Section: Acknowledgmentsmentioning

confidence: 99%

A potentiometric back‐titration method for determining sulfate in seawater and marine pore waters

Mucci

1991

Limnology & Oceanography

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Sulfate concentrations can be determined accurately by potentiometric back‐titration of excess Ba2+ with a mercury electrode following precipitation of BaSO4. The filtered seawater solution is eluted through a cation exchange column and the eluate reacted with excess BaCl2. The BaSO4 precipitate is removed by filtration and the solution titrated potentiometrically with EGTA. The method applies over a wide range of salinities and in the presence of 0.001 M HgCl2 which is used to inhibit bacterial activity during preservation. The oxidation of sulfides may interfere, but several remedial procedures can be adopted. The potentiometric titration and endpoint determination can be automated easily. The method determines the SO42− concentration in 1 ml or less of seawater with a SD of <0.6% (28.26±0.16 mmol kg−1 seawater, n = 28).

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Bacterial contribution to manganese oxidation in a deep coastal sediment

Cited by 27 publications

References 22 publications

Removal of Mn(II) ions from aqueous neutral media by manganese‐oxidizing fungus in the presence of carbon fiber

Removal of Mn(II) ions from aqueous neutral media by manganese‐oxidizing fungus in the presence of carbon fiber

Kinetics of manganese adsorption, desorption, and oxidation in coastal marine sediments

A potentiometric back‐titration method for determining sulfate in seawater and marine pore waters

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