Solubility of Carbon Dioxide in Natural Systems

Salminen, Justin; Kobylin, Petri; Ojala, Anne

doi:10.1016/b978-044452707-3/50012-4

Cited by 3 publications

(9 citation statements)

References 11 publications

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“…release of Ag + ions agrees with that under laboratory air (580 ppm, open symbols) indicating that acidification by CO 2 absorption25 plays a dominant role on metallic Ag dissolution in DI water. For all nanosilver sizes, the Ag mass fraction as Ag + ions increases with increasing CO 2 concentration.…”

supporting

confidence: 78%

“…On the other hand, under CO 2 -containing laboratory air (Figure 5b, open symbols), the pH of all nanosilver suspensions continuously decreases for 4 days, reaching a nearly steady state after 7 days. The pH of DI water (diamonds) reaches a true steady state after 4 days as the dissolved CO 2 attains its solubility limit 25 in water with pH ∼ 5.8. The pH evolution of the nanosilver suspensions is analogous to that of DI water, indicating that CO 2 absorption from air dominates 25 the change of the pH.…”

Section: ■ Materials and Methodsmentioning

confidence: 99%

“…The pH of DI water (diamonds) reaches a true steady state after 4 days as the dissolved CO 2 attains its solubility limit 25 in water with pH ∼ 5.8. The pH evolution of the nanosilver suspensions is analogous to that of DI water, indicating that CO 2 absorption from air dominates 25 the change of the pH. After 7 days exposed to laboratory air, the pH of all nanosilver suspensions is about 6.5.…”

Section: ■ Materials and Methodsmentioning

confidence: 99%

“…On the other hand, metallic Ag (without surface Ag 2 O) continuously dissolves for prolonged (>100 h) water exposure to ambient air. , Although metallic Ag dissolution consumes protons, the pH of the solution exposed to ambient air was constant because of CO 2 absorption . Therefore, the acidification of nanosilver suspensions by ambient CO 2 absorption could affect metallic Ag dissolution and needs to be better understood. This is important both for the prolonged performance of nanosilver products as well as their long-term environmental impact.…”

Section: Introductionmentioning

confidence: 99%

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Enhanced Ag⁺ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO₂

2015

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Nanosilver with closely controlled average particle diameter (7-30 nm) immobilized on nanosilica is prepared and characterized by X-ray diffraction, N2 adsorption, and transmission electron microscopy. The presence of Ag2O on the as-prepared nanosilver surface is confirmed by UV-vis spectroscopy and quantified by thermogravimetric analysis and mass spectrometry. The release of Ag(+) ions in deionized water is monitored electrochemically and traced quantitatively to the dissolution of a preexisting Ag2O monolayer on the nanosilver surface. During this dissolution, the pH of the host solution rapidly increases, suppressing dissolution of the remaining metallic Ag. When, however, a nanosilver suspension is exposed to a CO2-containing atmosphere, like ambient air during its storage or usage, then CO2 is absorbed by the host solution decreasing its pH and contributing to metallic Ag dissolution and further leaching of Ag(+) ions. So the release of Ag(+) ions from the above closely sized nanosilver solutions in the absence and presence of CO2 as well as under synthetic air containing 200-1800 ppm of CO2 is investigated along with the solution pH and related to the antibacterial activity of nanosilver.

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supporting

confidence: 78%

Section: ■ Materials and Methodsmentioning

confidence: 99%

Section: ■ Materials and Methodsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

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Enhanced Ag⁺ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO₂

2015

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“…Assuming that pH in Lake Valkea-Kotinen fluctuates in the same range the vast majority of inorganic carbon is always in form of CO 2 , and thus, changes in CO 2 equal changes in DIC (cf. Davies et al 2003;Hanson et al 2003;Salminen et al 2007). Thus, our data strongly suggests that the evaluated probes in connection with the constructed measuring system are well suited for high frequency CO 2 monitoring in aquatic environments with soft water.…”

Section: Discussion Comments and Recommendationsmentioning

confidence: 99%

High‐frequency measurements of productivity of planktonic algae using rugged nondispersive infrared carbon dioxide probes

Hari

Pumpanen

Huotari

et al. 2008

Limnology & Ocean Methods

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We have constructed a system based on commercially available inexpensive NDIR CO 2 sensors to continuously monitor CO 2 concentrations in water bodies. Here we demonstrate its use in a boreal humic lake. With the system, we collect high frequency data with a 10-min time resolution for determination of CO 2 consumption and production. We use and modify the computational methods commonly used in forest ecology to enable characterization of aquatic primary production. To demonstrate the advantages of the method, we present the results against the observations from the long-term monitoring program applying traditional bottle methods. With the probes, we can detect a clear, photosynthesis-driven daily pattern in the CO 2 concentration and determine the CO 2 consumption or production resulting in more than a 10-fold improvement in the time resolution when compared with traditional incubation methods. The measuring frequency is high enough to determine the dependence of photosynthesis on irradiance. The high-frequency data highlights the inherent problems of discrete bottle incubations and bring into question their reliability. Our free water approach yielded productivity and mineralization rates that were clearly higher than obtained with incubations.

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Extreme Carbon Dioxide Concentrations in Acidic Pit Lakes Provoked by Water/Rock Interaction

España

Boehrer

Yusta

2014

Environ. Sci. Technol.

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We quantify the gas pressure and concentration of a gas-charged acidic pit lake in SW Spain. We measured total dissolved gas pressure, carbon dioxide (CO2) concentration, major ion concentration, isotopic composition of dissolved inorganic carbon (δ(13)C(DIC)), and other physicochemical parameters. CO2 is the dominant dissolved gas in this lake and results mainly from carbonate dissolution during the interaction of acidic water with wall rocks, followed by diffusive and advective transport through the water column. The δ(13)C(DIC) values suggest that the biological contribution is comparatively small. Maximum CO2 concentrations higher than 0.1 M (∼5000 mg/L) have been measured, which are only comparable to those found in volcanic crater lakes. The corresponding gas pressures of CO2 alone (pCO2 ∼3.6 bar) imply 60% saturation relative to local pressure at 50 m depth. High CO2 concentrations have been observed in other pit lakes of the region. We recommend gas-specific monitoring in acidic pit lakes and, if necessary, the design of feasible degassing strategies.

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Solubility of Carbon Dioxide in Natural Systems

Cited by 3 publications

References 11 publications

Enhanced Ag⁺ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO₂

Enhanced Ag⁺ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO₂

High‐frequency measurements of productivity of planktonic algae using rugged nondispersive infrared carbon dioxide probes

Extreme Carbon Dioxide Concentrations in Acidic Pit Lakes Provoked by Water/Rock Interaction

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Solubility of Carbon Dioxide in Natural Systems

Cited by 3 publications

References 11 publications

Enhanced Ag+ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO2

Enhanced Ag+ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO2

High‐frequency measurements of productivity of planktonic algae using rugged nondispersive infrared carbon dioxide probes

Extreme Carbon Dioxide Concentrations in Acidic Pit Lakes Provoked by Water/Rock Interaction

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Enhanced Ag⁺ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO₂

Enhanced Ag⁺ Ion Release from Aqueous Nanosilver Suspensions by Absorption of Ambient CO₂