Japan Geoscience Union Meeting 2014

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Oral

Symbol S (Solid Earth Sciences) » S-MP Mineralogy & Petrology

[S-MP49_1PM2] Nano-Analyses of Natures and Origins of Earth and Planetary Solids

Thu. May 1, 2014 4:15 PM - 5:45 PM 314 (3F)

Convener:*Yohey Suzuki(Graduate School of Science, The University of Tokyo), Takashi Murakami(Department of Earth and Planetary Science, Graduate School of Science, University of Tokyo), Katsuhiro Tsukimura(National Institute of Advanced Industrial Science and Technology), Masaya Suzuki(AIST, Geological Survey of Japan), Tadashi Yokoyama(Department of Earth and Space Science, Graduate School of Science, Osaka University), Keisuke Fukushi(Institute of Nature & Environmental Technology, Kanazawa University), Satoshi Mitsunobu(University of Shizuoka, Institute for Environmental Sciences), Chair:Keisuke Fukushi(Institute of Nature & Environmental Technology, Kanazawa University), Tadashi Yokoyama(Department of Earth and Space Science, Graduate School of Science, Osaka University)

5:30 PM - 5:45 PM

[SMP49-P01_PG] Formation rate of iron colloids at pH 2-3

3-min talk in an oral session

*Sagakuni NAGASAKI1, Tadashi YOKOYAMA2, Osamu HISATOMI2, Satoru NAKASHIMA2 (1.Department of physics , Osaka University, 2.Department of Earth and Space Science, Graduate School of Science, Osaka University)

Keywords:鉄コロイド, 反応速度論, 動的光散乱法

Various types of iron colloids are widely distributed in the earth's surface conditions, and their formation process, adsorption characteristic, and the material transport mediated by iron colloids are receiving attention. Iron colloids are often formed through several reactions including the dissolution of Fe2+ and Fe3+ from minerals, oxidation from Fe2+ to Fe3+, hydrolysis, and crystallization. In the present study, the reaction rate was evaluated focusing on the process in which iron colloids are formed from dissolved Fe3+.A solution of Fe3+ 100 ppm was prepared by dissolving FeCl3 into pure water. This solution was reacted at 15, 25, 35, 45, and 55 ℃. At 25 ℃, pH of the solution was 〜2.7 at the start of the reaction and decreased to 〜2.2 as reaction time passed. Such change in pH is known to occur as a result of the following reactions: hydration of Fe3+ (release of H+) → formation of dissolved Fe(OH)3 → formation of solid Fe(OH)3 (Grundl and Delwiche, 1993). Therefore, information of the formation rate of iron colloids can be obtained by monitoring the pH of the solution. After the initial period of the reaction in which the rate of the decrease of dissolved Fe(OH)3 concentration was slow presumably due to nucleation, the concentration of dissolved Fe(OH)3 decreased in a manner like first-order reaction, and the reaction behavior deviated from the first-order reaction at the later stage. By assuming first-order reaction, rate constants of 3.3E-5 - 1.1E-2 s-1 were obtained at 15-55 ℃, and good linearity was confirmed in an Arrhenius plot of these rate constants. In addition to the above experiments in which time variation of the total amount of solid is considered, the time variation of the grain size of iron colloids was evaluated. A solution of Fe3+ 100 ppm was prepared and the change of grain size at 25 ℃ was continuously measured using a dynamic light scattering apparatus (Zetasizer μV, Malvern). As a result, enough scattering intensity began to be detected after the mean diameter of iron colloids grew to 10 nm, then the grain size increased. The increase of the grain size almost stopped after 8 hours, and mean diameter at this stage was approximately 30–40 nm. By evaluating the number of grains from the total amount of solid and mean grain size, the grain number was estimated to decrease with time.