GEOCHEMICAL JOURNAL
Online ISSN : 1880-5973
Print ISSN : 0016-7002
ISSN-L : 0016-7002
Volume 1, Issue 1
Displaying 1-5 of 5 articles from this issue
  • Yasushi Kitano, Nobuko Kanamori
    1966 Volume 1 Issue 1 Pages 1-10
    Published: 1966
    Released on J-STAGE: April 08, 2008
    JOURNAL FREE ACCESS
    As one of the steps that lead to an understanding of the secretion of magnesian calcite in skeletal parts of marine organisms, the laboratory synthesis of the mineral from aqueous solutions was carried out at low temperatures and pressures. The conditions of the laboratory synthesis of magnesian calcites are shown in this paper. Magnesian calcites are precipitated from calcium bicarbonate solutions containing magnesium ions and certain organic materials such as organic acids, which are found in the body fluids of carbonate-secreting organisms, in various concentrations.
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  • Akimasa Masuda
    1966 Volume 1 Issue 1 Pages 11-26
    Published: 1966
    Released on J-STAGE: April 08, 2008
    JOURNAL FREE ACCESS
    The lanthanides, La, Ce, Nd, Sm, Eu, Gd, Dy, Er and Yb were determined quantitatively for six basalts of Japan by the use of isotope dilution method. It is suggested that the high-alumina olivine basalt was a primary liquid-type material, the primary tholeiite was a primary solid-type material, and the alkali olivine basalt which was supposed to be primary was a secondary liquid-type material. This observation is in agreement with the consequence from the analysis of the relationship between thorium and uranium concentrations. The original depths for the aforementioned three magmas were estimated to be 200, 150 and 220 km, respectively, from the relative enrichment of lanthanides. A genetically close connection was corroborated for tholeiite and high-alumina basalt.
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  • Masako Shima, Masatake Honda
    1966 Volume 1 Issue 1 Pages 27-34
    Published: 1966
    Released on J-STAGE: April 08, 2008
    JOURNAL FREE ACCESS
    Distribution of lithium in several chondrites was examined by a fractional dissolution method. Water, bromine water, HCl, and HF were used to fractionally dissolve minerals comprising non-magnetic fractions of chondrites. From ordinary chondrites most of the lithium was extracted into HCl solutions. Although olivine was also decomposed with HCI, the degree of extraction of magnesium from olivine was different from that of lithium. In the case of Abee, an enstatite chondrite, bromine water extracted a major portion of lithium along with troilite. Other alkali metals remained in the acid insoluble silicates. These results indicate that lithium is located in a minor segregated constituent in stone meteorites. The isotopic compositions of lithium in the various fractions were found to be essentially identical to that of terrestrial lithium.
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  • Hitoshi Sakai, Masahiro Yamamoto
    1966 Volume 1 Issue 1 Pages 35-42
    Published: 1966
    Released on J-STAGE: April 08, 2008
    JOURNAL FREE ACCESS
    It is definitely shown that the main cause of error encountered in the precision isotope analysis of sulfur is in the isotope exchange reaction between SO2 and SO3 during the combustion process of SO2 preparation. The isotope fractionation factor between the two oxides is estimated to be 1.0035 at 1200°C. From this value, it is predicted that 3% fluctuation in the yield of SO2 would introduce uncertainty of 0.1‰ in the results of the ratio measurement. An improved combustion technique to maintain a constant yield of SO2 is described where pure oxygen is replaced by a nitroden-oxygen mixture (15: 1, v/v).
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  • Shinya Oana, Hitomi Ishikawa
    1966 Volume 1 Issue 1 Pages 45-50
    Published: 1966
    Released on J-STAGE: April 08, 2008
    JOURNAL FREE ACCESS
    Sulfur and sulfur compounds involved in the chemical reaction, 3H2SO3= 2H2SO4+S+H2O in the temperature range from 150 to 300°C have been quantitatively determined. After the disproportionation reaction of sulfurous acid is completed, sulfur decreases according to the chemical reaction, 4S+4H2O = 3H2S+H2SO4. These two reactions may be responsible for the production of sulfuric acid in hot spring water. 34S is enriched in sulfuric acid and depleted in sulfur revealing 16.1 to 21.1‰ fractionation between them. This would account for the enrichment of 34S in sulfuric acid encountered in hot spring water.
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