Kazuyoshi Takiyama

Analysis of metal chelates—III: Simultaneous determination by a.c. polarography of copper and nickel in copper-contaminated nickel dimethylglyoximate

Abstract A small amount of copper coprecipitates when nickel dimethylglyoximate is precipitated in the presence of copper. The simultaneous determination of this small amount of copper with the large amount of nickel has been carried out by a.c. polarography.

アルカリ土類炭酸塩の電子顕微鏡的研究(第1～2報)(第1報)炭酸ガス法による生成反応

S call U-effect I. In the case of glass-liquid interface we call it U-effect I, and in the case of mercury-solution interfaces U-effect II. The former is an effect of a.c. streaming potential generation and the latter is attributed to the periodical charging and discharging current of the interfacial double layer capacity. U-effect is applicable to all sorts of mechano-electric transducers, and it was proved that the apparatuses applying it were equally matched to those of Rochelle salt. Moreover, with regard to resistance against humidity and temperature change or easiness of fabrication, which Rochelle salt lacked, our device was superior. U-effect I can be used to measure streaming potentials by a.c. technique, which will provide more conventional method of its measurement by farther improvement. Counter U-effect can be observed by interchanging the input and output terminals of the elements. This gives an electroacoustical transducer, although the efficiency is very small. Electron Microscopic Studies on Alkaline Earth Carbonates. (I) Formation by Carbonic Acid Gas Method Eiji SUITO, Kazuyoshi TAKIYAMA and Makoto TAKAHASHI (Suit() Laboratory) Journal of the Chemical Society of Japan, Pure Chemistry Section (Nippon Kagahu Zasshi), 78, 1732 (1957) Calcium, strontium, and barium carbonates were prepared by introducing bubbles carbon dioxide gas into their hydroxide solutions or suspensions. Mixed carbonates were also prepared from the mixture of the hydroxides. The pH of the reaction mixture was about 12.5 at the outset and was almost constant during the course of the reaction and decreased rapidly directly before the end of the reaction. The rate of the formation reaction of barium carbonate was measured by titration and the reaction seemed to be nearly zero-order. Generally speaking, the reaction velocity was independent of the concentration of hydroxide and decreased with decreasing concentration of carbon dioxide gas. The reaction velocity was minimum at about 30C. When the reaction mixture was suspension before the reaction, the reaction velocity was dependent on the dissolution velocity of hydroxide and decreased with increasing content of calcium hydroxide. Formation of calcium carbonate in the presence of strontium or barium hydroxide occurred after that of strontium carbonate or barium carbonate.