On the Formation of Complex Ions Applied in Analytical Chemistry. VIII : Studies on Complexbilities of Ferric Compounds by the Use of Radioisotope Element

Applying the ion exchange method reported by J. Schubert, the complexbilities of ferric tartrate, citrate and malonate were measured by the use of the radioisotope element of Fe^ and the ion exchange resin of Amberlite 1R-120. The hydrogen ion concentrations of the solution were measured by the use of the quinhydrone electrode. All the measurements were made at 25℃ and the following results were obtained : ferric tartrate, K=3.1×10^ citrate, K=2.2×10^ ; malonate, K=2.5×10^

On the Formation of Complex Ions Applied in Analytical Chemistry. IV : Studies on Complexes of Lead and Cadmium Citrates

Complexbilities of various ions applied in chemical analysis, had been measured and reported in the previous papers. In the present study, the complexbilities of lead and cadmium citrates were measured by the usual potentiometric compensation method, using an ion concentration cell, a quinhydrone electrode and a hydrogen electrode. The following results were obtained at 25℃ : lead citrate, K=7.81×10^ ; cadmium citrate, K=5.70×10^

On the Formation of Complex Ions Applied in Analytical Chemistry. V : Studies on Complexes of Copper and Zinc Malonates

Complexbilities of various ions applied to chemical analysis have been measured and the results were reported in the previous papers. In the present research, the measurements of the complexbilities of copper and zinc malonates were made by the usual potentiometric compensation method, using the ion concentration cell and quinhydrone electrode and the following results were obtained : copper malonate, K=5.22×10^ ; zinc malonate, K=1.21×10^

On the Formation of Complex Ions Applied in Analytical Chemistry. III : Studies on Complexes of Copper and Zinc Citrates

From the standpoint of analytical chemistry, complexbilities of various ions applied to chemical analysis have been measured. In the present study, the complexbilities of copper and zinc citrates were measured by usual potentiometric compensation method, using the ion concentration cell and hydrogen electrode. The following results were obtained at 25℃ : copper citrate : K=3.37×10^ ; zinc citrate : K=2.19×10^

On the Formation of Complex Ions Applied in Analytical Chemistry. X : Studies on Complexbilities of Cobalt Compounds by the Use of Radioisotope Element

Using the radioisotope element of Co^ and the cation exchange resin Amberlite 1R-120, the complexbilities of cobalt tartrate, citrate and malonate were measured, and the following results were obtained : tartrate, K=2.5×10^ ; citrate, K=1.4×10 ; malonate, K=3.5×10^

On the Formation of Complex Ions Applied in Analytical Chemistry. VII : Studies on Complexes of Silver Citrate and Lead Acetate

Complexbilities of various ions applied to chemical analysis have been investigated. In the present experiment, the complexbilities of silver citrate and lead. acetate were measured by the usual potentiometric compensation method, using the ion concentration cell and quinhydrone electrode. The following results were obtained at 25℃ : for silver citrate K=1.14×10^ and for lead acetate K=1.45×10

On the Formation of Complex Ions Applied in Analytical Chemistry. I : Studies on Complexes of Copper and Zinc Tartarates

In this report, the measurements of the complexbilities of copper and zinc tartarates were made by the usual potentiometric compensation method, using the ion concentration cell and hydrogen electrode. The following results were obtained : copper tartarate : K=9.32×10^, zinc tartarate : K=4.44×10^<-4

The Chemistry of Protactinium. II : The Behavior of Pentavalent Protactinium in a Perchloric Acid Solution

Studies of the chemical behavior of protactinium (V) were carried out with the TTA-benzene extraction method, the ion exchange method and the filtration method. When the protactinium concentration is less than 10^M and the perchloric acid concentration is 0.3-2.0N, the reaction of TTA extraction may proceed as : PaO_m(OH)_n^+4HT⇄Pa(OH)T_4+(m+n-1)H_2O+(5-2m-n)H^+ where 2m+n is 3 and 4, or as : PaO_m(OH)_nT^+4HT⇄PaT_5+(m+n)H_2O+(4-2m-n)H^+ where 2m+n is 2 and 3. The cation exchange experiment gives results consistent with this conclusion. On the other hand, when the concentration of protactinium is higher than 10^M, the above relation does not hold, even in the 5N perchloric acid solution, because protactinium forms the aggregates to a great extent. This has been confirmed by the filtration experiment