<原報>銅イオン選択性電極を用いる混合試料溶液中の銅イオンの定量 : 電位差測定法と電位差滴定法の比較
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概要
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Cupric ion in 0.01 M acetate buffer can be determined by the measurement of electromotive force between Orion cupric ion electrode and Razaran calomel reference electrode. The response of the electrode is linear over the concentration ranges from (10)^<-1> to (10)^<-5> M and an Nernstian slope of 29 mV per concentration decade at 25.0℃ (Table I, Fig.1). The influence of the coexisting cations are represented in Table II, Table III and Fig. 2. It may be said that (10)^<-1> to (10)^<-5> M cupric ion can be determined even if equimolar Mg (II), Ca (II), Sr (II), Ba (II), Al (III), Mn (II), Co (II), Ni (II), Zn (II) and Pb (II) ions are coexisted, but Cr (III) considerablly disturbs the determination of cupric ion. 50 μ mole of cupric ion in the 0.1 M acetate buffer at about pH 5.5 can be titrated potentiometrically usiug Orion cupric ion electrode as indicator with 0.025 M EDTA. The effects of equimolar coexisting Mg (II), Ca (II), Sr (II) and Ba (II) ions to the determination of cupric ion are neglegible, but Al (III), Mn (II) and Cr (III) ions disturb the titration, and Co (II), Ni (II), Zn (II) and Pb (II) are titrated simultaneously with cupric ion. (Table IV and V) It appears that in the buffer of pH 3.5,the influence of Mn (II) or Al (III), and of pH 4.0,the affect of Cr (III) would be both neglected to the titration of cupric ion. (Table VI) It may be concluded that the electromotive force measurement method is more adventageous than the potentiometric titration method for the determination of cupric ion, but the latter method is more favarable than the former, when Cr (III) is present in the sample.
- 共立薬科大学の論文
- 1975-02-25
共立薬科大学 | 論文
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