Chelating agents as metal buffers in biological systems. I. Principles and use of ethylenediaminetetraacetic acid

Chaberek, S.; Bersworth, F. C.; Martell, Arthur E.

doi:10.1016/0003-9861(55)90415-x

Cited by 15 publications

(9 citation statements)

References 2 publications

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“…Fibres in a somewhat 'run down' state had smaller currents than fibres in a 'good condition'. The calcium-binding power of the EDTA is much greater than that of the citrate; the concentrations of unbound Ca in the EDTA and in the citrate solutions are about 10-10 M and 10-6M respectively, as calculated from the equations and constants given by Hastings, McLean, Eichel-berger, Hall & da Costa (1934), Schwarzenbach & Ackermann (1948 and Chaberek, Bersworth & Martell (1955), assuming 0-02-0-1 mm calcium contaminations in an ordinary 'Ca-free' Ringer's solution (see Frankenhaeuser, 1957). On the basis of this and the findings in the previous experiments it would be expected thatfibresin 'good condition,' also, would be completely inactivated at normal resting potential in the EDTA solution.…”

Section: Resultsmentioning

confidence: 99%

The effect of magnesium and calcium on the frog myelinated nerve fibre

Frankenhaeuser¹,

Meves²

1958

The Journal of Physiology

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Section: Resultsmentioning

confidence: 99%

The effect of magnesium and calcium on the frog myelinated nerve fibre

Frankenhaeuser¹,

Meves²

1958

The Journal of Physiology

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“…These calculations were conducted according to the method described by Chaberek et al (1954), in which only Fe 3+ and H 1 " concentrations and the Fe 3+ -chelate formation and H* association constants (at ja = 0.1 M) are used in the calculation. The equation (for HEED) is: pFe = log Kj-ßL -log alpha + log (free HBED/FeHBED) or, for 10 % chelator excess: pFe = 39.68 -log alpha -1.0 where alpha = loi 12 -46 " P») + io( 23 -46 -2*pH) + 10 (31.78 -3*pH) +10 (36.42 -4*pH) + !…”

Section: Methods and Materiaismentioning

confidence: 99%

“…and FeHBED in sinple aqueous solution (chelator = 11 pM, Fe 3+ = 10 ¿iM, u = 0.1). Calculations were conducted according to Chaberek et al (1954) using stability constants from Lindsay (1979) (see Table 2). The line for Fe(CH) 3 solubility is shown for ccnparison.…”

Section: Sourcementioning

confidence: 99%

Plants can utilize iron form Fe‐N,N'‐di‐(2‐hydroxybenzoyl)‐ethylenediamine‐N,N'‐diacetic acid, a ferric chelate with 10⁶greater formation constant than Fe‐EDDHA.

Chaney

1988

Journal of Plant Nutrition

105

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“…The physical chemistry of metal-EDT A equilibria has been examined by several workers (Chaberek, Bersworth & Martell, 1955;Raaflaub, 1956) and methods for calculating the concentrations of free metal ion at equilibrium outlined. These treatments, however, are limited to simple cases when only one chelating metal ion is present.…”

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The Chemistry of ethylenediamine Tetra-Acetic acid in sea water

Spencer

1958

J. Mar. Biol. Ass.

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(Text-figs. 1-10) 127 In recent years, ethylenediamine tetra-acetic acid (EDT A) has been extensively used in culture media for unicellular algae. This, and other chelating agents are also becoming widely used in toxicity studies with plants and animals, in analysis and for controlling the ionic concentration of certain metal ions in a wide variety of studies.EDT A forms complexes with a large number of metallic cations, and in the presence of sufficient EDT A only very small amounts of many metals can exist as free ions. The use of EDT A as a metal buffer system has been advocated by numerous workers. These metal buffer systems depend for their operation upon the equilibrium between the metal cations, the EDT A and the chelate. Providing that the concentrations of the chelate and the che1ating ion are large compared with that of the free metal ion, such a system will tend to maintain a constant concentration of metallic ions, should these be continuously removed by a biological system.The available data suggest that EDT A is not readily metabolized by most forms of life, and moreover it does not appear to be markedly toxic except by virtue of its meta1-che1ating reactions. Its use under the correct conditions for controlling metal ion concentrations in biological systems therefore has much to commend it.The physical chemistry of metal-EDT A equilibria has been examined by several workers (Chaberek, Bersworth & Martell, 1955;Raaflaub, 1956) and methods for calculating the concentrations of free metal ion at equilibrium outlined. These treatments, however, are limited to simple cases when only one chelating metal ion is present. The biologist is inevitably faced with working with systems containing many reacting metal ions (e.g. in sea water). Data regarding the free metal ion concentrations existing in equilibrium with EDT A in such systems is of obvious importance if the use of EDT A is to be fully exploited. This paper records some data on the equilibria set up when EDT A is added to sea water and on the effect of variations of certain controlling factors.

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Chelating agents as metal buffers in biological systems. I. Principles and use of ethylenediaminetetraacetic acid

Cited by 15 publications

References 2 publications

The effect of magnesium and calcium on the frog myelinated nerve fibre

The effect of magnesium and calcium on the frog myelinated nerve fibre

Plants can utilize iron form Fe‐N,N'‐di‐(2‐hydroxybenzoyl)‐ethylenediamine‐N,N'‐diacetic acid, a ferric chelate with 10⁶greater formation constant than Fe‐EDDHA.

The Chemistry of ethylenediamine Tetra-Acetic acid in sea water

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Chelating agents as metal buffers in biological systems. I. Principles and use of ethylenediaminetetraacetic acid

Cited by 15 publications

References 2 publications

The effect of magnesium and calcium on the frog myelinated nerve fibre

The effect of magnesium and calcium on the frog myelinated nerve fibre

Plants can utilize iron form Fe‐N,N'‐di‐(2‐hydroxybenzoyl)‐ethylenediamine‐N,N'‐diacetic acid, a ferric chelate with 106greater formation constant than Fe‐EDDHA.

The Chemistry of ethylenediamine Tetra-Acetic acid in sea water

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Plants can utilize iron form Fe‐N,N'‐di‐(2‐hydroxybenzoyl)‐ethylenediamine‐N,N'‐diacetic acid, a ferric chelate with 10⁶greater formation constant than Fe‐EDDHA.