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Equilibrium constant for calcium ion and ascorbate ion.

C S Tsao

    Experientia
    |February 15, 1984
    PubMed
    Summary
    This summary is machine-generated.

    Calcium and ascorbic acid form complexes in water. Researchers measured the equilibrium constant for this calcium-ascorbate complexation, finding it to be 2.1 M-1 at 25°C.

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    Area of Science:

    • Chemistry
    • Biochemistry
    • Physical Chemistry

    Background:

    • Calcium ions (Ca++) are essential in biological systems.
    • Ascorbic acid (Vitamin C) is a vital antioxidant.
    • Understanding their interactions is crucial for various applications.

    Purpose of the Study:

    • To investigate the complex formation between calcium ions and ascorbate ions in aqueous solution.
    • To quantify the equilibrium constant for this interaction.

    Main Methods:

    • Titration method used to measure free calcium ion concentration.
    • Controlled addition of ascorbate to calcium solutions at 25°C.
    • Determination of equilibrium constant at ionic strength (μ) of 0.1–0.2 M.

    Main Results:

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    • Complex formation between Ca++ and ascorbate ion was confirmed.
    • The equilibrium constant for the Ca++ and singly-charged ascorbate ion was determined to be 2.1 M⁻¹.
    • High precision (<5%) and accuracy (<20%) achieved for the equilibrium constant.

    Conclusions:

    • Calcium and ascorbate form stable complexes in solution.
    • The quantified equilibrium constant provides valuable data for chemical and biological modeling.
    • Further applications of these equilibrium constants are discussed.