The relation between composition and conductivity in solutions of meta- and orthophosphoric acids

E B R Prideaux

    Research output: Contribution to journalArticle

    Abstract

    When P2O5 is thrown into excess of water at room temperature, about 75 per cent. of the total dissolved acid is HPO3 and the rest H3PO4. There is no evidence of the formation of H4P2O7. This HPO3 exists as complex and simple molecules, and the proportions of the two may vary widely from one solution to another of the same total concentration. Two changes then take place, a depolymerisation of the (HPO3)n and a hydration of HPO3, of which the former is probably the quickest. The latter change (hydration) does not, as in the reaction studied by Sabatier, follow exactly the same exponential law until all the acid is changed. The two changes are seen most clearly in the G, K curves, Fig. 3, and from these it also appears that the conductivity of HPO3 is considerably greater than that of H3PO4.

    LanguageEnglish
    Pages37-44
    Number of pages8
    JournalTransactions of the Faraday Society
    Volume5
    Issue numberSEPTEMBER
    Publication statusPublished - 1909

    Fingerprint

    hydration
    conductivity
    acid
    temperature
    water

    Cite this

    @article{7d89a0f502294ed48ccb26549240673a,
    title = "The relation between composition and conductivity in solutions of meta- and orthophosphoric acids",
    abstract = "When P2O5 is thrown into excess of water at room temperature, about 75 per cent. of the total dissolved acid is HPO3 and the rest H3PO4. There is no evidence of the formation of H4P2O7. This HPO3 exists as complex and simple molecules, and the proportions of the two may vary widely from one solution to another of the same total concentration. Two changes then take place, a depolymerisation of the (HPO3)n and a hydration of HPO3, of which the former is probably the quickest. The latter change (hydration) does not, as in the reaction studied by Sabatier, follow exactly the same exponential law until all the acid is changed. The two changes are seen most clearly in the G, K curves, Fig. 3, and from these it also appears that the conductivity of HPO3 is considerably greater than that of H3PO4.",
    author = "Prideaux, {E B R}",
    year = "1909",
    language = "English",
    volume = "5",
    pages = "37--44",
    journal = "Transactions of the Faraday Society",
    issn = "0014-7672",
    publisher = "Faraday Division of the Chemical Society",
    number = "SEPTEMBER",

    }

    The relation between composition and conductivity in solutions of meta- and orthophosphoric acids. / Prideaux, E B R.

    In: Transactions of the Faraday Society, Vol. 5, No. SEPTEMBER, 1909, p. 37-44.

    Research output: Contribution to journalArticle

    TY - JOUR

    T1 - The relation between composition and conductivity in solutions of meta- and orthophosphoric acids

    AU - Prideaux, E B R

    PY - 1909

    Y1 - 1909

    N2 - When P2O5 is thrown into excess of water at room temperature, about 75 per cent. of the total dissolved acid is HPO3 and the rest H3PO4. There is no evidence of the formation of H4P2O7. This HPO3 exists as complex and simple molecules, and the proportions of the two may vary widely from one solution to another of the same total concentration. Two changes then take place, a depolymerisation of the (HPO3)n and a hydration of HPO3, of which the former is probably the quickest. The latter change (hydration) does not, as in the reaction studied by Sabatier, follow exactly the same exponential law until all the acid is changed. The two changes are seen most clearly in the G, K curves, Fig. 3, and from these it also appears that the conductivity of HPO3 is considerably greater than that of H3PO4.

    AB - When P2O5 is thrown into excess of water at room temperature, about 75 per cent. of the total dissolved acid is HPO3 and the rest H3PO4. There is no evidence of the formation of H4P2O7. This HPO3 exists as complex and simple molecules, and the proportions of the two may vary widely from one solution to another of the same total concentration. Two changes then take place, a depolymerisation of the (HPO3)n and a hydration of HPO3, of which the former is probably the quickest. The latter change (hydration) does not, as in the reaction studied by Sabatier, follow exactly the same exponential law until all the acid is changed. The two changes are seen most clearly in the G, K curves, Fig. 3, and from these it also appears that the conductivity of HPO3 is considerably greater than that of H3PO4.

    UR - http://www.scopus.com/inward/record.url?scp=37049171102&partnerID=8YFLogxK

    M3 - Article

    VL - 5

    SP - 37

    EP - 44

    JO - Transactions of the Faraday Society

    T2 - Transactions of the Faraday Society

    JF - Transactions of the Faraday Society

    SN - 0014-7672

    IS - SEPTEMBER

    ER -