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Shibata M, Sakaida H, Kakiuchi T. Determination of the activity of hydrogen ions in dilute sulfuric acids by use of an ionic liquid salt bridge sandwiched by two hydrogen electrodes. Anal Chem. 2010;83(1):164-8doi: 10.1021/ac1021216.
Shibata, M., Sakaida, H., & Kakiuchi, T. (2011). Determination of the activity of hydrogen ions in dilute sulfuric acids by use of an ionic liquid salt bridge sandwiched by two hydrogen electrodes. Analytical chemistry, 83(1), 164-8. https://doi.org/10.1021/ac1021216
Shibata, Manabu, et al. "Determination of the activity of hydrogen ions in dilute sulfuric acids by use of an ionic liquid salt bridge sandwiched by two hydrogen electrodes." Analytical chemistry vol. 83,1 (2011): 164-8. doi: https://doi.org/10.1021/ac1021216
Shibata M, Sakaida H, Kakiuchi T. Determination of the activity of hydrogen ions in dilute sulfuric acids by use of an ionic liquid salt bridge sandwiched by two hydrogen electrodes. Anal Chem. 2011 Jan 01;83(1):164-8. doi: 10.1021/ac1021216. Epub 2010 Dec 03. PMID: 21126098.
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Anal Chem. 2011 Jan 01;83(1):164-8. doi: 10.1021/ac1021216. Epub 2010 Dec 03.

Determination of the activity of hydrogen ions in dilute sulfuric acids by use of an ionic liquid salt bridge sandwiched by two hydrogen electrodes.

Analytical chemistry

Manabu Shibata, Hideaki Sakaida, Takashi Kakiuchi

Affiliations

  1. R&D Center, Horiba, Ltd., Kyoto 601-8510, Japan.

PMID: 21126098 DOI: 10.1021/ac1021216

Abstract

The activities of hydrogen ions in 20-200 μmol dm(-3) H(2)SO(4) solution were estimated by use of an ionic liquid salt bridge (ILSB), made of tributyl(2-methoxyethyl)phosphonium bis(pentafluoroethanesulfonyl)amide (TBMOEPC(2)C(2)N), sandwiched by two hydrogen electrodes. The experimental pH values (pH = -log a(H), where a(H) is the activity of hydrogen ions) were in good agreement, within 0.01 pH unit, with those calculated using the Pitzer model. The difference between the experimental and theoretical pH values at 50 μmol dm(-3) H(2)SO(4) solution was much smaller than that obtained by use of a glass electrode in combination with a reference electrode with a concentrated KCl salt bridge. The source of the small deviation can be explained by the residual diffusion potential due to the dissolution of TBMOEPC(2)C(2)N in the H(2)SO(4) solution (W) and the resultant increase in the ionic strength of W. The use of a reference electrode equipped with an ILSB opens the way to accurately estimate the pH in dilute aqueous solutions, for which we have not had effective means.

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