Electrometric Titration Research Articles

Bromide and Chloride Distribution Between Serum and Cerebrospinal Fluid

The report that bromide, after administration by mouth, exists in a higher concentration in the blood serum than in the cerebrospinal fluid attracted our attention because of the following considerations. If equilibrium exists between serum and cerebrospinal fluid, if bromide ions are freely diffusible, and if the protein ions are the only restraining factor, the application of the Gibbs-Donnan Law would lead to a predicted distribution ratio of (Br)s/(Br)csf = 0.95. The bromide distribution ratios of Malamud, Fuchs and Malamud were approximately 3.0 for normal individuals and did not fall below unity in patients with damaged permeability, as in paresis. Since the colorimetric method employed by these investigators did not permit the determination of actual bromide concentrations, observations have been made using the electrometric titration method previously described as well as the colorimetric gold chloride method. The procedure followed was to administer to the patients 0.01 gm. of sodium bromide per pound of body weight 3 times a day for 5 days. Twenty hours following the last dose of bromide, blood and cerebrospinal fluid were drawn for analysis. This procedure was followed with 5 patients. Two others, O and R, were given larger doses of sodium bromide for a longer period before analyses were made. The results of 3 paretic and 2 non-paretic patients are given in Table I. Concentrations have been expressed in millimols per kilogram of water. In all instances, with both methods, the ratio (Br)s:(Br)csf was greater than unity. This substantiates the theory that bromides are not freely diffusible between serum and cerebrospinal fluid. In all except one instance the bromide ratio determined electrometrically was lower than that obtained colorimetrically.

A NEW USE OF THE VACUUM TUBE IN ELECTROMETRIC TITRATIONS. I. POLARIZATION OF PLATINUM ELECTRODES IN OXIDATION AND REDUCTION REACTIONS1

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTA NEW USE OF THE VACUUM TUBE IN ELECTROMETRIC TITRATIONS. I. POLARIZATION OF PLATINUM ELECTRODES IN OXIDATION AND REDUCTION REACTIONS1J. L. Kassner, R. B. Hunze, and J. N. ChatfieldCite this: J. Am. Chem. Soc. 1932, 54, 6, 2278–2284Publication Date (Print):June 1, 1932Publication History Published online1 May 2002Published inissue 1 June 1932https://doi.org/10.1021/ja01345a016RIGHTS & PERMISSIONSArticle Views19Altmetric-Citations5LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (433 KB) Get e-Alerts Get e-Alerts

218. The properties of nicotine and its derivatives. Part VI. Electrical conductivities. Part VII. Electrometric titrations

218. The properties of nicotine and its derivatives. Part VI. Electrical conductivities. Part VII. Electrometric titrations

The Electrometric Titration of Copper Salts by Sodium Hydroxide

The Electrometric Titration of Copper Salts by Sodium Hydroxide

Colorimetric and potentiometric determination of pH: Outline of electrometric titrations. By L. M. Kolthoff, Ph.D. Pp. xi + 167. London: Champman & Hall. New York: J. Wiley & Sons, 1931. 11s

Journal of the Society of Chemical IndustryVolume 50, Issue 44 p. 877-877 Review Colorimetric and potentiometric determination of pH: Outline of electrometric titrations. By L. M. Kolthoff, Ph.D. Pp. xi + 167. London: Champman & Hall. New York: J. Wiley & Sons, 1931. 11s T. Callan, T. CallanSearch for more papers by this author T. Callan, T. CallanSearch for more papers by this author First published: 30 October 1931 https://doi.org/10.1002/jctb.5000504412AboutPDF ToolsRequest permissionExport citationAdd to favoritesTrack citation ShareShare Give accessShare full text accessShare full-text accessPlease review our Terms and Conditions of Use and check box below to share full-text version of article.I have read and accept the Wiley Online Library Terms and Conditions of UseShareable LinkUse the link below to share a full-text version of this article with your friends and colleagues. Learn more.Copy URL Share a linkShare onFacebookTwitterLinkedInRedditWechat No abstract is available for this article. Volume50, Issue4430 October 1931Pages 877-877 RelatedInformation

Oxidation of Cobaltous Cysteine.

Michaelis and Barron1 and Michaelis and Yamaguchi2 have shown that cobalt reacts with cysteine to form a product which has a high reduction intensity. They also showed that this reaction product can be oxidized with air, ferri-cyanide, and phenolindophenol to a brown cobaltic cysteine complex. We have found that cobaltous cysteine reacts in a different manner toward each one of these oxidants. Indigo disulfonate produces a quantitative conversion of cobaltous cysteine to the cobaltic cysteine complex. All other oxidants except those which contain a quinone group result in the formation of the cobaltic cysteine complex and cystine in different proportions.Oxidation with ferricyanide produces a unique type of electrometric titration curve because all of the cobaltous cysteine is removed from solution by addition of a half of the total amount of oxidant. The last half of the curve represents oxidation of cysteine to cystine.Cysteine reacts with quinone and with the quinone group of dibromophenol-indophenol w...

CCXCIV.—Electrometric titration curves of dibasic acids. Part IV. Corrections for interionic effects and for solvent electrostriction. First and second dissociation constants of some n-paraffin αω-dicarboxylic acids, alkyl- and dialkyl-malonic acids, s-di- and -tetra-alkylsuccinic acids, β-alkyl-and ββ-dialkyl-glutaric acids, and cyclic 1 : 1-di-acetic acids. Remarks on the configurations and molecular dimensions of these acids in dilute aqueous solution

CCXCIV.—Electrometric titration curves of dibasic acids. Part IV. Corrections for interionic effects and for solvent electrostriction. First and second dissociation constants of some n-paraffin αω-dicarboxylic acids, alkyl- and dialkyl-malonic acids, s-di- and -tetra-alkylsuccinic acids, β-alkyl-and ββ-dialkyl-glutaric acids, and cyclic 1 : 1-di-acetic acids. Remarks on the configurations and molecular dimensions of these acids in dilute aqueous solution

The Organic Acids of the Cerebro-Spinal Fluid

The electrometric titration method for the investigation of “organic acids,” as developed by Perlzweig and Delrue (1) and applied to the examination of sera, indicated a method of investigation of the organic acids of the cerebro-spinal fluid, and an attempt has been made in this paper to investigate the significance of the organic acid titration in mental disorders. Owing to the difficulty of obtaining normal cerebro-spinal fluid, the research had to be confined to the investigation of paretic and non-paretic cerebro-spinal fluids obtained from mental cases. In the former case adequate specimens were obtainable during the process of collection of fluid for diagnostic purposes, and the results obtained in some cases were confirmed by independent collection.

Apparatus for Rapid Electrometric Titration

This apparatus was assembled at Millport for the electrometric titration of solutions which, being highly coloured, cannot well be titrated with an indicator. It may be used also for highly dilute solutions, unless they are so slightly buffered that their pH value is appreciably changed by the addition of a small quantity of quinhydrone. Measurement of hydrogen-ion concentrations at the quinhydrone electrode has also been attempted with the apparatus. The apparatus is suitable for use at sea.

Societies and Academies

LONDON. Society of Public Analysts, Dee. 4.—A. P. Laurie: methods of examining pictures. An outline was given of the composition of the different pigments used for old illuminated MSS. and oil paintings, and methods of sampling by means of a micro-borer and examination by means of a microscope polariscope were described; a summary of micro-chemical tests the various classes of pigments was given. The of X-ray photography and ultra-violet rays was discussed, and it was shown how an examination of brush strokes in an oil painting, considered in conjunction with the chemical and optical properties the pigments, enabled a judgment to be formed as whether the whole work had been produced in one studio and at the same period.—S. Glasstone and C. Speakman: The quantitative analysis of mixtures nickel and cobalt. Electrometric titrations of nickel and cobalt solutions with potassium cyanide, with nickel and cobalt indicator-electrodes, respectively, have established the soundness of the theoretical basis of the Rupp and Pfennig method of determining these metals. A modified iodimetric method has also been developed for determining small amounts of cobalt in the presence of nickel.—J. C. Baird and H. Prentice: The changes with age of the hydrogen concentration of egg white and egg yolk. Determinations of hydrogen ion concentration by means quinhydrone electrode indicated that the normal pH value of fresh egg white is approximately 8.6, that there is a rapid rise in the course of the week of storage to a level of about pH 9.0, at which figure the reaction remains fairly constant. The fresh yolk has a reaction of approximately pH 6.0, which in the course of ten weeks rises to about 6.2. refractive index of the egg white is constant at about 1.360.

Societies and Academies

CAPE TOWN. Royal Society of South Africa, June 19.—Sir Thomas Muir: The literature of Cayleyan matrices.—A. Ogg: The space group and symmetry of potassium, ammonium, and rubidium suiphates. Taylor and Boyer have confirmed the space group for ammonium and cesium suiphates, and have given an atomic structure which is substantially the same as that given by the author. The space group Vhl3 given by F. P. Goeder for potassium, rubidium, and casium sulphates is untenable; the space group is Vhl6, as originally determined by the author and confirmed by Taylor and Boyer.—W. Pugh: Germanium dioxide in aqueous solution; germanic acid. Germanium hydroxide is truly amphoteric. As an acid, it forms the more characteristic series of salts, the germanates; as a base, it forms the less stable series of salts with the halogen acids. Electrometric titrations of sodium germanate solutions show that germanic acid is a dibasic acid; the existence of sodium bi-germanate in solution has been established. The degree of hydrolysis of sodium germanate has also been measured at various dilutions.

Determination of Tertiary Dissociation Constant of Phosphoric Acid.

Quantitative studies of the mechanism of calcification require a knowledge of the physico-chemical constants of the blood equilibria involved in the process. The tertiary dissociation constant of phosphoric acid, K3, thus far available seems incompatible with the apparent dissociation constant pK3 from the dissociation curve for the phosphates which is of an order of 1 x 1012.The value of K3 was determined experimentally from a study of aqueous systems of the tertiary sodium and potassium phosphates at equilibrium, from the standpoint of hydrolysis. The value thus obtained was correlated with calculations made from the data obtained by the electrometric titration of phosphoric acid.The tertiary phosphates hydrolyze to a great extent, the secondary and primary salts inappreciably. In the mechanism of the first stage hydrolysis of the tertiary salts, the essential equilibrium, may be expressed ionically:Where the brackets include the ion activities, and Kh is the activity hydrolysis constant.

Smooth Platinum Wire for Electrometric Titrations in Neutralization Reactions1

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTSmooth Platinum Wire for Electrometric Titrations in Neutralization Reactions1Stephen Popoff and Martin J. McHenryCite this: Ind. Eng. Chem. 1928, 20, 5, 534–538Publication Date (Print):May 1, 1928Publication History Published online1 May 2002Published inissue 1 May 1928https://doi.org/10.1021/ie50221a032RIGHTS & PERMISSIONSArticle Views14Altmetric-Citations2LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (599 KB) Get e-Alerts

Method for Electrometric Titration of Organic Acids of the Blood.

Repeated attempts were made to apply Van Slyke and Palmer's1 titrimetric method for the estimation of the organic acids of the blood plasma. These attempts were unsuccessful chiefly because with the small concentrations involved, no satisfactory end-point in the acid range could be obtained with the available indicators (thymol blue, bromphenol blue, Tropaeolin 00). In order to overcome this difficulty and also in the hope of gaining some information concerning the nature of the organic acids from the titration curves, the following method for the electrometric titration of these acids in the blood was developed.The proteins are removed by means of ultrafiltration through collodion membranes or by precipitation with metaphosphoric acid; the carbonates, phosphates, oxalates and sugar are removed by addition of CuSO4 and solid Ca(OH)2. The filtrate may at this point be evaporated on the water bath to a small volume. More calcium hydroxide, sulfate and carbonate as well as basic cupric carbonate usually crys...

THE DETERMINATION OF IRON IN GLASS SAND1

Data are presented in tabular form showing the determination of iron in the Bureau of Standards Sample of Glass Sand, No. 81. The electrometric titration method, the H2S reduction method, and the gravimetric method are described in detail.

STUDIES ON THE ACIDITIES OF CANE MOLASSES WORT

1. The hydrogen ion concentration of cane molasses wort has been investigated by gas chain method for distillery purpose. It varies from pH 5.06-5.93 at 20° Bolling. 2. On heating or reservation, the pH diminishes 0.3-0.56. 3. The buffer capacity has been shown by electrometric titration curve. 4. The titrable acidities of cane molasses wort by electrometric method were 18-36c.c. of 1/1.0 n NaOH on 100c.c. of wort, and by ordinary indicator method using litmus paper were 20-35c.c. and when used phenolphthalein as an indicator were 36-74c.c. of the same. 5. It is observed that the cane molasses wort ferments with good results on the pH range of 3.5-6.0 and the optimal range is pH 4.0-5.0 by the yeast No. 396 of our laboratory which is the powerful and widely distributed species in this land.

CCLXI.—Studies of valency. Part X. Electrometric titration of Vernon's α- and β-dimethyltelluronium bases

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Differential Electrometric Titration as a Precision Method

Differential Electrometric Titration as a Precision Method

Dissociation Constants of Hexosephosphoric Acids.

Hexosediphosphoric acid from yeast and hexosemonophosphoric acid from muscle (lactacidogen) were kindly made available from preparations by Professor Embden. Electrometric titration showed both stronger than pure phosphoric acid in the region of the first and, more conspicuously, in that of the second dissociation constant. In each case hexosemonophosphoric acid was the stronger. From titration data with pure phosphoric acid a second constant at 18 degrees of pK2 equals 6.82 was calculated, agreeing with the usual values given. For hexosediphosphoric acid only an apparent value of the constant corresponding to the actual third and fourth together was determined at pK2 = 6.25, corresponding with the value of Meyenhof and Suranyi of pK2, 6.2.

AMPHOTERIC BEHAVIOR OF COMPLEX SYSTEMS

Electrometric titrations of glycine, sulfanilic acid, and various mixtures of the two have been made. These mixtures are shown to give a curve which, between their respective isoelectric points, is different from that of either substance. These mixtures have a maximum buffering power at a pH which can be theoretically calculated, and which has the characteristics of an "isoelectric point of the system." Other pairs of ampholytes are shown to act in an analogous manner.