Lead Hydroxide Research Articles

ChemInform Abstract: CRYSTAL STRUCTURES OF LEAD (PB6)‐A AND LEAD HYDROXIDE HYDRATE (PB9(OH)8(H2O)3‐A. ZEOLITE A ION EXCHANGED WITH LEAD(2+) AT PH 4.3 AND 6.0 AND EVACUATED

Chemischer InformationsdienstVolume 16, Issue 31 Physical Inorganic Chemistry ChemInform Abstract: CRYSTAL STRUCTURES OF LEAD (PB6)-A AND LEAD HYDROXIDE HYDRATE (PB9(OH)8(H2O)3-A. ZEOLITE A ION EXCHANGED WITH LEAD(2+) AT PH 4.3 AND 6.0 AND EVACUATED C. RONAY, C. RONAYSearch for more papers by this authorK. SEFF, K. SEFFSearch for more papers by this author C. RONAY, C. RONAYSearch for more papers by this authorK. SEFF, K. SEFFSearch for more papers by this author First published: August 6, 1985 https://doi.org/10.1002/chin.198531007Read the full textAboutPDF 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. Volume16, Issue31August 6, 1985 RelatedInformation

The interaction of oxygen and carbon monoxide with a carbided Ni(111) surface

The oxidation of cleaved surfaces of galena (natural lead sulfide) in air at ambient temperature and humidity has been studied by X-ray photoelectron spectroscopy. Analyses were carried out with the sample held below 150 K, a temperature at which elemental sulfur was shown to be retained at a galena surface, and subsequently at ambient temperature. During the initial stages of air-oxidation, the surfaces became enriched with lead due to the formation of lead hydroxide, oxide and carbonate. No oxidised sulfur species were observed in this period and it was concluded that a metal-deficient sulfide was formed. Exposure of galena to air for extended periods resulted in the formation of sulfate. After oxidising galena in air-saturated acetic acid solution, the presence of polysulfide phases was revealed. Minor elements present in the galena were found to migrate to fill some of the vacancies in the metal-deficient sulfide and polysulfide phases.

An x-ray photoelectron spectroscopic study of the oxidation of galena

The oxidation of cleaved surfaces of galena (natural lead sulfide) in air at ambient temperature and humidity has been studied by X-ray photoelectron spectroscopy. Analyses were carried out with the sample held below 150 K, a temperature at which elemental sulfur was shown to be retained at a galena surface, and subsequently at ambient temperature. During the initial stages of air-oxidation, the surfaces became enriched with lead due to the formation of lead hydroxide, oxide and carbonate. No oxidised sulfur species were observed in this period and it was concluded that a metal-deficient sulfide was formed. Exposure of galena to air for extended periods resulted in the formation of sulfate. After oxidising galena in air-saturated acetic acid solution, the presence of polysulfide phases was revealed. Minor elements present in the galena were found to migrate to fill some of the vacancies in the metal-deficient sulfide and polysulfide phases.

The Formation and Solubility of Various Lead(II) Compounds Prepared by the Hydrolysis of Lead(II) Nitrate

Abstract Lead(II) nitrate was hydrolyzed by mixing with sodium hydroxide solutions at 25 and 50 °C. Four kinds of lead(II) hydroxide nitrates and two kinds of lead(II) oxides (massicot and litharge) were formed, depending on the pH, temperature, lead(II) nitrate concentration, and aging time of the suspension. The solubility of the products was also measured.

Thermal studies of lead(II) salts, VI

The kinetics and mechanisms of the thermal decomposition of lead(II) carbonate and lead(II) hydroxide carbonate have been studied over a range of temperatures and partial pressures of carbon dioxide using both isothermal and programmed heating. All stages in each decomposition are diffusion controlled and Arrhenius parameters have been determined. These values for loss of carbon dioxide are all extremely high for a diffusion process, but show a compensation effect, following the equation: logA=−5.02+0.067E The compensation effect is discussed and comparisons with other systems showing such effects are made.

Flotation of hydroxide precipitates

Bulky flocculent precipitates of hydroxides of Ti (IV), Zr(IV), In(III), Sn(IV), Fe(II), Ni(II), and Sb(III) {(2030) mg metal} in solutions (200ml) were rapidly floated with numerous tiny nitrogen bubbles (diameter below 0.5mm) after addition of an ethanolic solution of cationic surfactant (benzalkonium chloride) or anionic surfactant (sodium oleate or dodecylbenzenesulfonate). However, the flotation of fine precipitates of lead hydroxide was incomplete. Cadmium (1μg) in water (200ml) was coprecipitated with hydroxide precipitates of Ti(IV), Zr (IV), or In (III) (20mgmetal), which were then floated. The cadmium recovery was greater than 97%.

Polarographic determination of lead hydroxide formation constants at low ionic strength

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTPolarographic determination of lead hydroxide formation constants at low ionic strengthCarol J. LindCite this: Environ. Sci. Technol. 1978, 12, 13, 1406–1410Publication Date (Print):December 1, 1978Publication History Published online1 May 2002Published inissue 1 December 1978https://doi.org/10.1021/es60148a010RIGHTS & PERMISSIONSArticle Views67Altmetric-Citations4LEARN 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 (607 KB) Get e-Alerts Get e-Alerts

Reaction between hydrogen chloride and lead (II) salts

AbstractThe reactions occurring between gaseous hydrogen chloride and lead (II) carbonate and lead (II) hydroxide carbonate (white lead) have been studied over a range of temperatures and partial pressures of hydrogen chloride. The only solid reaction product is lead (II) chloride which is formed in a single stage. Kinetic studies show that the diffusion of HCI is probably the rate‐controlling step and Arrhenius parameters for this process are given.

The solubility products of some slightly soluble lead salts and the potentiometric titration of molybdate, tungstate, perrhenate and fluoride with use of a lead ion-selective electrode

The conditional solubility products of lead molybdate, lead tungstate and lead perrhenate were found to be 1.2 ± 0.3 × 10 −13, 8.4 ± 0.1 × 10 −11 and 6.9 ± 0.8 × 10 −9, respectively. In the case of lead perrhenate, the conditional stepwise formation constants for PbReO + 4 and Pb(ReO 4) 2 were found to be 1.2 ± 0.1 × 10 5 and 1.2 ± 0.2 × 10 3, respectively. Conditions for the potentiometric titration of molybdate, tungstate, perrhenate and fluoride with lead were established. The precipitates obtained during the titration of molybdate, perrhenate and fluoride mixtures have been proved to be physical mixtures of lead molybdate, perrhenate, fluoride and hydroxide, by infrared spectrometry. The p K sp-values of the lead salts of chromate, molybdate and tungstate are shown to increase linearly with increasing atomic number or electronegativity of the Group VI metal ion.

Thermal studies on lead(II) salts—II: The decomposition of lead hydroxide carbonate, Pb(OH)2·2PbCO3

The thermal decomposition of lead(II) hydroxide carbonate 2PbCO3·Pb(OH)2 (white lead) has been studied by thermogravimetry under various partial pressures of carbon dioxide. The TG curves have been followed by X-ray diffractometry and IR spectroscopy and the results interpreted by the reaction scheme: 2(2PbCO3.Pb(OH)2) = 2(2PbCO3.PbO)+ 2H2O2(2PbCO3.PbO) = 3(PbCO3.PbO) + CO23(PbCO3.PbO) = 2(PbCO3.2PbO) + CO22(2PbCO3.2PbO) = 6PbO + 2CO2.

Thermal studies on lead(II) salts

The thermal decomposition of synthetic lead(II) hydroxide chloride has been studied between 490 and 520 K over a range of partial pressures of water vapour. The reaction rate is controlled by diffusion of water vapour and Arrhenius parameters have been calculated. The activation energy varies between 92 and 145 kJ mol −1 and the frequency factor between 10 9 and 10 15 sec −1. Water vapour pressure has a profound effect on the reaction rate and a double minimum in the rate is observed. Enthalpimetric data are also presented for the decomposition.

The Use of Lead and Uranyl Ions As A Stain in Scanning Electron Microscopy

Cellular components can be identified in cryofractured surfaces of osmium impregnated tissue examined in the scanning electron microscope (SEM). The present study compares the staining properties of uranyl and lead ions used to selectively enhance the definition of cell organelles. Tissues used for this study were liver, kidney and testis from normal rats. All of the tissue in this study was treated with osmium-thiocarbohydrazide-osmium (OTO) as described by Munger and Mumaw (1). Following the OTO treatment some tissues were placed in 1% aqueous uranyl acetate for 4 hrs. at room temp. Tissue stained with lead was placed in a Millonig's lead hydroxide solution for 2 hrs. Some tissue blocks were stained with uranyl acetate for 4 hrs. followed with 2 hrs. staining in lead hydroxide. Following each staining period the tissue was rinsed several times with distilled water before proceeding with the next step.

Polarographic determination of lead (II) in a standard solution of lead tetraacetate; Application of separation method of lead (IV) hydroxide precipitates

Polarographic determination of lead (II) in a standard solution of lead tetraacetate; Application of separation method of lead (IV) hydroxide precipitates

Electrophoretic and tyndallometric studies on the hydrolysis of lead(II) in aqueous solutions

The hydrolysis of lead and the precipitation of lead hydroxide over a wide pH and concentration range of lead nitrate in 0·5 M sodium perchlorate and lead chloride in 0·15 M sodium chloride have been investigated by tyndallometric method, high voltage electrophoresis and adsorption chromatography on filter paper cellulose. The precipitation diagrams, represented as pH vs log concn of lead salts, show regions where Pb 2+ ionic species, cationic and anionic hydrolytic species, cationic chloro and chloro-hydroxo complexes, and electrically uncharged ion pairs of sodium ions with anionic hydroxo complexes of lead were found to exist. The solubility constant of lead hydroxide log Ks 0 = −19·3 was found at 20°C. The electrical charge of the lead hydrolytic species which form lead hydroxide precipitate at the precipitation boundary was found to be +2, whereas the electrical charge −2, was attributed to polynuclear anionic species formed after dissolution of lead hydroxide precipitate with alkali in excess.

Analytical Study of the Lead Ion-selective Ceramic Membrane Electrode

Abstract The lead(II) ion-selective ceramic membrane electrode developed by sintering a mixture of lead, silver, and cuprous sulfides showed sensitivity, selectivity, and other response characteristics well suited to analytical utilization. The Nernstian slope was obtained over a concentration range from 10−1 to 10−6m Pb2+ in activity, and the analytical range had a concentration of 10−1–10−7m when the membrane contained less than 30 wt% of cuprous sulfide and more than 1 wt% of lead sulfide. Among the common ions, silver, cupric, mercury(II), ferric, sulfide and iodide ions interfered seriously. About 10 times as many cadmium and bromide ions and more than 1000 times as many alkali metal, alkaline earth metal, zinc, aluminum, nickel, manganese(II), cobalt, and nitrate ions did not interfere with the lead ion, however. The electrode potentials did not change over a pH range from 2 to the pH at which the precipitation of lead hydroxide occurred. The electrode was safely used at temperatures from 0 to 95°C, and the potentials of the membrane satisfied the Nernstian equation within the limits of experimental error. The membrane electrode responded to activity changes very quickly: the rate of those changes was twice that in a lead sulfide-silver sulfide two-component ceramic electrode. A continuous potential measurement for 5 months promised long-term stability and accuracy. The rapid response rate and the long lifetime suggest that the continuous monitoring of some changing systems is feasible.

Uranyl Acetate as a Fixative—from pH 2.0 to 8.0

Numerous applications utilizing uranyl acetate as an electron stain for electron microscopy have been described. Uranyl acetate has become a routine stain used in conjunction with lead hydroxide for staining ultrathin sections. En bloc staining with uranyl acetate following osmium tetroxide post-fixation produces undesirable effects on some cytoplasmic components, especially glycogen. Recent studies using uranyl acetate as a fixative and en bloc stain at pH 7.2 before osmification has shown uranyl acetate to have desirable fixation and staining qualities. Tissues treated with uranyl acetate at a pH of 2.0-8.0 were studied. Normal rat tissue was fixed in Karnovsky's paraformaldehyde-glutaraldehyde fixative. The tissue was post-fixed in 0.5% uranyl acetate in water at pH 2.0 and 0.5% uranyl acetate in 0.1M s-collidine with 0.01M oxalic acid at pH 4, pH 6.0, pH 7.2, and pH 8.0 for 1 hour at 4°C. Following several rinses of 0.1M s-collidine buffer, the tissues were treated with 1.33% osmium tetroxide 1 hour at 4°C followed by rapid dehydration in ethanol and embedded in Durcupan ACM. Tissue sections were stained with lead hydroxide.

Ultrastructure of Alpha-Keratin Microfibrils

Tips from the quills of Erethyon dorsaturn (porcupine) were placed in 0.5 M thioglycollic acid at pH 5.6 for 24 hours, then fixed for 72 hours in 1% OsO4. Quills were also prepared without the thioglycollic acid treatment. The material was dehydrated in a series of ethyl alcohols and embedded in Spurr Low Viscosity Embedding Medium. Sections were cut on a Reichert 0mU2 ultramicrotome and stained for 40 minutes at 37°C with saturated lead hydroxide. Electron micrographs (primary magnification 150,000 x) were taken with an A.E.I. EM6B electron microscope at 60 KV equipped with 25 μ and 50 μ objective apertures and an anticontamination device. Focal series of silver to silver gray sections were taken with a 0.1 μ change of focus (1 click of fine focus control). For the Markham rotation technique a constant speed motor (The General Industries Co., Elyria, Ohio) and a Strobatac (Model 1538-A, General Radio) was used.

A reinvestigation of the chemistry of pinol : Oxygen migration in the electrophillic additions to a 7-oxabicyclo[3.2.1]oct-2-ene derivative

The addition of bromine to pinol is shown to give 6,7- diendo-dibromocineole ( 6) which on treatment with hydrogen bromide is converted into “pinol tribromide” which is now formulated as 2,6-dibromo-4-(α-bromoisopropyl)-1-methyl-1-cyclohexanol ( 7). The reaction of cineole dibromide 6 with lead hydroxide, epoxidation of pinol with performic acid or hydrolysis of pinol oxide afford 6,7- diendo-dihydroxycineole 21. Pinol epoxide on treatment with hydrogen chloride, hydrogen bromide or boron trifluoride is converted into the corresponding diendo 6-halo-7-hydroxycineole derivative. The reaction of pinol with potassium permanganate, osmium tetraoxide or nitrosyl chloride does not proceed with oxygen migration and yields pinol glycol 34 and chloro nitroso dimer 35, respectively.

Correlation between ultrastructure and histochemistry of lafora bodies.

Lafora bodies are composed of fibrillar and granular components in various concentrations. They are located in neuronal cell processes and perikarya and are frequently clearly intermingled with cytoplasmic elements. These components are electron-lucent, show a variable affinity for osmium, and are weakly stained by classical uranyl acetate stain following lead citrate. They exhibit a strong affinity for lead hydroxide and are periodic-acid reactive. They are not stained by the PTA technic for basic protein and/or acidic mucopolysaccharides. These results are in agreement with chemical studies according to which L. B are mostly composed of polyglucosans and suggest that both the granular and fibrillar ultrastructural components contain vic-glycol groups. The ultrastructure of L. B. is very similar to that of corpora amylacea, to deposits in basophilic degeneration of myocardium and in glycogenosis type IV.

Catalysts of the condensation of formaldehyde to sugars

According to the literature data, the condensation of formaldehyde to sugars occurs on calcium, magnesium, lead, and thallium hydroxides [1-4]. Theproeess occurs in neutral or weakly alkaline medium and is accelerated by the addition of certain organic substances. There is information [5] that complex formation of the reagents with the metal ions forming the hydroxide occurs during the synthesis. The hydroxides studied thus far contain metal ions, the radii of which lie within the interval from 0.78 to 0.99 A, while the ratio of the charge to the radius (e/R) varies from 2.56 to 2.01.