Hydrated Aluminum Sulfate Research Articles

Some Effects of High-Solids Matrices on the Sample Delivery System and the Meinhard Concentric Nebulizer during ICP Emission Analyses

Reports have challenged the viability of the concentric nebulizer for high-solids analyte injection in ICP spectrometers. Such samples, particularly those high in sulfates, have been said to cause emission signal drift and plasma instability due to salt deposits on the nebulizer nozzle tip which progressively obstruct argon supply to the plasma. It was of interest to test this hypothesis, particularly with respect to a comparison of the performance of a recently developed recessed capillary tip nozzle, the Meinhard Type C, with the performance of the widely used Types A and B. The aqueous test analyte contained 410 g/L hydrated aluminum sulfate with 1 mg/L manganese as internal standard. Nebulizer performance on a Perkin-Elmer ICP/5000 was monitored via the manganese emission signal and continuous readouts of the nebulizer argon flow rate and argon pressure. In each test, sample analyses continued to the point of plasma failure and instrument shutdown, after which the torch and nebulizer were removed and photographed. In all cases, failure due to salt deposits was discovered in the sample delivery tube of the torch, not in the nebulizers. However, the time before plasma failure occurred was significantly longer with the Type C nebulizer than with either the Type A or Type B units. Photographs and data tabulations are provided to illustrate these effects.

A new occurrence of the hydrated aluminium sulphate zaherite, from Pofadder, South Africa

AbstractA new occurrence of zaherite is reported from a sillimanite quarry 65 km west of Pofadder, Bushmanland, South Africa. It occurs as earthy white to light bluish-green cryptocrystalline material in narrow veins, in close association with natro-alunite and hotsonite, a new hydrated aluminium phosphate-sulphate. Scanning electron micrographs show an orientated wavy texture and tubular fibres. The optical and physical properties agree with those of the type material described from Pakistan, and it can be added that the mineral is biaxial positive with a moderate 2V and length-fast orientation. The new chemical analysis yields an ideal formula of Al12(SO4)5(OH)26·20H2O, which is identical to that of the type material. The white and light bluishgreen varieties are identical in major element composition but yielded trace Cu values of 1281 and 2408 ppm respectively. The X-ray powder diffraction pattern fits a triclinic symmetry (a 5.55, b 9.74, c 18.43Å, α 99.71°, β 89.13° γ 94.97°), and is dominated by one intense reflection at 18.12 Å, representing 001. The most important of the weak lines are (d, I, hkl): 9.56, 5, 010; 9.08, 4, 002; 4.82, 6, 01; 4.61, 8, 110; 4.56, 4, 02; 4.44, 4, 021; 3.61, 4, 1; 3.22, 8, 015. The differential thermal properties are characterized by endothermic peaks at 190, 470, and 685°C and a duplex at 880 and 910°C The infrared absorption spectrum is characterized by absorption bands centring about 905, 960, 985, 1150, 1700, and 3600 cm−1.

Surface and pore structure of some pyrogenic aluminas

Active γ-aluminas were prepared by thermolysis of hydrated aluminium nitrate, hydrated aluminium sulphate and ammonium alum at 1173 K. The specific surface area, pore volume and pore texture of these aluminas were determined by analysis of the corresponding nitrogen adsorption-desorption isotherms at 77 K. The material obtained from aluminium nitrate showed micro- and meso-porosity, a BET surface area of 86 m 2 g − and a pore volume of 0.094 cm 3 g − Thermolysis of aluminium sulphate and ammonium alum leads to mesoporous γ-aluminas with specific surface areas of 150 and 170 m 2 g −, respectively. The pore volume (V p) and most frequent pore radius (r p) are: V p = 0.723 cm 3 g −, r p = 7 nm for the aluminium sulphate-derived alumina; and V p = 1.097 cm 3 g −, r p = 10 nm for the material obtained from ammonium alum.

Thermal Decomposition Processes of Magnesium Aluminum Sulfate Hydrate Prepared with a Freeze-Dried Method

Thermal Decomposition Processes of Magnesium Aluminum Sulfate Hydrate Prepared with a Freeze-Dried Method

ChemInform Abstract: THERMAL DECOMPOSITION OF HYDRAZINIUM ALUMINUM SULFATE HYDRATE AND HYDRAZINATE

Chemischer InformationsdienstVolume 13, Issue 39 Preparative Inorganic Chemistry ChemInform Abstract: THERMAL DECOMPOSITION OF HYDRAZINIUM ALUMINUM SULFATE HYDRATE AND HYDRAZINATE S. GOVINDARAJAN, S. GOVINDARAJANSearch for more papers by this authorK. C. PATIL, K. C. PATILSearch for more papers by this author S. GOVINDARAJAN, S. GOVINDARAJANSearch for more papers by this authorK. C. PATIL, K. C. PATILSearch for more papers by this author First published: September 28, 1982 https://doi.org/10.1002/chin.198239032Read 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. Volume13, Issue39September 28, 1982 RelatedInformation

Decoration patterns on cleavage surfaces of ferroelectric crystals

Cleavage surfaces perpendicular to the polarization vector of the ferroelectric crystals guanidinium uranyl sulfate hydrate (GUSH), guanidinium aluminum sulfate hydrate (GASH) and triglycine sulfate (TGS) decorated with gold, tellurium and silver chloride were observed and compared with the patterns obtained in the non-ferroelectric crystals guanidinium zinc sulfate (GZnS), NaCl and LiF. It was shown that, while some of the decoration structures reproduce the shape of the ferroelectric domains, others are cleavage steps or fracture structures which are not always related to the presence of domains. Although decoration is a useful tool for the detection of ferroelectric domains in materials that are unstable under the conditions prevailing in the electron microscope, the decoration patterns should be carefully analyzed and the relationship between the cleavage plane, cleavage direction and the orientation of the electric polarization vector should be taken into account in order to distinguish between cleavage, fracture and domain structures.

Determination of Water-Soluble Polymers Containing Primary Amide Groups Using the Starch-Triiodide Method

Abstract Partially hydrolyzed, water-soluble polyacrylamide Partially hydrolyzed, water-soluble polyacrylamide polymers in oilfield brines were determined by polymers in oilfield brines were determined by oxidation with bromine at pH 3.5 to give a product that oxidized iodide ion to iodine. The iodine was measured spectrophotometrically as the starch-triiodide complex.Analyses of samples containing polyacrylamide polymers ranging from 10 to 100 ppm concentration polymers ranging from 10 to 100 ppm concentration gave results with a pooled standard deviation of 0.91 ppm and an average recovery of 104%. Separate ppm and an average recovery of 104%. Separate calibration for each batch of polymer was required because of the nonuniform composition of the product. product. Introduction Water-soluble polymers and copolymers of acrylamide and its derivatives are used to treat water and in oil recovery. These polymers are in the 3 to 15 million number-average molecular weight range and may have up to 50% of the amide groups hydrolyzed. A rapid method for determining less than 100 ppm of these materials in surface water and oilfield brine is described here.Turbidimetric techniques using a quaternary ammonium cation (Hyamine 1622 TM) or the hypochlorite ion as precipitants were applied to both polyacrylic acid and hydrolyzed polyacrylamide polyacrylic acid and hydrolyzed polyacrylamide polymers. While these techniques are rapid and polymers. While these techniques are rapid and sensitive, they are subject to heavy metal ion interference. Measurements used by others but deemed unsatisfactory for our work include total nitrogen, amide nitrogen, solution viscosity, and organic carbon.Post and Reynolds used a hypobromite oxidation-spectrophotometric titration to assay various aliphatic amides. Adapting this technique for analyzing acrylamide-based polymers yielded semiquantitative results. A polymer manufacturer recommended a similar procedure, based on this reaction, to form an N-bromoamide oxidation product. After destroying the excess oxidizing agent product. After destroying the excess oxidizing agent (bromine), the N-bromoamide oxidation product reacted with iodide ion to form iodine. Finally, the iodine was measured as the familiar starch-triiodide complex. Lambert described a superior iodide reagent using a linear A-fraction of potato starch/cadmium iodide solution as both the color reagent and source of iodide ion. We used this reaction to determine water-soluble amides. We have modified the bromine oxidation reaction conditions to make the reaction applicable for samples containing high concentrations of chloride ion. We combined this with the stable Lambert reagent to provide a reliable and sensitive procedure for determining polymers containing the primary amide group. Experimental Reagents and Apparatus Buffer solution was pH 3.5. We dissolved 25 g sodium acetate trihydrate in 0.80 dm3 water, added 0.11 dm3 glacial acetic acid and 0.75 g hydrated aluminum sulfate, adjusted the pH to 3.5 with acetic acid, and diluted the solution to 1 dm3. Starch-CdI2 color reagent was prepared as described in Ref. 7, except that we used J. T. Baker Iodometry Grade potato starch powder. Sodium formate (1 % solution) potato starch powder. Sodium formate (1 % solution) and saturated bromine water were required. Linear starches were obtained from Stein, Hall and Co. Inc. We measured absorbance on a Cary Model 11 spectrophotometer in 1-cm cells. SPEJ P. 151

Thermal Decomposition of Hydrated Aluminum Sulfate Precipitated from Acetic Acid Solution

Journal of the American Ceramic SocietyVolume 62, Issue 5-6 p. 313-313 Thermal Decomposition of Hydrated Aluminum Sulfate Precipitated from Acetic Acid Solution ETSURO KATO, ETSURO KATOSearch for more papers by this authorKEIJI DAIMON, KEIJI DAIMONSearch for more papers by this author ETSURO KATO, ETSURO KATOSearch for more papers by this authorKEIJI DAIMON, KEIJI DAIMONSearch for more papers by this author First published: May 1979 https://doi.org/10.1111/j.1151-2916.1979.tb09492.xCitations: 12 The writers are with the Nagoya Institute ot Technology. Gokiso-cho. Showa-ku. Nagoya-shi. Japan. AboutPDF 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 onFacebookTwitterLinked InRedditWechat No abstract is available for this article.Citing Literature Volume62, Issue5-6May 1979Pages 313-313 RelatedInformation

Evaluation of solid electrolytes for high temperature lithium batteries: A preliminary study

The lithium ionic conductivity of materials prepared by reaction of lithium iodide with anhydrous and hydrated aluminum sulfate has been investigated b

Editorial: Toxicity from aluminum antacids.

Alumina, from the Latin alumen (substance with as-tringent taste), constitutes nearly 8 per cent of the earth's crust. It is the most plentiful of rhetals and, of all elements, is exceeded in abundance only by oxygen and silicon. Alumina does not occur naturally in the metallic state; however, in combination with other elements, it is widely distributed in rocks, clay, and soils in the form of gems such as ruby, sapphire, and turquoise, and in minerals of industrial importance such as alum, bauxite, cryolite, corundum, and kaolin. Although aluminum was not isolated until 1825, alum (hydrated aluminum sulfate) has been . . .

Combustion characteristics of crystalline oxidizers.

Abstract : Various modifications to the monopropellant solid oxidizer ammonium perchlorate are described. Cation replacement, or 'doping' of AP by Sr(++) ion and deuteration to provide ND4ClO4 did not alter the burning rate from that of pure NH4ClO4 at 14.7 psia. Hydrated aluminum sulfate shows an ability to extinguish AP combustion at the 5% level, whereas 2% does not even alter the burning rate at atmospheric pressure. The theoretical adiabatic combustion species for AP and dihydroxy glyoxime (DHG) at 1, 34 and 68 atmospheres are given. DHG produces fuel rich rather than oxygen rich monopropellant combustion species.

Cathodo-luminescence of Samarium as Applied to the Structural Studies of Alumina. IV. On Alumina yielded by Thermal Decomposition of Hydrated Crystals of Aluminium Salts

Abstract Hydrated crystals of some aluminium salts, namely nitrate, chloride, sulphate and ammonium alum were subjected to heat treatments in the presence of a small amount of samarium ions. Cathodo-luminescence spectra were investigeted on the samarium-bearing aluminas thus resulted. A conversion of the luminescence spectrum takes place, as the temperature of the heat treatment has been elevated, from the prototype I to the prototype II, which corresponds to the γ-α transformation of an alumina. It was, however, confirmed that there are some differences in the facility of this conversion according to the kinds of aluminium salts employed for the preparation of alumina. Some alterations were, furthermore, perceived in the intensity of luminescence bands situating in the vicinity of 610 mμ, when the hydrated crystals of aluminium nitrate were submitted to the heat treatments of various elevated temperatures. Hydrated crystals of these aluminium salts were heated previously at various temperatures between 180 and 1200°C. After the addition of samarium ions, they were roasted. The resulting samarium-bearing aluminas give rise to cathodo-luminescence spectra, which reveal that a conversion to the genuine α-modification proceeds most readily in the case of aluminium nitrate, while it occurs with difficulty in the cases of hydrated aluminium sulphate and ammonium alum. It seems to be hard for samarium ions to enter into the configuration of alumina, when previous thermal treatments of aluminium salts have been carried out at much elevated temperatures.