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A simple and rapid technique for the estimation of lactose in fluid milk and whey, utilizing trichloroacetic acid (TCA) as a precipitating agent, is outlined. The color development is based on the reaction of picric acid with lactose in the presence of phenol, sodium hydroxide and sodium bisulfate. This method can be completed within 10 min. There is no significant difference ( p ≤ 0·05) between the results obtained by the proposed method and those obtained by the IDF method.

Observations and conclusions drawn from a model N-methylol reactant system have been used to study formaldehyde release from cotton fabric treated with N,N′-dimethylol-4,5-dihydroxy-ethyleneurea (DMDHEU). Reagent residues produced by DMDHEU in the presence of sodium bisulfate or zinc nitrate were found to be more complex than those formed from the N-methylolpyrrolidone (NMP) reactant system, and the exact nature of some of the residues from DMDHEU could not be established. Zinc nitrate produces higher fixation of DMDHEU on cotton as compared to sodium bisulfate and also reduces formaldehyde release. As is the case with the NMP system, the lower amount of formaldehyde release with zinc nitrate catalyst is believed to be at least partially due to the formation of a complex between the N-methylol reactant, DMDHEU, and zinc nitrate. The COCell bonds in both finishes resist acid-catalyzed cleavage but cleavage of the NC bonds in N-methylol groups (to release formadehyde) in the presence of acid is greater for the DMDHEU system than for the NMP system. Results with the DMDHEU and NMP systems are similar, but because of the complex nature of the products formed in the DMDHEU system it is very difficult to correlated formaldehyde release with specific chemical structures of residues or reactants.

Raman spectra of supersaturated solution droplets of ammonium bisulfate, potassium bisulfate and sodium bisulfate were obtained in the region 800–1300 cm−1 with a resolution of 1 cm−1. Under supersaturation condition, these solution droplets show new molecular vibrations, not found in the spectra of either the bulk crystalline or the solution samples. The results demonstrate the existence of an ion pair in the supersaturated bisulfate solution, which consists of both the cation and the anion of the dissociated solute as well as the solvent molecules. They also provide a new interpretation of the asymmetry commonly found in the 1050 cm−1 bisulfate ion vibration band.

Hydrolysis was over 90% in a 30% (wt/vol) solution of lactose in 2N sulfuric acid at 60 C for 36 h. The brown color that developed during hydrolysis was removed easily with activated carbon. Slight off-flavors were removed completely by treatment with calcium hydroxide to about pH 6 followed by activated carbon, yielding a syrup of excellent color and flavor. This process minimized anions and cations in the hydrolyzed syrup. Neutralization with lime and treatment with activated carbon gave a syrup with equisweetness to 20.8% sucrose (g/100 ml). Acid hydrolysis of concentrated whey with sulfuric acid produced a more severe browning reaction and off-flavor. Treatments with calcium hydroxide and activated carbon that were effected in aqueous lactose hydrolysates were ineffective in hydrolyzed whey. Sodium bisulfate inhibited color development during hydrolysis of whey but slowed hydrolysis, affected flavor, and interfered with analytical methods.

The applicability of the Lee-Wheaton conductance equation to the problem of accounting for the variation of the conductivity of moderately complex electrolyte solutions containing more than two kinds of ionic species and involving one or more ion-association equilibria is demonstrated using the chemically interesting examples of sulfuric acid, sodium bisulfate, and hydrofluoric acid, as well as naphthalene trisulfonic acid, sodium naphthalene trisulfonate, and lanthanum naphthalene trisulfonate. The question of retention of the C7 and V2 terms in the Lee-Wheaton equation is discussed.

A molecular orbital study of sodium sulfate and hydrogen chloride formation from sulfur trioxide, water, and sodium chloride shows no activation barrier, in agreement with recent experimental work of Kohl, Fielder, and Stearns. Two overall steps are found for the process. First, gas-phase water reacts with sulfur trioxide along a pathway involving a linear O-H-O transition state yielding closely associated hydroxyl and bisulfite which rearrange to become a hydrogen sulfate molecule. Then the hydrogen sulfate molecule transfers a hydrogen atom to a surface chloride in solid sodium chloride while an electron and a sodium cation simultaneously transfer to yield sodium bisulfate and gas-phase hydrogen chloride. This process repeats. Both of these steps represent well-known reactions for which mechanisms have not been previously determined.

Residues remaining after drying and curing cotton fabric with either sodium bisulfate or zinc nitrate and N-methylolpyrrolidone, a monofunctional model durable press agent, have been quantitated by high performance liquid chromatography. The residues were identified as pyrrolidone, N-methylolpyrrolidone, N,N′-methylene-bis-2-pyrrolidone, and N,N′-(oxydimethylene)bis-2-pyrrolidone. The two catalysts fixed approximately the same amount of the N-methylolpyrrolidone to cellulose, but generated different ratios of the extractable residues. A comparison of the levels of these residues that are capable of releasing formaldehyde is given. The dominant residue from the NaHSO4 treatment was N-methylolpyrrolidone, while zinc nitrate generated more N,N′-(oxydimethylene)bis-2-pyrrolidone.

Recent epidemiologic studies have emphasized a relationship between alteration in lung function, respiratory symptoms in asthmatics, and elevated levels of sulfate air pollutants. In asthmatics, it has been reported that 1) the more acidic sulfate aerosols, sulfuric acid (H2SO4) and ammonium bisulfate (NH4HSO4), provoked the greatest changes in lung function and 2) a definite exposure-response relationship exists for H2SO4 inhalation. To determine if sulfate aerosol exposure caused increased reactivity to a known bronchoconstrictor, normal and asthmatic subjects inhaled subthreshold doses of carbachol after the following sulfates: H2SO4, NH4HSO4, and sodium bisulfate. A NaCI aerosol served as a control. Exposure times averaged 16 minutes with sulfate concentrations ranging from 100 μ/m3 to 1000 jtg/m3. In normal subjects, prior inhalation of either 1000 yug/m3 H2SO4 or NH4HSO4 significantly potentiated (P < 0.05) the bronchoconstrictor action of carbachol on airway conductance compared to NaCI and carbach...

Under hydrothermal conditions sulfuric acid, sodium bisulfate and sodium sulfate solutions were reduced by dextrose to hydrogen sulfide in order to clarify the origin of sulfide species in hot-springs, geothermal water and ore-forming fluids. At temperatures above 250°C, reduction of sulfuric acid and at above 300°C of sodium bisulfate and sodium sulfate was observed. The reduction rate depends fairly well on the temperatures, pH and sulfate species. The reduction of sulfate seems to be a first-order reaction. Sulfur-isotope compositions of sulfate and hydrogen sulfide were measured in order to disclose isotope effects in the reduction of sulfate. The reduction of sulfuric acid and sodium bisulfate solution results in enrichment of 3S in the hydrogen sulfide and of the heavy isotope into residual sulfate. The fractionation factor in the reduction is independent of the temperature and is seen to be 1.007 to 1.009, in agreement with previously published values.

The herbicides applied as sprays in the present study, with the exception of sodium nitrate and ammonium sulfate, show approximately the same degree of lethality for a given strength, whether applied to plants grown at a mean temperature of 12 degrees or 18 degrees C. Sodium nitrate and ammonium sulfate, on the other hand, when used at a strength destructive to plants grown at 18 degrees C are relatively inocuous to plants grown at 12 degrees C. The rate at which the herbicides used as sprays are dried does not materially affect their toxicity, except in the case of iron sulfate which is approximately twice as active dried slowly as when dried quickly. In practice, a high degree of toxicity per unit weight is desirable. The herbicides used as sprays destroyed 90% of the mustard when used at the strengths indicated below, the substances being listed in decreasing order and assuming average conditions: (...). The figures show that copper sulfate occurs in a group of substances in which the toxic equivalent is rather close, and ranges from 1 to 5, but that iron sulfate occupies a low position in the scale. It has been pointed out that the toxicity of sodium nitrate and ammonium sulfate is affected by the temperature at which the sprayed plants were grown and that the toxicity of iron sulfate is markedly affected by the rate of drying. When we add further that these three substances possess a low toxic value per unit weight, their retention on a list of herbicides useful for the control of mustard seems no longer desirable. we assume that the substances possessing a toxic equivalent of 1 to 5 are all equally satisfactory as herbicides, then a selection from this group will be based upon relative cost, ease of handling, and corrosion of spray machinery. The substances in the group mentioned are not equally corrosive. A bright steel nail partially immersed in them for 6 minutes at room temperature showed the following reaction upon being withdrawn: (...). Four of the sprays most effective for the control of mustard have little or no action on iron. Copper nitrate is too expensive to be given serious consideration at the present time, but copper sulfate and sodium nitrate mixed, sodium bisulfate, and sodium bichromate should be given extensive field trials. With the exception of iron sulfate, the dusts used in the experiments proved very effective. Weight for weight, cyanamide is eight times as effective as kainit ground to pass a 65-mesh sieve, but as it is a nitrogenous fertilizer its use for the control of mustard in oats is generally inappropriate. Kainit, on the other hand, is a potash fertilizer and oats do not lodge following its use. Both kainit and cyanamide must be applied to wetted foliage, but after they have been applied, the rate at which the leaves dry is not important.

The authers made the preliminary research with commercial aluminum (1S and 2S) to comply with the recent requirment for protective and transparent anodized films.Chemically rolished 1S aluminum was anodized in various concentration of oxalic, sulfuric, sulfamic, phosphoric, chromic acid and sodium bisulfate, sodium carbonate, by applying D. C. 1.0A/dm2, for 5min, at 25°C. The variations of reflectivity of polished surfaces and anodized surfaces were measured. Abrasion and corrosion resistance was measured according to specification of JIS.Next the effect of current density were studied with the two typical baths, 10vol% sulfuric acid 5wt% oxalic acid. Further, decrease of reflectivity with anodizing time was measured by both D. C. and A. C. using 1S and 2S which were polished chemically or electrically.

Table OF Contents I, Introduction. II, Physical Extraction: (1) classifying, (2) calcination, (3) hydration, (4) leaching, (5) flotation, (6) crystallization, and (7) miscellaneous physical methods. III, Chemical Extraction: (1) forming carbonates and formates, (A) carbon dioxide, (B) carbonates, and (C) carbon monoxide; (2) chlorine compounds, (A) chlorine, (B) hydrochloric acid, (C) calcium chloride, (D) magnesium chloride, (E) cyclic process, (F) hydrochloric acid manufacture; (3) nitric acid; (4) sulfur compounds, (A) sulfuric acid, (B) sodium sulfate, (C) sodium bisulfate, (D) calcium sulfate, (E) magnesium sulfate, (F) sulfur dioxide, (G) sulfites, and (H) sulfur, sulfides, hydrogen sulfide; (5) ammonia and ammonium salts; (6) alkalis, (A) calcium hydroxide, and (B) sodium hydroxide; (7) organic compounds, (A) acetic acid, and (B) sugar; (8) sea water, (9) electrochemical methods; (10) ion exchange, (11) miscellaneous chemical methods. IV Miscellaneous. V. Conclusions VI, Bibliography VII, Author Index.

A number of studies on sulfur dioxide (SO2) in toxicology and pharmacology have been reported, however spectral properties of SO2 and its derivatives were seldom investigated. We investigated the absorption spectra of SO2, sodium sulfite (Na2SO3), sodium bisulfite (NaHSO3) and sodium metabisulfite (Na2S2O5) in aqueous solution. In the meanwhile, the effects of HCl on spectral properties of SO2 and its derivatives were also investigated. We found that gaseous SO2 in ethanol, n-butyl-alcohol and glycerol had a characteristic absorption peak at 276 nm. Na2S2O5 and NaHSO3 exhibited an absorption peak at 257 nm. Absorption of SO2 at 276 nm was strongly enhanced in the presence of HCl. NaHSO3, Na2SO3 and Na2S2O5 also exhibited absorption at 276 nm with the addition of HCl, which was enhanced with the increase of HCl concentration. Importantly, two conclusions have been reached on the basis of our results. First, we attributed the absorbing power of SO2 to SO2 molecule, rather than hydrated sulfur dioxide. Second, absorption of SO2 strongly enhanced by HCl at 276 nm was due to H+, instead of the formation of a complex SO2Cl-. Primary studies also indicated that NaHSO3 and Na2S2O5 with HCl had a similar effect as SO2 did in rat thoracic aortic rings, which prompted us believe that NaHSO3 and Na2S2O5 with HCl may be acted as a donor of SO2 in biology and other area.

Epidemiologic studies support an association between elevated levels of sulfates and increased symptoms in asthmatics. To determine if these pollutants produce airway responses, 17 asthmatics inhaled the following sulfates: sodium bisulfate, ammonium sulfate, ammonium bisulfate (NH4HSO4), or sulfuric acid (H2SO4) aerosols with an aerodynamic diameter of 0.80 micron at concentrations of 100 micrograms/m3, 450 micrograms/m3, and 1,000 micrograms/m3. A sodium chloride (NaCl) aerosol of similar characteristics, administered by double-blind randomization, served as a control. Subjects breathed these aerosols for a 16-minute period via a mouthpiece. Deposition studies showed 54 to 65% retention of the inhaled aerosols. At the 1,000 micrograms/m3 concentration, the Threshold Limit Value for occupational exposure, H2SO4 and NH4HSO4 inhalation produced significant reductions in specific airway conductance (SGaw) (p less than 0.05) and forced expiratory volume in one second (p less than 0.01) compared with NaCl or pre-exposure values. At the 450 micrograms/m3 concentration, only H2SO4 inhalation produced a significant reduction in SGaw (p less than 0.01). At 100 micrograms/m3, a level 3 to 5 times greater than peak urban levels, no significant change in airway function occurred after any sulfate exposure. These data indicate that asthmatics demonstrate bronchoconstriction after brief exposure to common acidic sulfate pollutants.

Epidemiological studies support an association between elevated levels of sulfates and acute respiratory disease. To determine if these pollutants produce airway hyperreactivity, 16 normal and 17 asthmatic subjects inhaled a control NaCl aerosol and the following sulfates: ammonium sulfate, sodium bisulfate, ammonium bisulfate, and sulfuric acid. A Lovelace generator produced particles with an average MMAD of approx. 1.0 ..mu..m (sigma/sub g/ approx. = 2.0) and concentrations of 0.1 and 1.0 mg/m/sup 3/. By double-blind randomization, all subjects breathed these aerosols for a 16-minute period. To determine if sulfate inhalation caused increased reactivity to a known bronchoconstrictor, all subjects inhaled carbachol following each 16-minute exposure. Before, during, and after exposure, pulmonary function studies were performed. When compared to NaCl, sulfate (1 mg/m/sup 3/) produced significant reductions in airway conductance and flow rates in asthmatics. The two most sensitive asthmatics demonstrated changes even at 0.1 mg/m/sup 3/ sulfate. To a far more significant degree, the bronchoconstrictor action of carbachol was potentiated by sulfates more or less in relation to their acidity in normals and asthmatics.

In order to investigate the effects of sulfuric acid and sulfate salts mist on the respiratory system, guinea pigs were exposed to acute conditions of sulfuric acid, ammonium bisulfate, ammonium sulfate, sodium bisulfate, sodium sulfate of 50mg-SO4/m3, respectively. Animals developed laboured breathing, only when exposed to acidic mist. Furthermore, it was shown that laboured breathing might be related to the acidity of mist. No significant differences in respiratory frequency (f), total respiratory system resistance (T. R. S. R) and pseudo-flow rate (Vpse) were observed between ammonium bisulfate (acidic) exposed group and ammonium sulfate (neutralized salt) exposed group, before laboured breathing development. Histamine content of lung and tracheal tissues were also examined. Tracheal histamine level of ammonium salts exposed group was reduced compared to the control group, but the relationship between laboured breathing development and histamine content was not observed.

The standard colorimetric procedure for thorium was improved by using lanthanum carrier precipitation of thorium fluoride, conversion to sulfate, and colorimetric measurement with thoron. Four types of anion-exchange resins were evaluated using breakthrough capacity, elution volume, and the neptunium-plutonium ratios in both wash solutions and ion-column eluates as criteria, and 100 to 200 mesh Dowex 1 x 4 resin had the most favorable separation characteristics. Use of commercially available aqueous cleaner followed by water and acetone rinses was found to be superior to other techniques for cleaning uranium samples prior to carbon analysis. The substitution of sodium bisulfate for potassium pyrosulfate in the fusion procedure has lead to a more efficient dissolution process for oxide samples undergoing plutonium assay and the determination of uranium impurities. Sealed-capillary differential thermal analysis experiments were performed to assess the relative reactivities of iron, stainless steel, copper, beryllium, aluminum, and plutonium with trichloroethylene, methyl chloroform, and Freon TF. Results obtained by a method involving reduction of plutonium with titanium (III) chloride followed by titration with standard cerium (IV) sulfate solution are comparable to those obtained by an established amperometric-titration method.

To the Editor.— Untoward effects stemming from the mixing of common household cleaners may include acute chlorine poisoning, a fact evidently better known to housewives than to physicians, and emphasized more in ladies' magazines than in scientific publications.1My experience with an elderly woman who developed near fatal pulmonary edema within minutes after cleaning her bathtub with a mixture of two ubiquitous household products prompted this report. Report of a Case.— This 83-year-old diabetic woman was admitted with severe pulmonary edema. Her symptoms had developed abruptly half an hour earlier while she was cleaning her bathtub. Provoked by a stubborn stain unresponsive to soap, she had emptied into the tub about a half gallon of undiluted Clorox (an aqueous solution of 5.25% sodium hypochlorite) and thereupon added most of a can of Sani-Flush, a dry powder for cleaning toilets that contains 80% sodium bisulfate. Almost immediately she experienced intense

Cerium sulfate purified by D2EHPA in Semiworks can be precipitated by adjusting pH to between 1 and 2 in tank 6 with 50% caustic. The solution can then be transferred through tank 1 to tank 67, where sodium bisulfate is added to make the solution 0.5M sulfate. A stoichiometric amount (mole for mole) of 50% caustic is added to just neutralize the sodium bisulfate. The precipitate is digested one hour at 60 C, then filtered.