Ammonium Acetate Citrate Solution

Synonym Ammonia Water Amfbnioformaldehyde Ammonium Acetate Ammonium Acid Fluoride Ammonium Amidosulfonate Ammonium Amidosulphate Ammonium Benzoate Ammonium Bicarbonate Ammonium Bichromate Ammonium Bifluoride Ammonium Carbonate Ammonium Chloride Ammonium Citrate Ammonium Citrate, Dibasic Ammonium Decaborate Octahydrate Ammonium Dichromate Ammonium Disulfate-Nickelate (II) Ammonium Ferric Citrate Ammonium Ferric Oxalate Trihydrate Ammonium Ferrous Sulfate Ammonium Fluoride Ammonium Fluosilicate Ammonium Formate Ammonium Gluconate Ammonium Hydrogen Carbonate Ammonium Hydrogen Fluoride Ammonium Hydrogen Sulfide Solution Ammonium Hydroxide Ammonium Hypo Ammonium Hyposulfite Ammonium Iodide Ammonium Iron Sulfate Ammonium Lactate Ammonium Lactate Syrup Ammonium Lauryl Sulfate Ammonium Molybdate Ammonium Muriate Ammonium Nickel Sulfate Ammonium Nitrate Ammonium Nitrate-Urea Solution Ammonium Oleate... 

Many of the classical methods grew out of the earliest synthesis of imidazole, which was achieved in 1858 by Debus [1] when he allowed glyoxal, formaldehyde and ammonia to react together. Although the earliest modifications of this method used a-diketones or a-ketoaldehydes as substrates [2, by the 1930s it was well established that a-hydroxycarbonyl compounds could serve equally well, provided that a mild oxidizer (e.g. ammoniacal copper(ll) acetate, citrate or sulfate) was incorporated [3. A further improvement was to use ammonium acetate in acetic acid as the nitrogen source. All of these early methods have deficiencies. There are problems associated with the synthesis of a wide range of a-hydroxyketones or a-dicarbonyls, yields are invariably rather poor, and more often than not mixtures of products are formed. There are, nevertheless, still applications to the preparation of simple 4-alkyl-, 4,5-dialkyl(diaryl)- and 2,4,5-trialkyl(triaryl)imidazoles. For example, pymvaldehyde can be converted quite conveniently into 4-methylimidazole or 2,4-dimethylimidazole. However, reversed aldol reactions of pyruvaldehyde in ammoniacal solution lead to other imidazoles (e.g. 2-acetyl-4-methylimidazole) as minor products [4]. Such... 

Figures 1 and 2 show relationships among concentrations of U and selected major and trace elements in spinach leaves and petioles, respectively. It is noteworthy that concentrations of U in spinach were significantly positively correlated (p<0.01) with concentrations of Fe and A1 in both leaves and petioles. These relationships suggested that the absorption and transport processes of U in spinach could be related to those of Fe and Al, as was also suggested by Kametani et al. who showed that plants with higher Fe concentrations tended to absorb more U. Less U was extracted by 1 mol L ammonium acetate solution from soil (Table 2), meaning that U in soil was less available to plants. Spinach favours neutral-to-weak alkaline conditions and has the ability to acquire insoluble mineral nutrients such as Fe under neutral-to-alkaline conditions. Helal et al. compared spinach and beans with respect to the ability of the root to uptake Fe and found that spinach root absorbed Fe more efficiently. The differences in Cu, Zn, and Cd uptake by two spinach cultivars were attributed to different abilities to exude oxalate, citrate, and malate from root l The application of organic acids to soil facilitated the phytoextraction of U by hyperaccumulator plants thus, those root exudates could induce U dissolution from soil. Since part of U is associated with Fe and Al minerals in the soil it was likely that the absorption of U was accompanied by Fe and Al absorption, possibly triggered by the secretion of protons or organic acids to solubilise Fe and Al from soil.

Primer Removal 1 pi of a 0.5 M acetic add solution was added to the processed primer extension reaction resulting in a reaction pH < 7. Then 2 pi of phosphodiesterase II that was previously dialysed against ammonium citrate (0.1 M, pH 6.0) were added and the reaction was incubated for 1 h at 37°C. 

Aminobiphenyl, 4-Aminocarb Aminopyridine, 4-Amiton Amitrole Ammonia Ammonia solutions Ammonium acetate Ammonium benzoate Ammonium bicarbonate Ammonium bisulphite Ammonium carbamate Ammonium carbonate Ammonium chlorate Ammonium chloride Ammonium chromate Ammonium citrate Ammonium dichromate Ammonium fluoride Ammonium hydrogen fluoride Ammonium hydrogen sulfate Ammonium hydroxide Ammonium nitrate Ammonium nitrate fertihzers Ammonium oxalate Ammonium phosphates Ammonium picrate Ammonium sulfamate Ammonium sulfate Ammonium sulfide Ammonium sulfite Ammonium tartrate Amyl acetate... 

For Bi, B2, B3, and Bg, a ground sample (1 g) was autoclaved with HCl (120° C, 30 min), cooled, diluted to known volume with aqueous ammonium acetate, vortexed, and centrifuged. The filtered supernatant was injected onto the LC column. For B5, a ground sample (4 g), was treated with acetate buffer (pH = 5.6) and autoclaved (121° C, 15 min), cooled, diluted to known volume with aqueous ammonium formate, vortexed, and centrifuged. The filtered supernatant was injected onto the LC column. For B9, ground sample (2.5 g) was mixed with a sodium phosphate—sodium citrate/ ascorbate buffer (pH = 8), heated, cooled, and incubated with papain and di-a-amylase (40°C, 2 hr). The solution was diluted to known volume with aqueous ammonium formate, vortexed, and centrifuged. 

Werde K.V., Mondelaers D., Vanhoyland G., Nelis D., Van Bael M.K., Mullens J., Van Poucke L.C., Van der Veken B., Desseyn H.O. Thermal decomposition of the ammonium zinc acetate citrate precursor for aqueous chemical solution depositions ofZnO.J. Mater. Sci.2002 37 81-88... 

Complexing agents, which act as buffers to help control the pH and maintain control over the free metal—salt ions available to the solution and hence the ion concentration, include citric acid, sodium citrate, and sodium acetate potassium tartrate ammonium chloride. Stabilizers, which act as catalytic inhibitors that retard the spontaneous decomposition of the bath, include fluoride compounds thiourea, sodium cyanide, and urea. Stabilizers are typically not present in amounts exceeding 10 ppm. The pH of the bath is adjusted. 

The clear solution, obtained by centrifuging a solution of the oxide in aqueous ammonia which had been treated with silver nitrate until precipitation started, exploded on two occasions after 10-14 days storage in closed bottles in the dark. This was ascribed to slow precipitation of amorphous silver imide, which is very explosive even when wet [1], When silver oxide is dissolved in ammonia solution, an extremely explosive precipitate (probably Ag3N4) will separate. The explosive behaviour is completely inhibited by presence of colloids or ammonium salts (acetate, carbonate, citrate or oxalate). Substitution of methylamine for ammonia does not give explosive materials [2],... 

Distilled water at 125F/52C, 500.0ml Ferric ammonium citrate, 8.0g Potassium ferricyanide, 8.0 g Acetic acid, 28% solution, 265.0ml Distilled water to make 1.0 liter... 

The resulting salt, whilst readily soluble in dilute mineral acids, is insoluble in cold acetic acid, phosphoric acid, and sodium phosphate. It is slightly soluble in citric and tartaric acid solutions, and readily dissolves m neutral aqueous ammonium citrate, yielding a green solution with a brownish tint.3 The salt is insoluble in water, but hot water hydrolyses it, and boiling with excess of ammonia solution converts it into a mixture of ferric hydroxide 4 and ferric phosphate, or if the ammonia is present in great excess the ferric phosphate may be entirely decomposed. Thus —... 

The dialyzed enzyme solution was now subjected to a repetition of the preceding procedures admixture of suflBcient calcium phosphate gel to adsorb protein but leave the enzyme in solution centrifugation and addition of more gel to the supernatant to adsorb the enzyme elution of the enzyme from the gel with a mixture of 0.15 M acetate and 0.015 M citrate at pH 4.5 addition of solid ammonium sulfate to the eluate to 55% saturation and precipitation of the enzyme. At this stage, the purifications ranged from 650- to 1100-fold with a recovery of approximately 20-30% of the activity present in the crude red cell hemolysate. Solution of this precipitate, dialysis treatment with solid ammonium sulfate and collection of the precipitate appearing between 40 and 55% saturation yielded a preparation that represented a 1500-fold purification. The preparations were stable when left sedimented in the ammonium sulfate solution. 

The reactions were monitored by thin layer chromatography (silica TLC plates developed with n-butanol/acetic acid/H20, 1.5 1 1 or 1 1 1) and napthoresorcinol staining (0.2% w/v in 96% ethanol/4% sulfuric acid 100°C). For mass spectrometry (MALDI-TOF MS), the matrix solution (50 mg/ml 6-aza-2-thiothymine in 50% acetonitrile, 49.9% water, 0.1% trifluoroacetic acid, 10 mM ammonium citrate) was mixed 1 1 with the samples containing 0.1 pg/pl oligosaccharide in water, spotted onto the target plate, and vacuum dried. The samples were analyzed in the negative ion, reflectron mode on a Voyager Elite DE mass spectrometer. 

---