Ammonium acid formate chloride

Qualitative. The classic method for the quaUtative determination of silver ia solution is precipitation as silver chloride with dilute nitric acid and chloride ion. The silver chloride can be differentiated from lead or mercurous chlorides, which also may precipitate, by the fact that lead chloride is soluble ia hot water but not ia ammonium hydroxide, whereas mercurous chloride turns black ia ammonium hydroxide. Silver chloride dissolves ia ammonium hydroxide because of the formation of soluble silver—ammonia complexes. A number of selective spot tests (24) iaclude reactions with /)-dimethy1amino-henz1idenerhodanine, ceric ammonium nitrate, or bromopyrogaHol red [16574-43-9]. Silver is detected by x-ray fluorescence and arc-emission spectrometry. Two sensitive arc-emission lines for silver occur at 328.1 and 338.3 nm. 

Plumes from biomass burning can also have unique signatures. For example, organics, ammonium, potassium, sodium, nitrate, nitrite, sulfate, chloride, phosphate, elemental carbon, and the anions of organic acids (formate, acetate, oxalate, etc.) have all been measured in particles in the plumes from burning vegetation (e.g., see Cofer et al., 1988 Andreae et al., 1988 and Artaxo et al., 1994). 

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... 

A considerable increase in conversion of Morwell brown coal occurs when dilute sodium hydroxide was used in place of water (see Table VIII and Figure 8). Dilute sodium carbonate and formate had a similar effect (see Table VIII) as did n-pentylamine (see Table IX), but no improvement was found with dilute hydrochloric acid, sodium chloride or ammonium hydroxide nor with 20% phenol/80% water and methanol/water mixtures. The conversion and extract yield increases with the molarity of the sodium hydroxide (Figure 8). 

Color reactions Boric acid (hydroxyquinones). Dimethylaminobenzaldehyde (pyrroles). Ferric chloride (enols, phenols). Haloform test. Phenylhydrazine (Porter-Silber reaction). Sulfoacetic acid (Liebermann-Burchard test). Tetranitromethane (unsaturation). Condensation catalysts /3-Alanine. Ammonium acetate (formate). Ammonium nitrate. Benzyltrimethylammonium chloride. Boric acid. Boron trilluoride. Calcium hydride. Cesium fluoride. Glycine. Ion-exchange resins. Lead oxide. Lithium amide. Mercuric cyanide. 3-Methyl-l-ethyl-2-phosphoiene-l-oxlde. 3-Methyl-1-phenyi-3-phoipholene-1-oxide. Oxalic acid. Perchloric acid. Piperidine. Potaiaium r-butoxIde. Potassium fluoride. Potassium... 

The most convenient method for preparing 2,1 -benzisoxazolin-3-ones is by zinc-ammonium acetate (or chloride) reduction of o-nitrobenzoates.248,249 The resulting o-hydroxyaminoesters undergo rapid acid- or base-catalyzed intramolecular displacement of alcohol with concomitant formation of the benzisoxazolin-3 -one. 

AMMONIUM NITRATE (6484-52-2) A strong oxidizer. An ingredient in dynamite. Violent reaction and/or the formation of explosive mixtures with hot water, reducing agents, combustible materials, organic materials, ammonium dichromate, barium chloride, barium nitrate, charcoal, cyanoguanidine, phosphorus, potassium chromate, potassium dichromate, potassium nitrate, potassium permanganate, sodium chloride, finely divided metals. Forms explosive or heat- and shock-sensitive compounds with acetic acid, alkali metals (potassium, sodium, etc.), ammonia, nitric acid, sodium hypochlorite, sulfur, urea. At elevated temperatures, contained or confined material may explode violently. 

Directions (a) Saturate 10 c.c. of ammonium hydroxide solution with sodium chloride in a large test tube by adding an excess of the salt, shaking the mixture vigorously, and then filtering out the undissolved remainder. Set up a generator for carbon dioxide as in Experiment 38 6, and pass the gas into the solution until a heavy precipitate is obtained. Filter out the precipitate and dry it by pressing it between sheets of filter paper. (1) What is this substance (2) Write two equations for the reactions which takes place and cause the formation of the precipitated substance. (3) What caused the second reaction to take place (4) Why is not a solution of ammonium acid carbonate used to produce this reaction with a solution of sodium chloride ... 

Analytical Characters.—(1.) Add a little alcoholic solution of potash and 3--3 drops of anilin and warm a disagreeable odor resembling that of witch-hazel, is produced. (3.) Vapor of CHCls,. when passed through a red-hot tube, is decomposed with formation of HCl and Cl, the former of -which is recognized by the pro duction of a white ppt., soluble in ammonium hydroxid, in ai> acid solution of silver nitrate. This test does not afford reliable results when the substance tested contains a free acid and chlorids. (3.) Dissolve about 0.01 gin. of /3 naphthol in a small quantity of KHO solution, warm, and add the suspected liquid a blue color is produced. (4.) Add about 0.3 grm. resorcin in solution, and 3 gtts. NaHO solution and boil strongly. In the presence of CHCli or of chloral a yellowish-red color is produced, and the liquid exhibits a beautiful yellow-green fluorescence. 

Chloride ions, when added in excess as hydrochloric acid, sodium chloride, or ammonium chloride, act to solubilize the relatively insoluble cuprous chloride and thereby maintain stable etch rates. The complex ion formation can be shown as... 

The enantioselective ester syntheses from acid salts, chlorides and anhydrides with racemic alkyl halides, catalysed by optically active polyaminesalmost certainly proceed via in situ formation of chiral ammonium salts, and therefore fall within the scope of phase transfer catalysts. Though the optical yields obtained are low, the work is important because it explores the use of polyamine species with a potential chirality derived from the polymerization of optically active oxazolines, and as such is again a novel approach. 

Notice that salt formation, though very favorable, is nonetheless reversible. Upon heating, a slower but thermodynamically favored reaction between the acid and the amine can take place. The acid and the amine are removed from the equilibrium, and eventually salt formation is completely reversed. In this second mode of reaction, the nitrogen acts as a nucleophile and attacks the carbonyl carbon. Completion of an addition-elimination sequence leads to the amide. Although it is convenient, this method suffers from the high temperatures required to reverse ammonium carboxylate formation. Therefore, better procedures rely on the use of activated carboxylic acid derivatives, such as acyl chlorides (Chapter 20). 

A simpler nonphosgene process for the manufacture of isocyanates consists of the reaction of amines with carbon dioxide in the presence of an aprotic organic solvent and a nitrogeneous base. The corresponding ammonium carbamate is treated with a dehydrating agent. This concept has been apphed to the synthesis of aromatic and aUphatic isocyanates. The process rehes on the facile formation of amine—carbon dioxide salts using acid haUdes such as phosphoryl chloride [10025-87-3] and thionyl chloride [7719-09-7] (30). 

The ammonium sulfate and sodium chloride are simultaneously dissolved, preferably ia a heel of ammonium chloride solution. The sodium chloride is typically ia excess of about 5%. The pasty mixture is kept hot and agitated vigorously. When the mixture is separated by vacuum filtration, the filter and all connections are heated to avoid cmst formation. The crystalline sodium sulfate is washed to remove essentially all of the ammonium chloride and the washings recycled to the process. The ammonium chloride filtrate is transferred to acid resistant crystallising pans, concentrated, and cooled to effect crystallisation. The crystalline NH Cl is washed with water to remove sulfate and dried to yield a product of high purity. No attempt is made to recover ammonium chloride remaining ia solution. The mother Hquor remaining after crystallisation is reused as a heel. 

Reactions of the Side Chain. Benzyl chloride is hydrolyzed slowly by boiling water and more rapidly at elevated temperature and pressure in the presence of alkaHes (11). Reaction with aqueous sodium cyanide, preferably in the presence of a quaternary ammonium chloride, produces phenylacetonitrile [140-29-4] in high yield (12). The presence of a lower molecular-weight alcohol gives faster rates and higher yields. In the presence of suitable catalysts benzyl chloride reacts with carbon monoxide to produce phenylacetic acid [103-82-2] (13—15). With different catalyst systems in the presence of calcium hydroxide, double carbonylation to phenylpymvic acid [156-06-9] occurs (16). Benzyl esters are formed by heating benzyl chloride with the sodium salts of acids benzyl ethers by reaction with sodium alkoxides. The ease of ether formation is improved by the use of phase-transfer catalysts (17) (see Catalysis, phase-thansfer). 

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