Silver ammonium nitrate

Boronic acids can be reversibly esterified with resin-bound diols (Figure 3.15). The resulting boronic esters are stable under the standard conditions of amide bond formation, but can be cleaved by treatment with water under acidic or neutral conditions to yield boronic acids. Treatment of the resin-bound boronic esters with alcohols yields the corresponding boronic esters [197]. Resin-bound boronic esters are suitable intermediates for the Suzuki reaction [198], Treatment with H202 leads to the formation of alcohols (Entry 8, Table 3.36), while treatment of resin-bound aryl boronates with silver ammonium nitrate leads to the conversion of the C-B bond into a C-H bond (Entry 14, Table 3.46). 

Arylboronic acids esterified with support-bound 1,2-diols undergo Suzuki reaction with aryl iodides, whereby biaryls are released into solution (Entry 13, Table 3.46). This technique has also been used to prepare (3-turn mimetics by simultaneous macro-cyclization and cleavage from the support [766]. Alternatively, the C-B bond of a resin-bound boronate may be converted to a C-H bond by treatment with aqueous silver ammonium nitrate (Entry 14, Table 3.46). 

Protonolysis in the last step can also be achieved with aqueous silver ammonium nitrate for acid sensitive molecules as in a simple stereoselective route to prostaglandins (Eq. 70) 128>. 

The Zweifel traws-alkene synthesis from dialkyl-1-alkenylboranes involves the hy-droboration of 1-halo-l-alkynes with dialkylborane (Eq. 69) It is of interest that the base produces a transfer with inversion Protonolysis in the last step can also be achieved with aqueous silver ammonium nitrate for acid sensitive molecules as in a simple stereoselective route to prostaglandins (Eq. 70)... 

The cleavage of alkenylboranes may be carried out under non-acidic conditions by converting the alkenylborane into the ate complex with n-BuLi prior to hydrolysis with aqueous NaOH. " Also, alkenylboranes derived from internal alkynes may be protonated under neutral conditions using catalytic amounts of Pd(0Ac)2 in THF or acetoneor with aqueous silver ammonium nitrate [Ag(NH3)2 N03]. ... 

Thexylborane-sodium alcohol-silver ammonium nitrate... 

The dimethyl ethers of hydroquiaones and 1,4-naphthalenediols can be oxidized with silver(II) oxide or ceric ammonium nitrate. Aqueous sodium hypochlorite under phase-transfer conditions has also produced efficient conversion of catechols and hydroquiaones to 1,2- and 1,4-benzoquiaones (116), eg, 4-/-butyl-l,2-ben2oquinone [1129-21-1] ia 92% yield. 

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. 

Thiosulphate as Ag2S. Add a slight excess of 0.1 M silver nitrate solution to the cold, almost neutral, thiosulphate solution. Heat at 60 °C in a covered vessel and, after cooling, filter and wash the silver sulphide precipitate with ammonium nitrate solution, water and finally with ethanol. Dry at 110°C and weigh as Ag2S (Section 11.76). 

Cl2, ammonium nitrate on Clayfen, Oxone on wet alumina, silver nitrate and iodine,2,3-dichloro-5,6-dicyano -1,4-benzoquinone (DDQ) in acetonitrile... 

Among other oxidizing agents that have been used to accomplish the conversion of ArCHs to ArCHO are ceric ammonium nitrate, ° ceric trifluoroa-cetate, and silver(II) oxide.Oxidation of ArCHa to carboxylic acids is considered at 19-11. 

Metal oxosalts MRH Ammonium nitrate 8.79/69, potassium nitrate 7.57/58, silver nitrate 6.95/70, barium sulfate 4.27/71, copper(II) sulfate 7.03/58, sodium sulfate 5.86/60, potassium carbonate, 3.10/66. 

Yellow phosphorus ignites in molten ammonium nitrate, and mixtures of phosphorus with ammonium nitrate, mercuiy(I) nitrate or silver nitrate explode on impact. Red phosphorus is oxidised vigorously when heated with potassium nitrate [1]. During development of new refining agents for aluminium manufacture, a mixture containing red phosphorus (16%) and sodium nitrate (35%) was being pressed into 400 g tablets. When the die pressure was increased to 70 bar, a violent explosion occurred [2],... 

Iodoform Iodomethane Iron disulfide Isothiourea Ketones Lactonitrile Lead Acetone, lithium, mercury(II) oxide, mercury(I) chloride, silver nitrate Silver chlorite, sodium Water, powdered pyrites Acrylaldehyde, hydrogen peroxide, nitric acid Aldehydes, nitric acid, perchloric acid Oxidizing materials Ammonium nitrate, chlorine trifluoride, hydrogen peroxide, sodium azide and carbide, zirconium, oxidants... 

Production of ammonia (NH ) Anhydrous (dry) ammonia is the fifth most produced industrial compound. The Haber-Bosch process uses steam on hot coke, which is mostly used in South Africa. In the United States, it is mostly produced from partial combustion of natural gas (methane) or by combining several gases using steam. Other methods use coke-oven gas, refinery gas (mostly methane), or even solar energy. Ammonia is toxic if inhaled and has a high pH value when mixed with water (hydration) to form ammonium hydroxide (NH OH), which has many uses, including as a household cleaner. Ammonia forms many compounds, including ammonium nitrate in fertilizer, rocket fuel, and explosives. Ammonia is also explosive when mixed with mercury or silver or when mixed as part of nitrocellulose. 

Partial oxidation of 158 by bromine yields bromine-free 159 together with mono-, di-, and tribromo derivatives. Other useful reagents are nitrous acid (54JCS286) or the one-electron oxidants silver acetate (in substoichio-metric quantity) and cerium(IV) ammonium nitrate (only for the methyl ether of 158 86BCJ511). 

A mixture of silver nitrite and iodine reacts with alkenes to give jS-nitroalkyl iodides, and therefore, provides a convenient route to a-nitroalkenes. Treatment of alkenes with ammonium nitrate and trifluoroacetic anhydride in the presence of ammonium bromide, followed by... 

Nitric acid has a 65 25 fertilizer explosive end use ratio. The production of ammonium nitrate makes up nearly all of these two uses. The other 10% is made into miscellaneous compounds adipic acid, nitroglycerin, nitrocellulose, ammonium picrate, trinitrotoluene, nitrobenzene, silver nitrate, and various isocyanates. 

Ammonium nitrate, Aluminum powder, Polyester resin, Ammonium bichromate, Charcoal powder Silver perchlorate, 5-Aminotetrazole, Perchloric acid Glycerin, Potassium permanganate Potassium permanganate, Glycerin Silver nitrate, Nitric acid, Ethanol Silver nitrate, Nitric acid, Ethanol... 

Diammino-silver Nitrate, [Ag(NII3)2]N03.—When aqueous ammonia is added to a solution of silver nitrate until the precipitate first formed redissolves and the solution is evaporated, a crystalline substance separates of composition [Ag(NH3)2]N03. The compound can also be formed by dissolving silver oxide in an anunoniaeal solution of ammonium nitrate, or by dissolving silver nitrate in benzonitrile and passing ammonia gas into the solution.2... 

Diammino-silver nitrate forms glistening rhombic or prismatic crystals which blacken on exposure to light. It is fairly stable, and may be heated to 100° C. without loss of ammonia. Further heating causes it to decompose, and finally to melt with evolution of nitrogen and ammonia, leaving a residue of metallic silver and ammonium nitrate. It is soluble in water, but partial dissociation takes place so that the solution is alkaline in reaction, and it therefore yields a precipitate of silver chloride and soluble chlorides. Certain of the metals—for example, zinc, cadmium, and copper—quickly reduce the ammine in solution to metallic silver. 

Chretien and Woringer [34] described the preparation of silver cyanamide from calcium cyanamide by the action of silver nitrate and also described its explosive properties. Montagu-Pollock [35] described a method for growing large crystals of the salt from its aqueous solution in the presence of ammonium nitrate, ammonia and a surface active agent. Bowden and Montagu-Pollock [36] and Montagu-Pollock [35] studied the slow decomposition of the crystals when heated at temperatures from 150 to 360°C. The course of decomposition was studied by electron microscope. 

Chlorides. — On dissolving 1 gm. of ammonium nitrate in 10 cc. of water, and adding a few drops of nitric acid, followed by silver nitrate solution, the liquid should remain unchanged. 

Silver Arsenates.—Silver nitrate reacts with solutions of arsenic acid or arsenates, giving a chocolate-coloured precipitate of silver orthoarsenate, Ag3As04, containing a small proportion of silver nitrate, possibly in solid solution.1 The adsorption of silver nitrate is prevented by the presence of ammonium nitrate. The precipitation is incomplete in acid solution.2 The orthoarsenate cannot be completely dried except by fusion. 

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