Ammonium Oxalate Hydrate

Chemical Designations - Synonyms Ammonium Oxalate Hydrate Diammonium Oxalate Oxalic Acid, Diammonium Salt Chemical Formula (NH,)2C204 H20. 

Ammonium Oxalate Ammonium Oxalate Hydrate Ammonium Pentaborate Ammonium Pentaborate Tetrahydrate Ammonium Pentachlorozincate Ammonium Perchlorate Ammonium Peroxydisulfate Ammonium Persulfate Ammonium Phosphate Ammonium Phosphate, Dibasic Ammonium Rhodanate Ammonium Rhodanide Ammonium Silicofluoride Ammonium Stearate Ammonium Sulfamate Ammonium Sulfate Ammonium Sulfhydrate Solution Ammonium Sulfide Ammonium Sulfide Solution Ammonium Sulfite Ammonium Sulfocyanate Ammonium Sulfocyanide Ammonium Tartrate Ammonium Thiocyanate Ammonium Thiosulfate Ammonium Zinc Chloride Amorphous Phosphorus AMS... 

Vulcan pyrolyzed at 1000°C in acetonitrile-enriched Ar for 2 h, weight gain 65% phenanthroline -l- ammonium oxalate hydrate precursor... 

Ammonium Oleate Ammonium Oxalate Ammonium Oxalate Hydrate Ammonium Pentaborate Ammonium Pentaborate Tetrahydrate... 

Sinsheimer and Poswalk determined water in several matrices [14]. Solid samples were analyzed for hydrous and anhydrous forms of strychnine sulfate, sodium tartrate, and ammonium oxalate mixed with KC1 and compressed into disks containing 100 mg KC1 and 25 mg of drug. The water band at 1940 nm was seen in the hydrates for some samples. 

A solution of 0.711 g. (0.005 mol) of ammonium oxalate 1-hydrate in 20 ml. of boiUng water is added in 1-ml. portions with continuous stirring to 4.42 g. (0.010 mol) of ammonium hexachloroiridate(IV)f contained in a 100-ml. round-bottomed flask Caution. Effervescence). The dark reddish brown solution is warmed on the steam bath for 10 minutes to ensure complete reduction. J After the solution has cooled to room temperature, 8.06 ml. (7.91 g. 0.100 mol) of pyridine (density, 0.892) dissolved in 3.33 ml. 

The compound is only slightly soluble in water and dilute acids but is soluble in warm concentrated hydrochloric acid to form a dark green solution. It can be reprecipitated by cooling or by diluting such a solution. Concentrated nitric acid effects oxidation to the uranyl salt. With solutions of the alkali carbonates or hydrogen carbonates, uranium(IV) hydroxide is formed. With an excess of a solution of potassium carbonate and by atmospheric oxidation, potassium uranyl carbonate results. Uranium(IV) oxalate 6-hydrate is also soluble in solutions of alkali and ammonium oxalates to form the tetraoxalatouranate(IV)... 

Carboxylic acids and their salts, as well as alcohols and alkoxides, are common ligands and this has limited their use as reductants in synthesis. Potassium hexachloroplatinate(IV), for example, is reduced by ammonium oxalate.63 Che and coworkers 4 have shown that the reaction of aqueous solutions of ascorbic acid with the complex, [Ru02(NH3)4]Cl2, in the presence of NaX (X = Cl, I, CNS) yields the complexes, [RuX2(NH3)4]X. The reduction of a mixture of hydrated ruthenium(III) chloride and ruthenium(IV) chloride by glucose or ascorbic acid in water in the presence of 2,2 -bipyridyl results in the formation of [Ru(bipy)3]Cl2 7H20. 5 Additionally, the reduction of the [Tc04] anion by gluconic acid has been studied. ... 

Dihydrazinium oxalate is prepared by reacting hydrazine hydrate with ammonium oxalate and the reaction can be written as follows ... 

Reaction of Metal Powder with Ammonium Oxalate in Hydrazine Hydrate... 

When a metal powder M° is added to a solution of ammonium oxalate in hydrazine hydrate it dissolves with the evolution of gases like hydrogen and ammonia, together with liberation of heat. The product obtained is... 

When an aqueous solution of the metal salt of Fe, Co, and Ni is mixed with ammonium oxalate in hydrazine hydrate, the corresponding metal oxalate hydrazines are precipitated ... 

Similar to the above, mixed metal oxalate hydrazines can be prepared with cobalt being the common metal. Stoichiometric quantities of the respective metal powders of magnesium and nickel are dissolved in a solution of ammonium oxalate in hydrazine hydrate. It takes a few hours for the metal powders to completely disperse into the solution. After their complete dissolution, alcohol is added to precipitate out the complex. The precipitate is further washed with alcohol and diethyl ether [18] ... 

If the metallisable dye is insoluble in water, a miscible solvent such as ethanol or ethylene glycol may be added. Polar solvents such as formamide or molten urea have sometimes been preferred. It is likely that such solvents will preferentially displace water molecules and coordinate with the chromium (III) ion as the first step in the reaction. If colourless organic chelates of chromium, such as those derived from oxalic or tartaric acid, are used instead of or in addition to hydrated chromium (III) salts, the difficulty of replacing the strongly coordinated water molecules in the first stage of the reaction is eliminated. In this way the initial reaction can be carried out at high pH without contamination by the precipitation of chromium hydroxide. Use of the complex ammonium chromisalicylate (5.12) in this connection should also be noted (section 5.4-1). 

The effect of the hydration radius of these cations is very important, and mobilities are sometimes very close or the same as for potassium and ammonium. For this reason, a complexing agent is added to the buffer. Several complexing agents such as a-hydroxyiso-butyric acid (HIBA), 18-crown-6, phthalic, malonic, tartaric, lactic, citric, oxalic, or glycolic acid may be used. 

Fifteen grams of Mohr s salt (ferrous ammonium sulfate 6-hydrate) are dissolved In 50ml of water containing one ml of ZM sulfuric acid. The solution is stirred well while it is mixed with 7.5g of oxalic acid 2-hydrate in 75ml of water. The mixture, which now contains a yellow precipitate of ferrous oxalate, is carefully [CAUTION bumping ] heated to the boiling point, allowed to settle, and cooled somewhat The supernatant liquid is decanted and the solid washed once by decantation with about 50ml of hot water. 

Although the alkali-metal ions are hydrated in aqueous solution, only the lithium and sodium ions retain their water of hydration in their solid salts. Hydrated potassium salts are known, but the water in such hydrates is generally anion water (Chap. 4) the ammonium ion often forms hydrated salts with the same anions as does the potassium ion (carbonate, oxalate, sulfite). 

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