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Ammonium nitrate is a chemical compound with the formula NH 4 NO 3. It is a white crystalline salt consisting of ions of ammonium and nitrate . It is highly soluble in water and hygroscopic as a solid, but does not form hydrates .
Enthalpy change of solution in water at 25 °C for some selected compounds [2] Compound ΔH o in kJ/mol; hydrochloric acid: −74.84 ammonium nitrate +25.69 ammonia: −30.50 potassium hydroxide: −57.61 caesium hydroxide: −71.55 sodium chloride +3.87 potassium chlorate +41.38 acetic acid: −1.51 sodium hydroxide: −44.50
Solutions of urea and ammonium nitrate in water (UAN) are commonly used as a liquid fertilizer. In admixture, the combined solubility of ammonium nitrate and urea is so much higher than that of either component alone that it gives a stable solution with a total nitrogen content (32%) approaching that of solid ammonium nitrate (33.5%), though ...
Ammonia solution, also known as ammonia water, ammonium hydroxide, ammoniacal liquor, ammonia liquor, aqua ammonia, aqueous ammonia, or (inaccurately) ammonia, is a solution of ammonia in water. It can be denoted by the symbols NH 3 (aq). Although the name ammonium hydroxide suggests a salt with the composition [NH + 4][OH −
Ammonium nitrite is a chemical compound with the chemical formula [NH 4]NO 2. It is the ammonium salt of nitrous acid. It is composed of ammonium cations [NH 4] + and nitrite anions NO − 2. It is not used in pure isolated form since it is highly unstable and decomposes into water and nitrogen, even at room temperature.
The idea that oxidation of ammonia to nitrate is in fact a biological process was first given by Louis Pasteur in 1862. [22] Later in 1875, Alexander Müller, while conducting a quality assessment of water from wells in Berlin, noted that ammonium was stable in sterilized solutions but nitrified in natural waters. A.
Nitrate is a polyatomic ion with the chemical formula NO − 3. Salts containing this ion are called nitrates. Nitrates are common components of fertilizers and explosives. [1] Almost all inorganic nitrates are soluble in water. An example of an insoluble nitrate is bismuth oxynitrate.
Most simple ammonium salts are very soluble in water. An exception is ammonium hexachloroplatinate, the formation of which was once used as a test for ammonium. The ammonium salts of nitrate and especially perchlorate are highly explosive, in these cases, ammonium is the reducing agent. In an unusual process, ammonium ions form an amalgam.