Calcium nitrate fertilizer

Nitrophosphate fertilizer is made by digesting phosphate rock with nitric acid. This is the nitrophosphate route leading to NPK fertilizers as in the mixed-acid route, potassium and other salts are added during the process. The resulting solution is cooled to precipitate calcium nitrate, which is removed by filtration methods. The filtrate is neutralized with ammonia, and the solution is evaporated to reduce the water content. The process of prilling may follow. The calcium nitrate filter cake can be further treated to produce a calcium nitrate fertilizer, pure calcium nitrate, or ammonium nitrate and calcium carbonate. 

Instead of using sulfuric or phosphoric acid, nitric acid can be used to treat the phosphate lock to produce calcium nitrate fertilizer. Instead of neutralizing phosphoric acid with calcium which is useless, ammonia can be used to give ammonium phosphate, hence, two fertilizing elements. 

Calcium nitrate fertilizer, controlled-release Oxamide fertilizer, soluble Potassium phosphate fertilizer, specialty Potassium tripolyphosphate fertilizer, trace element Cobalt fiber... 

Nitric acid acidulation of phosphate rock produces phosphoric acid, together with dissolved calcium nitrate. Separation of the phosphoric acid for use as an intermediate in other fertilizer processes has not been developed commercially. Solvent extraction is less effective in the phosphoric—nitric system than in the phosphoric—hydrochloric system. Instead, the nitric acid acidulate is processed to produce nitrophosphate fertilizers. 

Some commonly used primary nutrient fertilizers are incidentally also rich sources of calcium. Ordinary superphosphate contains monocalcium phosphate and gypsum in amounts equivalent to all of the calcium originally present in the phosphate rock. Triple superphosphate contains soluble monocalcium phosphate equivalent to essentially all the P2 5 product. Other fertilizers rich in calcium are calcium nitrate [10124-37-5] calcium ammonium nitrate [39368-85-9] and calcium cyanamide [156-62-7]. The popular ammonium phosphate-based fertilizers are essentially devoid of calcium, but, in view of the natural calcium content of soils, this does not appear to be a problem. 

Calcium. Calcium is the fifth most abundant element in the earth s cmst. There is no foreseeable lack of this resource as it is virtually unlimited. Primary sources of calcium are lime materials and gypsum, generally classified as soil amendments (see Calcium compounds). Among the more important calcium amendments are blast furnace slag, calcitic limestone, gypsum, hydrated lime, and precipitated lime. Fertilizers that carry calcium are calcium cyanamide, calcium nitrate, phosphate rock, and superphosphates. In addition, there are several organic carriers of calcium. Calcium is widely distributed in nature as calcium carbonate, chalk, marble, gypsum, fluorspar, phosphate rock, and other rocks and minerals. 

AMMONIUM NITRATE FERTILIZER, uith CALCIUM CARBONATE 2068 ... 

CAN [calcium ammonium nitrate] A process for making calcium ammonium nitrate fertilizer. Developed by BASF (hence the alternative process name BASF/CAN) and engineered by Uhde. 

Cemy A process for crystallizing calcium nitrate tetrahydrate, used as a fertilizer, by cooling the saturated solution with drops of cold petroleum. 

Calcium magnesium acetate, 1 127 Calcium magnesium carbonate, health and safety factors related to, 15 74 Calcium monosulfoaluminate, 5 477t Calcium montmorillonite, 6 686, 696 structure and composition, 6 668-669 Calcium nitrate, in nitrogen fertilizers,... 

Calcium nitrate [Ca(NO )2] is known as Norwegian saltpeter. It is a strong oxidi2er (because of the NOj) that is flammable in the presence of organic materials (such as hands). It explodes when given a hard shock. It is used in fireworks, matches, and fertilizers. 

Nitric acid is one of the most important industrial chemicals in the world. Its largest use is in the fertdizer industry for producing various nitrate fertd-izers. Such fertilizers include ammonium-, sodium-, potassium-, and calcium nitrates. Other major apphcations of nitric acid are in making nitrates and nitrooganics for use in explosives, gunpowder, and fireworks. Ammonium nitrate, nitroglycerine, nitrocellulose, and trinitrotoluenes are examples of such explosives, while barium and strontium nitrates are used in fireworks. 

The expl may also be agitated at room or elevated temp with hydroxides of alkali or alka-line earth metals (pref calcium hydroxide) with or without application of pressure (Ref 4) [See also Ammonium Nitrate, Fertilizer Grade (FGAN) in Vol 1 of Encycl, p A364]... 

To grow sufficient crops, you will need large amounts of calcium phosphate fertilizer. You can make this compound by combining the phosphate solution in the stream with calcium cations. Simulate this reaction in the laboratory. Design a procedure to find the mass of dry calcium phosphate precipitate. Mix 50 mL of a 0.10 mol/L aqueous solution of sodium phosphate with sufficient calcium nitrate to obtain a precipitate. Filter the precipitate, dry it, and determine its mass. 

One process modification that overcomes these difficulties uses only nitric acid for acidulation the extraction slurry is cooled to crystallize calcium nitrate, which then is removed by centrifugation. This process is referred to as the Odda process. The calcium nitrate byproduct is either sold as a fertilizer or converted to co-product ammonium nitrate. The extraction slurry, with its lowered calcium content, then is ammoniated and granulated. 

AMMONIUM NITRATE FERTILIZER, with CALCIUM CARBONATE... 

Alkali metal nitrates have comparatively low-melting points and the solid nitrates are excellent oxidizers at higher temperatures. Potassium nitrate is used as an oxidizer in black powder (75wt% KNO3, 15% charcoal, 10% sulfur). Fertilizer mixtures commonly contain ammonium nitrate or potassium nitrate, sometimes sodium or calcium nitrate as nitrogen compounds. Ammonium nitrate is also used as an explosive or as an oxidizer in an explosive mixture. Some properties of important nitrate fertilizers are summarized in Table 31. 

Calcium nitrate is produced as a byproduct in the manufacture of fertilizers (see Section 2.1.2.4). 

Other calcium compounds include calcium chloride (CaCl2), which can be spread on sidewalks and roads as a deicer in winter calcium hypochlorite (Ca(ClO)2), which is a form of powdered bleach calcium nitrate (Ca(N03)2), which is a fertilizer calcium carbide (CaC2), which is the primary ingredient used to produce acetylene in miners lamps and calcium sulfide (CaS), which is used sometimes as a hair remover. 

Calcium dinitrate Calcium nitrate Calcium saltpeter Calcium(ll) nitrate (1 2) EINECS 233-332-1 HSDB 967 Ume nitrate Ume saltpeter Nitric xid, calcium salt Nltrxalcite Norge saltpeter Norway saltpeter Norwegian saltpeter Saltpeter Synfat 1006 UN14M W l saltpeter. Usually crystallizes as the tetrahydrate [13477-344] or the trihydrale [15M2-292]. Used to support combustion in matches, explosives, as a fertilizer and corrosion inhibitor. Solid mp = 560 very soluble in H2O, MeOH, EtOH, MezCO, inxiuble in other organic solvents. 

Inorganic nitrogen fertilizers mostly contain nitrogen in the ammonium and/or nitrate form (ammonium nitrate, potassium nitrate, calcium nitrate, ammonium sulfate, ammonium phosphates). In the case of urea, ammonia (NH3) is set free by hydroly-... 

Ammonium nitrate production became a major fiictor towards the end of World War I once the merits of amatol, an 80 20 mixture of ammonium nitrate and TNT, had been accepted by the Services as the most expedient method of extending the hmited TNT supplies. Nitrogen fixation for fertilizers was the objective of the Haber process for ammonia and the successful chenjical engineering of this process had made Germany independent of the Chile nitrate supplies by 1918. The plant at Oppau made 25 tons/day of ammonia. The British requirement for ammonium nitrate was 4000 tons/week by the end of the war, which was met largely with gas works ammonia, Chile nitrate, and some manu cture via a Birkland-Eyre oxidation furnace and calcium nitrate. 

This unfavorable effect of low pH is usually intensified by the nitrogen fertilizers themselves, because most of them increase soil acidity. This may be due to the added acid, as in the case of S04 in ammonium sulfate. It may also be due to the NOs added as neutral salts, or to that formed in the nitrification process. If the NOs formed by nitrification is assimilated by plants and converted into protein, there is no appreciable direct effect on soil pH, but if the acid is leached out in the form of nitrate salts then the increase in soil acidity is marked. Even anhydrous ammonia, which is strongly basic, will produce acidity to the extent that it is nitrified and lost to the drainage waters as calcium nitrate or as some other neutral salt. Even if biologically-fixed nitrogen, present in plants as protein, undergoes decomposition to ammonia and oxidation to nitrate, it increases acidity if leaching occurs. Most of the increase in soil acidity is due to the removal of bases as nitrate salts. The possible reactions are explained in detail by Allison (1931). 

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