Ammonia from nitrate

Many of the reactions producing imidazoles in tobacco and tobacco smoke involve the interaction of carbohydrates with ammonia, which has several precursors in tobacco. Amino acids and proteins can contribute to the formation of smoke amines and the formation of ammonia. Johnson et al. (1964) conclusively demonstrated through experiments with W-glycine that it is an ammonia source. In addition to amino acids, nitrates have been shown to be efficiently converted during the smoking of a cigarette to ammonia (1964). This ammonia from nitrates was shown to participate in the formation of many nitrogenous compounds in smoke. Thus, leaf nitrates as well as amino acids and proteins are considered the major sources of ammonia in tobacco smoke. 

Analytical Procedures. Standard methods for analysis of food-grade adipic acid are described ia the Food Chemicals Codex (see Refs, ia Table 8). Classical methods are used for assay (titration), trace metals (As, heavy metals as Pb), and total ash. Water is determined by Kad-Fisher titration of a methanol solution of the acid. Determination of color ia methanol solution (APHA, Hazen equivalent, max. 10), as well as iron and other metals, are also described elsewhere (175). Other analyses frequendy are required for resia-grade acid. For example, hydrolyzable nitrogen (NH, amides, nitriles, etc) is determined by distillation of ammonia from an alkaline solution. Reducible nitrogen (nitrates and nitroorganics) may then be determined by adding DeVarda s alloy and continuing the distillation. Hydrocarbon oil contaminants may be determined by ir analysis of halocarbon extracts of alkaline solutions of the acid. 

Ammonia from coal gasification has been used for fertilizer production at Sasol since the beginning of operations in 1955. In 1964 a dedicated coal-based ammonia synthesis plant was brought on stream. This plant has now been deactivated, and is being replaced with a new faciUty with three times the production capacity. Nitric acid is produced by oxidation and is converted with additional ammonia into ammonium nitrate fertilizers. The products are marketed either as a Hquid or in a soHd form known as Limestone Ammonium Nitrate. Also, two types of explosives are produced from ammonium nitrate. The first is a mixture of fuel oil and porous ammonium nitrate granules. The second type is produced by emulsifying small droplets of ammonium nitrate solution in oil. 

Let us first segregate the two sources forming the feed to the incinerator. As can be seen from the source-sink mapping diagram (Fig. 9.20), the gaseous emission from the ammonium nitrate process (R2) is within the acceptable zone for the incinerator. Therefore, it should not be mixed with R] then separated. Instead, the ammonia content of Ri should be reduced to 0.10 wt% then mixed with R2 to provide an acceptable feed to the incinerator as shown by Fig. 9.20. The task of removing ammonia from Rj to from 1.10 wt% to 0.10 wt% is identical to the case study solved in Section 9.3. Hence, the solution presented in Fig. 9.18 can be used. 

Ammonia also may be present as the result of the partial breakdown of amines used for condensate system protection, from hydrazine, or potentially even from nitrate. 

Although perhaps not an attraction to nutrients in a strict sense, symbiotic dino-flagellates (zooxanthellae) have been known for some time to be attracted to host invertebrates (which ultimately provide them with nutrients), presumably via chemical cues from the hosts (Kinzie 1974 Fitt 1984). These cues may include ammonia and nitrate released from the host (Fitt 1984). Recently Pasternak et al. (2004) demonstrated chemoattraction by Symbiodinium sp. to cell-free homogenates of juvenile soft coral polyps, which did not previously have symbiotic zooxanthellae, but not to adult polyps, which did already have symbiotic algae. The attraction was subsequently shown to be a true chemotactic response with an additional chemoki-netic effect of the algae swimming slower in the presence of host chemical cues (Pasternak et al. 2006). 

This chapter is concerned with the three primary nutrients making up most fertilizers nitrogen, phosphorus, and potassium. The usual sources of nitrogen are ammonia, ammonium nitrate, urea, and ammonium sulfate. Phosphorus is obtained from phosphoric acid or phosphate rock. Potassium chloride is mined or obtained from brine and the sulfate is mined in small amounts. Potassium nitrate is made synthetically. These chemicals have already been described under inorganic chemicals of the top 50. Sources for the three primary nutrients are given in Fig. 21.1. 

HA can be produced by catalytic oxidation of ammonia with hydrogen peroxide or by catalytic reduction of nitrates with hydrogen . Analogously, oxidative and reductive enzymic pathways in which HA is produced from either ammonia or nitrate have been identified in a variety of biological systems. 

Nitric and sulfuric acids readily dissolve in water drops, lowering the vapor pressure of the water and stabilizing the smog aerosols. Ammonia from animal feedlots also dissolves in these drops, creating ammonium sulfate and ammonium nitrate. 

La-hexaaluminate Ammonia route coprecipitation from nitrates aqueous solution La and A1 nitrates and ammonia solution 1000-1100 La-P-Al203, Sa=10-15 m2/g Catalytic combustion 21... 

Ammonium nitrate mixed with litharge expels ammonia from the solid salt at ordinary temp. T. J. Pelouze found that when ammonium nitrate is treated with a little sulphuric acid, ammonium sulphate and nitric acid are formed the same result obtains with the dried salt in fifty times itB weight of sulphuric acid provided the temp, is below 120° but at 150°, nitrous oxide mixed with a little nitric oxide and nitric acid vapour is evolved, and sulphuric acid and water remain. If the salt be mixed with ten times its weight of sulphuric acid, about 75 per cent, of the. salt forms nitric acid and ammonium sulphate, and 25 per cent, forms nitrous... 

One of the important problems of compatibility in explosive mixtures is whether ammonium nitrate can react with nitro compounds, such as TNT. This was discussed by Lang and Boileau [64]. These authors concluded that no reaction can occur between TNT and ammonium nitrate when they are pure. The evolution of ammonia from ammonium nitrate on storage at room temperature does not suffice to produce any reaction with TNT. 

The nitrogen cycle entails formation of ammonia by bacterial fixation of N2, nitrification of ammonia to nitrate by soil organisms, conversion of nitrate to ammonia by higher plants, synthesis of amino acids from ammonia by all organisms, and conversion of nitrate to N2 by denitrifying soil bacteria. 

Ammonium nitrate is the most readily available and cheapest salt of nitric acid, now manufactured wholly from synthetic ammonia and from nitric acid obtained by oxidation of ammonia. Ammonium nitrate was prepared for the first time as early as in 1659 by Glauber. The original experiments with it as a component of explosive mixtures began in the second half of the nineteenth century. Ammonium nitrate is the most widely used oxygen carrier, since it is an ingredient of the commonest group of high explosives. The reasons for this are to be seen in its properties and those of its explosive mixtures appreciable chemical stability, and low sensitiveness to friction and to shock. 

Nitrogen (from Nitrates and Ammonia). — Dissolve 10 gm. of zinc dust in a mixture of 20 cc. of sulphuric acid (sp. gr. 1.84) and 200 cc. of water. Add to the solution 100 cc. of sodium hydroxide solution I, distil off about 50 cc., and collect the distillate in a receiver containing about 20 cc. of water and 2 to 3 cc. of decinormal hydrochloric acid. Titrate the distillate with decinormal potassium hydroxide, using methyl orange as the indicator. Not more than 0.2 cc. of the acid should have been consumed by the ammonia. 

One procedure that is widely used to circumvent these complications is to remove ambient ammonia from the sampled air without removing particles by inserting one of several types of diffusion denuders upstream from the filter(s). In fact, in a recent Environmental Protection Agency (EPA)-sponsored intercomparison of methods for determination of strong acid content of aerosols, all but one protocol utilized an ammonia denuder (63), and all used an impactor or cyclone to remove coarse particles. The presence of this denuder clearly prevents neutralization of acidic aerosols by ammonia but also disturbs the gas-aerosol equilibrium between sulfate-nitrate aerosols and gaseous species. Ammonia and nitric acid are released from the depositing particles (64, 65) and must be collected downstream if accurate particulate ammonium and nitrate determinations are to be made. If equal amounts of ammonia and nitric acid are released, then the absolute [H+] (neq/m3) will not be altered. No specific evidence is available in the literature to demonstrate alteration of the observed [H+] as the result of reequilibration, but this area deserves further study. 

The oxide, a-Mn304, used in this study was prepared by thermal decomposition of manganese(II)hydroxide in air at 390K. The mentioned hydroxide was precipitated with ammonia from a manganese(II)nitrate solution (Mn(N03)2, 4H20, Fluka, Switzerland) at... 

Condensation Product of EDNA, Formaldehyde Ammonia, On thei basis of a British report, the condensation product of EDNA, formaldehyde ammonia was nitrated to yield a compd (mp 167° dec 208° nonhygroscopic) which was reported to be of interest as an explosive. The structure of the compd resembled that of RDX. It appeared, from its physical expl props, to offer no advantage over Tetryl or RDX as an expl. The un-nitrated condensation product was indicated to be of interest for use in pyrotechnic compns... 

Amatol is made up in various proportions of ammonium nitrate to trinitrotoluene, such as 50/50, 60/40, and 80/20. The granulated, dried, and sifted ammonium nitrate, warmed to about 90°, is added to melted trinitrotoluene at about 90°, and the warm mixture, if 50/50 or 60/40, is ladled into the shells which have been previously warmed somewhat in order that solidification may not be too rapid, or, if 80/20, is stemmed or extruded into the shells by means of a screw operating within a steel tube. Synthetic ammonium nitrate is preferred for the preparation of amatol. The pyridine which is generally present in gas liquor and tar liquor ammonia remains in the ammonium nitrate which is made from these liquors and causes frothing and the formation of bubbles in the warm amatol—with the consequent probability of cavitation in the charge. Thiocyanates which are often present in ammonia from the same sources likewise cause frothing, and phenols if present tend to promote exudation. 

The nitric acid of the original 2 mols of ammonium nitrate is exactly sufficient for the formation of 2 mols of guanidine nitrate. But the intermediate biguanide is a strong diacid base the ammonium nitrate involved in its formation supplies only one equivalent of nitric acid and there is a point during the early part of the process when the biguanide mononitrate tends to attack the unchanged ammonium nitrate and to liberate ammonia from it. For this reason the process works best if a small excess of... 

---