14797-55-8 Usage
Chemical Description
Nitrate and nitrite are secondary products that can be produced during the decomposition of liquid nitric peroxide by alkalis and acids.
Description
Nitrate is commonly found in drinking water sources especially
in agricultural areas where nitrogen fertilizer is used, and where
unregulated shallow private wells are more at the risk of
contamination. The World Health Organization (WHO)
guideline of 50 ppm and the US maximum contaminant level
(MCL) of 45 ppm for nitrate in drinking water have been
established for protecting infants from methemoglobinemia,
commonly known as blue baby syndrome. The health protective
value continues to be a subject of public health interest for
many years, with varying opinion on whether it is too high or
too low. Evaluation of nitrate will need to include consideration
of nitrite because both are closely related in the nitrogen
cycle in the environment and the body, and nitrite plays
a major role in inducing toxicity after its formation from
nitrate. More recently, reports of nitrate in drinking water,
especially at levels higher than 50 ppm, have been associated
with other health effects other than methemoglobinemia. This
toxicological review provides an update on the health effects of
nitrate with a focus on methemoglobinemia, reproductive and
developmental effects, potential carcinogenicity, and especially
endocrine/thyroid effects.
Chemical Properties
A colorless liquid.
Uses
Different sources of media describe the Uses of 14797-55-8 differently. You can refer to the following data:
1. Nitrate is the salt of nitric acid. it is used in meat curing to develop
and stabilize the pink color associated with cured meat. by itself, it
is not effective in producing the curing reaction until it is chemi-
cally reduced to nitrite. it has an effect on flavor and also functions
as an antioxidant. it is available as sodium and potassium nitrate,
with the sodium form being more common.
2. In the treatment of angina pectoris; in the manufacture of inorganic and organic nitrates and nitro
compounds for fertilizers, dye intermediates, explosives, and many different organic chemicals.
3. Nitrate is used in fertilizers; in the manufacture of nitrites,
nitrous oxide, explosives, pyrotechnics, matches, freezing
mixtures, and special cements; as a coloring agent and
preserving additive in food; for coagulation of latexes; in the
nuclear industry; and for odor (sulfide) and corrosion control
in aqueous systems.
Definition
Different sources of media describe the Definition of 14797-55-8 differently. You can refer to the following data:
1. ChEBI: A nitrogen oxoanion formed by loss of a proton from nitric acid. Principal species present at pH 7.3.
2. A salt or ester of nitric
acid.
3. nitrate: A salt or ester of nitric acid.
General Description
Crystalline solids. Salts of nitrate, such as ammonium nitrate, potassium nitrate, and sodium nitrate.
Air & Water Reactions
Most are water soluble.
Reactivity Profile
Mixtures of metal/nonmetal nitrates with alkyl esters may explode, owing to the formation of alkyl nitrates; mixtures a nitrate with phosphorus, tin (II) chloride, or other reducing agents may react explosively [Bretherick 1979. p. 108-109].
Hazard
Moderately toxic.
Health Hazard
Inhalation, ingestion or contact (skin, eyes) with vapors or substance may cause severe injury, burns or death. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may cause pollution.
Fire Hazard
These substances will accelerate burning when involved in a fire. Some may decompose explosively when heated or involved in a fire. May explode from heat or contamination. Some will react explosively with hydrocarbons (fuels). May ignite combustibles (wood, paper, oil, clothing, etc.). Containers may explode when heated. Runoff may create fire or explosion hazard.
Environmental Fate
Nitrate (NO3
-), a product of nitrogen oxidation, is a naturally
occurring ion in the environment and integrated into complex
organic molecules such as proteins and enzymes required by
living systems. Nitrate is a more stable form of oxidized
nitrogen than nitrite; however, it can be reduced by microbial
action to nitrite, which, in turn, can be reduced to various
compounds or oxidized to nitrate by chemical and biological
processes. Nitrates occur naturally in soil from microbial
oxidation of ammonia derived from organic nitrogenous
materials such as plant proteins, animals, and animal excreta.
Other source contributions are wastewater, septic tank runoffs,
airborne nitrogen compounds emitted by industry and automobiles,
nitrogen fertilizer, and manure from animal feeding.
Nitrate in groundwater is generally found below 10 ppm, with
higher levels in areas of high agricultural activities.
Toxicity evaluation
The acute oral LD50 values for sodium nitrate range from 2480
to 9000 mg kg-1 in rats, mice, and rabbits. Acute, subchronic,
and chronic animal toxicity studies showed low toxicity for
nitrate as sodium or potassium nitrate. A long-term study
showed a slight depression in growth rate. Nitrite, but not
nitrate, is capable of inducing methemoglobinemia (see
Nitrites, for more details).
Nitrate has been reported to be associated with thyroid
effects in experimental animals and humans. Possible mode of
action includes inhibition of iodine uptake to thyroid, serum
T3 and T4 changes, and tissue T3 changes. However, there is
a lack of knowledge on the differences in the mode of action to
permit animal-to-human extrapolation. While the data indicate
humans and rats exhibit similar dose–response relationships
in acute inhibition of thyroidal iodide uptake, they show
differences in thyroid hormone response following iodide
uptake inhibition. Comparative data are needed for serum and
brain tissue levels of thyroid hormones and characterization of
the dose–response relationship between changes of thyroid
hormone levels and adverse effects.
Early experimental and field studies in mammals have
found inorganic nitrate to be goitrogenic. The effects were
observed in rats following oral and parenteral administration
of potassium and sodium nitrate, whereas antithyroid effects
were also reported in sheep and pigs administered potassium
nitrate. Nitrate exposure through diet or drinking water caused
functional and histological changes to the thyroid gland in rats
and pigs. More recent investigations between 2000 and 2010
reported changes in thyroid and thyroid activity following
exposure to nitrate. In these more recent studies, nitrate exposure
has consistently resulted in increases in thyroid weight
and/or changes to the follicle cell; however, the reported
thyroidal hormone changes have not been as consistent. The
studies reported increased thyroid weights with a decrease in
thyroid hormones (i.e., T3 and T4) and/or decrease in thyroid
stimulating hormone. However, not all the results are consistent
with the expected outcome of a sodium–iodide symporter
(NIS) inhibitor, which can be seen as supplementation of
iodine in the diet that did not result in thyroid changes.
Overall, the data support that nitrate impairs thyroid function
involving the hypothalamic–pituitary–adrenal axis.
Check Digit Verification of cas no
The CAS Registry Mumber 14797-55-8 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,4,7,9 and 7 respectively; the second part has 2 digits, 5 and 5 respectively.
Calculate Digit Verification of CAS Registry Number 14797-55:
(7*1)+(6*4)+(5*7)+(4*9)+(3*7)+(2*5)+(1*5)=138
138 % 10 = 8
So 14797-55-8 is a valid CAS Registry Number.
InChI:InChI=1/NO3/c2-1(3)4/q-1
14797-55-8Relevant articles and documents
Chemical and Electrochemical Oxidation of Solutions of Silver Nitrate in Acetonitrile
Tracy, Mark L.,Nash, Charles P.
, p. 1239 - 1242 (1985)
In anhydrous acetonitrile the unstable, brown species Ag(NO3)42-, I, can be produced either by the electrolysis of silver nitrate or by the equilibrium reaction N2O5 + Ag+ + 3NO3- ->/-3.The ESR spectrum of I at 77 K is that of a Ag(II) ion in a field with pronounced axial distortion.Its resonance Raman spectrum indicates square-planar coordination of the metal ion by unidentate nitrate ligands.The complex decomposes to form cyanomethyl nitrate and nitric acid by the rate law -d/dt = k/->.In the presence of p-xylene a major organic product is p-methylbenzyl nitrate.Equilibrium and electrochemical studies lead to estimated ΔG0298 values for the free radical and ionic dissociation pathways of N2O5 in acetonitrile solution of +38 and -26 kJ, respectively.
Nucleophile Assistance of Electron-Transfer Reactions between Nitrogen Dioxide and Chlorine Dioxide Concurrent with the Nitrogen Dioxide Disproportionation
Becker, Robert H.,Nicoson, Jeffrey S.,Margerum, Dale W.
, p. 7938 - 7944 (2003)
The reaction of chlorine dioxide with excess NO2- to form ClO2- and NO3- in the presence of a large concentration of ClO2- is followed via stopped-flow spectroscopy. Concentrations are set to establish a preequilibrium among ClO2, NO2-, ClO2-, and an intermediate, NO2. Studies are conducted at pH 12.0 to avoid complications due to the ClO2-/NO2- reaction. These conditions enable the kinetic study of the ClO2 reaction with nitrogen dioxide as well as the NO2 disproportionation reaction. The rate of the NO2/ClO2 electron-transfer reaction is accelerated by different nucleophiles (NO2- > Br- > OH- > CO32- > PO43- > ClO2- > H 2O). The third-order rate constants for the nucleophile-assisted reactions between NO2 and ClO2 (kNu, M -2 s-1) at 25.0 °C vary from 4.4 × 10 6 for NO2- to 2.0 × 103 when H2O is the nucleophile. The nucleophile is found to associate with NO2 and not with ClO2 in the rate-determining step to give NuNO2+ + ClO2-. The concurrent NO2 disproportionation reaction exhibits no nucleophilic effect and has a rate constant of 4.8 × 107 M-1 s -1. The ClO2/NO2/nucleophile reaction is another example of a system that exhibits general nucleophilic acceleration of electron transfer. This system also represents an alternative way to study the rate of NO2 disproportionation.
HYPOCHLORITE OXIDATION OF AMMONIA. EFFECTIVE REMOVAL OF AMMONIA FROM WASTE WATER BY UV-IRRADIATION.
Kimura,Suzuki,Ogata
, p. 3198 - 3201 (1980)
The hypochlorite oxidation of ammonia giving rise to nitrogen evolution was carried out in the dark or under irradiation in order to study the reaction mechanism and application to waste water treatment. UV-irradiation accelerates remarkably the rate of decomposition of unfavorable chloramines. The acceleration covers the pH region 2-12, where corresponding dark reactions are slow. The irradiation also affects the formation of byproducts such as NO//2** minus and NO//3** minus , the effect being a slight increase in NO//2** minus formation in the pH range 2-12. These results suggest an effective industrial application to avoid eutrophication in seas and lakes. The irradiation effect is discussed in relation to reaction mechanism, in which the irradiation possibly facilitates the N-N bond formation after chloramine formation.
NMR study of reactions between Pd, Ru, and Rh nitrite complexes with sulfamic acid
Belyaev,Emel'yanov,Khranenko,Fedotov
, p. 184 - 194 (2001)
Reactions of nitrite complexes of Pd, Ru, and Rh with sulfamic acid were studied by the 14, 15N, and 17O NMR method. Chemical shifts were assigned, and the predominant forms of the complexes were established. The reaction products at room temperature are cis-nitroaqua complexes. Coordination of the sulfamate ion upon storage for a long time or on heating was detected.
Nanopore enriched hollow carbon nitride nanospheres with extremely high visible-light photocatalytic activity in the degradation of aqueous contaminants of emerging concern
Yang, Yuxin,Hu, An,Wang, Xinyue,Meng, Jiaqi,Guo, Yihang,Huo, Mingxin,Zhu, Suiyi
, p. 355 - 365 (2019/01/28)
Construction of highly efficient hollow nanosphere photocatalytic systems has been strongly attracting the attention of researchers. In the present work, nanopore enriched hollow carbon nitride nanospheres (HCNNSs) with a smaller particle size (200 nm) and a thinner shell thickness (40 nm) are successfully fabricated by a silica-nanocasting strategy. Such unique structures possess many advantages such as large BET surface area (122 m2 g-1), high light-harvesting ability, fast charge separation and transfer efficiency, plentiful exposed active sites and enhanced oxidation ability of photogenerated holes (h+VB). Therefore, HCNNSs in smaller sizes (HCNNS-200) exhibit extremely excellent visible-light photocatalytic efficiency towards the degradation of contaminants of emerging concern, e.g. levofloxacin (LEVO), in comparison with bulk g-C3N4 and HCNNSs in larger sizes (HCNNS-500). And it takes less than 10 min to finish the degradation of LEVO. The experimental results including those from indirect chemical probing, electron spin resonance, ion chromatography and high performance liquid chromatography-mass spectrometry confirm that h+VB and O2- are the active species that are responsible for the mineralization of LEVO to NO3-, F-, H2O and CO2 under visible-light irradiation. Additionally, the degradation pathway of LEVO in the HCNNS-200 photocatalytic system is also proposed. It is expected that HCNNS-200 can be used as a promising photocatalyst for environmental remediation.
Design and construction of a bifunctional magnetically recyclable 3D CoMn2O4/CF hybrid as an adsorptive photocatalyst for the effective removal of contaminants
Zheng, Jianhua,Hu, Yandong,Zhang, Lei
, p. 25044 - 25051 (2017/09/29)
Herein, a magnetic microsphere CoMn2O4 (MS-CoMn2O4) with a 3D architecture was constructed directly on cellulose fiber (CF) substrates from wastepaper by a solvothermal synthesis method with further calcination treatment. The designed hybrid shows excellent dual functions including rapid catalytic oxidation of tetracycline (TC)/methylene blue (MB) and a high adsorption capacity. What's more, the hybrid is easily recycled using an external magnetic field. In comparison with that of pure MS-CoMn2O4, the enhanced adsorption ability and photocatalytic activity of MS-CoMn2O4/CFs can mainly be attributed to the introduced cellulose fiber supporter in the hybrid system. MS-CoMn2O4 incorporated CFs can improve the efficient separation of photogenerated electron-hole pairs and the transport pathway of electrons. More importantly, introduction of CFs can help to enrich and further improve the degradation efficiency of organic contaminants. The possible mechanism for the enhancement of the photocatalytic activity has been elucidated in detail. The reusability analysis revealed that the MS-CoMn2O4/CF hybrid exhibited superb cycling stability after 5 cycles. This study provides novel insights into the design and construction of high capacity sorbents as strongly adsorptive photocatalysts to perform catalytic degradation of organic contaminants.
