13587-52-5Relevant articles and documents
Infrared Spectra of Solid Films Formed from Vapors Containing Water and Nitric acid
Smith, Roland H.,Ming-Taun, Leu,Keyser, Leon F.
, p. 5924 - 5930 (1991)
Infrared spectra have been recorded at 188 K for crystalline mono- and trihydrates of nitric acid formed by vapor deposition.In addition, spectra of fully deuterated forms of these same compounds have been obtained.These spectra have been interpreted in terms of the known ionic structures of the hydrates and the known spectra of oxonium and nitrate ions.Two other less stable solids were formed, a molecular hydrogen-bonded HNO3*H2O complex, stable only at temperatures below 120 or 150 K, and a substance thought to be a crystalline mixture of trihydrate and ice which sometimes formed from water-rich vapors and which upon pumping and/or warming could be converted into crystalline trihydrate.While these four substances appear to be the four species recently reported by Ritzhaupt and Devlin, we disagree with their allocation of structures to two of them.In particular, we disagree with their claims that a stable dihydrate exists.The relevance of the results to the stratosperic ozone hole problem is discussed.
Nitric acid-water complexes: Theoretical calculations and comparison to experiment
McCurdy, Patrick R.,Hess, Wayne P.,Xantheas, Sotiris S.
, p. 7628 - 7635 (2002)
The formation of HNO3·(H2O)n complexes is studied both theoretically and experimentally. First principles electronic structure calculations were used to produce minimum structures and harmonic vibrational frequencies of HN
AgNO3?NH4NO3 – an enigmatic double-salt type “decomposition intermediate” of diamminesilver(I) permanganate
Béres, Kende Attila,Petru?evski, Vladimir,Holló, Berta Barta,Németh, Péter,Foga?a, Lara,Paiva Franguelli, Fernanda,Farkas, Attila,Menyhárd, Alfréd,Szilágyi, Imre Miklós,Kótai, László
, p. 1166 - 1174 (2021)
The 1 : 1 type double salt of AgNO3 and NH4NO3 (NH4NO3 ? AgNO3, compound 1) was prepared and its Raman spectrum was evaluated. IR and far-IR spectra of compound 1 and its deuterated analog (ND4NO3 ? AgNO3, compound 1-D) were also studied. We identified two types of nitrate ions, one had a relatively strong, whereas the other is only weakly hydrogen bonded to the surrounding ammonium ions. The thermal decomposition features of compound 1 and its formation mechanism from [Ag(NH3)2]MnO4 (compound 2) at 80 °C with consecutive aqueous leaching of the decomposition residue has been elucidated. The solid phase decomposition product of compound 2 is presumably [Ag(NH3)NO3] (compound 3), which disproportionates into AgNO3 and [Ag(NH3)2]NO3 (compound 4). Compound 4 thermally decomposes in the solid phase into Ag+MnOx, while in aqueous solution its hydrolysis results in NH4NO3, which crystallizes out with an equimolar amount of AgNO3 formed during the disproportionation as compound 1.
Direct experimental evidence for reactions between dissolved acid halide and chlorine nitrate
Giligan,Castleman Jr.
, p. 1028 - 1032 (2001)
Cluster chemistry employing a fast flow reactor was used to evaluate the enhanced reactivity of chlorine nitrate (ClONO2) with dissolved acid halide. Reactions of ClONO2 with deuterium chloride doped deuterated water clusters [D+(D2O)m(DCl)n, (m = 10-14, n = 1,2)] were investigated under thermal conditions over a temperature range of 148-158 K; deuterated species were employed in place of light hydrogen containing molecules to facilitate the determination of reaction mechanisms. Chemical reactions were found to occur between water clusters and chlorine nitrate only under conditions where dissolved deuterium chloride was present. Nitric acid is found to remain within the water cluster to yield gaseous chlorine (Cl2) from the water cluster. These results provide direct evidence that an ionic reaction mechanism is involved in the heterogeneous reaction of hydrogen chloride and chlorine nitrate on clusters that mimic polar stratospheric cloud surfaces.
The crystal structures of the low-temperature and high-pressure polymorphs of nitric acid
Allan,Marshall,Francis,Oswald,Pulham,Spanswick
, p. 3736 - 3743 (2010)
A new high-pressure phase of pure nitric acid (HNO3) has been characterised at 1.6 GPa at room temperature by high-pressure neutron powder and X-ray single-crystal diffraction techniques. This is the first crystalline phase obtained upon compression of liquid nitric acid at room temperature and appears to be the stable phase up to pressures of at least 4 GPa. The crystal structure of this new phase shows some similarities to that of the low-temperature phase of nitric acid at ambient pressure, which has been redetermined as part of this study. Both structures share a herringbone packing of hydrogen-bonded molecular catemers, although the presence of disorder within the hydrogen bonds within one of the catemers of the low-temperature phase makes its structure comparatively more complex.
Kinetics of the Removal of OH(v = 1) and OD(v = 1) by HNO3 and DNO3 from 253 to 383 K
MeCabe, David C.,Brown, Steven S.,Gilles, Mary K.,Talukdar, Ranajit K.,Smith, Ian W. M.,Ravishankara
, p. 7762 - 7769 (2003)
The reaction of OH with HNO3 involves both HOX (HOX ≡ OH + HO2) and NOX (NOX ≡ NO + NO2 + NO3) species and plays two important roles in the atmosphere. The rate coefficients for the removal of OH(ν = 1) and OD(ν = 1) by HNO3 and DNO3 as a function of temperature from 253 to 383 K. The measured rate coefficients at 295 K ranged from 2.5 × 10-11 cc/molecule-sec for the removal of OH(ν = 1) by HNO3 to 6 × 10-12 cc/molecule-sec for the removal of OH(ν = 1) by DNO3; the rate coefficients for the like-isotope processes [removal of OH(ν = 1) by HNO3 and removal of OD(ν = 1) by DNO3] were 2-4 times higher than the rate coefficients for the unlike-isotope processes. All four rate coefficients showed negative temperature dependences that were too strong to be attributable only to long-range interactions between the reactions. The higher rate coefficients of the like-isotope processes (relative to the unlike-isotope processes) was attributed to faster, resonant, intramolecular vibrational energy redistribution within the reaction complexes containing the same isotopes. The yields of OH(ν = 1) were estimated to be ～ 1% and OH(ν = 2) to be ～ 0.4% of that of OH(ν = 0) from the photolysis of HNO3 at 248 nm.
Absorption and Oxidation of Nitrogen Oxide in Ionic Liquids
Kunov-Kruse, Andreas J.,Thomassen, Peter L.,Riisager, Anders,Mossin, Susanne,Fehrmann, Rasmus
, p. 11745 - 11755 (2016)
A new strategy for capturing nitrogen oxide, NO, from the gas phase is presented. Dilute NO gas is removed from the gas phase by ionic liquids under ambient conditions. The nitrate anion of the ionic liquid catalyzes the oxidation of NO to nitric acid by atmospheric oxygen in the presence of water. The nitric acid is absorbed in the ionic liquid up to approximately one mole HNO3per mole of the ionic liquid due to the formation of hydrogen bonds. The nitric acid can be desorbed by heating, thereby regenerating the ionic liquid with excellent reproducibility. Here, time-resolved in-situ spectroscopic investigations of the reaction and products are presented. The procedure reveals a new vision for removing the pollutant NO by absorption into a non-volatile liquid and converting it into a useful bulk chemical, that is, HNO3.
Microwave spectrum of DNO3, and average structures of nitric and nitrous acids
Cox, A. P.,Ellis, M. C.,Attfield, C. J.,Ferris, A. C.
, p. 91 - 106 (1994)
The rotational spectrum of DNO3 in the ground vibrational state has been investigated in the region 16-40 GHz and analysed to give rotational constants and centrifugal distortion constants.Microwave data for eight isotopomers of HNO3 have been used to der
Heterogeneous reactivity of gaseous nitric acid on Al2O3, CaCO3, and atmospheric dust samples: A Knudsen cell study
Hanisch,Crowley
, p. 3096 - 3106 (2007/10/03)
The heterogeneous reaction between HNO3 and various authentic and synthetic mineral dust/mineral oxide surfaces has been investigated using a low-pressure Knudsen reactor operating at 298 K. The surfaces used were Saharan dust from Cape Verde, Arizona dust, CaCO3, and Al2O3. In all cases, a large irreversible uptake was observed. An uptake coefficient of γ = (11 ± 3) × 10-2 was determined for Saharan dust, and γ= (6 ± 1.5) × 10-2 was obtained for Arizona dust. The uptake coefficients for HNO3 on heated CaCO3 and on unheated CaCO3 are given by γ = (10 ± 2.5) × 10-2 and (18 ± 4.5) × 10-2, respectively, and are in good agreement with previous results. CO2 and H2O were formed as gas-phase products. Measurements of the uptake coefficient of HNO3 on grain-size selected samples of Al2O3, γ = (13 ± 3.3) × 10-2, and systematic variation of sample mass enabled us to show that the geometrical surface area of the dust sample is appropriate for calculation of uptake coefficients in these experiments. The high reactivity of HNO3 toward dust samples highlights the potentially important role of mineral dust in redistributing nitrate from the gaseous to the particulate phase and modifying tropospheric photochemical oxidation cycles.
Reaction of hydroxyl radical with nitric acid: Insights into its mechanism
Brown, Steven S.,Burkholder, James B.,Talukdar, Ranajit K.,Ravishankara
, p. 1605 - 1614 (2007/10/03)
The rate constant for the reaction of hydroxyl radicals with nitric acid has an unusual pressure and temperature dependence. To explore the mechanism for this reaction, we have measured rate constants for reactions of isotopically substituted species OD+DNO3, OH+DNO3, OD+HNO3, and 18OH+HNO3 and the yield of NO3 product. Deuterium substitution on nitric acid results in more than a 10-fold reduction in the rate constant, removes the pressure dependence (over the observed range of 20-200 Torr in He and SF6), and leads to a strongly curved Arrhenius temperature dependence. Deuterium substitution on hydroxyl increases the rate constant slightly but does not change the pressure dependence. There is no evidence for exchange reactions in the isotopically mixed reactions. Absorption measurements of the NO3 product yield show that the title reaction produces nitrate radical with unit efficiency over all temperatures and pressures studied. We discuss the implications of the measured rate constants, product yields, and lack of isotopic exchange in terms of a mechanism that involves formation of a hydroxyl radical-nitric acid complex and its subsequent reaction to give NO3 and H2O.
