Nitric acid monohydrate

Nitric acid is one of the three major inorganic acids in the chemical industry. Its structural parameters in the gaseous state are shown in Fig. 15.2.2(d). The crystals of nitric acid monohydrate consist of H30+ and N0, which are connected by strong hydrogen bonds. In the acid salts, HNO3 molecules are bound to nitrate ions by strong hydrogen bonds. For example, the structures of [H(N03)2r in K[H(N03)2] and [H2(N03)3] in (NH4)H2(N03)3 are as follows ... 

In equimolar mixtures of nitric acid and water a monohydrate is formed whose Raman spectrum has been observed. There is no evidence for the existence of appreciable concentrations of the nitric acidium ion in aqueous nitric acid. 

The vapour pressure of nitric acid, over solutions in sulphuric acid, reaches a maximum with 84-5 % sulphuric acid, the acidity corresponding to the formation of the monohydrate. ... 

Lead styphnate monohydrate is precipitated as the basic salt from a mixture of solutions of magnesium styphnate and lead acetate followed by conversion to the normal form by acidification using dilute nitric acid (97—99). 

Manganese Nitrate. Manganese nitrate [10377-66-9] is prepared from manganese(II) oxide or carbonate using dilute nitric acid, or from Mn02 and amixture of nitrous and nitric acids. Mn(N02)2 exists as the anhydrous salt [10377-66-9]-, the monohydrate [3228-81-9]-, ttihydrate [55802-19-2],... 

Qua.driva.Ient, Zirconium tetrafluoride is prepared by fluorination of zirconium metal, but this is hampered by the low volatility of the tetrafluoride which coats the surface of the metal. An effective method is the halogen exchange between flowing hydrogen fluoride gas and zirconium tetrachloride at 300°C. Large volumes are produced by the addition of concentrated hydrofluoric acid to a concentrated nitric acid solution of zirconium zirconium tetrafluoride monohydrate [14956-11-3] precipitates (69). The recovered crystals ate dried and treated with hydrogen fluoride gas at 450°C in a fluid-bed reactor. The thermal dissociation of fluorozirconates also yields zirconium tetrafluoride. 

Zirconium tetrafluoride dissolves in dilute acid without hydrolysis, and can be recovered as the monohydrate [14956-11-3] by crystallization from nitric acid solutions. If the solution is acidified with hydrofluoric acid, ZtF 3H20 [14517-16-9] crystallizes at 10—30 wt % HF HZtF 20 [18129-16-9] crystallizes at 30—35 wt % HF, and at higher HF concentrations H2ZtF -2H20 [12021 -95-3] can be recovered. 

Maltose (H2O) [6363-53-7] M 360.3, m 118 . Purified by chromatography from aqueous soln on to a charcoal/Celite (1 1) column, washed with water to remove glucose and other monosaccharides, then eluted with aqueous 75% EtOH. Crystd from water, aqueous EtOH or EtOH containing 1% nitric acid. Dried as the monohydrate at room temperature under vacuum over H2SO4 or P2O5. 

Mercury(II) nitrate monohydrate Mercury(II) chloride Nitric acid 0.1 mol/1 Titrisol Nitric acid (65%)... 

Mercury (II) nitrate solution. Dissolve 1.713 g pure mercury(II) nitrate monohydrate in 500 mL of 0.05 M nitric acid. 

The Raman spectrum of the monohydrate, HN03.H20, shows it to exist as the hydroxoni-um salt, H30+N03 13. Also, according to analyses of the Raman spectrum, nitric acid exists in aq solns either as a pseudo-acid, N02.0H or as a true acid, N03".H+. In 10 molar aq soln, both acids are present in equal amounts, being caused by the self-dissociation of nitrogen pentoxide (NjOj), while in a 6 molar soln, the pseudo acid is present only to the extent of 2%. and the more dilute the soln, the less pseudo acid is present. In very coned solns, the true acid is present only in small quantities (Refs 32 33)... 

Indium dissolves in mineral acids. Concentration or evaporation of the solution produces corresponding salts. With sulfuric acid, it forms indium trisulfate, In2(S04)s and indium hydrogen sulfate, In(HS04)2. The latter salt is obtained upon concentration of trisulfate solution. With nitric acid, the salt is indium nitrate trihydrate, In(N03)s 3H2O [13770-61-1] which on dehydration yields monohydrate, In(N03)3 H20. 

The monohydrate is a white crystalline or powdery substance density 4.3g/cm3 decomposes on heating soluble in water and nitric acid insoluble in alcohol. 

Mercury(II) nitrate is prepared by dissolving mercury in excess hot concentrated nitric acid. Upon evaporation of the solution, large colorless deliquescent crystals of monohydrate, Hg(N03)2 H2O, form. 

The monohydrate is prepared by treating a molybdate solution with nitric acid, followed by crystallization which may take several weeks to separate out as a yellow solid. The anhydrous molybdic acid is obtained as a white crystalline substance by careful dehydration of the yellow monohydrate. 

The individuality of this acid has not yet been established. According to H. Lescceur (1889), the crystals of iodic acid deposited from its soln. in dil. nitric acid are monohydrated iodic add, HI03.H20 from soln. in cone, nitric acid, anhydrous iodic acid, HI03 and from soln. of nitric acid of intermediate cone., mixtures of monohydrated and anhydrous iodic acid. 

Strontium iodate furnishes two hydrates According to C. F. Rammelsberg, monohydrated strontium iodate, Sr(I03)2.H20, is formed as a white crystalline powder when hot soln. of strontium chloride and sodium iodate are mixed together and, according to A. Ditte, the same hydrate is formed by crystallization from cold nitric acid soln. C. F. Rammelsberg also claims that if soln. of strontium chloride and sodium iodate are mixed together in the cold, small crystals of hexa-hydrated strontium iodate are formed. 

C. W. Kimmins 9 study of the periodates of silver has shown that the composition of the precipitate depends upon the concentration of the nitric acid in which the sodium periodate is dissolved when the silver nitrate is added. If the amount of nitric acid be just sufficient to effect the dissolution of the sodium salt, a dark brown precipitate of secondary silver mesoiodate, Ag2HI03, is formed if but a slight excess of nitric acid is used dark-red secondary silver paraperiodate is formed, Ag2H3I06 if a further excess of nitric acid is used, slate-coloured tertiary silver paraperiodate, Ag3H2I06, is formed and if cone, nitric acid be used in excess, monohydrated silver metaperiodate, AgI04.H20, is formed in orange crystals. 

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