Nitrates solubility

The carbonates, sulfates, nitrates, and haUdes of lead (except the yeUow iodide) are colodess. Bivalent lead forms a soluble nitrate, chlorate, and acetate a slightly soluble chloride and an insoluble sulfate, carbonate, chromate, phosphate, molybdate, and sulfide. Highly crystalline basic lead salts of both anhydrous and hydrated types are readily formed. Tetrabasic lead sulfate [52732-72-6] 4PbO PbSO, and the hydrated tribasic salt [12397-06-7] ... 

Rhodium complexes with oxygen ligands, not nearly as numerous as those with amine and phosphine complexes, do, however, exist. A variety of compounds are known, iucluding [Rh(ox)3] [18307-26-1], [Rh(acac)3] [14284-92-5], the hexaaqua ion [Rh(OH2)3] [16920-31 -3], and Schiff base complexes. Soluble rhodium sulfate, Rh2(804 )3-a H2 0, exists iu a yellow form [15274-75-6], which probably coutaius [Rh(H20)3], and a red form [15274-78-9], which contains coordinated sulfate (125). The stmcture of the soluble nitrate [Rh(N03)3 2H20 [10139-58-9] is also complex (126). Another... 

Nitric acid dissolves silver at all concentrations. This is the principal chemical reaction for the dissolution of silver into the soluble nitrate, which is the chemical intermediate for the production of electroplated ware, catalysts, battery plates, pharmaceuticals, mirrors, and silver haUdes for photographic materials. Nitric acid removes silver from the residual pellet in the gold fire assay. 

Ce(III) forms a water-insoluble hydroxide, carbonate, oxalate, phosphate, and fluoride sparingly soluble sulfate and acetate and soluble nitrate and chloride (and bromide). In solution the salts are only slightly hydrolyzed. The carbonate is readily prepared and is a convenient precursor for the preparation of other derivatives. The sparingly soluble sulfate and acetate decrease in solubihty with an increase in temperature. Calcination of most Ce(III) salts results in Ce02. 

Purified by recrystn from dioxane (white needles) and sublimes above 120°. It has been distilled, b 132-140°/4-8mm. It forms complexes with metals and gives a sparingly soluble nitrate salt, m 205 (dec), which crystallises from H2O and is dried at 150 . [UV Bosnich et al. Inorg Chem 4 1102 1963, van Alphen Reel Trav Chim Pays-Bas 56 343 1937.]... 

Both are unmelted at 320°, form the characteristic, sparingly soluble nitrate, and give with sulphuric acid the specific colour reaction, cheriy-red changing to blue on warming. 

Sulphates, silicates, carbonates, colloids and certain organic compounds act as inhibitors if evenly distributed, and sodium silicate has been used as such in certain media. Nitrates tend to promote corrosion, especially in acid soil waters, due to cathodic de-polarisation and to the formation of soluble nitrates. Alkaline soils can cause serious corrosion with the formation of alkali plumbites which decompose to give (red) lead monoxide. Organic acids and carbon dioxide from rotting vegetable matter or manure also have a strong corrosive action. This is probably the explanation of phenol corrosion , which is not caused by phenol, but thought to be caused by decomposition of jute or hessian in applied protective layers. ... 

It, or further hydrolysis products should be water soluble. Water soluble nitrate-containing material was found in the wash water during separation of PETN from the rest of the residue in the bomb... 

The rare earth oxides of lanthanum, samarium and gadolinium were converted into soluble nitrate salts by dissolving them in the minimum amount of concentrated nitric acid. Then two sets were prepared by adding 2.0 ml of aqueous solution of La(N03)3.6H20 [0.2 M] and 0.01 ml of (n-BuO)4Ti to 25 ml of aqueous solution of Cu(N03)2 [1.0 M]. Similarly, two sets were prepared with Co(N03)3. Same procedures were followed for Sm(N03)3 [0.2 M] and Gd(N03)3 [0.2 M], One set of all these solutions were sonicated under ultrasonic bath (Model - Meltronics, 20 kHz, 250 W) for half an hour. The solutions prepared in normal and sonicated conditions were kept in muffle furnace (Model - Deluxe Zenith) first at 100°C for 2 h and then the temperature of the furnace was raised up to 900°C and calcined for 2 h. The solid composites prepared were then cooled to room temperature and treated as catalyst for phenol degradation. 

O Consider a solution that contains Pb ", Cu ", and Mg " cations, present as their (soluble) nitrate salts. How could you selectively precipitate these cations, given solutions of NaCl, Na2S, and Na3P04 Present your answer as a flowchart, with a chemical equation accompanying each step. 

Several tetrammino-derivatives of gold salts have been prepared. When dilute ehloraurie acid saturated with ammonium nitrate is added to a cold saturated solution of ammonium nitrate and the mixture treated with ammonia gas at ordinary temperature, a precipitate of fetrammino-auric nitrate, [Au(NH3)4](N03)3, is obtained. Tctrammino-aurie nitrate is soluble in water and may be crystallised from warm water. It may be precipitated from solution by the addition of any soluble nitrate, but with potassium, sodium, or ammonium nitrate it forms double salts. Thus, potassium nitrate if added to a concentrated solution of tetrammino-auric nitrate forms the compound [Au (NH 3).,] (NO 3)j.KNO. j, which crystallises from solution in needles. 

Hexammino-ehromic Nitrate, [Cr(NH3)6](N03)3, is obtained by the method described above.1 It crystallises in brilliant orange-yellow plates or prisms, is insoluble in alcohol and soluble in cold water, one part dissolving in forty parts of water the addition of soluble sulphates to the solution causes the precipitation of the less soluble nitrate-sulphate, [Cr(NH3)6](N03)(S04), which crystallises in glistening yellow octahedra. Sodium chloroplatinate added to an aqueous solution of the nitrate precipitates the nitrate-chloroplatinaie, [Cr(NH3)6](N03).(PtCl6).H20. 

Shoun, H., Suyama, W., and Yasui, T. (1989). Soluble, nitrate/nitrite-inducible cytochrome P-450 of the fungus Fusarium oxysporum. FEBS Lett. 244, 11-14. 

Many of the resulting compounds form crystalline picrates, and are isolated as such. The compounds with aromatic aldehydes are isolated as difficultly soluble nitrates. 

When exposed to oxygen in air, dissolved metals precipitate in unpreserved water as oxides or hydroxides. This process is prevented by the addition of 1 1 nitric acid solution to water samples. Metals in water with the pH of less than 2 will be permanently dissolved in a form of highly soluble nitrates. 

Often, with precipitation reactions the starting materials are limited to whatever salts are soluble in the solvent of choice. For water systems this is often limited to metal salts of halides, nitrates, and some sulfates and phosphates. Halides, in particular chlorides, have a pronounced effect on precipitation reactions. Chlorine is able to form bridged complexes much like the hydroxides or oxides of the desired compounds. In addition, acidic environments make possible the oxidation of chloride to chlorine gas, which can further complicate the synthesis. Sulfates and phosphates are typically easier to work with since they do not have the complicated redox behavior of the halides, but they typically have reduced solubilities. Nitrates, although they do not have the solubility concerns of sulfates and phosphates, do have redox complications, which typically result in oxidation of cations. So, the anion, which is expected to act solely as a spectator, in many cases is actually acting as a catalyst. 

Nature uses nitrogen fixation to combine free nitrogen with other elements. Nodules on the roots of many plants contain bacteria that extract nitrogen from the air and convert it into soluble nitrates that fertilize the soil. Most nitrogen products are based on nitrogen oxides and ammonia, as described on the following pages. 

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