Nitrate salts, solubility

Silver nitrate forms colorless, rhombic crystals. It is dimorphic and changes to the hexagonal rhombohedral form at 159.8°C. It melts at 212°C to a yellowish Hquid which solidifies to a white, crystalline mass on cooling. An alchemical name, lunar caustic, is stiU appHed to this fused salt. In the presence of a trace of nitric acid, silver nitrate is stable to 350°C. It decomposes at 440°C to metallic silver, nitrogen, and nitrogen oxides. Solutions of silver nitrate are usually acidic, having a pH of 3.6—4.6. Silver nitrate is soluble in ethanol and acetone. 

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.]... 

Nitrogen sources include proteins, such as casein, zein, lactalbumin protein hydrolyzates such proteoses, peptones, peptides, and commercially available materials, such as N-Z Amine which is understood to be a casein hydrolyzate also corn steep liquor, soybean meal, gluten, cottonseed meal, fish meal, meat extracts, stick liquor, liver cake, yeast extracts and distillers solubles amino acids, urea, ammonium and nitrate salts. Such inorganic elements as sodium, potassium, calcium and magnesium and chlorides, sulfates, phosphates and combinations of these anions and cations in the form of mineral salts may be advantageously used in the fermentation. 

The predictions of the pH/potential diagram are generally fulfilled, but in very concentrated acid solutions, attack may diminish, owing to the relative insolubility of the relevant salt in the acid. Thus, lead nitrate, although soluble in water, has (owing to common ion effect) only slight solubility in concentrated nitric acid, and the corrosion rate is reduced. Similarly, lead chloride is less soluble in moderately concentrated hydrochloric acid than... 

All sodium salts are soluble, and so are all nitrate salts, so It makes sense that neither of these ions participates in a solubility equilibrium. Furthermore, nitrate and sodium cations are neither acidic nor basic, so it makes sense that neither participates in an acid-base equilibrium. 

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. 

Comparisons of solubilities of trichlorides, tribromides, and triiodides of the lanthanides in a variety of nonaqueous solvents can be found in a Russian review (310). Perhaps the widest range of solubilities of lanthanide(III) salts in nonaqueous media refers not to the trihalides but to the nitrates, whose solubilities in 31 solvents have been measured (312). Unfortunately, these measurements were carried out on the hexahydrates rather than anhydrous materials. 

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. 

When cleaning with acid, the usual choice is nitric (of relatively high concentration), since virtually all nitrate salts are water soluble, thereby ensuring that the products of contamination are removed readily by rinsing. 

Chemical/Physical. Products identified from the gas-phase reaction of ozone with N,N-dimethylaniline in synthetic air at 23 °C were A-methylformanilide, formaldehyde, formic acid, hydrogen peroxide, and a nitrated salt having the formula [C0H6NH(CH3)2] NO3 (Atkinson et al, 1987). Reacts with acids forming water-soluble salts. 

Silver is a white, ductile metal occurring naturally in its pure form and in ores (USEPA 1980). Silver has the highest electrical and thermal conductivity of all metals. Some silver compounds are extremely photosensitive and are stable in air and water, except for tarnishing readily when exposed to sulfur compounds (Heyl et al. 1973). Metallic silver is insoluble in water, but many silver salts, such as silver nitrate, are soluble in water to more than 1220 g/L (Table 7.3). In natural environments, silver occurs primarily in the form of the sulfide or is intimately associated with other metal sulfides, especially fhose of lead, copper, iron, and gold, which are all essentially insoluble (USEPA 1980 USPHS 1990). Silver readily forms compounds with antimony, arsenic, selenium, and tellurium (Smith and Carson 1977). Silver has two stable isotopes ( ° Ag and ° Ag) and 20 radioisotopes none of the radioisotopes of silver occurs naturally, and the radioisotope with the longest physical half-life (253 days) is "° Ag. Several compounds of silver are potential explosion hazards silver oxalate decomposes explosively when heated silver acetylide (Ag2C2) is sensitive to detonation on contact and silver azide (AgN3) detonates spontaneously under certain conditions (Smith and Carson 1977). 

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. 

According to the ionic hypothesis, if the solubility product [Li]2[C0"3] is not altered, the solubility can be increased by the union of one or other of the ions of the carbonate forming complexes with the added salt. This effect is not very marked with potassium or sodium chloride or nitrate. The marked increase in the solubility with sodium and potassium sulphates is due to the formation of lithium sulphate, but with the ammonium salts soluble complexes like Li(NH3) and NH2C00 may be formed just as is the case with magnesium carbonate in the presence of ammonium salts. 

Sodium and potassium nitrates are soluble in liquid ammonia,38 and the soln. are good electrical conductors. According to F. M. Raoult, the dry salts absorb no ammonia, but a cone. soln. of sodium nitrate dissolves as much ammonia as an equal volume of water, and a cone. soln. of potassium nitrate, more ammonia than water. R. Abegg and H. Riesenfeld found the tension of N, N-, and l 5A-soln. of potassium nitrate in A-soln. of ammonia at 25°, had vap. press. 14 59, 15 61, and 16 75 mm. respectively, when the A-ammonia alone had a vap. press, of 13 45 mm. F. Ephraim prepared lithium tetrammino-nitrate, LiN03.4NH3, as a syrup more stable than the corresponding tetrammino-chloride. The electrical conductivities and the lowering of the f.p. of soln. of potassium nitrate 39 in soln. 

The elements have remarkably low specific gravity, and a high atomic volume (q.v.). The oxides and hydroxides are markedly basic they do not exhibit acidic qualities. The physical properties of the salts—solubility in water, molecular volume, optical properties, and the variation in the form of the crystals show the same order of variation as the atomic weights of the elements. Lithium differs in mafiy respects from the other members of the family. The salts of the alkali metals —nitrates, chlorides, sulphides, sulphates, phosphates, carbonates, etc.—are nearly all soluble in water, although lithium, carbonate, phosphate, and fluoride are very... 

Partyka s method [20]). Powder may also be made porous by the previous introduction into the powder mass of salts soluble in water which are extracted by soaking. Potassium nitrate is generally used for this purpose so that a certain amount of it remains in the powder and enhances its vivacity. 

Naoiim [68] has drawn attention to the nitric acid salts of ethanolamine nitric esters (O-nitrated etlianolamines), i.e. mono-, di- and triethanolamine nitrate salts, as substances suitable for explosives. Nitration of a mixture of all three ethanolamines furnishes an oil-like, insufficiently stable product, readily decomposed with the evolution of oxides of nitrogen. The individual substances are crystal products soluble in water, in which they are hydrolysed. e... 

After the two solutions are mixed, the combined solution contains Pb2+, NO3-, Na +, and Cl- ions and has a volume of 0.150 L + 0.100 L = 0.250 L. Because sodium salts and nitrate salts are soluble in water, the only compound that might precipitate is PbCl2, which has Ksp = 1.2 X 10-5 (Appendix C). To calculate the value of IP for PbCl2, first calculate the number of moles of Pb2+ and Cl- in the combined solution ... 

Nitric acid is usually monobasic, forming a series of salts, the nitrates. The basic salts have been discussed by A. Ditte,11 E. Groschuff, and others—see, for example, the basic lead nitrates. The nitrates are usually made by the action of the acid on the metal, hydroxide, oxide, carbonate, etc. According to H. Braconnot, the cone, acid does not decompose dehydrated sodium, barium, calcium, or lead carbonate, even when boiling, because the nitrates of these bases are insoluble in the cone, acid, and a surface film of nitrate protects the remainder of the carbonate from the acid. Potassium carbonate is decomposed by the cone, acid because the nitrate is soluble in the cone. acid. J. Pelouze said that an alcoholic soln. of nitric acid does not act on potassium carbonate, but it acts slowly on sodium, barium, and magnesium carbonates, and rapidly on calcium and strontium carbonates because, added H. Braconnot, calcium and strontium nitrates are readily dissolved by alcohol, whereas potassium nitrate is but sparingly soluble in that menstruum. Potassium hydroxide resists attack by a soln. of nitric acid in ether unless the mixture is boiled or shaken. A. A. Kazantzeff discussed the influence of nitric acid on the solubilities of the nitrates. 

Since practically all nitrates are soluble in water, one would not expect to find extensive deposits of these salts in nature excepting in arid or semiarid regions. In addition to the nitrate deposits in Chile, limited quantities of potassium nitrate occur in East Asia. Most of the potassium nitrate used at the present time is made by the metatheti-cal reaction between sodium nitrate and potassium chloride,... 

Trivalent chromium compounds, with the exception of acetate, hexahydrate of chloride, and nitrate salts, are generally insoluble in water (Table 3-2). Some hexavalent compounds, such as chromium(VI) oxide (or chromic acid), and the ammonium and alkali metal salts (e.g., sodium and potassium) of chromic acid are readily soluble in water. The alkaline metal salts (e.g., calcium, strontium) of chromic acid are less soluble in water. The zinc and lead salts of chromic acid are practically insoluble in cold water (Table 3-2). The hexavalent chromium compounds are reduced to the trivalent form in the presence of oxidizable organic matter. However, in natural waters where there is a low concentration of reducing materials, hexavalent chromium compounds are more stable (EPA 1984a). 

The acidopentamminecobalt(III) salts have characteristic colors dependent upon the atom coordinated, i.e., salts in which there is a cobalt-oxygen bond vary in color from pink to red the fluoro complex is pink the chloro, red the bromo, purple the iodo, olive green and the nitro, orange. The nitrate salts of most of these complexes are only slightly soluble in water. None of these compounds is soluble in nonpolar solvents. Solutions of the compounds may decompose after long standing, liberating ammonia and cobalt hydroxide. Rates of aquation and of hydrolysis... 

Dilute nitric acid attacks copper, forming copper nitrate, a soluble salt, so that the surface of the metal remains free until the copper has all reacted. Copper oxide may be obtained by heating the solution, first to expel the water, and then with a somewhat stronger heat to decompose the residue of copper nitrate oxides of nitrogen escape as red fumes, and copper oxide remains as a black solid. This is the method by which zinc was converted quantitatively into zinc oxide, page 24. 

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