Lithium bromide nitrate

Lithium bromide also combines with gaseous ammonia to form four solid deliquescent substances. The monammine, [Li(NH3)]Br, is formed above 95° C. the diammine, [Li(NIi3)2]Br, between 87° and 95° C. the triammine, [Li(NH3)3]Br, between 71° and 87° C. and the tetrammine about —18° C.2 Ephraim prepared other ammino-salts of lithium, as, for example, tetrammino-lithium nitrate, [Li(NH3)J(N03), which is a colourless syrup at ordinary temperature and is more stable than the chloride tetrammino-lithium chlorate, [Li(NII3)Ll]C103, which is a fairly mobile liquid and tetrammino-lithium perchlorate, [Li(NH3)4]C104, a white solid which liquefies and decomposes at ordinary temperature.3... 

With 5-33.3 vol.% water/acetone mixtures, it is found136 that common-ion salts have no effect on the rate of hydrolysis of benzoyl chloride whereas the rate in 15% (but not 33.3%) water is increased by the addition of neutral salts such as lithium bromide or potassium nitrate. The increase in ionic strength on the addition of neutral salts is not the major reason for the increase in rate and nucleophilic catalysis via the more easily hydrolysed benzoyl bromide was postulated. 

Alkylation of potassium enolates is not always fruitful, and so counterion exchange with lithium bromide prior to addition of the electrophile has been recommended. Reduction of aromatic esters instead of acids provides a number of potential advantages. The esters tend to be more soluble than carboxylate salts, hydrogenolysis of 2-alkoxy substituents does not appear to present the s me problem, and the products are more stable. This can be important when enol ether functions are generated, allowing the necessarily acidic work-up procedures for carboxylic acids to be avoided. Indeed, the hydrolysis of enol ether functions may be very slow in aqueous acid and is best achieved through catalysis by mercury(II) nitrate. ... 

Dimerizations of aryldiazomethanes to 1,2-diarylethylenes were reported to be catalyzed by cerium(IV) ammonium nitrate (4J), lithium bromide (42), copper(II) salts (43), and rhodium(II) acetate (44) and to be induced by photolysis (45). Catalysis of copper ion-exchanged zeolite (CuNaY) was compared with reactions of copper salts supported on AI2O3 and a homogeneous catalyst, Cu(C104)2, for the dimerization [Eq. (11)] of aryldiazomethane (Table XIII) (-/6). 

Lithium Bromide Lithium Chloride Lubricating Oils Magnesium Carbonate Magnesium Chloride Magnesium Citrate Magnesium Hydroxide Magnesium Nitrate Magnesium Sulfate... 

Potassium chloride "1 bromide 1 iodide j Ammonium chloride J Sodium bromide chloride / Lithium Potassium nitrate Silver nitrate Potassium hydroxide Hydrochloric acid 0503 0528 0174 0503 0528 0x74 0503 0 604 0 680 0528 0174 0687 0 497 0528 0 735 0 697 0 496 0527 0736 0 492 0519 0 738... 

Development of a Stable Aqueous Membrane. An aqueous LiBr membrane was fabricated by soaking a porous 47 mm diameter cellulose acetate/nitrate membrane in a 3 M LiBr solution for 24 hours. The membrane was then exposed to a vacuum for 5 hours to remove the water while leaving the lithium bromide. It was then placed into the apparatus shown in Figure 7 and exposed to a nitrogen mixture containing approximately 10 mmHg water vapor until the pores filled via condensation. 

Lithium monobromide. See Lithium bromide Lithium monohydride. See Lithium hydride Lithium monoxide. See Lithium oxide Lithium nitrate... 

Lithium carbonate Lithium hydroxide Lithium chloride Lithium bromide Lithium phosphate Lithium nitrate Battery material special glass For carbon dioxide absorbent and grease Aluminum welding material humidity control material For freezer and air conditioner Electronic and electric material Electronic and electric material... 

LiBr, lithium bromide Mg(I04)2, magnesium periodate AgN03, silver nitrate MnCl3, manganese(III) chloride Hg2Br2, mercuryfl) bromide... 

C HigBrLiN, Bis(ethylenediamine)lithium bromide, 32B, 267 C4H1gCaNaOi0r Calcium nitrate - methanol, 40B, 650 C H eCaNeOsS, Calcium sulfate urea complex, 41B, 60... 

The chlorides, bromides, iodides, and cyanides are generally vigorously attacked by fluorine in the cold sulphides, nitrides, and phosphides are attacked in the cold or may be when warmed a little the oxides of the alkalies and alkaline earths are vigorously attacked with incandescence the other oxides usually require to be warmed. The sulphates usually require warming the nitrates generally resist attack even when warmed. The phosphates are more easily attacked than the sulphates. The carbonates of sodium, lithium, calcium, and lead are decomposed at ordinary temp, with incandescence, but potassium carbonate is not decomposed even at a dull red heat. Fluorine does not act on sodium bofate. Most of these reactions have been qualitatively studied by H. Moissan,15 and described in his monograph, Lefluor et ses composes (Paris, 1900). 

According to F. C. Franklin and C. A. Kraus,40 liquid ammonia readily dissolves sodium and potassium iodides. The partial press, of ammonia in soln. of potassium iodide at 25°, as measured by R. Abegg and H. Riesenfeld, is raised from 13 45 mm. of water to 13 28, and 14 88 mm. for 0 5W-, N-, and l 5Ar-soln. respectively. H. M. Dawson and J. McCrae have shown that the distribution of ammonia between water and chloroform is generally lowered by the addition of various salts of the alkali metals and ammonium which they tried—halides, nitrates, chlorates, oxalates, sulphates, carbonates, hydroxides this means that the solvent power of aq. soln. of the alkali salts is in general less than that of pure water—lithium chloride, ammonium bromide, and sodium iodide act in the opposite way. The other halide salts of lithium were not tried. The change produced in the partition coeff. by the halides, at 20°, is as follows ... 

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