Magnesium nitrate, formation

Bis (ethylenediamine)copper (II) diiodocuprate(I), 5 16, 17 Bis (ethylenediam ine) copper (II) iodide, formation of, from bis-(ethy lenediamine) copper (II) diiodocuprate(I), 5 18 Bis(ethylenediamine)nickel(II) chloride, 6 198 Bismuth(III) iodide, 4 114 Bismuth magnesium nitrate, 2Bi-(N0,)3-3Mg(N0,), 24H,0, separation of europium from samarium and gadolinium by, 2 57... 

Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. This mass of the white precipitate formed is 0.641 g. 

We predict that reaction occurs because silver chloride is insoluble and precipitates from the reaction mixture. Figure 4.6 shows the formation of the white silver chloride from this reaction. If you separate the precipitate from the solution by pouring it through filter papCT, the solution that passes through (the filtrate) contains magnesium nitrate, which you could obtain by evaporating the water. The molecular equation is a summary of the actual reactants and products in the reaction. ... 

Free styphnic acid is not a suitable starting material due to its low solubility in water and formation of nitric acid as a by-product of the reaction (nitric acid decomposes LS). When the sodium or magnesium salt of styphnic acid is used, innocuous sodium or magnesium nitrate forms as a by-product [33]. The reagents for LS production are used in equimolar quantity. However, when excess lead acetate is used as a starting substance, the double salt of LS and lead acetate is formed. But the double salt of LS and an initial lead salt only forms when the lead salt of a weak organic acid is used (e.g., lead acetate) [58]. 

Hetero-phase additions can influence both the transition alumina sequence and the temperature at which alpha alumina forms. For example, magnesium oxide additions introduced via addition of a magnesium nitrate salt to the boehmite precursor sol induces the formation of eta alumina after heating to 500°C rather than gamma alumina. This eta phase has a very diffuse X-ray diffraction patem at 500°C which sharpens with heating to 1000°C. The magnesium alumina spinel precipitates as a distinct fine crystal upon finther heating. 

To use potassium nitrate in colored flame mixtures, it is necessary to include magnesium as a fuel to raise the flame temperature. A source of chlorine is also needed for formation of volatile BaCl (green), or SrCl (red) emitters. The presence of chlorine in the flame also aids by hindering the formation of magnesium oxide and strontium or barium oxide, all of which will hurt the color quality. Shidlovskiy suggests a minimum of 15% chlorine donor in a color composition when magnesinm metal is nsed as a fuel [5]. 

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. 

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