Mercury nitrite nitration with

Mercuric and mercurous nitrates have the same oxidising properties as nitrates. The first has been involved in accidents with phosphine (formation of a complex, which detonates on impact) and alkaline cyanides. In the latter case, it is assumed that the danger arises from the formation of mercury nitrite, which is highly unstable in one particular accident the use of an apparatus with a narrow neck aggravated the effect, causing an effect of confinement. The second nitrate led to more or less strong detonations with carbon (red-hot) and phosphorus (on impact). 

Sodium hypnnitrite Na N 0 is formed (I) by reaction of sodium nitrate or nitrite solution with sodium amalgam (sodium dissolved in incrcuryl, alter which acetic acid is added to neutralize the alkali. Sodium stannite ferrous hydroxide, or electrolytic reduction w ith mercury cathode may also be utilized. (2) by reaclion of hydroxylamine sulfonic acid and sodium hydroxide. Silver hyponitrite is formed by reaclion of silver nitrate solution and sodium hyponitrite. 

P. C. Ray and 8. C. Mukherjee found the degree of ionization to be 0-11 for a mol of the salt in 32 litres. P. C. Ray and N. Dhar found that if the aq. soln. be kept in a closed vessel for some time, some of the mercuric nitrite forms mercurous nitrate and a basic salt is formed thus in 3 weeks, a soln. of sp. gr. 1-065 contained mercuric mercurous mercury as 13-7 1. P. C. Ray and N. Dhar found that the conductivity measurements of aq. soln. of mercurous nitrite agree with the assumption that a complex Hg2(N02) 5-ion is present this corresponds with mercurosic nitrite, HgN02.2Hg(N02)2. For a dilution v=187, A—62-33, and when c=561, A=80-10. With dil. soln., hydrolysis occurs. If the aq. soln. be sealed up in an... 

Test for nitrate (andI or nitrite) If ammonium is found, transfer the solution from test 5 with the aid of 0-5 ml water to a semimicro boiling tube (or crucible), add 0 5 ml sodium hydroxide solution and evaporate down to a volume of about 0-2 ml - this treatment completely decomposes the ammonium salt. Transfer the residue to a semimicro test-tube, rinse the vessel with 0-5 ml sodium hydroxide solution and add this to the contents of the test-tube. Then add 10 mg of Devarda s alloy (or of aluminium powder or thin foil), introduce a Pyrex filter tube provided with a loose plug of cotton wool at the lower end and containing a strip of red litmus paper or mercury(I) nitrate paper (Fig. II.29a), and place the assembly in the hot water rack. If frothing occurs, remove the apparatus from the water bath until the vigorous reaction has subsided. 

If ammonia is evolved, as detected by its action upon red litmus paper or upon mercury(I) nitrate paper, the presence of a nitrate or nitrite is indicated. Nitrite will also be detected in the reaction with dilute sulphuric acid (see test 7) if nitrite is absent, the presence of nitrate is established. 

Potassium tetranitrodiamminecobaltate(III) is a lustrous yellow to brown solid, the exact color depending on the crystal size. It is only very slightly soluble in cold water the solubility at 100° is about 5 g./lOO ml. of water. Prolonged contact with water at temperatures above 50 to 60° causes decomposition. Treatment with excess 10% aqueous oxahc acid yields potassium dinitrooxalatodiamminecobal-tate(III). Silver or mercury (I) nitrate causes the precipitation of the corresponding sparingly soluble metal salts of the anion. The free acid is also relatively stable. Aqueous ethylenediamine displaces nitrite from the complex to give the nonelectrolyte trinitro (ethylenediamine) amminecobalt-(III). ... 

In the new procedure described below the potassium dinitrodiglycinatocobaltate(III) is prepared by a simpler, direct method consisting of the oxidation of cobalt(II) to cobalt(III) in the presence of potassium glycinate and potassium nitrite. The corresponding silver and mercury (I) salts are obtained by double decomposition of the potassium salt with silver and mercury(I) nitrates, respectively. 

MERCURY CYANIDE or MERCURY(II) CYANIDE (592-04-1) Hg(CN)2 Slowly decomposes in light. A moderate impact- and heat-sensitive explosive. Violent reaction with metal chlorates, fluorine, hydrogen cyanide, magnesium, nitrates, nitrites, metal perchlorates, sodium nitrite. Contact with strong acids evolves flammable and poisonous hydrogen cyanide gas, which can be detonated by this material. Thermal decomposition releases toxic nitrogen oxides, mercury, and hydrogen cyanide. On... 

The reaction is exothermic, and multitubular reactors are employed with indirect cooling of the reactor via a heat transfer medium. A number of heat transfer media have been proposed to carry out the reactor cooling, such as hot oil circuits, water, sulfur, mercury, etc. However, the favored heat transfer medium is usually a molten heat transfer salt which is a eutectic mixture of sodium-potassium nitrate-nitrite. 

Atomic hydrogen is a powerful reducing agent, even at room temperature. For example, it reacts with the oxides and chlorides of many metals, including silver, copper, lead, bismuth, and mercury, to produce the free metals. It reduces some salts, such as nitrates, nitrites, and cyanides of sodium and potassium, to the metallic state. It reacts with a number of elements, both metals and nonmetals, to yield hydrides such as NH3, NaH, KH, and PH3. Sulfur forms a number of hydrides the simplest is H2S. Combining with oxygen, atomic... 

In a similar procedure [32] the sediment is wet oxidised with dilute sulphuric acid and nitric acids in an apparatus in which the vapour from the digestion is condensed into a reservoir from which it can be collected or returned to the digestion flask as required. The combined oxidised residue and condensate are diluted until the acid concentration is IN and nitrate is removed by addition of hydroxylammonium chloride with boiling. Fat is removed from the cooled solution with carbon tetrachlodithizone in carbon tetrachloride. The extract is shaken with 0.1M hydrochloric acid and sodium nitrite solution and, after treatment of the separated aqueous layer with hydroxylammonium chloride a solution of urea and then EDTA solution are added to prevent subsequent extraction of copper. The liquid is then extracted with a 0.01% solution of dithizone in carbon tetrachloride and mercury estimated in the extract spectrophotometrically at 485nm. 

Nitrotetrazole is readily prepared from the diazotization of 5-aminotetrazole in the presence of excess sodium nitrite and is best isolated as the copper salt complex with ethylenediamine. The salts of 5-nitrotetrazole have attracted interest for their initiating properties. The mercury salt is a detonating primary explosive. The amine salts of 5-nitrotetrazole are reported to form useful eutectics with ammonium nitrate. ... 

The commercial preparation of mercury fulminate is carried out by a process which is essentially the same as that which Howmrd originally recommended. Five hundred or 600 grams of mercury is used for each batch, the operation is practically on the laboratory scale, and several batches are run at the same time. Since the reaction produces considerable frothing, capacious glass balloons are used. The fumes, which are poisonous and inflammable, are passed through condensers, and the condensate, which contains alcohol, acetaldehyde, ethyl nitrate, and ethyl nitrite, is utilized by mixing it with the alcohol for the next batch. 

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