Manganese salts nitrate

An alternative method for carrying out the test is to employ the manganese(II) nitrate-silver nitrate reagent. Upon treating a neutral solution of manganese(II) and silver salts with ammonia, a black precipitate is formed ... 

Praseodymium is difficult to obtain in pure compounds buffi because of its scarcity and close resemblance to other elements. The best methods of separation are as follows (1) Hot. out from a double magnesium nitrate scries such fractions us contain only lanthanum and praseodymium continue the fractionation of the same salt or of double ammonium nitrate, Praseodymium appears at the soluble end, but usually neodymium appears there also, even if its presence is unsuNficctcd at first. (2) Remove from the magnesium double nitrate series the fractions which contain only praseodymium and neodymium and continue the fractionation as the manganese double nitrate, when praseodymium separates in the least soluble portions, Other methods used are Crystallization of the oxalates from nitric add of the double ammonium nitrate or double carbonate. 

Different, more specific, separation techniques were developed, each one having its special characteristics. It could be separation of other double salts - nitrates, oxalates - composed of a RE metal ion and another cation present in the solution, for example K+, Na+, NH or Mg. Double ammonium nitrate may be used for removal of lanthanum and the separation of neodymium from praseodymium. Members within the cerium group may be separated using double manganese nitrates, while elements in the yttrium group are separated using the differences in solubihty of their bromates. Auer von Welsbach did much work with RE-ammonium oxalate systems. Charles James in the USA developed an effective technique with RE-magne-sium double salts. 

A variation of this method is the impregnation of layers with metal ions that act as central atoms. For example, thin-layer plates impregnated with cadmium, zinc, or manganese salts, have been used to separate alkaloids (201,202), amino acids (203), and sulfonamides (204). Impregnation with silver nitrate is especially important in this connection. The Ag ions are able to form complexes with n systems. In this way, selectivity is achieved with respect to the number, position, and geometry of double bonds. This property is used to separate chinones (205), fatty acid derivatives (206,207), lipids (208,210), and sterols (211,212). 

Alkali bromides, chlorides, sulfates, and nitrates interfere only when very small amounts of iodide are to be detected. Bromides have the greatest deleterious effect however, when the amount of bromide is approximately known, small amounts of iodine may still be detected if a comparative test is carried out. Metal salts which give colored aqueous solutions interfere (Fe , UOa, Ni, Cu, Co). Cyanides, mercuric, silver, and manganese salts impair the reaction, as do compounds which reduce Ce. In such cases the difficulty may occasionally be averted by using more concentrated ceric solutions. Under the experimental conditions, barium and strontium salts are precipitated as sulfates, which are colored yellow by coprecipitation of ceric salt. Osmium salts behave similarly to iodides. 

Solutions of manganese and manganese salts are quite stable towards 2.5 iV hydrochloric acid at room temperature, and liberate little or no chlorine. On the addition of dilute silver nitrate, these brown solutions rapidly lose their color with evolution of chlorine. Ceric salts in hydrochloric acid solutions behave similarly when alone, their yellow color fades very slowly with development of chlorine, but on the addition of silver nitrate the reaction is instantaneous. The fact that silver chloride has a catalytic effect only in the presence of hydrochloric acid is due to its activation by silver chloride. The compound H[AgCl2], which may be formed under these conditions, probably takes part in the reaction. This catalyzed liberation of chlorine is effected by such small amoimts of silver that the reaction may be used as a test for silver. It is carried out most conveniently as a spot test. 

Manganese nitrate - 842, 870 Manganese oxide 402, 409 Manganese oxide-sulfuric acid 384 Manganese salts 132, 156, 278 Manganese solution - 62... 

Manganese Nitrate. Manganese nitrate [10377-66-9] is prepared from manganese(II) oxide or carbonate using dilute nitric acid, or from Mn02 and amixture of nitrous and nitric acids. Mn(N02)2 exists as the anhydrous salt [10377-66-9]-, the monohydrate [3228-81-9]-, ttihydrate [55802-19-2],... 

Acidic Properties. As a typical acid, it reacts readily with alkaUes, basic oxides, and carbonates to form salts. The largest iadustrial appHcation of nitric acid is the reaction with ammonia to produce ammonium nitrate. However, because of its oxidising nature, nitric acid does not always behave as a typical acid. Bases having metallic radicals ia a reduced state (eg, ferrous and staimous hydroxide becoming ferric and stannic salts) are oxidized by nitric acid. Except for magnesium and manganese ia very dilute acid, nitric acid does not Hberate hydrogen upon reaction with metals. 

Dissolved mineral salts The principal ions found in water are calcium, magnesium, sodium, bicarbonate, sulphate, chloride and nitrate. A few parts per million of iron or manganese may sometimes be present and there may be traces of potassium salts, whose behaviour is very similar to that of sodium salts. From the corrosion point of view the small quantities of other acid radicals present, e.g. nitrite, phosphate, iodide, bromide and fluoride, have little significance. Larger concentrations of some of these ions, notably nitrite and phosphate, may act as corrosion inhibitors, but the small quantities present in natural waters will have little effect. Some of the minor constituents have other beneficial or harmful effects, e.g. there is an optimum concentration of fluoride for control of dental caries and very low iodide or high nitrate concentrations are objectionable on medical grounds. 

BOD, inorganic salts, heavy metals pathogens, refractory organic compounds, plastics nitrate metals including iron, copper, manganese suspended solids... 

Many of the following powdered metals reacted violently or explosively with fused ammonium nitrate below 200°C aluminium, antimony, bismuth, cadmium, chromium, cobalt, copper, iron, lead, magnesium, manganese, nickel, tin, zinc also brass and stainless steel. Mixtures with aluminium powder are used as the commercial explosive Ammonal. Sodium reacts to form the yellow explosive compound sodium hyponitrite, and presence of potassium sensitises the nitrate to shock [1], Shock-sensitivity of mixtures of ammonium nitrate and powdered metals decreases in the order titanium, tin, aluminium, magnesium, zinc, lead, iron, antimony, copper [2], Contact between molten aluminium and the salt is violently explosive, apparently there is a considerable risk of this happening in scrap remelting [3],... 

In 1948, Bloch, Hansen, and Packard reported first the use of a paramagnetic salt, ferric nitrate to enhance the relaxation rates of water protons (8). In 1987, Lauterbur et al. (9) applied a manganese(II) salt to distinguish between different tissues based on the differential relaxation times. The first commercial MRI... 

A galvanic cell involves the overall reaction of iodide ions with acidified permanganate ions to form manganese(II) ions and iodine. The salt bridge contains potassium nitrate. 

Oxygen can be produced by electrolysis of water using a salt as an electrolyte that produces hydrogen at the opposite electrode. When potassium chlorate (KClOj) is heated in a test tube with a small amount of manganese dioxide (MnO ) as a catalyst, the chemical reaction that releases the oxygen from potassium chlorate will be accelerated. Use of potassium nitrate (KNOj) will also produce small amounts of oxygen. 

The simple hydrated ionic salt, chromic nitrate, has a spectrum quite distinct from the ionic salts of cobalt and manganese. The principal peak shows a splitting. This may be related to the very strong aflSnity which chromium displays toward its first coordination sphere of water. 

To synthesize Pa-233, thorium nitrate is irradiated with neutron. Pa-233 formed, as shown above, is dissolved in 3M nitric acid. The solution is heated. A manganous salt and permanganate are added to this solution. Manganese dioxide, Mn02, is precipitated. Pa-233 co-deposits onto this precipitate. The precipitate is washed with water. It is then dissolved in 6M hydrochloric acid. 

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