Manganous Chloride Sulphate

Polissar has observed 100 % exchange between Mn(III), as the oxalato ion Mn(Ox)J, and manganous sulphate. Adamson, using manganic chloride as the source of Mn(III), has observed the exchange to be incomplete in a time 15 sec with reactant concentrations 10 M. Both workers used a separation technique based on the precipitation of Mn(IV), present via the equilibrium... 

Sulphates. Dissolve I gm. of manganous chloride in 10 cc. of water, add 0.2.r> cc, of hydrochloric acid, and some barium chloride solution. No change should be noticeable,... 

E. P. Alvarez 2 found that the pemitrates react with soln. of lead acetate (white precipitate), silver nitrate (white precipitate), mercurous nitrate (white precipitate with rapid decomposition), mercuric chloride (red precipitate), copper sulphate (blue precipitate), zinc and cadmium sulphates (white precipitate), bismuth nitrate (white precipitate), gold chloride (slight effervescence and escape of oxygen), manganous chloride (pink precipitate), nickelous chloride or sulphate (greenish-white precipitate), cobaltous nitrate and chloride (pink precipitate), ferrous sulphate (green or bluish-green precipitate), ferric chloride (red ferric hydroxide), and alkaline earth chlorides (white precipitates). The precipitates are all per-salts of the bases in question. 

Cr(OH)2, manganic and manganous, ferric and ferrous, cobaltous and nickelous in short, from all elements which form basic hydroxides. And from almost all these the oxides may be obtained by heating the hydrates to redness. Excess of the precipitant, however, must be avoided in many cases, for some of these hydroxides display acid properties if in presence of excess of alkali. Thus, for example, if excess of sodium hydroxide or potassium hydroxide be added to the solution of a soluble salt of zinc, such as the chloride, nitrate, or sulphate, the first change, as already shown, is the precipitation of the hydroxide but on addition of excess of alkali, the precipitate redissolves, forming the... 

Sodium chloride Sodium bromide Sodium iodide Sodium sulphate Sodium silicate Potassium sulphate Lithium chloride Calcium carbonate Calcium sulphate Magnesium sulphate Manganous carbonate Ferrous carbonate. Aluminium phosphate Ammonium nitrate Organic matter... 

Manganous sulphate5 and ferric salts in general accelerate the decomposition of hydrogen peroxide.6 The sulphate is less active than the chloride or nitrate. With dilute solutions of the salts the effect is proportional to the concentration of the peroxide and that of the iron ions, whilst in the presence of acids it is inversely proportional to the hydrogen-ion concentration. The temperature coefficient of the reaction is 3 25 for ten degrees. ... 

Calcium bromide Citric acid Ferric oxide Hydrated lime Manganic oxide Natural fatty acids Potassium bromide Potassium chloride Potassium sulphate Phosphate esters Silicates (inorganic)... 

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