Manganese bromate

The products of the reaction between bromide ions and permanganate ions, Mn04, in basic aqueous solution are solid manganese(IV) oxide, MnO>, and bromate ions. Balance the net ionic equation for the reaction. 

Barium-bearing manganese silicon, 22 519 Barium P-alumina, 2 406t Barium bromate, 4 335 Barium bromide, 3 355... 

Lead dioxide Lead perchlorate Lithium chlorate Lithium hypochlorite Lithium perchlorate Lithium peroxide Magnesium bromate Magnesium chlorate Magnesium perchlorate Magnesium peroxide Manganese dioxide Mercurous chlorate Mono-(trichloro)-tetra-(mono-potassium dichloro)-penta-s-triazinetrione... 

Intimate mixtures of chlorates, bromates or iodates of barium, cadmium, calcium, magnesium, potassium, sodium or zinc, with finely divided aluminium, arsenic, copper carbon, phosphorus, sulfur hydrides of alkali- and alkaline earth-metals sulfides of antimony, arsenic, copper or tin metal cyanides, thiocyanates or impure manganese dioxide may react violently or explosively, either spontaneously (especially in presence of moisture) or on initiation by heat, friction, impact, sparks or addition of sulfuric acid [1], Mixtures of sodium or potassium chlorate with sulfur or phosphorus are rated as being exceptionally dangerous on frictional initiation. 

The violence of the explosion is feebler with iodates than it is with chlorates or bromates. The chlorates transform lead oxide to the dioxide manganese oxide in fused alkalies to manganates etc. Ammonium iodate explodes when heated alone. Chloric, bromic, and iodic acids with their salts are energetic oxidizing agents. 

Tetra(3-aminopropanethiolato)trimercury perchlorate, 3576 Tetraacrylonitrilecopper(I) perchlorate, 3504 Tetraammine-2,3-butanediimineruthenium(III) perchlorate, 1788 Tetraamminebis(dinitrogen)osmium(II) perchlorate, 4065 Tetraamminecadmium permanganate, 3950 Tetraamminecopper(II) bromate, 0263 Tetraamminecopper(II) nitrate, 4270 Tetraamminecopper(II) nitrite, 4269 Tetraamminecopper(II) sulfate, 4268 Tetraamminedithiocyanatocobalt(III) perchlorate, 0965 Tetraamminehydroxynitratoplatinum(IV) nitrate, 4589 Tetraamminepalladium(II) nitrate, 4583 Tetraamminezinc peroxodisulfate, 4581 1,4,8,1 l-Tetraazacyclotetradecanenickel(II) perchlorate, 3370 Tetrakis(3-methylpyrazole)cadmium sulfate, 3710 Tetrakis(3-methylpyrazole)manganese(II) sulfate, 3711... 

Manganese fluoride trioxide, 4295 Manganese tetrafluoride, 4337 Manganese(IV) oxide, 4700 Manganese(VII) oxide, 4704 Mercury(II) bromate, 0269 Mercury(II) nitrate, 4598 Mercury(II) oxide, 4600 Monofluoroxonium hexafluoroarsenate, 0097 Neptunium hexafluoride, 4360 Nickel(II) nitrate, 3583... 

Concentrated HCI Manganese (II) sulfate + phosphoric acid Chlorine dioxide gas evolved, imparts yellow color to acid Violet coloration due to diphosphatomanganate formation peroxydisulfate nitrates, bromates, iodates, and periodates react similarly... 

Manganese (II) sulphate test If a bromate solution is treated with a little of a 1 1 mixture of saturated manganese(II) sulphate solution and m sulphuric acid, a transient red colouration (due to manganese(III) ions) is observed. Upon concentrating the solution rapidly, brown, hydrated manganese dioxide separates. The latter is insoluble in dilute sulphuric acid, but dissolves in a mixture of dilute sulphuric and oxalic acids (difference from chlorates and iodates, which neither give the colouration nor yield the brown precipitate). 

To 2 ml of the soda extract add 1 ml concentrated hydrochloric acid and 2 ml of the manganese(II) chloride reagent. A brown (or black) colouration indicates the presence of nitrate, nitrite, hexacyanoferrate(III), chlorate, bromate, iodate, chromate or permanganate. A negative test indicates the absence of the above oxidizing agents except small amounts of nitrates and nitrites and of arsenate if reducing anions have been found, this test is inconclusive. 

Indications. A blue colour indicates the presence of an oxidising agent such as bromate, chlorate, chromate, dichromate, iodate, lead (IV), manganese (III, IV, VII), nitrate, nitrite, permanganate, or vanadate. 

Ignites on contact with metal oxides (e.g., barium peroxide, chromium trioxide, copper oxide, lead dioxide, manganese dioxide, nickel oxide, silver(I) oxide, silver(II) oxide, sodium peroxide, thallium(III) oxide, mercury oxide, calcium oxide, nickel oxide), oxidants (e.g., silver bromate, heptasilver nitrate octaoxide, dibismuth dichromium nonaoxide, mercury(I) bromate, lead(II) hypochlorite, copper chromate, fluorine, nitric acid, sodium peroxide, lead(IV) oxide), rust, soda-lime + air. Reacts violently with NI3, NF3, p-bromobenzenediazonium chloride, OF2, F2, Cu, CIO, BrFs,... 

The Belousov-Zhabotinsky reaction demonstrated here is set in train by the reduction of potassium bromate to elemental bromine by malonic acid and manganese(II) sulfate this is shown by the orange coloration. The reaction of the bromine with malonic acid to give mono or dibromomalonic acid leads to decolorisation. At the same time more bromine is formed in the initial redox process, and this again replaces one or two hydrogen atoms of the malonic acid. The process is repeated many times the start reaction is inhibited by complexa-tion of the brominated malonic acid by Mn(ll) ions, so that the oscillation slowly comes to an end. ... 

IIIC, D) Geiseler, W. Multiplicity, Stability and Oscillations in the Stirred Flow Oxidation 1982-2 of Manganese(II) by Acidic Bromate. J. Phys. Chem. 86(22) 4394-4399. 

IIIC, D) Maselko, J. Experimental Studies of Complicated Oscillations. The System Manganese 1980-1 (2+) ion-malonic acid-potassium bromate-sulfuric acid. Chem. Phys. 51(3) 473-480... 

Example 14.3. The Belousov-Zhabotinsky reaction [22,27-29], The reaction is an oxidation of malonic acid by bromate ion in sulfuric acid, catalyzed by a Ce(III)/Ce(IV) redox couple. Many variations with other organic acids and transition-metal ions are possible [22] (Belousov used citric acid, and manganese, ruthenium, or iron can replace cerium). The color of the solution alternates between clear [Ce(III)] and pale yellow [Ce(IV)], and more dramatically between red and blue if ferroin is added as indicator. 

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