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Updated: June 18, 2025
!Answer!: 35.89% FeO; 10.03% Al O . A sample of magnesia limestone has the following composition: Silica, 3.00%; ferric oxide and alumina, 0.20%; calcium oxide, 33.10%; magnesium oxide, 20.70%; carbon dioxide, 43.00%. In manufacturing lime from the above the carbon dioxide is reduced to 3.00%. How many cubic centimeters of normal KMnO will be required to determine the calcium oxide volumetrically in a 1 gram sample of the lime?
This is possible even under the most favorable conditions, and for this reason the iron precipitate is redissolved and again precipitated to free it from calcium. The aluminium is then determined by difference, after subtracting the weight of ferric oxide corresponding to the amount of iron found.
Ferrous salts may be promptly and completely oxidized to ferric salts, even in cold solution, by the addition of potassium bichromate, provided sufficient acid is present to hold in solution the ferric and chromic compounds which are formed. The acid may be either hydrochloric or sulphuric, but the former is usually preferred, since it is by far the best solvent for iron and its compounds.
The precipitate is first submitted to the action of ferric chloride to dissolve the copper, and the residue is fused with charcoal and soda to separate the selenium. The regulus from this operation is dissolved, and a compound of selenium and palladium, or of these with platinum, is obtained. They are composed of equal atoms of the two metals and form hard brilliant plates.
Whatever the character of the compound may be, it has been shown that it loses sulphuric anhydride upon ignition, causing low results, even though the precipitate contains iron. The contamination of the barium sulphate by iron is much less in the presence of ferrous than ferric salts.
Iodine sol. = 15.59; 1 cc. Iodine sol. = 1.086 cc. Na S O sol.; 1 cc. Na S O = 0.005044 gram Cu. Calculate the percentage of sulphur. !Answer!: 0.107%. Given the following data, calculate the percentage of iron in a sample of crude ferric chloride weighing 1.000 gram.
The ferric thiocyanate differs from the great majority of salts in that it is but very little dissociated in aqueous solutions, and the characteristic color appears to be occasioned by the formation of the un-ionized ferric salt. If the ammonium thiocyanate is used, the amount is 76.08 grams.
Its value as a paint is due to the presence of ferric oxide, of which it contains more than any of the French, Australian, American, Irish, or Welsh ochres. Ferric oxides have long been recognized as the essential constituents of such paints as Venetian red, Turkish red, oxide red, Indian red, and scarlet. They are most desirable, being quite permanent when exposed to light and air.
If a solution of ferric oxide and manganese ammonium oxalate is submitted to electrolysis, without the previous addition of ammonium oxalate, the characteristic color of permanganic acid immediately makes its appearance, and the peroxide gradually precipitates itself on the positive, while the iron is deposited on the negative electrode.
The addition of a solution of potassium or ammonium thiocyanate to one of silver in nitric acid causes a deposition of silver thiocyanate as a white, curdy precipitate. If ferric nitrate is also present, the slightest excess of the thiocyanate over that required to combine with the silver is indicated by the deep red which is characteristic of the thiocyanate test for iron.
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