Ferrous Ammonium Sulphate

Besides Fe-, other reducing agents that may be used in conjunction with H2O2 are aliphatic amines, Na2S203 thiourea, ascorbic acid, glyoxal, sulfuric acid, NaHSOs, sodium nitrite, ferric nitrate, peroxidase, AgNOs, tartaric acid, hydroxylamine, ethylene sulfate, sodium phosphite, formic acid, ferrous ammonium sulphate, acetic acid, ferrous sulphate, and HNO2, etc,... 

Ferroin 175, 365, 381 modification by substituents, 366 prepn. of indicator solution, 175, 365 Ferromanganese analysis of, (ti) 336 Ferrous ammonium sulphate see Ammonium iron(II) sulphate Ferrous iron see Iron(II)... 

Cellulose Chemistry , London (1947), 245—47 22) B.T. Fedoroff, Rapid Method for the Determination of Nitrogen Content of Nitrocellulose by the Ferrous Ammonium Sulphate Method , PACLR 122871 (1948) 23) J. Pearson... 

Ferrous ammonium sulphate Ferrous chloride Ferrous sulphate Lead nitrate Lithium chloride... 

To examine the oxidation of Fe2+ to Fe3+, in the second experiment, 10 ml solution of 0.1 M ferrous ammonium sulphate was taken separately in four different beakers and sonicated for 15, 30, 45 and 60 min, before transferring the solution to a 25 ml volumetric flask and adding to it 10 ml of 0.01 M KSCN and making upto the mark with deionised water. The absorbance of these solutions was measured at 4-,iax 451 nm. Sonication of ferrous ammonium sulphate solutions oxidised ferrous ions to ferric ions, which in the presence of thiocyanate ions, produced an intense red coloured complex Fe(SCN)63, in proportions to the oxidation of ferrous ions to ferric ions, as could be seen in Fig. 10.1. 

Ferrous ammonium sulphate, approximately 0.4 M - carefully add 5 ml sulphuric acid (98% m/m H SO ) to 1.5 I water, stir slowly to dissolve, then add 314 g ammonium ferrous sulphate [(NH4)2S04.FeS04.6H20, mol. wt 392.14] stir to dissolve and dilute to 2 I. 

If the standardization titration was 26 ml ferrous ammonium sulphate solution, it had reacted with 25 ml acid-dichromate containing 1.668 mmol. If the back-titration of the residual acid-dichromate was 10 ml ferrous ammonium sulphate solution, then the residual acid-dichromate amounted to 10 x 1.668/26 = 0.642 mmol. The amount used to oxidize the organic carbon is therefore... 

A simple test for ether peroxides is to add 10ml of the ether to a stoppered cylinder containing 1ml of freshly prepared 10% solution of potassium iodide containing a drop of starch indicator. No colour should develop during one minute. Alternatively, a 1% solution of ferrous ammonium sulphate, O.IM in sulphuric acid and O.OIM in potassium thiocyanate should not increase appreciably in red colour when shaken with two volumes of the ether. 

Ally I acetate [591-87-7] M 100.1, b 103°, d 0.928, n4 1.40488, nD27 1.4004. Freed from peroxides by standing with crystalline ferrous ammonium sulphate, then washed with 5% NaHCC, followed by saturated CaCl2 soln. Dried with Na2S04 and fractionally distd in an all-glass apparatus. 

Sydrosulphites may also be determined accurately by titration with standard ferricyanide 6 solution using ferrous ammonium sulphate as indicator the reaction is expressed by the equation ... 

Pale, bluish-green crystals, or light, bluish-green crystalline powder, soluble in 6 parts of cold water. Ferrous ammonium sulphate contains exactly one seventh of its weight of Fe in the ferrous condition. 

Ferric Salts,—The solution of 1 gm. of powdered ferrous ammonium sulphate in 20 cc. of boiled and cooled water (freed from oxygen), with 1 cc. of hydrochloric acid, should not afford an immediate red color on adding a few drops of potassium sulphocyanate solution. 

Copper, Zinc, and Alkali Salts. — Dissolve 5 gm. of ferrous ammonium sulphate in 50 cc. of water, add 5 cc. of nitric acid (sp. gr. 1.3), and boil the solution for a few minutes then add to the liquid 15 cc. of ammonia water, let stand for about one hour, and filter. The filtrate must be colorless (copper). 

Quantitative Determination. — Dissolve 1 gm. of ferrous ammonium sulphate in 50 cc. of well-boiled and cooled water, add 10 cc. of dilute sulphuric acid, and titrate with decinormal potassium permanganate solution. 

The estimation of a vanadate solution by direct titration with ferrous sulphate or ferrous ammonium sulphate solution has been worked out, and is found to be specially applicable to the analysis of vanadium alloys. The vanadate is again reduced to tire tetravalent state by the ferrous salt, the end point being obtained by the use of potassium ferricyanide as internal indicator alternatively, a known excess of the ferrous salt solution is added to the vanadate, the amount unused... 

The conditions under which the formation of the arsenides Fe3As and Fe5As4 may occur are indicated on p. 65. The former was obtained by Brakl 1 as a black precipitate by the action of arsine on an alcoholic solution of ferrous ammonium sulphate. The product was only slightly attacked by concentrated hydrochloric or sulphuric acid but was soluble in nitric acid, aqua regia and bromine water. 

Many alloys and compounds have an equal claim to be considered in two or more volumes of this series, but this would entail unnecessary duplication. For example, alloys of copper and tin might be dealt with in Volumes II. and V. respectively. Similarly, certain double salts—such, for example, as ferrous ammonium sulphate—might very logically be included in Volume II. under ammonium, and in Volume IX. 

Standardisation.—3-5 gms. of pure ferrous ammonium sulphate are dissolved in distilled water, 100 c.cs. of 5N sulphuric acid added, and the whole made up to 250 c.cs. 25 c.cs. of this are oxidised with potassium... 

T. Curtius and J. Rissom showed that the evaporation of a soln. of manganese carbonate in hydrazoic acid gives a pulverulent, non-crystalline manganese hydroxyazide, Mn(OH)(N3)2, which cannot be purified by re-crystallization. The product is sparingly soluble in water it does not explode by percussion, but does so on a hot plate. L. Wohler and F. Martin gave 203° for the explosion temp, of manganese azide. T. Curtius and J. Rissom obtained a colourless soln. of ferrous azide by the action of sodium azide on a soln. of ferrous ammonium sulphate when boiled, the salt decomposes and when shaken in air, a blood-red soln. of ferric azide is formed. The same salt can also be obtained directly from ferric salts. When the soln. of ferric azide is boiled, ferric hydroxide is precipitated and, added T. Curtius and A. Darapsky, if allowed to stand in... 

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