Ferrous tartrate

Tartratea—Ferrous Tartrate—FeC H O, -f- 2 Aq—203.9 -f 36.— A white, crystalline powder formed by dissolving Fe in hot concentrated solution of tartaric acid. 

Fenton s reagent. To a solution of tartaric acid or a tartrate add 1 drop of freshly prepared ferrous sulphate solution, i drop of hydrogen peroxide solution and then excess of NaOH solution an intense violet coloration is produced, due to the ferric salt of dihydroxyfumaric acid, HOOC C(OH) C(OH)COOH. 

DOUBLE SALT. A hydrated compound resulting from crystallization ol a mixture of ions in aqueous solution. Common examples arc the alums, made by ciystallizing from solution either potassium or ammonium sulfate and aluminum sulfate Rochelle salt (potassium sodium tartrate), made from a water solution of potassium acid tartrate treated with sodium carbonate and Mohr s salt (fertous ammonium sulfate), crystallized Iruin mixed solutions of ferrous sulfate and ammonium sulfate. 

The most unstable form of the amorphous variety is colloidal silver, prepared by reduction of an ammoniacal or dilute alcoholic solution of silver nitrate with sodium citrate, sodium potassium tartrate, dextrin, tannin, or formaldehyde, with subsequent addition of ferrous sulphate.13 If forms a chocolate, pale-lilac, blue, or green mass, and dissolves in water to a deep-red solution. The colour depends partly on the mode of... 

Tartaric acid (200 g., 1.33 moles) is dissolved in 140 ml. of warm water, and to the cooled solution is added a solution of 5 g. of sodium potassium tartrate in 40 ml. of water. The mixture is cooled to —10°, and a solution of 4 g. of ferrous sulfate in 40 ml. of water is added in one portion. The mixture is stirred vigorously and the temperature is held at —5° while 145 ml. of 30% hydrogen peroxide is added slowly (addition requires 5-6 hours). The reaction mixture is stirred for ah additional 2.5 hours at —5° after completion of the addition. The mixture is allowed to stand for a week in an ice chest, and then the precipitated dihydroxymaleic acid is collected by filtration and dried over phosphorus pentoxide. The product contains some iron salt of dihydroxymaleic acid which gives it a pale yellow color. The yield is 42 g. or 24%. 

Salts Compounds formed by the union of acids and bases, by the action of alkalies upon metals, or by the direct union of elements. The term is often incorporated in the common name of salts used as pharmaceuticals bitter salts, epsom salt, or Seidlitz salt (magnesium sulfate), preparing salt (sodium stannate), Preston s salts (ammonium chloride), Rochelle salt or Seignette s salt (potassium and ammonium tartrate), salt of Mars (ferrous sulfate), salt of Saturn (lead acetate), salt of tartar (potassium carbonate), salt of tin (stannous chloride), salt of wisdom (mercury bichloride and ammonium chloride), sore-throat salt (fused potassium nitrate), vinegar salts (calcium acetate), and vomiting salt (zinc sulfate). The term is also applied to some acids, such as salt of lemon or sour salt (citric acid), salt of sorrel (oxalic acid), and spirit of salt (muriatic acid). ... 

The nature of the metal-ions in the active site also varies between species. Whereas the purple acid phosphatase isolated from red kidney beans (rkbPAP) contains Fe and Zn", the tartrate-resistant acid phosphatase isolated from rat osteoclasts (TRAcP) contains two iron atoms in different oxidation states, an stabilized Fe ion and a redox-active Fe ion. In this way, the ability of the ferrous ion to act as an electron donor confers to the enzyme an alternative function as generator of reactive oxygen species (ROS) [20, 21]. The enzyme may appear in an inactive purple form when the redox-active iron is oxidized to the ferric state, or it can be in an active pink form where the redox-active iron is reduced to the ferrous state [22]. In particular, the tartrate-resistant acid phosphatase isolated from osteoclasts is synthetized as a precursor which is activated by cysteine proteinases resulting in an active two subunit enzyme [23]. 

Electrolytes which do not afford ionic complexes with common hexitols and reducing sugars are aqueous solutions of lead acetate, copper sulfate, zinc sulfate, ferrous ammonium sulfate, calcium chloride, potassium dichromate, ferric chloride (pH 3), aluminum sulfate, magnesium sulfate, sodium sulfate, potassium antimonyl tartrate, sodium arsenate or arsenic acid, sodium phosphate, and hydrochloric acid. It is not certain whether sodium aluminate (in 0.1 N sodium hydroxide) affords ionic complexes with carbohydrates, as aqueous alkali, alone, permits their migration during electrophoresis. 

Beside the tartrate, other organic salts—notably the oxalate and the formate—yield the more easily produced pyrophoric metals, i.e. lead, nickel, and cobalt, if the pyrogenic decomposition is performed at low temperature. These organic salts or the oxides of nickel, cobalt, and iron, under hydrogen at about 300X, also furnish the self-flammable metals, but in the case of iron, a pyrophoric ferrous oxide (FeO) may first appear by reduction with hydrogen as well as by reduction under carbon monoxide. 

Salicylsulfonic acid. See 5-Sulfosalicylic acid Saline. See Sodium chloride Salinide. See Salicylanilide Salix alba Salix alba bark extract. See Willow (Salix alba) bark extract Salmiac. See Ammonium chloride Sal mine sulfate. See Protamine sulfate Salol. See Phenyl salicylate SALP. See Sodium aluminum phosphate acidic Sal soda. See Sodium carbonate Salt. See Sodium chloride Sal tartar. See Sodium tartrate Salt cake. See Sodium sulfate Salt of Mohr. See Ferrous ammonium sulfate Saltpeter. See Potassium nitrate Salt of Saturn. See Lead acetate Salt of tartar. See Potassium chlorate Potassium carbonate Salt of tarter. See Potassium chlorate Salt of tin. See Stannous pyrophosphate Salvia. See Sage (Salvia officinalis)... 

Insoluble salts can be made to mask an unpleasant taste or to prevent local irritation of the gastrointestinal tract. Well-known examples are ferrous fumarate suspension and potassium hydrogen tartrate suspension. In Sect. 5.4.10 more examples of insoluble salts to mask unpleasant tastes are discussed. 

Examples of other substances that may contain more than 4 % impurities are dexamethasone sodium phosphate, ergotamine tartrate, erythromycin, codergocrine mesilate, cyanocobalamin, hydroxycobalamin, thiamine hydrochloride and ferrous fumarate. 

Yoshiaki Miura has published [1] a procedure for the determination of iron and copper in aluminum alloys, using ethylenediamine tartrate (EDT) and potassium pyrophosphate as base electrolyte. As a result of this investigation, polarographic procedures using ethylenediamine tartrate complexes have been developed for the determination of iron (ferrous), nickel, cadmium, and copper, as well as for mixtures of the latter three elements. 

Tartrates give soluble, more or less stable, complexes with miscellaneous cations such as copper, bismuth, and iron, with some metallic hydroxides, acids (such as boric acid), and antimony oxide. The cations become masked by complexation. The identity reaction is carried out, according to the European pharmacopeia, with Fenton s reagent (ferrous sulfate and perhydrol). In a first step, dihydroxyftimaric acid is formed ... 

To 10 ml of the injection add 20 mg of sodium metabisulphite, 0 1 ml of freshly-prepared ferrous sulphate-citrate solution and 1 ml of the buffer reagent. Mix, allow to stand for ten minutes and extract with 10 ml of ether. Reject the ether after separation and measure the extinction at 540 m/i. Calculate the adrenaline content by reference to a curve prepared by treating suitable quantities of a standard solution of adrenaline acid tartrate by the same process. 

Freeman and Morrison (1949) have given a detailed procedure for the production of this antibiotic from T. roseum F227. The medium contained 50g of glucose, 2 g of ammonium tartrate, 0.5 g of magnesium sulfate, 1 g of potassium hydrogen phosphate, 0.5 g of potassium chloride, 0.01 g of ferrous sulfate, 10 ml of corn steep liquor, and sufficient water to make 1000 ml of solution. After the pH was adjusted to 5, the culture was allowed to stand for 28 days at 25 , filtered, the filtrate extracted with chloroform, and the chloroform evaporated. Final purification was effected by chromatography on alumina, and gave about 36 mg of trichothecin (I) per 1 of culture filtrate. 

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