Potassium Acetate Solution Acid Tartrate

Add a few drops of acetic acid and a little ammonium or potassium acetate solution to a moderately strong solution of tartaric acid or a neutral tartrate. On stirring with a glass rod, the acid potassium or ammonium tartrate will be precipitated. 

Potassium acetate, 20 629-630 Potassium acid tartrate, 20 637 Potassium alkoxides, 20 604-605 Potassium a-hydrohexafluoroisobutanoyl fluoride, 13 724 Potassium amides, 20 605 Potassium analysis, of water, 26 31 Potassium arsenite (Fowler s solution), 3 276... 

Lead acetate solution white precipitate of lead sulphate, PbS04, soluble in hot concentrated sulphuric acid, in solutions of ammonium acetate and of ammonium tartrate (see under Lead, Section III.4, reaction 5), and in sodium hydroxide solution. In the last case sodium tetrahydroxoplumbate(II) is formed, and on acidification with hydrochloric acid, the lead crystallizes out as the chloride. If any of the aqueous solutions of the precipitate are acidified with acetic acid and potassium chromate solution added, yellow lead chromate is precipitated (see under Lead, Section III.4, reaction 6). 

Potassium chloride solution When a concentrated neutral solution of a tartrate is treated with a solution of a potassium salt (e.g. potassium chloride or potassium acetate) and then acidified with acetic acid, a colourless crystalline precipitate of potassium hydrogen tartrate, KH.C4H406, is obtained. The precipitate forms slowly in dilute solutions crystallization is induced by vigorous shaking or by rubbing the walls of the vessel with a glass rod. 

Tartaric Acid (Dextrorotary).—For our knowledge of the deportment of this acid on electrolysis we are also indebted to Bourgoin. The free acid is partially oxidized to carbon dioxide and carbon monoxide, while the solution contains acetic acid. Neutral potassium tartrate gives principally carbon dioxide besides a little carbon monoxide and oxygen, acid potassium tartrate being at the same time deposited. In alkaline solutions the gases carry with them traces of ethane, the formation of which is due to potassium acetate which is found present in the solution at the end of the operation. 

Complexing agents, which act as buffers to help control the pH and maintain control over the free metal—salt ions available to the solution and hence the ion concentration, include citric acid, sodium citrate, and sodium acetate potassium tartrate ammonium chloride. Stabilizers, which act as catalytic inhibitors that retard the spontaneous decomposition of the bath, include fluoride compounds thiourea, sodium cyanide, and urea. Stabilizers are typically not present in amounts exceeding 10 ppm. The pH of the bath is adjusted. 

After having been washed with 50 cc of water the benzene layer is dried over potassium carbonate, filtered, allowed to stand over 10 g of alumina for about VA hours for partial decolorization, filtered again and concentrated under reduced pressure. The oily base which remains as a residue is directly converted into the tartrate. A solution cooled to 0°C, of 6.50 g of the free base in 100 cc of acetic acid ethyl ester is thoroughly shaken and poured into an ice cold solution of 2.66 g of tartaric acid in 410 cc of acetic acid ethyl ester. The precipitated, analytically pure, tartrate of 3-methylsulfinyl-10-[2 -N-methyl-piperidyl-2")-ethyl-1 ]-phenothiazine melts at 115° to 120°C (foam formation) and sinters above B0°C. The base Is reacted with benzene sulfonic acid in a suitable solvent to give the besylate. 

Calcium. — On dissolving 1 gm. of potassium and sodium tartrate in 10 cc. of water, and adding to the solution 5 cc. of dilute acetic acid, and then shaking for a few minutes, a crystalline precipitate forms. On filtering off the latter, diluting the filtrate with an equal volume of water, and then adding 8 to 10 drops of ammonium oxalate solution, no turbidity should develop within one minute. 

Sodium hexanitrocobaltate (III) (Na3[Co(N02)6]) Tartaric acid solution (sodium acetate buffered) Yellow precipitate of potassium hexanitrocobaltate (III) insoluble in acetic acid White precipitate of potassium hydrogen tartrate... 

Place a drop of the reagent upon drop-reaction paper, add one drop of the test solution (which should be slightly acidified with acetic acid (2m) containing a little sodium potassium tartrate), and then one drop potassium hydroxide (2m). A bright-pink spot, surrounded by a blue circle, is produced. 

Copper hydroxide test Tartrates dissolve copper hydroxide in the presence of excess alkali hydroxide solution to form the dark-blue ditartratocuprate(II) ion, [Cu(C4H406)2]2-, which is best detected by filtering the solution. If only small quantities of tartrate are present, the filtrate should be acidified with acetic acid and tested for copper by the potassium hexacyanoferrate(II) test. 

The experimental details are as follows. Treat the test solution with an equal volume of 2m sodium or potassium hydroxide (or treat the test solid directly with a few ml of the alkali hydroxide solution, warm for a few minutes with stirring and then cool), add a few drops of 0-25m copper sulphate solution (i.e. just sufficient to yield a visible precipitate of copper(II) hydroxide), shake the mixture vigorously for 5 minutes, and filter. If the filtrate is not clear, warm to coagulate the colloidal copper hydroxide and filter again. A distinct blue colouration indicates the presence of a tartrate. If a pale colouration is obtained, it is advisable to add concentrated ammonia solution dropwise when the blue colour intensifies it is perhaps better to acidify with 2m acetic acid and add potassium hexacyanoferrate(II) solution to the clear solution whereupon a reddish-brown precipitate or (with a trace of a tartrate) a red colouration is obtained. 

Acetic acid (2 mL) was added to a stirred suspension of tetramethylanunonium triace-toxyborohydride (1.54 g, 5.85 nunol) in acetonitrile (2 mL) at room temperature. The mixture was stirred at room temperature for 30 min and then cooled to -40 °C. The P-hydroxyketone (300 mg, 0.731 mmol) in acetonitrile (2 mL) was added dropwise at this temperature. A solution of camphorsulfonic acid (85 mg, 0.366 mmol) in a mixture of acetic acid acetonitrile (1 1,4 mL) was added, and the mixture was allowed to warm to -22 °C over 18 h. The mixture was poured into saturated aqueous NaHCOs (50 mL). A saturated aqueous solution of sodium potassium tartrate (50 mL) was added, followed by ether (100 mL), and the mixture was stirred vigorously at room temperature for 8 h. The layers were separated, and the aqueous layer was extracted with EtOAc (3 x 50 mL). The combined organic extracts were washed with water (50 mL), brine (50 mL), and dried (MgSO4). The solvent was removed under vacuum to afford 300 mg (99.5%, dr >97 3) of the anz/-l,3-diol as a colorless oil. 

Separation of Pd with a collector. To the sample solution (-100 ml) in 0.1 M HCl, containing not more than 50 pg of Pd and heated to 80°C, add a macerated filter paper and 1 ml of 5% oxalic acid solution. Keep the solution at 80°C for 1 h, then allow it to cool. Filter off the precipitate of elemental gold and silver chloride together with the paper. To the filtrate add successively 2 mg of nickel (as its sulphate solution), 2 ml of 20% potassium sodium tartrate solution [to mask Fe(IIl), Al, Ti, etc.], 2 g of sodium acetate, 1 ml of 0.1 A/ EDTA, and 2 ml of the H2Dm solution (pH -6.5). After 30 min, filter off the precipitate of nickel- and palladium dimethylglyoximates. Wash the precipitate from the filter paper into a beaker, add 1 ml of cone. HCl, and evaporate to 5-10 ml, depending on the quantity of Pd in the solution. 

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. 

The fraction of more soluble Chelidonium alkaloids from which most of the bases have been removed is treated in dilute acid solution with an excess of aqueous potassium cyanide. The precipitate is separated by filtration and washed thoroughly with dilute acetic acid. After drying it is repeatedly crystallized from acetone until most of the chelerythrine -cyanide is recovered in the least soluble fractions. The more soluble product is then decomposed by boiling in ethanol with hydrochloric acid, and the free base is recovered and converted to its hydrogen tartrate. The tartrate crystallizing from the more soluble fractions is that of pure sanguinarine, does not have methoxyl, and is identical with -chelerythrine (19). 

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