Sodium pyrosulfate

Alcohol sulfates decompose at high temperature. At 100°C they lose any associated water and at 150°C thermal decomposition begins. The organic part of the molecule is completely decomposed at 285 °C. Main decomposition substances of sodium lauryl sulfate are dilauryl ether and sodium pyrosulfate [64]. 

An older Be method, P CAM 121, discusses air, dust, ore, and swipe samples. More vigorous digestion procedures such as hydrofluoric nitric acid for filters or potassium fluoride sodium pyrosulfate fusion and nitric acid digestion for ores. A nitrous oxide/acetylene flame is suggested for this method rarely used (Table HI). 

SYNS GBS NITRE CAKE SODIUM ACID SULFATE SODIUM BISULFATE, FUSED SODIUM HYDROGEN SULFATE, soUd (UN 1821) (DOT) SODIUM HYDROGEN SULFATE, solution (LiN 2837) (DOT) SODIUM PYROSULFATE SULFURIC ACID, MONOSODIUM SALT... 

In some cases, the contents can be dissolved with warm hydrochloric acid or chlorine-free nitric acid. If this does not sirffice, sodium pyrosulfate is heated in the Pt crucible imtil liberation of SO3, the molten liquid is poured out, and the material still adhering to the walls is dissolved with hot water (O. Brunck). The crucible is not damaged at all by this treatment. If the edges of the crucible lid become bent out of shape, they can be smoothed out against a glass plate with a spatula made of horn or plastic. A very badly dented crucible should best be repaired by a goldsmith or other expert. 

The temperature regimes in which this corrosion occurs are summarized in Figure 3.2. The data generally show that K2S2O7 will form from K2SO4 and SO3 at 400°C when SO3 concentration is at least 150 ppm as the temperature increases, the SO3 requirement increases, so that, at 500°C, at least 2000 ppm SO3 will be required to form liquid K2S2O7. Sodium pyrosulfate can form at 390°C with = 2500 ppm SO3, but at 485°C, 2% by volume SO3 will be required. Based on these results and the anticipated maximum level of 3500 ppm SO3 in a pulverized-coal boiler, Reid (1971) concluded that pyrosulfates can contribute to metal loss in the waterwall and economizer tubes but may not be a cause of corrosion in superheaters and reheaters in conventional systems (Natesan 2002). 

Synonyms Acid sodium sulfate Nitre cake Sodium acid sulfate Sodium acid sulfate solid Sodium bisulfate, fused Sodium bisulfate solid Sodium hydrogen sulfate Sodium pyrosulfate Sulfuric acid monosodium salt Empin cal HNa04S Formula NaHS04... 

Sodium pyrosulfate. See,Sodium bisulfate Sodium pyrosulfite. See Sodium metabisulfite Sodium DL-2-pyrrolidone-5-carboxylate Sodium L-2-pyrrolidone-5-carboxylate. See Sodium PCA... 

When beryllium is an essential constituent of tin-free minerals and alloys, its presence can be established by isolating beryllium hydroxide and noting the fluorescence reaction with morin (page 124). Silicate-bound beryllium requires fuming with ammonium fluoride for its release. Solution in dilute hydrochloric acid is sufificient in the case of non-ferrous alloys. Chrysoberyl (AlgOg-BeO) must be fused with sodium pyrosulfate. 

Procedure. The sample should be divided into as small pieces as possible. One or two milligrams are sintered in a platinum spoon with ammonium fluoride, or fused with sodium pyrosulfate, or dissolved in hydrochloric acid and evaporated. The product is rinsed into a micro crucible with as little water as possible. A drop of the liquid is transferred to a depression of a spot plate and the following are stirred in three drops of a saturated solution of Complexone III (versene) in ammonia (1 10) one drop of 0.002 % solution of morin in acetone then one drop of concentrated ammonia. If beryllium is present, the mixture exhibits a strong yellow-green fluorescence in ultraviolet light. 

Sodium pyrosulfate Molten Dissolves metal rapidly over 752°F (400°C)... 

Kiely, P. V., and M. L. Jackson, 1965. Quartz, feldspar, and mica determination for soils by sodium pyrosulfate fusion. Soil Sci. Soc. Am. Proc. 29 159-163. 

The analytical chemistry of titanium has been reviewed (179—181). Titanium ores can be dissolved by fusion with potassium pyrosulfate, followed by dissolution of the cooled melt in dilute sulfuric acid. For some ores, even if all of the titanium is dissolved, a small amount of residue may still remain. If a hiU analysis is required, the residue may be treated by moistening with sulfuric and hydrofluoric acids and evaporating, to remove siUca, and then fused in a sodium carbonate—borate mixture. Alternatively, fusion in sodium carbonate—borate mixture can be used for ores and a boiling mixture of concentrated sulfuric acid and ammonium sulfate for titanium dioxide pigments. For trace-element deterrninations, the preferred method is dissolution in a mixture of hydrofluoric and hydrochloric acids. 

The active phase, which is soHd at room temperature, is comprised of mixed potassium and sodium vanadates and pyrosulfates, whereas the support is macroporous siUca, usually in the form of 6—12 mm diameter rings or pellets. The patent Hterature describes a number of ways to prepare the catalyst a typical example contains 7 wt % vanadium pentoxide, 8% potassium added as potassium hydroxide or carbonate, 1% sodium, and 78 wt % siUca, added as diatomaceous earth or siUca gel, formed into rings, and calcined in the presence of sulfur dioxide or sulfur trioxide to convert a portion of the alkah metal salts into various pyrosulfates (81,82). 

The determination of arsenic by atomic absorption spectrometry with thermal atomisation and with hydride generation using sodium borohydride has been described by Thompson and Thomerson [29], and it was evident that this method couldbe modified for the analysis of soil. Thompson and Thoresby [30] have described a method for the determination of arsenic in soil by hydride generation and atomic absorption spectrophotometry using electrothermal atomisation. Soils are decomposed by leaching with a mixture of nitric and sulfuric acids or fusion with pyrosulfate. The resultant acidic sample solution is made to react with sodium borohydride, and the liberated arsenic hydride is swept into an electrically heated tube mounted on the optical axis of a simple, lab oratory-constructed absorption apparatus. 

Morphin was extracted from the plant vegetable (the poppy) by the mixture of water and methanol or the aqueous solution of potassium pyrosulfate. The precipitation of the morphin was carried out by addition to the extract the aqueous solution of sodium carbonate. 

B. Fuse about 1 mg of sample with about 50 mg of potassium pyrosulfate in a porcelain crucible, cool, and break up the mass with a glass rod. Add 3 mL of water, and dissolve by boiling. Add 1 drop of phenolphthalein TS, mix, and then add drops of a 1 10 solution of sodium hydroxide until just pink. Add 500 mg of sodium acetate, 0.5 mL of 1 N acetic acid, and 0.5 mL of a 1 500 solution of nitroso R salt. A red or orange-red color appears at once. Add 0.5 mL of hydrochloric acid, and boil for 1 min. The red color persists. 

With few exceptions, the common fluxes used in analysis are compounds of the alkali metals. Alkali metal carbonates, hydroxides, peroxides, and borates are basic fluxes used to attack acidic materials. The acidic fluxes are pyrosulfates, acid fluorides, and boric oxide. If an oxidizing flux is required, sodium peroxide can be used. As an alternative, small quantities of the alkali nitrates or chlorates can be mixed with sodium carbonate. 

Monohydrate, odorless crystals. When strongly heated it changes into pyrosulfate. Sol in about 0.8 part water dec by alcohol into sodium sulfate and free HjS04 The eq soln is strongly acid. pH of 0.1 molar soln ].4. 

In sulfonating hydroxyanthraquinones, boric acid is often added to block the free phenolic group by the formation of boric esters, thereby inhibiting oxidation as a destructive side reaction. Sodium sulfate is also added to such sulfonation mixtures presumably pyrosulfate is formed, which is more moderate in its action than oleum. 

Chlorids of Antimony.— Antimony trichlorid—Protochlortd or butter of antimony—SbCla—226.5—is obtained by passing dry Cl over an excess of Sb. S> by dissolving SbjSa in HCl or by distilling mixtures, either of SbjS and mercuric chlorid, or of Sb and mercuric chlorid, or of antimonyl pyrosulfate and sodium, chlorid. 

It is also worth noticing that weighing to constant mass is not a requirement, if the result obtained is below the prescribed limit. This is new in the revised sulfated ash that became official in European Pharmacopoeia IV, which is a result of the international pharmacopoeia harmonization effort. Another difference in the new test is that the old test included a step where sodium carbonate was added to the residue with the purpose of eliminating certain pyrosulfates that allegedly could build up as a result of igniting with sulfuric acid. 

The literature data show that many mediods were used for oxoacidity studies and estimation of the acidic properties of melts. One simplest mefliod involves indicator. Acid-base indicators usually employed in aqueous solutions for protic aeidity measurements have been used for acidity studies in molten KNOj-LiNOj at 210 C and KSCN at 200"C. The color of indicator solution, relative to acidity, changes during titration of bases (sodium hydroxide or peroxide) by potassium pyrosulfate, KjSjOy ... 

These ethers can now be sulfated using any known sulfation agent such as chlorosulfonic acid, sulfur trioxide, pyrosulfate, or oleum to yield the final glyceryl ether sulfates (Figure 8.6) and then neutralized with an alkali metal hydroxide such as sodium hydroxide. The main difference between this molecule and the one described earlier is that all of the hydroxyls will be sulfated whereas the earlier process retains one of the hydroxyl groups. 

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