Sodium citrate.5 hydrate

Viossat B, Rodier N, Eberly J (1986) Crystal stmeture of sodium citrate hydrate. Bull Soc Chim France 522-525... 

H =0.1 M sodium citrate dihydrate (29.41 g in 1000 ml) avoid using any other hydrated salt I = 0.2 M acetic acid... 

All consistency measurements were conducted by adding 0.2-g sodium citrate to 100 mL of gaging water to prevent premature stiffening caused by hydration of the stucco. 

Fig. 1 ID NMR spectra (800 MHz for H) of CN-bR (a), HDCN-bR (b), and DCN-bR (c), fully hydrated in sodium citrate buffer and collected under very similar conditions. Adapted from [119] with permission from Elsevier B.V...

The tissue mass was dried at ambient temperature until no detectable residual solvent was evident. Aqueous extractions of the 93% moisture washed orange pulp were performed with 0.4 M sodium citrate, 0.2 M EDTA, 0.1% H PO, 0.5% Na2C0, and 5% NaOH solutions in respective experiments In each case 200 ml of extracting solution was added to 100 grams of pulp and stirred for three hours of 25 C. After filtration the extracted tissue was washed three times with 200-250 ml of 50°C distilled water and filtered. Those samples for OHC or WHC were then freeze dried. Samples for microscopic examination were kept in the hydrated state. 

CAS 68-04-2 (anhyd.) 6132-04-3 (dihydrate) 6858-44-2 (hydrate) EINECS/ELINCS 200-675-3 FEMA 3026 INS331(iii) E331 Synonyms Citric acid trisodium salt Sodium citrate (INCI) Sodium citrate anhydrous Sodium citrate tertiary Trisodium 2-hydroxypropane-1,2,3-tricarboxylate Empirical CeHsNasO (anhyd.) CeHsNasO 2H2O (dihydrate)... 

There are a number of reports on the synthesis of Au NPs-rGO composites by adopting in situ methods such as chemical reduction, electrochemical deposition, microwave irradiation, and sonochemical reduction [14, 18, 23]. In most of the reduction methods, a GO suspension in water or ethanol is mixed with Au salt, the resulting mixture is then reduced with different reducing agents like sodium borohydride, hydrazine hydrate, glucose, ascorbic acid, sodium citrate, beer solution, oleylamine, ethylene glycol, etc., which results in. simultaneous reduction of the Au ions and GO to form Au NPs-rGO composites. 

Morris speculated that the precipitate was a ferrous [Fe(ll)] salt. Hamm et al. identified three Fe(ll) complexes in aqueous solutions of citric acid and ferrous iron FeHCit, FeCit, and FeOHCit. Because FeHCit is the only identified uncharged species, the precipitate probably contained this compound. The aqueous chemistry of ferric/citric acid is more complex than the ferrous chemistry. The known Fe(lll) complexes include FeHCit, FeCit FeOHCit, and Fe(OH)2Cit. In addition, Bobtelsky and Jordan identified additional iron complexes (such as Fe2Cit3) in solutions containing sodium citrate and Fe(lli). These authors also offer evidence that hydrated species may be present. One composition that solved the iron precipitate problem was patented by Reich. He made mixtures of citric acid with formic acid that did not produce precipitates during the removal of mill scale from steel pipes. 

Ciavatta L, De Tommaso G, luliano M (2001) The solubility of calcium citrate hydrate in sodium perchlorate solutions. Anal Lett 34 1053-1062... 

Ramachandran and LoweryP l applied conduction calorimetry to the study of the relative effects of various retarders on the hydration of cement. The retarders used were calcium gluconate, glucose, glycolic acid, molasses, sodium borate, sodium citrate, sodium heptonate, sodium hexametaphosphate, sodium pyrophosphate, sugar-free lignosulfonate, and sucrose. The dosage of the chemicals varied between 0.025 and 1.2%. 

Tyrosinase (PPO) [E.C 1.14.18.1] was purchased from Sigma. Pyrrole was purchased from Aldrich and sodium dodecyl sulfate (SDS) from Sigma. Pyrrole was distilled before use. MBTH, acetone and sulfuric acid used in spectrophotometric activity determination of PPO were also obtained from Sigma. For preparation of citrate buffer, tri-sodium citrate-2 hydrate and citric acid were used as received. 

ACETIC ACID, LEAD(II) SALT TRIHYDRATE (6080-56-4) Pb(C2H302)2 3H20 Contact with acids forms acetic acid. Incompatible with oxidizers, bases, acetic acid alkalis, aUcylene oxides, ammonia, amines, bromates, carbonates, citrates, chlorides, chloral hydrate cresols, epichlorohydrin, hydrozoic acid, isocyanates, methyl isocyanoacetate, phenols, phosphates, salicylic acid sodium salicylate, sodium peroxyborate, potassium bromate resorcinol, salicylic acid, strong oxidizers, sulfates, sulfites, taimin, tartrates, tinctures trinitrobenzoic acid, urea nitrate. On small fires, use dry chemical, Halori, or CO2 extinguishers. 

C4H604Pb Pb(CH3COO)2 Violent reaction with bromates, carbonates, phenols, phosphates potassium bromate (possible explosion). Contact with strong acids forms acetic acid. Reacts with strong oxidizers. Incompatible with alkalis, alkylene oxides, ammonia, amines, carbonates, citrates, cresols, chloral hydrate, chlorides, epichloro-hydrin, hydrozoic acid, isocyanates, methyl isocyanoacetate, phenol, phosphates, potassium bromate, resorcinol, salicylic acid, sodium salicylate, sodium peroxyborate soluble sulfates sulfites, tannin, tartrates, some tinctures triiutrobenzoic acid, urea nitrate. In the heat of fire lead oxides and acetic acid fumes are formed. 

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