124-43-6

Usage

Uses

Used in Pharmaceutical and Cosmetic Industries:
Urea hydrogen peroxide is used as an antiseptic, disinfectant, and bleaching agent in the pharmaceutical and cosmetics industries. It is particularly effective in the whitening of teeth and provides relief for minor inflammation of gums, oral mucosal surfaces, and lips.
Used in Dental Care:
In dental care, urea hydrogen peroxide is used as a whitening agent for teeth and as a treatment for minor gum inflammation.
Used in Plastics Production:
Urea hydrogen peroxide finds application in the preparation of plastics, making it a valuable component in the manufacturing process.
Used in Blueprint Development:
It is also utilized in the development of blueprints, contributing to its versatility in various industries.
Used in Starch Modification:
Urea hydrogen peroxide is employed in the modification of starch, enhancing its properties for different applications.
Used as a Source of Hydrogen Peroxide in Laboratories:
In addition to its other uses, urea hydrogen peroxide is used as a source of hydrogen peroxide that is easily handled in laboratory settings.
Used for Extemporaneous Preparation of H2O2:
Urea hydrogen peroxide is also used for the extemporaneous preparation of hydrogen peroxide, providing a convenient and efficient method for producing this important compound.
Brand Name Example:
One brand that utilizes urea hydrogen peroxide is Murine Ear Drops (Ross).

Air & Water Reactions

Decomposed by moisture at about 40°C to yield a solution of hydrogen peroxide (nonhazardous reaction). Water soluble.

Reactivity Profile

Urea hydrogen peroxide is an oxidizing agent. Liable to spontaneous combustion when heated or in contact with organic materials. The contents of a screw-capped brown glass bottle spontaneously erupted after four years storage at ambient temperature. [MCA Case History No. 719]. Combustion may release Irritating ammonia gas.

Health Hazard

Inhalation of dust causes irritation of nose from hydrogen peroxide formed when heated. Contact with eyes causes severe damage. Contact with moist skin causes temporary itching or burning sensation. Ingestion causes irritation of mouth and stomach.

Flammability and Explosibility

Notclassified

Clinical Use

Carbamide peroxide (Gly-Oxide) is a stable complex of ureaand hydrogen peroxide. It has the molecular formulaH2NCONH2 H2O2. The commercial preparation is a solutionof 12.6% carbamide peroxide in anhydrous glycerin.When mixed with water, hydrogen peroxide is liberated.Carbamide peroxide is used as both an antiseptic and disinfectant.The preparation is especially effective in the treatmentof oral ulcerations or in dental care. The oxygen bubblesthat are liberated remove debris.

Purification Methods

It is a safe alternative to H2O2 in various oxidation reactions. It is commercially available in tablets (“rapidly soluble”, equivalent to ~30% H2O2) or as a white powder (with 15-17% active oxygen). It is usually used without purification after assaying for active oxygen. This is done by titration with potassium permanganate or by iodometry, i.e. titration of liberated iodine when glacial acetic acid containing Fe3+ and NaI are added. It can be recrystallised from 30% H2O2 in a molar ratio of ~2:3 by heating in a pyrex dish for a few minutes at ~60o, cooling and allowed to crystallise slowly by evaporation in a crystallising dish. It forms elongated white needles, but if the solution is seeded just before crystallisation and shaken gently for as few seconds, then small plates are formed. Perferably collect the crystals by centrifugation at low temperature and dry them at 0o in vacuo. When dry, it is stable at room temperature and it has been reported that the available oxygen content had not decreased noticeably after 12 months. However, it is best to store it dry at low temperature. It is soluble in organic solvents e.g. EtOH, Et2O, CHCl3, CH2Cl2 and Me2CO with slow decomposition, and its solubility in H2O is 40% where it also decomposes slowly. It decomposes slowly at 40-60o/20mm and at 55-70o/760mm in air, but decomposition appears to accelerate above 80o. It is very useful (and in many cases superior to p-chloroperbenzoic acid) in the oxidation of alkenes, (epoxides), aromatic hydrocarbons (to phenols), ketones (Baeyer-Villiger), sulfides (to sulfones) and N-heterocycles (to N-oxides) when using 5 to 10 molar ratios of oxidant in the presence of acetic or trifluoroacetic anhydrides. Care should be used with this reagent as it is potentially explosive. [Lu et al. J Am Chem Soc 63 1508 1941, Cooper et al. Synlett 533 1990, Beilstein 3 H 54, 3 I 25, 3 II 45, 3 III 105, 3 IV 102.]

InChI:InChI=1/CH4N2O3/c4-1(2-5)3-6/h2-3H2

Synthetic route

sodium molybdate + ammonium dihydrogen phosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
Stage #1: sodium molybdate; ammonium dihydrogen phosphate With caesium carbonate In neat (no solvent, solid phase) at 850℃; for 24h; Stage #2: In neat (no solvent, solid phase) at 680℃; for 85h; Stage #3: In neat (no solvent, solid phase) at 20℃; for 66h;

ammonium dihydrogen phosphate + sodium carbonate (497-19-8) → sodium pyrophosphate (124-43-6)

Conditions	Yield
Stage #1: ammonium dihydrogen phosphate; sodium carbonate In neat (no solvent, solid phase) at 350℃; for 24h; Stage #2: In neat (no solvent, solid phase) at 600℃; for 120h; Calcination;

sodium phosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With silver cyanide In neat (no solvent) byproducts: NaCN, NaCNO, Ag; heating with AgCN in presence of (CN)2 to 270°C;;	75%
With sulfur In neat (no solvent) grinding phosphate with sulfur; heating to 1000°C in quartz crucible in a stream of air (10 K/min);; detn. by 31P-NMR;
With mercury(II) cyanide In neat (no solvent) molar ratio Na3PO4:Hg(CN)2=1:1 or 2:1, heating for 1.5h;;	74-77
With oxygen; Nitrogen dioxide In neat (no solvent) Kinetics; byproducts: NaNO3; mixing with NO2 and O2 directly in the quartz reaction vessel contg. Na3PO4, heating on a platinum support at different temp. for different times; not isolated; Raman, NMR;

tetrasodium pyrophosphate decahydrate → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) byproducts: H2O; heating to 300°C for several days;;
byproducts: H2O; heating at 100-105°C to const. mass;
In solid byproducts: H2O; dehydrating the decahydrate at 130°C to constant weight;

sodium phosphate dibasic dodecahydrate → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) byproducts: H2O; dehydration at elevated temp., decompn. at red heat (Pt-vessel);;
In melt; neat (no solvent) byproducts: H2O; dehydration of melt in presence of 2-25% condensed phosphates; heating resulting dihydrate to 300-400°C;;
In melt; neat (no solvent) byproducts: H2O; dehydration of melt, heating resulting dihydrate to 300-400°C;;

sodium metaphposphate → sodium pyrophosphate (124-43-6) + sodium phosphate

Conditions	Yield
With H2O In water formation of orthophosphate and pyrophosphate by hydratation of metaphosphate in alkaline solns.;;

disodium hydrogenphosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
sodium nitrate In neat (no solvent) increase of react. rate by NaNO3 (decompn. of impurities);;
With sodium nitrate In neat (no solvent) oxidation of organic material in educt mixt. by NaNO3, light product;;
With thionyl chloride In neat (no solvent) byproducts: SO2, HCl; heating on a water bath;;

sodium fluorophosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
In melt thermal decompn.;;
With water In water byproducts: HF; hydrolyzed at 883 K;
In neat (no solvent) on heating;;
In neat (no solvent) on heating;;

phosphorus → sodium pyrophosphate (124-43-6)

Conditions	Yield
With air In neat (no solvent) spraying Na posphates (Na2O:P2O5 >2:1) into a P flame, temp. up to 1000°C;;
With air In sodium hydroxide P flame, react. vessel coated with a layer of alk. orthophosphate-soln. (Na2O:P2O5=2:1), dehydration of resulting soln., calcination to Na4P2O7;;
With air In neat (no solvent) spraying sodium-phosphates-hydrate melts (Na2O:P2O5 >2:1) into a P flame, temp. up to 1000°C;;

Sodium trimetaphosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With oxygen In neat (no solvent) Kinetics; on heating;;
With sodium nitrite In neat (no solvent) 240-570°C, different molar ratios of Na2O and P2O5;;
With NaNO2 In neat (no solvent) 240-570°C, different molar ratios of Na2O and P2O5;;
With O2; Na-acetate or NaNO3 or Na2CO3 In neat (no solvent) Kinetics; on heating;;

tetrasodium pyrophosphate decahydrate → sodium pyrophosphate (124-43-6) + water (7732-18-5)

Conditions	Yield
In water at 80°C;;
In neat (no solvent) complete dehydration in a stream of dry NH3 within 8d;;
In neat (no solvent) isothermic dehydration at 23°C;;
In ammonia NH3 (liquid); dehydration with liquid NH3 at -78.5°C;;

phosphorus + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With air In sodium hydroxide spraying NaCl into a P flame (introduction of excess air and H2O vapor), sepn. of volatile impurities, react. of generated metaphosphates with aq. NaOH; apparatus described;;
With oxygen In neat (no solvent) byproducts: metaphosphate; combustion of P in a vessel coated with NaCl, react. of P2O5 with molten NaCl;;
With air In sodium hydroxide spraying NaCl into a P flame (introduction of excess air and H2O vapor), sepn. of volatile impurities, react. of generated metaphosphates with aq. NaOH;;

Graham's salt → sodium pyrophosphate (124-43-6)

Conditions	Yield
With zinc diacetate In water heating an aq. soln. with zinc acetate at 40 °C;;
With zinc acetate In water heating an aq. soln. with zinc acetate at 40 °C;;

sodium dihydrogenphosphate dihydrate → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent, solid phase) at 900℃; Heating;

disodium dihydrogen diphosphate 6-hydrate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With ammonia In neat (no solvent) byproducts: (NH4)2H2P2O7, H2O; with NH3-gas at 100°C;; product-mixture;;
With NH3 In neat (no solvent) byproducts: (NH4)2H2P2O7, H2O; with NH3-gas at 100°C;; product-mixture;;

sodium imido diphosphate 10-hydrate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With water In solid byproducts: NH3; moist air, at 200°C, for 0.5 and for 3 h; not isolated, detected by (31)P-NMR;

sodium monothiophosphate → sodium pyrophosphate (124-43-6) + sodium sulfate (7757-82-6)

Conditions	Yield
With air In neat (no solvent, solid phase) 315°C;

sodium phosphite → sodium pyrophosphate (124-43-6) + Sodium trimetaphosphate + sodium peroxodiphosphate + sodium phosphate

Conditions	Yield
With sodium hydroxide In water Electrolysis; 16 mM sodium phosphite was electrolyzed on B-doped diamond electrode at pH 12 (1 N NaOH) and 20°C for 500 min; ion chromy.;
With sulfuric acid In water Electrolysis; 9.7-29 mM sodium phosphite was electrolyzed on B-doped diamond electrodeat pH 2 or 7 (1 N H2SO4) and 10-40°C for 500 min; ion chromy.;

sodium cyanide (773837-37-9) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With sodium hypophosphate; oxygen In neat (no solvent) byproducts: (CN)2; heating at 500°C, 1h;;
With NaPO3; O2 In neat (no solvent) byproducts: (CN)2; heating at 500°C, 1h;;

sodium subphosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With nitric acid In not given evapn. of Na2PO3 soln. in platinum crucible; oxidation (HNO3) and calcination;;
With HNO3 In not given evapn. of Na2PO3 soln. in platinum crucible; oxidation (HNO3) and calcination;;

NaHPO3 → sodium pyrophosphate (124-43-6)

Conditions	Yield
With nitric acid In not given evapn. of Na2PO3 soln. in platinum crucible; oxidation (HNO3) and calcination;;
With HNO3 In not given evapn. of Na2PO3 soln. in platinum crucible; oxidation (HNO3) and calcination;;

disodium pyrophoshate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With sodium hydroxide In not given pptn. of Na4P2O7 from a soln. satd. with NaOH;;
With NaOH In not given pptn. of Na4P2O7 from a soln. satd. with NaOH;;

Sodium tripolyphosphate → sodium pyrophosphate (124-43-6) + Phosphate (14265-44-2)

Conditions	Yield
With water In water Kinetics; 100°C; NMR monitoring;
With water; urea In water Kinetics; 100°C; NMR monitoring;

tetrasodium hypophosphate*10H2O → sodium pyrophosphate (124-43-6)

Conditions	Yield
With nitric acid In neat (no solvent) oxidation with HNO3 and then calcinated;;	>99
With HNO3 In neat (no solvent) oxidation with HNO3 and then calcinated;;	>99

{Co(NH3)6}(3+)*Na(1+)*P2O7(4-)*11.5H2O={Co(NH3)6}NaP2O7*11.5H2O → sodium pyrophosphate (124-43-6) + 4{Co(NH3)6}(3+)*3P2O7(4-)*20H2O={Co(NH3)6}4(P2O7)3*20H2O

Conditions	Yield
With water In water hot H2O;;
With H2O In water hot H2O;;

sodium phosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With silver cyanide In neat (no solvent) byproducts: NaCN, NaCNO, Ag; heating with AgCN in presence of (CN)2 to 270°C;;	75%
With sulfur In neat (no solvent) grinding phosphate with sulfur; heating to 1000°C in quartz crucible in a stream of air (10 K/min);; detn. by 31P-NMR;
With mercury(II) cyanide In neat (no solvent) molar ratio Na3PO4:Hg(CN)2=1:1 or 2:1, heating for 1.5h;;	74-77
With oxygen; Nitrogen dioxide In neat (no solvent) Kinetics; byproducts: NaNO3; mixing with NO2 and O2 directly in the quartz reaction vessel contg. Na3PO4, heating on a platinum support at different temp. for different times; not isolated; Raman, NMR;

aluminum oxide (1333-84-2, 1344-28-1) + Sodium tripolyphosphate + phosphorus oxynitride (23369-45-1) → sodium pyrophosphate (124-43-6) + Na3AlP3O9N

Conditions	Yield
In neat (no solvent) heating in a sintered corund crucible at 800°C for 90 min, at 480°C for 120 min.;; extn. of byproducts (aq. HCl); elem. anal.;;	A n/a B 64.9%

silver(I) cyanide (506-64-9) + sodium phosphate → sodium cyanide (773837-37-9) + sodium pyrophosphate (124-43-6) + sodium isocyanate (917-61-3)

Conditions	Yield
In neat (no solvent) byproducts: Ag; heating dry Na3PO4 with AgCN at 270°C;;
In neat (no solvent) byproducts: Ag; at 270°C;;
In neat (no solvent) byproducts: Ag; heating dry Na3PO4 with AgCN at 270°C;;

disodium hydrogenphosphate + sodium phosphite → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) byproducts: H2; 400-900°C, small excess of Na2HPO4 needed to avoid formation of PH3;;

zinc pyrophosphate + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) byproducts: ZnCl2; calcination;;
In neat (no solvent) byproducts: ZnCl2; calcination;;

zinc pyrophosphate + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6) + zinc(II) chloride (7646-85-7)

Conditions	Yield
In neat (no solvent) calcination of NaCl with Zn2P4O7;; evaporation of ZnCl2;;

iron(III) oxide + Sodium tripolyphosphate + Sodium trimetaphosphate → sodium pyrophosphate (124-43-6) + 6Na(1+)*2Fe(3+)*3P2O7(4-)=Na6Fe2(P2O7)3

Conditions	Yield
In further solvent(s) dissolution mechanism for 30 mole% NaCl + 70 mole% NaPO3 at 700°C;

sodium dihydrogenphosphate (10049-21-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
In water spraying method using NaH2PO4 soln. (from neutralization of H3PO4 with Na2CO3);;
In neat (no solvent) prepn. by calcination at 800°C;

sodium dihydrogenphosphate (10049-21-5) + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With ammonia In neat (no solvent) byproducts: NH4Cl; heating in presence of NH3, sublimation of NH4Cl;;

sodium dihydrogenphosphate (10049-21-5) + sodium hydrogen monothiophosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) byproducts: Na4P2O6S; at 224°C;;
In neat (no solvent) byproducts: Na4P2O6S; at 224°C;;

disodium hydrogenphosphate + sodium dihydrogenphosphate (10049-21-5) → disodium pyrophoshate + sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) on heating a stoichiometric mixture;; product mixture;;

sulfur dioxide (7446-09-5) + sodium phosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
With oxygen Kinetics; byproducts: Na2SO3, Na2SO4; at heating from 200°C up to 1000°C; raman spectroscopy; NMR;

sulfur dioxide (7446-09-5) + sodium phosphate → sodium pyrophosphate (124-43-6) + sodium sulfate (7757-82-6)

Conditions	Yield
In neat (no solvent) byproducts: sulfur; heating of Na3PO4 in a SO2 atmosphere at 400-1000°C; not separated, detected by Raman-, (31)P-NMR-spectroscopy and X-ray diffraction;;

mercury(II) cyanide (592-04-1) + sodium phosphate → sodium cyanide (773837-37-9) + sodium pyrophosphate (124-43-6) + sodium isocyanate (917-61-3)

Conditions	Yield
In neat (no solvent) heating at 300°C;;
In neat (no solvent) heating at 300°C;;

sodium metaphposphate + sodium fluoride → sodium pyrophosphate (124-43-6) + fluorine (7782-41-4)

Conditions	Yield
With oxygen

phosphorus + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With air In sodium hydroxide spraying NaCl into a P flame (introduction of excess air and H2O vapor), sepn. of volatile impurities, react. of generated metaphosphates with aq. NaOH; apparatus described;;
With oxygen In neat (no solvent) byproducts: metaphosphate; combustion of P in a vessel coated with NaCl, react. of P2O5 with molten NaCl;;
With air In sodium hydroxide spraying NaCl into a P flame (introduction of excess air and H2O vapor), sepn. of volatile impurities, react. of generated metaphosphates with aq. NaOH;;

lead(II) pyrophosphate + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) byproducts: PbCl2; calcination;;
In neat (no solvent) byproducts: PbCl2; calcination;;

lead(II) pyrophosphate + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6) + lead(II) chloride

Conditions	Yield
In neat (no solvent) calcination of NaCl with Pb2P4O7;; evaporating of PbCl2;;

phosphoric acid (86119-84-8, 7664-38-2) + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
In water byproducts: HCl; heating H3PO4 and NaCl until formation of HCl is finished, concg. of melt with H2O (150-250°C, 7-14 atm); addn. of Ca(OH)2 to the filtarte until a ratio of Na2P:P2O5=2;1 is reached, evapn. of filtrate, heating to ca. 550° for 45-60 min;;
In neat (no solvent) byproducts: HCl, H2O; calcination;;
In neat (no solvent) byproducts: HCl; heating to red heat in presence of SiO2;;
In neat (no solvent) byproducts: HCl, H2O; calcination;;

phosphorus pentoxide + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With oxygen In neat (no solvent) byproducts: Cl2; at about 1000°C, exclusion of H2O;;

sodium metaphposphate + sodium chloride (7647-14-5) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With O2

tellurium(IV) oxide (7446-07-3) + sodium metaphposphate → sodium pyrophosphate (124-43-6) + sodium tetraphosphate + sodium phosphate

Conditions	Yield
In neat (no solvent) 1123 K, 0.5 h; quenching, paper chromy.;

phosphoric acid (86119-84-8, 7664-38-2) + sodium cation (17341-25-2) → sodium pyrophosphate (124-43-6)

Conditions	Yield
In water evapn. of a mixt. of H3PO4 with Na salts of volatile acids, molar ratio Na2O:P2O5=2:1;;
In water purifn. of H3PO4 by addn. of Ca(OH)2 or CaO, pptn. of impurities, addn. of Na(1+) to the filtrate until a ratio Na2O:P2O5=2:1 is reached;;

phosphorus → sodium pyrophosphate (124-43-6)

Conditions	Yield
With air In neat (no solvent) spraying Na posphates (Na2O:P2O5 >2:1) into a P flame, temp. up to 1000°C;;
With air In sodium hydroxide P flame, react. vessel coated with a layer of alk. orthophosphate-soln. (Na2O:P2O5=2:1), dehydration of resulting soln., calcination to Na4P2O7;;
With air In neat (no solvent) spraying sodium-phosphates-hydrate melts (Na2O:P2O5 >2:1) into a P flame, temp. up to 1000°C;;

phosphorus + sodium hydroxide (1310-73-2) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With air In neat (no solvent) spraying solid NaOH into a P flame, temp. up to 1000°C;;

Sodium trimetaphosphate + silicon (7440-21-3) → sodium pyrophosphate (124-43-6) + phosphorus + silica gel (112926-00-8, 7631-86-9)

Conditions	Yield
In neat (no solvent) Kinetics; evacuated quartz vessel, 700-1000°C, condensation in cold zone; yield depending on educt ratio, reaction time and temperature; product mixt. not sepd., detd. by powder X-ray diffraction and (31)P-NMRspectroscopy;

disodium dihydrogen pyrophosphate → sodium pyrophosphate (124-43-6)

Conditions	Yield
In neat (no solvent) heating recrystd. educt to about 110°C, then for 1h to red heat;; recrystn., heating; very pure product;;
In neat (no solvent) heating recrystd. educt to about 110°C, then for 1h to red heat;; recrystn., heating; very pure product;;

disodium hydrogenphosphate + thionyl chloride (7719-09-7) → sodium pyrophosphate (124-43-6)

Conditions	Yield
In not given byproducts: SO2, HCl; heating Na2HPO4 with SOCl2 on a water bath;;
In not given byproducts: SO2, HCl; heating Na2HPO4 with SOCl2 on a water bath;;

sodium cyanide (773837-37-9) → sodium pyrophosphate (124-43-6)

Conditions	Yield
With sodium hypophosphate; oxygen In neat (no solvent) byproducts: (CN)2; heating at 500°C, 1h;;
With NaPO3; O2 In neat (no solvent) byproducts: (CN)2; heating at 500°C, 1h;;

sodium pyrophosphate (124-43-6) + tin(II) chloride dihdyrate (10025-69-1) → tin(II) pyrophosphate

Conditions	Yield
In water at 60℃; for 0.5h;	95%

[2,2]bipyridinyl (366-18-7) + sodium pyrophosphate (124-43-6) + palladium diacetate (3375-31-3) → [(Pd(2,2'-bipyridine))2(μ-P2O7)]*5.5H2O

Conditions	Yield
In water Pd salt, bipyridine and Na salt were dissolved with stirring in H2O at 60°C; left for 2 h; slowly evapd. at room temp. for few d; dried in vac. overnight; elem. anal.;	85%

[2,2]bipyridinyl (366-18-7) + sodium pyrophosphate (124-43-6) + water (7732-18-5) + copper hydroxide (20427-59-2) → ([(2,2'-bipyridine)Cu(H2O)(μ-P2O7)Na2(H2O)6]*4H2O)

Conditions	Yield
In water aq. suspn. Cu(OH)2 was treated with 2,2'-bipyridine at room temp. and stirred for 15 min, Na4P2O7 was added and stirred for 4 h; soln. was allowed to stand over several days; elem. anal.;	80%

[2,2]bipyridinyl (366-18-7) + sodium pyrophosphate (124-43-6) + VO(4+)*2SO4(2-)*2H2O=VO(SO4)2*2H2O → ([(2,2'-bipyridine)(VO)2]2(μ-P2O7)]*3.5H2O)

Conditions	Yield
In water 2,2'-bipyridine was added to aq. soln. VO(SO4)2*2H2O, aq. soln. Na4P2O7 was added; ppt. was filtered, washed with water and air dried; elem. anal.;	80%

sodium pyrophosphate (124-43-6) + perchloric acid (7601-90-3) + [Ga2(2,6-bis((N,N′-bis(2-picolyl)amino)methyl)-4-tertbutylphenolate)(OH)2(H2O)2](ClO4)3·4H2O + water (7732-18-5) → [Ga2(2,6-bis((N,N′-bis(2-picolyl)amino)methyl)-4-tertbutylphenolate)(HP2O7)](ClO4)2·3H2O

Conditions	Yield
In methanol; acetone at 20℃;	77%

sodium pyrophosphate (124-43-6) + sodium tetrachloropalladate(II) + N-(pyridin-2-yl)formamidine + water (7732-18-5) → C12H14N6O7P2Pd2*4H2O

Conditions	Yield
With nitric acid; potassium hydroxide In ethanol; water at 60℃; for 15h; pH=8;	74.6%

Upstream product

• 57-13-6 urea 
• 7722-84-1 dihydrogen peroxide 
• 506-64-9 silver(I) cyanide 
• 10049-21-5 sodium dihydrogenphosphate 
• 7647-14-5 sodium chloride 
• 7446-09-5 sulfur dioxide 
• 592-04-1 mercury(II) cyanide 
• 7681-49-4 sodium fluoride 
• 7446-07-3 tellurium(IV) oxide 
• 1310-73-2 sodium hydroxide 
• 7440-21-3 silicon 
• 7719-09-7 thionyl chloride 
• 773837-37-9 sodium cyanide 
• 12185-10-3 phosphorous 

Downstream Products

• 477252-61-2 N-cyclopropyl-1-[3-(6-methylsulfonyl-1-oxidopyridin-3-yl)phenyl]-1,4-dihydro[1,8]naphthyridin-4-one-3-carboxamide 
• 12055-23-1 hafnium dioxide 
• 12027-05-3 hafnium hydroxide 
• 91223-89-1 hafnium dihydroxide 
• 7722-84-1 dihydrogen peroxide 
• 57-13-6 urea 
• 258884-24-1 cis-dichloro(5,11,17,23-tetra-tert-butyl-25,26-bis(diphenylphosphinomethoxy)-27-diphenylphosphinoylmethoxy-28-methoxycalix[4]arene-P,P')platinum(II) 
• 79-21-0 peracetic acid 
• 591-07-1 acetylurea 
• 10058-44-3 ferric pyrophosphate 
• 7647-14-5 sodium chloride 
• 7782-41-4 fluorine 
• 1310-73-2 sodium hydroxide 

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Urea hydrogen peroxide (cas 124-43-6) determination in whole blood using europium tetracycline probe09/27/2019

We introduce the use of a lanthanide complex, tetracycline–europium, for the clinical diagnosis of urea hydrogen peroxide in human whole blood. The values obtained agree with the urea concentration variation verified in 49 patients, including 12 predialysis, 12 peritoneal, and 15 dialysis subje...detailed

Relevant academic research and scientific papers

Kinetics of solid-phase H+/M+ ion exchange on hafnium hydrogen phosphate

The kinetics of solid-phase reactions between hafnium hydrogen phosphate and alkali metal chlorides were studied by thermogravimetry with subsequent analysis of leaving gases. For sodium and potassium chlorides, the reaction occurs in two stages; the firs

Effects of P2O7 clusters arrangement on second harmonic generation responses of pyrophosphates

Phosphates with rich structural diversities and novel physicochemical properties can be regarded as the indispensible sources of optical functional materials. Therefore, the extensive research has been performed to search the suitable nonlinear optical (NLO) materials and unveil the relationship among the crystal structures, properties and functions of phosphates system. Herein, two pyrophosphates, namely, Na4P2O7 and β-Ca2P2O7 have been obtained and characterized. Results show that the two title compounds can achieve the coexistence of deep-ultraviolet (UV) cutoff edges (2PO4 (KDP)). Besides, the positive roles of alkaline and alkaline earth metals with larger radii or higher ratios of M/P2O7 on SHG effects of pyrophosphates can be concluded. Theoretical analysis reveals that their NLO effects mainly originate from O-2p and P-2p orbitals near to the Fermi level. In addition, their thermal properties, infrared spectra and elemental analysis were also discussed.

Crystal Structures and Low-Dimensional Ferromagnetism of Sodium Nickel Phosphates Na5Ni2(PO4)3·H2O and Na6Ni2(PO4)3OH

Two new sodium nickel phosphates, Na5Ni2(PO4)3·H2O (I) and Na6Ni2(PO4)3OH (II), have been synthesized hydrothermally and characterized by synchrotron X-ray diffraction, electron diffraction, low-temperature thermodynamic and magnetic measurements, and ab initio calculations. Unlike the majority of Ni2+ compounds, I and II show predominant ferromagnetic exchange couplings. I crystallizes in the monoclinic space group P21/n (a = 14.0395(4) ?, b = 5.1847(14) ?, c = 16.4739(4) ?, β = 110.4186(14)°) and features chains of ferromagnetically coupled Ni2+ ions. In II with the orthorhombic space group Pcmb (a = 7.5007(15) ?, b = 21.4661(4) ?, c = 7.1732(15) ?), the ferromagnetically coupled Ni2+ ions form dimers arranged on a spin ladder. Both compounds represent rare examples of quasi-one-dimensional ferromagnets. Structural features behind this unusual magnetic behavior are discussed.

Ionic conductivity and Raman investigations on the phase transformations of Na4P2O7

The ionic conductivity and thermo-Raman spectra of anhydrous sodium pyrophosphate Na4P2O7 were measured dynamically in the temperature range from 25 to 600 °C with a heating rate of 2 °C min-1 to understand the structural evolution and phase transformation involved. The DSC thermogram was also measured in the same thermal process for the phase transformation investigation. The spectral variations observed in the thermo-Raman investigation indicated the transformation of Na4P2O7 from low temperature phase (ε) to high temperature phase (α) proceeded through pre-transitional region from 75 to 410 °C before the major orientational disorder at 420 °C and minor structural modifications at 511, 540 and 560 °C. The activation energies and enthalpies of the proposed phase transformations were determined. The possible mechanism for temperature dependent conductivity in Na4P2O7 was discussed with the available data.

Synthesis of substitutional solid solutions in Na2O-P 2O5-In2O3- MI 2I IO3 (MIII = Cr, Fe, and Mn) systems

Solid solutions based on Na7(InP2O7) 4PO4 and Na3In2(PO4) 3, where chromium, iron, and manganese substitute for indium, have been prepared. When chromium and iron substitute for indium in Na 7(InP2O7)4PO4, a continuous solid solution series exists. When manganese substitutes for indium, it enters the compound in the oxidation state +3. The substitution of chromium for indium in Na3In2(PO4)3 occurs within the range from 0.11 to 0.74 (mol/mol), and that of iron for indium, from 0.09 to 0.62 (mol/mol). When manganese substitutes for indium, it enters the structure of the crystalline phase in insignificant amounts as a two-charged cation.

Phase relations and flux research for zinc oxide crystal growth in the ZnO-Na2O-P2O5 system

The subsolidus phase relations of the ternary system ZnO-Na2O-P2O5 were investigated by means of X-ray diffraction (XRD). There are 7 binary compounds, 4 ternary compounds and 16 three-phase regions in this system. The pha

Monitoring dehydration and condensation processes of Na2HPO4 · 12H2O using thermo-Raman spectroscopy

Thermal dehydration and condensation processes of disodium hydrogen phosphate dodecahydrate (Na2HPO4 · 12H2O) were monitored by thermo-Raman spectroscopy (TRS). Various hydrated forms Na2HPO4 · 12H2O, Na2HPO4 · 8H2O, Na2HPO4 · 7H2O, Na2HPO4 · 2H2O, Na2HPO4 · H2O and Na2HPO4 were observed, followed by condensation of Na2HPO4 to sodium pyrophosphate (Na4P2O7) in a dynamic thermal process. Representative Raman spectra of all the hydrated forms Na2HPO4 · 12H2O, Na2HPO4 · 8H2O, Na2HPO4 · 7H2O, Na2HPO4 · 2H2O, Na2HPO4 · H2O and Na2HPO4 were detected in both H2O and PO43- regions are reported. The thermo-Raman intensity (TRI) thermogram also showed systematic loss of water in five steps of dehydration, with the differential TRI thermogram in agreement shows five dips corresponding to the five steps of dehydration, respectively. Thermogravimetry (TG) and differential thermogravimetry (DTG) are in harmony with the results of TRS, though, the two could not resolve the steps involved.

Modified Pechini synthesis of Na3Ce(PO4) 2and thermochemistry of its phase transition

Effect of the synthesis conditions of Pechini technique on crystallinity and purity of Na3Ce(PO4)2compound was investigated. Nano-sized cerium-sodium phosphate obtained when EDTA was used as an additional chelating agent f

Crystal structure and properties of the new vanadyl(IV)phosphates Na 2MVO(PO4)2, M=Ca and Sr

Two new complex vanadyl(IV)phosphates Na2MVO(PO 4)2 (M=Ca, Sr) were synthesized in evacuated quartz ampoules and investigated by means of X-ray diffraction, electron microscopy, DTA, ESR and magnetic susceptibility measurements. The crystal structure of Na2SrVO(PO4)2 was solved ab initio from X-ray powder diffraction data. Both compounds are isostructural: a=10.5233(3)A, b=6.5578(2)A, c=10.0536(3)A and a=10.6476(3)A, b=6.6224(2)A, c=10.2537(3)A for Ca and Sr, respectively; S.G. Pnma, Z=4. The compounds have a three-dimensional structure consisting of V 4+O6 octahedra connected by PO4 tetrahedra via five of the six vertexes forming a framework with cross-like channels. The strontium and sodium atoms are located in the channels in an ordered manner. Electron diffraction as well as high-resolution electron microscopy confirmed the structure solution. The new vanadylphosphates are Curie-Weiss paramagnets in a wide temperature range down to 2K with θ=12 and 5K for Ca and Sr phases, respectively.

Spectroscopic and thermal behavior of Na6[(VO)3(P2O7)3] ·7H2O

The electronic (absorption and reflectance) as well as the infrared and Raman spectra of Na6[(VO)3(P2O7)3] ·7H2O were recorded and discussed. Its thermal behavior was investigated by means of TG and DTA measurements. After a two-step dehydration, the compound melts at 464°C and, apparently, depolymerization takes place during this process. The characteristics of the pyrolysis residues, collected at different temperatures, were spectroscopically investigated.