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Cas Database

13446-18-9

13446-18-9

Identification

Synonyms:Nitric acid, magnesiumsalt, hydrate (2:1:6);Dusicnan horecnaty;

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Safety information and MSDS view more

  • Pictogram(s):CorrosiveC,IrritantXi,OxidizingO

  • Hazard Codes:C,Xi,O,T

  • Signal Word:No signal word.

  • Hazard Statement:none

  • First-aid measures: General adviceConsult a physician. Show this safety data sheet to the doctor in attendance.If inhaled If breathed in, move person into fresh air. If not breathing, give artificial respiration. Consult a physician. In case of skin contact Wash off with soap and plenty of water. Consult a physician. In case of eye contact Rinse thoroughly with plenty of water for at least 15 minutes and consult a physician. If swallowed Never give anything by mouth to an unconscious person. Rinse mouth with water. Consult a physician.

  • Fire-fighting measures: Suitable extinguishing media Use water spray, alcohol-resistant foam, dry chemical or carbon dioxide. Wear self-contained breathing apparatus for firefighting if necessary.

  • Accidental release measures: Use personal protective equipment. Avoid dust formation. Avoid breathing vapours, mist or gas. Ensure adequate ventilation. Evacuate personnel to safe areas. Avoid breathing dust. For personal protection see section 8. Prevent further leakage or spillage if safe to do so. Do not let product enter drains. Discharge into the environment must be avoided. Pick up and arrange disposal. Sweep up and shovel. Keep in suitable, closed containers for disposal.

  • Handling and storage: Avoid contact with skin and eyes. Avoid formation of dust and aerosols. Avoid exposure - obtain special instructions before use.Provide appropriate exhaust ventilation at places where dust is formed. For precautions see section 2.2. Store in cool place. Keep container tightly closed in a dry and well-ventilated place.

  • Exposure controls/personal protection:Occupational Exposure limit valuesBiological limit values Handle in accordance with good industrial hygiene and safety practice. Wash hands before breaks and at the end of workday. Eye/face protection Safety glasses with side-shields conforming to EN166. Use equipment for eye protection tested and approved under appropriate government standards such as NIOSH (US) or EN 166(EU). Skin protection Wear impervious clothing. The type of protective equipment must be selected according to the concentration and amount of the dangerous substance at the specific workplace. Handle with gloves. Gloves must be inspected prior to use. Use proper glove removal technique(without touching glove's outer surface) to avoid skin contact with this product. Dispose of contaminated gloves after use in accordance with applicable laws and good laboratory practices. Wash and dry hands. The selected protective gloves have to satisfy the specifications of EU Directive 89/686/EEC and the standard EN 374 derived from it. Respiratory protection Wear dust mask when handling large quantities. Thermal hazards

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  • Manufacture/Brand:Usbiological
  • Product Description:Magnesium Nitrate hexahydrate ACS
  • Packaging:25g
  • Price:$ 389
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  • Manufacture/Brand:Strem Chemicals
  • Product Description:Magnesium nitrate hexahydrate, 99% (ACS)
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  • Manufacture/Brand:Strem Chemicals
  • Product Description:Magnesium nitrate hexahydrate, 99% (ACS)
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  • Manufacture/Brand:Strem Chemicals
  • Product Description:Magnesium nitrate hexahydrate (99.999%-Mg) PURATREM
  • Packaging:25g
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  • Manufacture/Brand:Strem Chemicals
  • Product Description:Magnesium nitrate hexahydrate (99.999%-Mg) PURATREM
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  • Manufacture/Brand:Sigma-Aldrich
  • Product Description:Magnesium nitrate hexahydrate BioXtra, ≥98%
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  • Manufacture/Brand:Sigma-Aldrich
  • Product Description:Magnesium nitrate hexahydrate for analysis EMSURE ACS,Reag. Ph Eur
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  • Manufacture/Brand:Sigma-Aldrich
  • Product Description:Magnesium nitrate hexahydrate BioUltra, ≥99.0% (KT)
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  • Manufacture/Brand:Sigma-Aldrich
  • Product Description:Magnesium nitrate hexahydrate for analysis EMSURE? ACS,Reag. Ph Eur
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  • Manufacture/Brand:Sigma-Aldrich
  • Product Description:Magnesium nitrate hexahydrate 99.99 Suprapur . CAS 13446-18-9, EC Number 233-826-7, chemical formula Mg(NO ) * 6 H O., 99.99 Suprapur
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Relevant articles and documentsAll total 13 Articles be found

Pb0.5 + xMg xZr2 – x(PO4)3(x = 0, 0.5) Phosphates: Structure and Thermodynamic Properties

Asabina, E. A.,Kovalsky, A. M.,Markin, A. V.,Mayorov, P. A.,Pet’kov, V. I.,Smirnova, N. N.

, p. 711 - 719 (2020)

Abstract—Crystalline Pb0.5 + xMgxZr2 – x(PO4)3 (x = 0, 0.5) phosphates of NaZr2(PO4)3 (NZP) structural type were synthesized. The heat capacity of Pb0.5Zr2(PO4)3 was measured by adiabatic vacuum and differential scanning calorimetry (DSC) within the temperature range 8–660 K. The studied phosphates were found to experience a reversible phase transition in the region 256–426 K. According to the results of Rietveld structural study, this transition occurred due to an increase in disorder of lead cation positions in cavities of the NZP structure. The measurements of PbMg0.5Zr1.5(PO4)3 heat capacity in the temperature range 195–660 K showed that it experienced a similar phase transition at 255–315 K. Based on the measured experimental data, the thermodynamic functions of Pb0.5Zr2(PO4)3, such as Cp 0(T) [H0(T) – H0(0)], S0(T), and [G0(T) – H0(0)] were calculated for the temperature range 0–660 K. The standard formation enthalpy of Pb0.5Zr2(PO4)3 was determined at 298.15 K.

On the photophysics and speciation of actinide ion in MgAl2O4spinel using photoluminescence spectroscopy and first principle calculation: A case study with uranium

Gupta, Santosh K.,Pathak, Nimai,Ghosh,Kadam

, p. 337 - 343 (2017)

Actinide chemistry is very interesting not from scientific perspective but also from technological importance. Elucidating the valence state and coordinating environment of actinide ion like uranium in technologically important magnesium aluminate spinel (MAS) is important to fully understand its hazardous and other harmful effect in human as well as environment. Magnesium aluminate spinel doped with 1.0?mol % of Uranium ion has been synthesized using citric acid assisted gel-combustion route at 800?°C. The as prepared powder is characterised using X-ray diffraction (XRD), time resolved photoluminescence spectroscopy (TRPLS) and density functional theory (DFT) calculations. Uranium is an interesting element because it exhibits multiple oxidation state and each one of them is having characteristics fluorescence behavior. TRPLS is used to investigate the oxidation state and coordination behavior of uranium in MgAl2O4. Indeed in our earlier work on undoped and lanthanide ion doped MAS; it was oberved that in undoped sample itself defect induced emission could be seen in visible region which was probed using DFT. Here on doping uranium in MAS; complete energy of host is transferred to uranium ion which is explained using DFT. From excitation and emission spectroscopy it was observed that uranium stabilizes in?+6 oxidation state in the form of UO22+ ion. Based on luminescence lifetime and its comparison with the emission profile of uranyl fluoride crystal it was inferred that majority of uranium is occupying relatively asymmetric MgO4polyhedra and minority substitutes AlO6. The site stability of the uranyl ion in MAS was also validated using DFT based first principle calculations. Time resolved emission shows the uranyl at Mg2+site differs from the one at Al3+site in terms of peak position and intensity.

Paulik, F.,Paulik, J.,Arnold, M.,Naumann, R.

, p. 627 - 636 (1988)

Synthesis of MgAl2O4 nanopowders

Kuznetsov,Fedorov,Voronov,Osiko

, p. 895 - 898 (2011)

A procedure has been developed for the synthesis of MgAl2O 4 nanopowders with a characteristic particle size of 10-40 nm. Translucent hydrous xerogels have been synthesized as precursors to MgAl 2O4. The synthesized magnesium aluminum spinel nanopowders are promising for the fabrication of optical ceramics.

Preparation of MgO nanoparticles

Fedorov,Tkachenko,Kuznetsov,Voronov,Lavrishchev

, p. 502 - 504 (2007)

MgO nanoparticles have been prepared via hydroxide precipitation from aqueous solutions, followed by the thermal decomposition of the hydroxide. The nanoparticles inherit the platelike shape from the hydroxide and break into isometric particles upon signi

Enhanced photoredox chemistry in surface-modified Mg2TiO4 nano-powders with bidentate benzene derivatives

Medi?, Mina M.,Vasi?, Marija,Zarubica, Aleksandra R.,Trandafilovi?, Lidija V.,Dra?i?, Goran,Drami?anin, Miroslav D.,Nedeljkovi?, Jovan M.

, p. 94780 - 94786 (2016)

Magnesium-orthotitanate (Mg2TiO4) nano-powder was synthesized using a Pechini-type polymerized complex route. Microstructural characterization involving transmission electron microscopy, X-ray diffraction analysis and nitrogen adsorption-desorption isotherms indicated that well-crystallized Mg2TiO4 nanoparticles are small in size (about 10 nm) with large specific surface area (72 m2 g-1). The surface modification of Mg2TiO4 nano-powders with 5-amino salicylic acid and catechol induced a significant shift of absorption to the visible spectral region due to charge transfer complex formation. It should be emphasized that tunable optical properties of Mg2TiO4 nano-powders have never been reported in the literature. Degradation reactions of an organic dye (crystal violet) were used to test the photocatalytic ability of pristine and surface-modified Mg2TiO4 nano-powders under illumination in different spectral regions. Excitation with UV light indicated, for the first time, photocatalytic ability of Mg2TiO4. Also, improved photocatalytic performance of surface-modified Mg2TiO4 nano-powders was found in comparison to unmodified ones.

Metal-organic phase-change materials for thermal energy storage

McGillicuddy, Ryan D.,Thapa, Surendra,Wenny, Malia B.,Gonzalez, Miguel I.,Mason, Jarad A.

supporting information, p. 19170 - 19180 (2020/12/01)

The development of materials that reversibly store high densities of thermal energy is critical to the more efficient and sustainable utilization of energy. Herein, we investigate metal-organic compounds as a new class of solid-liquid phase-change materials (PCMs) for thermal energy storage. Specifically, we show that isostructural series of divalent metal amide complexes featuring extended hydrogen bond networks can undergo tunable, high-enthalpy melting transitions over a wide temperature range. Moreover, these coordination compounds provide a powerful platform to explore the specific factors that contribute to the energy density and entropy of metal-organic PCMs. Through a systematic analysis of the structural and thermochemical properties of these compounds, we investigated the influence of coordination bonds, hydrogen-bond networks, neutral organic ligands, and outer-sphere anions on their phase-change thermodynamics. In particular, we identify the importance of high densities of coordination bonds and hydrogen bonds to achieving a high PCM energy density, and we show how metal-dependent changes to the local coordination environment during melting impact the entropy and enthalpy of metal-organic PCMs. These results highlight the potential of manipulating order-disorder phase transitions in metal-organic materials for thermal energy storage.

Process route upstream and downstream products

Process route

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

Conditions
Conditions Yield
magnesium oxide

magnesium oxide

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

Conditions
Conditions Yield
In nitric acid; mgO dissolved in HNO3;
In water; drying the mixing soln. of MgO and HNO3;
In nitric acid; prepn. by dissolving MgO in threefold excess of HNO3;
Heating;
In water;
ammonium nitrate

ammonium nitrate

magnesium oxide

magnesium oxide

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

Conditions
Conditions Yield
In neat (no solvent); byproducts: NH3, H2O; MgO reacted with molten NH4NO3 with formation of Mg(NO3)2, NH3 and H2O;;
byproducts: NH3; H2O;
In neat (no solvent); byproducts: NH3, H2O; MgO reacted with molten NH4NO3 with formation of Mg(NO3)2, NH3 and H2O;;
magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

Conditions
Conditions Yield
With magnesium chloride; evapn. with excess of HNO3 soln.;
>99
With magnesium chloride; no reaction at low temp.;
0%
With MgCl2; no reaction at low temp.;
0%
With MgCl2; evapn. with excess of HNO3 soln.;
>99
ammonium nitrate

ammonium nitrate

magnesium
7439-95-4

magnesium

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

ammonia
7664-41-7

ammonia

water
7732-18-5

water

Conditions
Conditions Yield
byproducts: N2; 10-20°C above the melting-point;
Nitrogen dioxide
10102-44-0

Nitrogen dioxide

magnesium
7439-95-4

magnesium

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

Conditions
Conditions Yield
byproducts: MgO; Mg in form of filings, at dark red heat;
byproducts: MgO; Mg in form of filings, at dark red heat;
magnesium(II) nitrate hexahydrate

magnesium(II) nitrate hexahydrate

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

Conditions
Conditions Yield
In neat (no solvent); byproducts: H2O; thermal dehydration to Mg(NO3)2*2H2O at 95 - 280 °C, and Mg(NO3)2at 390 °C; Q-TG, Q-DTA;
In melt; byproducts: H2O; Mg(NO3)2*6H2O was dehydrated at temp. above 200 °C, crystn. of Mg(NO3)2 from the melt;;
In neat (no solvent); byproducts: H2O, basic magnesium nitrate; Mg(NO3)2*6H2O was rapidly dehydrated at high temp. forming Mg(NO3)2 with 5% basic magnesium nitrate;;
In neat (no solvent); byproducts: H2O; no formation of Mg(NO3)2 on heating Mg(NO3)2*6H2O at 100 °C over P2O5 in high vacuum for 4 days;;
0%
In neat (no solvent); byproducts: H2O; thermal decomposition; TG, DTA;
In neat (no solvent); byproducts: H2O; air or N2 atmosphere; heating to 310°C; Kinetics;
In neat (no solvent); sample placed in a Pt crucible, covered with a lid, heated (5 deg/min, O);
0%
In neat (no solvent); byproducts: H2O; Mg(NO3)2*6H2O was dried over P2O5 at ambient temp. with formation of Mg(NO3)2*2H2O, then heated at 130.5 °C in an desiccator with formation of Mg(NO3)2;;
In melt; byproducts: H2O; Mg(NO3)2*6H2O was dehydrated at temp. above 200 °C, crystn. of Mg(NO3)2 from the melt;;
In neat (no solvent); byproducts: H2O, basic magnesium nitrate; Mg(NO3)2*6H2O was rapidly dehydrated at high temp. forming Mg(NO3)2 with 5% basic magnesium nitrate;;
In neat (no solvent); byproducts: H2O; no formation of Mg(NO3)2 on heating Mg(NO3)2*6H2O at 100 °C over P2O5 in high vacuum for 4 days;;
0%
In neat (no solvent); melting (95 - 140°C);
In neat (no solvent); byproducts: H2O; heated at 523.15 K in stainless steel crucible on hot plate under Ar for2 h; slowly heated to 573.15 K;
lead(II) nitrate

lead(II) nitrate

magnesium chloride
7786-30-3

magnesium chloride

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

Conditions
Conditions Yield
In water; MgCl2 was treated with Pb(NO3)2 with formation of Mg(NO3)2 soln.;;
In water; MgCl2 was treated with Pb(NO3)2 with formation of Mg(NO3)2 soln.;;
In water; MgCl2 was treated with Pb(NO3)2 with formation of Mg(NO3)2 soln.;;
dinitrogen trioxide
10544-73-7,96607-26-0

dinitrogen trioxide

water
7732-18-5

water

magnesium
7439-95-4

magnesium

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

magnesium nitrite

magnesium nitrite

Conditions
Conditions Yield
In water; liquid N2O3 was dissolved in ice water with formation of a soln. of free HNO2 which was treated with Mg at tempp. below 5 °C, very slow reaction with formation of Mg(NO2)2 and Mg(NO3)2;;
In water; liquid N2O3 was dissolved in ice water with formation of a soln. of free HNO2 which was treated with Mg at tempp. below 5 °C, very slow reaction with formation of Mg(NO2)2 and Mg(NO3)2;;
magnesium phosphide

magnesium phosphide

magnesium(II) nitrate
13446-18-9

magnesium(II) nitrate

phosphoric acid
86119-84-8,7664-38-2

phosphoric acid

Conditions
Conditions Yield
In nitric acid; reaction of Mg3P2 with concd. HNO3 under ignition and formation of Mg(NO3)2 and H3PO4;;
In nitric acid; aq. HNO3; reaction of Mg3P2 with concd. HNO3 under ignition and formation of Mg(NO3)2 and H3PO4;;

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  • Shanghai Upbio Tech Co.,Ltd
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