Formula Mass Of Calcium Nitrate

Magnesium nitrate
Names


IUPAC name Magnesium nitrate
Other names Nitromagnesite (hexahydrate)
Identifiers
CAS Number	10377-threescore-three ^Y 15750-45-five (dihydrate)^N 13446-18-9 (hexahydrate)^Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:64736 ^Y
ChemSpider	23415 ^Y
ECHA InfoCard	100.030.739
EC Number	233-826-7
PubChem CID	25212
RTECS number	OM3750000 (anhydrous) OM3756000 (hexahydrate)
UNII	77CBG3UN78 ^Y V85K20LJMK (hexahydrate)^Y
United nations number	1474
CompTox Dashboard (EPA)	DTXSID4049664
InChI InChI=1S/Mg.2NO3/c;ii2-one(iii)four/q+2;2-1^{Due north} Key: YIXJRHPUWRPCBB-UHFFFAOYSA-North^N InChI=1/Mg.2NO3/c;iiii-one(iii)4/q+2;two-one Key: YIXJRHPUWRPCBB-UHFFFAOYAA
SMILES [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Mg+2]
Properties
Chemic formula	Mg(NO₃)_two
Molar mass	148.32 chiliad/mol (anhydrous) 184.35 g/mol (dihydrate) 256.41 g/mol (hexahydr.)
Advent	White crystalline solid
Density	2.iii g/cm³ (anhydrous) 2.0256 one thousand/cm³ (dihydrate) 1.464 thousand/cm^three (hexahydrate)
Melting point	129 °C (264 °F; 402 K) (dihydrate) 88.9 °C (hexahydrate)
Boiling betoken	330 °C (626 °F; 603 Yard) decomposes
Solubility in water	71 thou/100 mL (25 ºC)^[ane]
Solubility	moderately soluble in ethanol, ammonia
Refractive index (n _D)	1.34 (hexahydrate)
Construction
Crystal structure	cubic
Thermochemistry
Rut capacity (C)	141.9 J/mol K
Std molar entropy (S ^⦵ ₂₉₈)	164 J/mol K
Std enthalpy of formation (Δ_f H ^⦵ ₂₉₈)	-790.seven kJ/mol
Gibbs energy (Δ_f Thousand ^⦵)	-589.four kJ/mol
Hazards
Occupational prophylactic and wellness (OHS/OSH):
Principal hazards	Irritant
GHS labelling:
Pictograms
Point word	Warning
Hazard statements	H272, H315, H319, H335
Precautionary statements	P210, P220, P221, P261, P264, P271, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P370+P378, P403+P233, P405, P501
NFPA 704 (fire diamond)	1 0 0 OX
Rubber information canvas (SDS)	External MSDS
Related compounds
Other anions	Magnesium sulfate Magnesium chloride
Other cations	Beryllium nitrate Calcium nitrate Strontium nitrate Barium nitrate
Except where otherwise noted, information are given for materials in their standard country (at 25 °C [77 °F], 100 kPa). Nverify (what is^{Y N} ?) Infobox references

Chemical compound

Magnesium nitrate refers to inorganic compounds with the formula Mg(NO_three)₂(H₂O)_ten, where x = vi, two, and 0. All are white solids.^[2] The anhydrous material is hygroscopic, quickly forming the hexahydrate upon continuing in air. All of the salts are very soluble in both water and ethanol.

Occurrence, preparation, structure [edit]

Existence highly water soluble, magnesium nitrate occurs naturally only in mines and caverns as nitromagnesite (hexahydrate form).^[3]

The magnesium nitrate used in commerce is made by the reaction of nitric acid and diverse magnesium salts.

Structure of [Mg(H₂O)₆]²⁺ in the dinitrate common salt.^[4]

Use [edit]

The principal apply is as a dehydrating amanuensis in the preparation of concentrated nitric acid.^[2]

Its fertilizer grade has 10.5% nitrogen and ix.4% magnesium, so it is listed as 10.5-0-0 + nine.4% Mg. Fertilizer blends containing magnesium nitrate also have ammonium nitrate, calcium nitrate, potassium nitrate and micronutrients in almost cases; these blends are used in the greenhouse and hydroponics merchandise.

Reactions [edit]

Magnesium nitrate reacts with alkaline metal hydroxide to form the corresponding nitrate:

Mg(NO_three)₂ + 2 NaOH → Mg(OH)₂ + 2 NaNO₃.

Since magnesium nitrate has a high analogousness for water, heating the hexahydrate does not result in the dehydration of the salt, but rather its decomposition into magnesium oxide, oxygen, and nitrogen oxides:

2 Mg(NO_three)₂ → 2 MgO + four NO₂ + O_two.

The assimilation of these nitrogen oxides in water is 1 possible route to synthesize nitric acid. Although inefficient, this method does not require the utilize of whatsoever strong acrid.

Information technology is also occasionally used as a desiccant.

References [edit]

^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Printing. ISBN0-8493-0487-iii.
^ ^a ^b Thiemann, Michael; Scheibler, Erich and Wiegand, Karl Wilhelm (2005). "Nitric Acrid, Nitrous Acrid, and Nitrogen Oxides". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:x.1002/14356007.a17_293. ISBN3527306730. {{cite encyclopedia}}: CS1 maint: uses authors parameter (link)
^ Mindat, http://www.mindat.org/min-2920.html
^ Schefer, J.; Grube, M. (1995). "Low temperature construction of magnesium nitrate hexahydrate, Mg (N O3)two . vi(H2 O): a neutron diffraction written report at 173 K". Materials Research Bulletin. thirty: 1235–1241. doi:ten.1016/0025-5408(95)00122-0. {{cite journal}}: CS1 maint: uses authors parameter (link)