Draw the Lewis Diagram for Mg3N2 (magnesium nitride)
Draw the Lewis Diagram for Mg3N2 (magnesium nitride)

Magnesium nitrate

Names
IUPAC name

Magnesium nitrate

Other names

Nitromagnesite (hexahydrate)

Identifiers

3D model (JSmol)

ChEBI
ChemSpider
ECHA InfoCard 100.030.739
EC Number

PubChem CID

RTECS number
UNII
UN number 1474

CompTox Dashboard (EPA)

Properties
Mg(NO3)2
Molar mass 148.32 g/mol (anhydrous)

184.35 g/mol (dihydrate)

256.41 g/mol (hexahydr.)

Appearance White crystalline solid
Density 2.3 g/cm3 (anhydrous)

2.0256 g/cm3 (dihydrate)

1.464 g/cm3 (hexahydrate)

Melting point 129 °C (264 °F; 402 K) (dihydrate)

88.9 °C (hexahydrate)

Boiling point 330 °C (626 °F; 603 K) decomposes
71 g/100 mL (25 °C)[1]
Solubility moderately soluble in ethanol, ammonia

Refractive index (nD)

1.34 (hexahydrate)
Structure
cubic
Thermochemistry

Heat capacity (C)

141.9 J/mol K

Std molar

entropy (S⦵298)

164 J/mol K

Std enthalpy of

formation (ΔfH⦵298)

-790.7 kJ/mol

Gibbs free energy (ΔfG⦵)

-589.4 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):

Main hazards

Irritant
GHS labelling:

Warning
H272, H315, H319, H335
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)
Safety data sheet (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, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Magnesium nitrate refers to inorganic compounds with the formula Mg(NO3)2(H2O)x, where x = 6, 2, and 0. All are white solids.[2] The anhydrous material is hygroscopic, quickly forming the hexahydrate upon standing in air. All of the salts are very soluble in both water and ethanol.

Occurrence, preparation, structure[edit]

Being 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 various magnesium salts.

Use[edit]

The principal use is as a dehydrating agent in the preparation of concentrated nitric acid.[2]

Its fertilizer grade has 10.5% nitrogen and 9.4% magnesium, so it is listed as 10.5-0-0 + 9.4% Mg. Fertilizer blends containing magnesium nitrate also have ammonium nitrate, calcium nitrate, potassium nitrate and micronutrients in most cases; these blends are used in the greenhouse and hydroponics trade.

Reactions[edit]

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

Mg(NO3)2 + 2 NaOH → Mg(OH)2 + 2 NaNO3.

Since magnesium nitrate has a high affinity 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(NO3)2 → 2 MgO + 4 NO2 + O2.

The absorption of these nitrogen oxides in water is one possible route to synthesize nitric acid. Although inefficient, this method does not require the use of any strong acid.

It is also occasionally used as a desiccant.

References[edit]

  1. ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  2. ^ a b Thiemann, Michael; Scheibler, Erich and Wiegand, Karl Wilhelm (2005). “Nitric Acid, Nitrous Acid, and Nitrogen Oxides”. Ullmann’s Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_293. ISBN 3527306730.{{cite encyclopedia}}: CS1 maint: uses authors parameter (link)
  3. ^ Mindat, http://www.mindat.org/min-2920.html
  4. ^ Schefer, J.; Grube, M. (1995). “Low temperature structure of magnesium nitrate hexahydrate, Mg (N O3)2 . 6(H2 O): a neutron diffraction study at 173 K”. Materials Research Bulletin. 30: 1235–1241. doi:10.1016/0025-5408(95)00122-0.
HNO3 He
LiNO3 Be(NO3)2 B(NO3)−4 RONO2 NO−3

NH4NO3

HOONO2 FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3

Al(NO3)−4

Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)2

Fe(NO3)3

Co(NO3)2

Co(NO3)3

Ni(NO3)2 CuNO3

Cu(NO3)2

Zn(NO3)2 Ga(NO3)3 Ge As Se BrNO3 Kr
RbNO3 Sr(NO3)2 Y(NO3)3 Zr(NO3)4 NbO(NO3)3 MoO2(NO3)2 Tc Ru(NO3)3 Rh(NO3)3 Pd(NO3)2

Pd(NO3)4

AgNO3

Ag(NO3)2

Cd(NO3)2 In(NO3)3 Sn(NO3)4 Sb(NO3)3 Te INO3 Xe(NO3)2
CsNO3 Ba(NO3)2 Lu(NO3)3 Hf(NO3)4 TaO(NO3)3 W Re Os Ir Pt(NO3)2

Pt(NO3)4

Au(NO3)3 Hg2(NO3)2

Hg(NO3)2

TlNO3

Tl(NO3)3

Pb(NO3)2 Bi(NO3)3

BiO(NO3)

Po(NO3)4 At Rn
FrNO3 Ra(NO3)2 Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
La(NO3)3 Ce(NO3)3

Ce(NO3)4

Pr(NO3)3 Nd(NO3)3 Pm(NO3)3 Sm(NO3)3 Eu(NO3)3 Gd(NO3)3 Tb(NO3)3 Dy(NO3)3 Ho(NO3)3 Er(NO3)3 Tm(NO3)3 Yb(NO3)3
Ac(NO3)3 Th(NO3)4 PaO2(NO3)3 UO2(NO3)2 Np(NO3)4 Pu(NO3)4 Am(NO3)3 Cm(NO3)3 Bk(NO3)3 Cf Es Fm Md No

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