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Nickel nitrate is the inorganic compound Ni(NO 3) 2 or any hydrate thereof. The anhydrous form is not commonly encountered, thus 'nickel nitrate' usually refers to nickel(II) nitrate hexahydrate. The formula for this species is written in two ways: Ni(NO 3) 2. 6H 2 O and, more descriptively Ni(H 2 O) 6 (NO 3) 2. Links with this icon indicate that you are leaving the CDC website. The Centers for Disease Control and Prevention (CDC) cannot attest to the accuracy of a non-federal website. Linking to a non-federal website does not constitute an endorsement by CDC or any of its employees of the sponsors or the information and products presented on the website.
Names | |
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IUPAC name | |
Other names Nickel nitrate Nickelous nitrate Nitric acid, nickel(2+) salt | |
Identifiers | |
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ChemSpider | |
ECHA InfoCard | 100.032.774 |
EC Number |
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Properties | |
Ni(NO3)2 | |
Molar mass | 182.703 g/mol (anhydrous) 290.79 g/mol (hexahydrate) |
Appearance | emerald green hygroscopic solid |
Odor | odorless |
Density | 2.05 g/cm3 (hexahydrate) |
Melting point | 56.7 °C (134.1 °F; 329.8 K) (hexahydrate) |
Boiling point | 136.7 °C (278.1 °F; 409.8 K) (hexahydrate) |
243 (hexahydrate) g/100ml (0 °C)[1] | |
Solubility | soluble in ethanol |
+4300.0·10−6 cm3/mol (+6 H2O) | |
Refractive index (nD) | 1.422 (hexahydrate) |
Structure | |
monoclinic (hexahydrate) | |
Hazards | |
Safety data sheet | External MSDS |
EU classification (DSD) (outdated) | Oxidant (O) Carc. Cat. 1 Muta. Cat. 3 Repr. Cat. 2 Toxic (T) Harmful (Xn) Irritant (Xi) Dangerous for the environment (N) |
R-phrases(outdated) | R49, R61, R8, R20/22, R38, R41, R42/43, R48/23, R68, R50/53 |
S-phrases(outdated) | S53, S45, S60, S61 |
NFPA 704 (fire diamond) | |
Flash point | Non-flammable |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 1620 mg/kg (oral, rat) |
Related compounds | |
Nickel(II) sulfate Nickel(II) chloride | |
Other cations | Palladium(II) nitrate |
Cobalt(II) nitrate Copper(II) nitrate | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
verify (what is ?) | |
Infobox references |
Nickel nitrate is the inorganic compound Ni(NO3)2 or any hydrate thereof. The anhydrous form is not commonly encountered, thus 'nickel nitrate' usually refers to nickel(II) nitrate hexahydrate. The formula for this species is written in two ways: Ni(NO3)2.6H2O and, more descriptively [Ni(H2O)6](NO3)2. The latter formula indicates that the nickel(II) center is surrounded by six water molecules in this hydrated salt. In the hexahydrate, the nitrate anions are not bonded to nickel. Also known are three other hydrates: Ni(NO3)2.9H2O, Ni(NO3)2.4H2O, and Ni(NO3)2.2H2O. Anhydrous Ni(NO3)2 is also known.[2]
It is prepared by the reaction of nickel oxide with nitric acid:
- NiO + 2 HNO3 + 5 H2O → Ni(NO3)2.6H2O
The anhydrous nickel nitrate is typically not prepared by the heating the hydrates. Rather is generated by reaction of hydrates with dinitrogen pentoxide or of nickel carbonyl with dinitrogen tetroxide:[2]
- Ni(CO)4 + 2 N2O4 → Ni(NO3)2 + 2 NO + 4 CO
The hydrated nitrate is often used as a precursor to supported nickel catalysts.
Safety[edit]
Like other nitrates, nickel nitrate is oxidizing. It is also irritating to the eyes, skin and, upon inhalation of the dust, respiratory tract. It may cause skin allergy. Nickel nitrate is a carcinogen, along with most other nickel compounds. The nickel ion is also toxic to aquatic organisms.
Uses[edit]
Nickel(II) nitrate is used as the precursor for the explosive Nickel Hydrazine Nitrate, which is used as lead-free and safer alternative to Lead Azide and Lead Styphnate. https://networksnew535.weebly.com/ring-for-lighitng-dmg-poe.html.
References[edit]
- ^Perry's Chem Eng Handbook, 7th Ed
- ^ abKeith Lascelles, Lindsay G. Morgan, David Nicholls, Detmar Beyersmann, 'Nickel Compounds' in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a17_235.pub2
![Nickel chloride plating Nickel chloride plating](/uploads/1/3/4/2/134281459/822803546.jpeg)
Salts and covalent derivatives of the nitrate ion
Nickel Chloride 2 Disposal
HNO3 | He | ||||||||||||||||
LiNO3 | Be(NO3)2 | B(NO 3)− 4 | C | NO− 3, NH4NO3 | O | FNO3 | Ne | ||||||||||
NaNO3 | Mg(NO3)2 | Al(NO3)3 | 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)3, Fe(NO3)2 | Co(NO3)2, Co(NO3)3 | Ni(NO3)2 | Cu(NO3)2 | Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | Br | Kr |
RbNO3 | Sr(NO3)2 | Y(NO3)3 | Zr(NO3)4 | Nb | Mo | Tc | Ru | Rh | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In | Sn | Sb(NO3)3 | Te | I | Xe(NO3)2 |
CsNO3 | Ba(NO3)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(NO3)2, Hg(NO3)2 | Tl(NO3)3, TlNO3 | Pb(NO3)2 | Bi(NO3)3 BiO(NO3) | Po | At | Rn | |
FrNO3 | Ra(NO3)2 | 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 | Nd(NO3)3 | Pm | Sm | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy | Ho | Er | Tm | Yb | Lu | |||
Ac(NO3)3 | Th(NO3)4 | Pa | UO2(NO3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr |
Nickel Chloride Phase
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