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Nickel nitrate | |
---|---|
Names: | nickel nitrate nickelous nitrate |
Formula: | Ni(NO3)2 (anhydrous) Ni(NO3)2 · 6H2O (hexahydrate) |
Molar mass: | 182.701 g/mol (anhydrous) 290.790 g/mol (hexahydrate) |
Density: | 2.05 g/cm3 (hexahydrate) |
Crystal system: | triclinic (hexahydrate) monoclinic (dihydrate) a=5.7664 Å, b=5.907 Å, c=8.4676 Åα=90°, β=90.966°, γ=90° cubic (anhydrous) a=7.31 Å, b=7.31 Å, c=7.31 Åα=90°, β=90°, γ=90° |
Shapes: |
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Color: | blue-green turquoise |
Melting point: | 56.7 °C329.85 K <br />134.06 °F <br />593.73 °R <br /> (hexahydrate) |
Decomposition point: | 136.7 °C409.85 K <br />278.06 °F <br />737.73 °R <br /> (hexahydrate) ~200 °C"~" is not declared as a valid unit of measurement for this property. (anhydrous) |
Refractive index: | 1.422 (hexahydrate) |
Magnetic properties: | paramagnetic χ=4.30 · 10-3cm³/mol |
Stability: | stable (hexahydrate) hygroscopic (anhydrous) |
Hardness: | fragile |
Toxicity: | slightly toxic LD50=1620mg/kg |
Description
Inorganic compound, salt of bivalent transitional metal nickel and inorganic nitric acid. From water solutions crystallizes as hexahydrate.
Precursors
Reaction between nickel oxide, hydroxide or hydroxycarbonate and nitric acid
Chemical equation:
100.00
g of nickel nitrate hexahydrate
а 25.69
g of nickel oxide or 31.88
g of hydroxide or 36.35
g of hydroxycarbonate and 66.67
g of 65%
acid is required.Add acid to the flask, then add small parts of nickel compound with stirring until it will totally dissolve or, if you use carbonate, until carbon dioxide emission will stop. After reaction will stop, filter the solution and use it for crystal growing.
Reaction between metal nickel and diluted nitric acid
Chemical equation:
100.00
g of nickel nitrate hexahydrate
а 20.18
g of pure nickel and 88.90
g of 65%
acid is required.Add diluted acid solution to the flask, then add nickel pieces, shavings or powder and stir it until gas emission will stop.
Reaction between nickel sulfate and calcium or lead(II) nitrate
You can use nickel chloride instead of sulfate if you use lead salt..
Chemical equation:
100.00
g of nickel nitrate hexahydrate
а 81.74
g of nickel chloride hexahydrate
or 96.58
g of nickel sulfate heptahydrate
and 113.90
g of nitrate lead(II) or 81.21
g of calcium nitrate tetrahydrate
is required.Add to the flask with calcium or lead nitrate solution small parts of nickel salt solution and stir. The large amount of poorly soluble precipitate will form. Settle it out and discard, then filter the solution carefully.
Reaction between nickel hydroxide or hydroxycarbonate and ammonium nitrate
Chemical equation:
100.00
g of nickel nitrate hexahydrate
а 31.88
g of hydroxide or 36.35
g of nickel hydroxycarbonate and 55.05
g of ammonium nitrate is required.Add to the flask suspended in water nickel compounds and then add small parts of hot ammonium nitrate solution with heating and stirring. Emission of large amount of ammonia will begin.Attention, exuding ammonia irritates eyes and lungs! The synthesis should be carried out only in a fume hood or outdoors!
Storage conditions
Keep in its original form or under several layers of varnish at average humidity and room temperature. Do not keep crystals near heaters.
Solubility
Temperature | g/100,00 g water | g/100,00 g ethylene glycol | g/100,00 g hydrazine | g/100,00 g dimethylformamide | |
---|---|---|---|---|---|
(anhydrous) | (hexahydrate) | (anhydrous) | (anhydrous) | (anhydrous) | |
0°C273.15 K <br />32 °F <br />491.67 °R <br /> | 79.2 | 243 | |||
20°C293.15 K <br />68 °F <br />527.67 °R <br /> | 94.17 | 8.1 | 3 | ||
25°C298.15 K <br />77 °F <br />536.67 °R <br /> | 99.2 | 20 | |||
30°C303.15 K <br />86 °F <br />545.67 °R <br /> | ~105 | ||||
40°C313.15 K <br />104 °F <br />563.67 °R <br /> | 118.4 | ||||
50°C323.15 K <br />122 °F <br />581.67 °R <br /> | 139.2 | ||||
60°C333.15 K <br />140 °F <br />599.67 °R <br /> | 157.7 | ||||
70°C343.15 K <br />158 °F <br />617.67 °R <br /> | 180.1 | ||||
100°C373.15 K <br />212 °F <br />671.67 °R <br /> | 255 |
Gallery
Sources
Nickel compounds | |
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Salts |
Nickel (Ni) • Nickel acetate (Ni(CH3COO)2) • Nickel nitrate (Ni(NO3)2) • Nickel sulfate (NiSO4) • Nickel tartrate (NiC4H4O6) |
Double salts |
Nickel-ammonium sulfate ((NH4)2Ni(SO4)2) • Nickel-potassium sulfate (K2Ni(SO4)2) |
Complexes |
Hexaamminenickel chloride ([Ni(NH3)6]Cl2) • Tris(ethylenediamine)nickel(II) oxalate ([Ni(H2NCH2CH2NH2)3]C2O4) |