Nickel nitrate

From Crystal growing
Jump to: navigation, search



  Nickel nitrate   
Names: nickel nitrate

Formula: Ni(NO3)2
Ni(NO3)2 · 6H2O
SMILES: [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Ni+2]
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
5.7664 Å
0.5766 nm
, b=5.907 Å
5.9070 Å
0.5907 nm
, c=8.4676 Å
8.4676 Å
0.8468 nm
α=90°
90°  
, β=90.966°
90°57′57.6″  
, γ=90°
90°  

cubic (anhydrous)
a=7.31 Å
7.3100 Å
0.7310 nm
, b=7.31 Å
7.3100 Å
0.7310 nm
, c=7.31 Å
7.3100 Å
0.7310 nm
α=90°
90°  
, β=90°
90°  
, γ=90°
90°  

Forms:
https://media.crystalls.info/w/uploads/media/Prolongated_rhombic_prism.json
https://media.crystalls.info/w/uploads/media/Truncated_rhombic_prism.json
https://media.crystalls.info/w/uploads/media/Prolongated_hexagonal_prism.json


Color: blue-green

turquoise

Melting point: 56.7°C
329.85 K
134.06 °F
593.73 °R
(hexahydrate)
Decomposition point: 136.7°C
409.85 K
278.06 °F
737.73 °R
(hexahydrate)
~200°C
473.15 K
392 °F
851.67 °R
(anhydrous)
Refractive index: 1.422 (hexahydrate)
Electrical properties: dielectric
Magnetic properties: paramagnetic
χ=4.3 · 10-3 cm³/mol
Stability: stable (hexahydrate)
hygroscopic (anhydrous)
Hardness: fragile
Toxicity: slightly toxic

Description

Inorganic compound, salt of bivalent transitional metal nickel and inorganic nitric acid. From water solutions crystallizes as hexahydrate.

Synthesis

Reaction between nickel oxide, hydroxide or hydroxycarbonate and nitric acid

Chemical equation:

NiO + 2HNO3 = Ni(NO3)2 + H2O
Ni(OH)2 + 2HNO3 = Ni(NO3)2 + 2H2O
Ni2CO3(OH)2 + 4HNO3 = 2Ni(NO3)2 + CO2↑ + 3H2O

For preparation 100g of nickel nitrate hexahydrate a 25.69g of nickel oxide, 31.88g of hydroxide or 36.35g of hydroxycarbonate and 66.67g 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:

3Ni + 8HNO3 = 3Ni(NO3)2 + 2NO2↑ + 4H2O

For preparation 100g of nickel nitrate hexahydrate a 20.18g of pure nickel and 88.90g 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:

NiSO4 + Ca(NO3)2 = CaSO4↓ + Ni(NO3)2
NiSO4 + Pb(NO3)2 = PbSO4↓ + Ni(NO3)2
NiCl2 + Pb(NO3)2 = PbCl2↓ + Ni(NO3)2

For preparation 100g of nickel nitrate hexahydrate a 81.74g of nickel chloride hexahydrate, 96.58g of nickel sulfate heptahydrate or 90.39g of nickel sulfate hexahydrate and 113.90g of nitrate lead(II), 81.21g of calcium nitrate tetrahydrate or 56.43g of anhydrous calcium nitrate 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:

Ni(OH)2 + 2NH4NO3 = Ni(NO3)2 + 2H2O + 2NH3
Ni2CO3(OH)2 + 4NH4NO3 = 2Ni(NO3)2 + 3H2O + 2NH3↑ + CO2

For preparation 100g of nickel nitrate hexahydrate a 31.88g of hydroxide or 36.35g of nickel hydroxycarbonate and 55.05g 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

Store in its original form or under several layers of varnish at average humidity and room temperature. Do not store in matchboxes or cotton wool and do not heat.

Solubility

Temperatureg/100g of waterg/100g of ethylene glycolg/100g of hydrazineg/100g of dimethylformamide
(anhydrous)(hexahydrate)(anhydrous)(anhydrous)(anhydrous)
0°C
273.15 K
32 °F
491.67 °R
79.2
79.2 g/100g
44.196 %
243
243 g/100g
70.845 %
10°C
283.15 K
50 °F
509.67 °R
~86.7
86.7 g/100g
46.438 %
15°C
288.15 K
59 °F
518.67 °R
~90.4
90.4 g/100g
47.479 %
20°C
293.15 K
68 °F
527.67 °R
94.17
94.17 g/100g
48.499 %
8.1
8.1 g/100g
7.493 %
3
3 g/100g
2.913 %
25°C
298.15 K
77 °F
536.67 °R
99.2
99.2 g/100g
49.799 %
20
20 g/100g
16.667 %
30°C
303.15 K
86 °F
545.67 °R
~105
105 g/100g
51.22 %
40°C
313.15 K
104 °F
563.67 °R
118.4
118.4 g/100g
54.212 %
50°C
323.15 K
122 °F
581.67 °R
139.2
139.2 g/100g
58.194 %
60°C
333.15 K
140 °F
599.67 °R
157.7
157.7 g/100g
61.195 %
70°C
343.15 K
158 °F
617.67 °R
180.1
180.1 g/100g
64.298 %
80°C
353.15 K
176 °F
635.67 °R
~205
205 g/100g
67.213 %
90°C
363.15 K
194 °F
653.67 °R
~230
230 g/100g
69.697 %
100°C
373.15 K
212 °F
671.67 °R
255
255 g/100g
71.831 %
Soluble in ethanol, DMSO, ammonia and acetonitrile.

Gallery


Video


Sources


Navigation