Copper(II) sulfate
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Copper(II) sulfate | |
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Names: | cupric sulfate copper vitriol blue vitriol bluestone Е519 food additive
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Formula: | CuSO4 (anhydrous) CuSO4 · 5H2O (pentahydrate) |
SMILES: | [O-]S(=O)(=O)[O-].[Cu+2] |
Molar mass: | 159.607 g/mol (anhydrous) 249.681 g/mol (pentahydrate) |
Density: | 3.6 g/cm3 (anhydrous) 2.7 g/cm3 (trihydrate) 2.286 g/cm3 (pentahydrate) |
Crystal system: | orthorhombic (anhydrous) a=8.409 Å, b=6.409 Å, c=4.833 Åα=90°, β=90°, γ=90° monoclinic (trihydrate) a=5.59 Å, b=13.03 Å, c=7.34 Åα=90°, β=97.1°, γ=90° triclinic (pentahydrate) a=5.986 Å, b=6.141 Å, c=10.736 Åα=77.333°, β=82.267°, γ=72.567° |
Shapes: | |
Color: | bright-blue blue |
Decomposition point: | 650 °C923.15 K <br />1,202 °F <br />1,661.67 °R <br /> (anhydrous) |
Refractive index: | 1.732 (anhydrous) 1.529 (pentahydrate) |
Magnetic properties: | paramagnetic χ=1.33 · 10-3cm³/mol |
Stability: | slightly erodes (pentahydrate) hygroscopic (anhydrous) |
Hardness: | strong (2.5 on Moh's scale) |
Toxicity: | slightly toxic LD50=612.9mg/kg |
Description
Inorganic compound, salt of bivalent transitional metal copper and inorganic sulfuric acid. From water solutions crystallizes as pentahydrate.
Minerals
Occurs in nature as chalcanthite, chalcocyanite, bonattite and boothite minerals.
Where to buy
In fertilizers store (as "blue vitriol").
Precursors
Reaction between copper(II) hydroxycarbonate, hydroxide or oxide copper (II) and sulfuric acid
Chemical equation:
100.00
g of copper(II) sulfate pentahydrate
а 39.07
g of hydroxide or 31.86
g of oxide and 106.16
g of 37%
sulfuric acid is required.Add acid to the flask, then add small parts of copper 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 pure copper, sulfuric acid and hydrogen peroxide
Chemical equation:
100.00
g of copper(II) sulfate pentahydrate
а 25.45
g of copper, 454.10
g of 3%
peroxide and 106.16
g of 37%
sulfuric acid is required.Add hot acid solution to the flask, then add peroxide and copper pieces, shavings or powder and stir and heat it until gas emission will stop.
Reaction between pure copper and concentrated sulfuric acid
Chemical equation:
100.00
g of copper(II) sulfate pentahydrate
а 25.45
g of copper and 78.56
g of concentrated
sulfuric acid is required.Add concentrated acid solution to the flask, then add copper pieces, shavings or powder and stir and heat it until gas emission will stop.
Electrolysis of sulfuric acid solution with copped anode
Chemical equation:
100.00
g of copper(II) sulfate pentahydrate
а 25.45
g of copper and 106.16
g of 37%
sulfuric acid is required.Add to the flask sulfuric acid solution, then place there copper electrodes and plug them to 1.5-5 V power supply. After some time crystal growth will begin at cathode.
Reaction between copper(II) chloride, sulfate or nitrate and excess of concentrated sulfuric acid
Chemical equation:
100.00
g of copper(II) sulfate pentahydrate
а 68.28
g of copper(II) chloride dihydrate
or 79.96
g of copper(II) acetate monohydrate
or 118.41
g of copper(II) nitrate hexahydrate
and 39.28
g of concentrated
sulfuric acid is required.Add to the flask concentrated sulfuric acid and then add small parts of hot copper compound solution with heating and stirring. Emission of large amount of gas will begin.Attention, exuding gas irritates eyes and lungs! The synthesis should be carried out only in a fume hood or outdoors! After reaction will stop, filter the solution and use it for crystal growing.
Influence of temperature
Growing from a hot solution leads to forming polycrystals.
Influence of impurities
The technical compound impurities slightly affect a growth of crystals. Usually these impurities are copper hydroxychloride, which is insoluble and can be removed by solution filtration, or iron salts, which can be removed only by several stages of recrystallization.
Addition of glycerol leads to flat crystals forming.
Influence of pH level
Addition of hydrochloric acid leads to crystals cleavage into plates.
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
Temperature | гр/100,00 гр water | гр/100,00 гр ethanol | гр/100,00 гр ethanol 40% | гр/100,00 гр methanol | гр/100,00 гр glycerol | гр/100,00 гр ethylene glycol | гр/100,00 гр formic acid 95% | гр/100,00 гр sulfuric acid | гр/100,00 гр dimethylformamide | |||
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(anhydrous) | (pentahydrate) | (pentahydrate) | (pentahydrate) | (anhydrous) | (pentahydrate) | (anhydrous) | (anhydrous) | (pentahydrate) | (pentahydrate) | (anhydrous) | (anhydrous) | |
0°C273.15 K <br />32 °F <br />491.67 °R <br /> | 14.16 | 23.1 | 1.1 | |||||||||
10°C283.15 K <br />50 °F <br />509.67 °R <br /> | 16.82 | 27.5 | ||||||||||
15°C288.15 K <br />59 °F <br />518.67 °R <br /> | ~18.4 | ~30.1 | 0.77 | 30.3 | 8.2 | |||||||
20°C293.15 K <br />68 °F <br />527.67 °R <br /> | 20.05 | 32.6 | 0.25 | 1.04 | 15.6 | 0.05 | ||||||
25°C298.15 K <br />77 °F <br />536.67 °R <br /> | 21.95 | ~35.2 | 1.42 | 0.13 | 1.8 | |||||||
30°C303.15 K <br />86 °F <br />545.67 °R <br /> | 23.92 | 37.8 | ~1.73 | 0.5 | ~0.14 | |||||||
40°C313.15 K <br />104 °F <br />563.67 °R <br /> | 28.54 | 44.6 | ~2.36 | 0.16 | ||||||||
50°C323.15 K <br />122 °F <br />581.67 °R <br /> | 34.05 | ~53.2 | 2.99 | ~0.20 | ||||||||
60°C333.15 K <br />140 °F <br />599.67 °R <br /> | 40.45 | 61.8 | ~0.25 | |||||||||
70°C343.15 K <br />158 °F <br />617.67 °R <br /> | 47.93 | ~72.8 | 0.29 | |||||||||
80°C353.15 K <br />176 °F <br />635.67 °R <br /> | 56.99 | 83.8 | ||||||||||
90°C363.15 K <br />194 °F <br />653.67 °R <br /> | 67.5 | ~99.4 | ||||||||||
100°C373.15 K <br />212 °F <br />671.67 °R <br /> | 76.99 | 115 |
Gallery
Growth in 2 monthsCopper(II) sulfate, Aleksandr Chernikh, VKontakteVKontakte
Growth in 3 weeksCopper(II) sulfate, Maxim Martinov, VKontakteVKontakte
Video
Sources
- R.A.Kiper Properties of compounds. Handbook
- R.A.Kiper Properties of compounds. Handbook
- R.A.Kiper Properties of compounds. Handbook
- C.Beevers, The crystal structure of copper(II) sulfate pentahydrate
- P.Kokkoros, The crystal structure of the anhydrous sulfates of copper and zinc
- Etacude.com reference
- Piece of Science blog
Copper compounds | |
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Salts |
Copper (Cu) • Copper(II) acetate (Cu(CH3COO)2) • Copper(II) dihydrophosphate (Cu(H2PO4)2) • Copper(II) formate (Cu(COOH)2) • Copper(II) lactate (Cu(C3H5O3)2) • Copper(II) nitrate (Cu(NO3)2) • Copper(II) sulfamate (Cu(NH2SO3)2) • Copper(II) sulfate (CuSO4) • Copper(II) tartrate (CuC4H4O6) • Copper(II) chloride (CuCl2) |
Double salts |
Copper-calcium acetate (CuCa(CH3COO)4) • Copper(II)-iron(II) sulfate ((Cu,Fe)SO4) • Copper(II)-ammonium sulfate ((NH4)2Cu(SO4)2) • Copper(II)-potassium sulfate (K2Cu(SO4)2) |
Complexes |
Dicarbonatocuprates • Dioxalatocuprates • Bis-thetramethylethylenediaminecopper(II) nitrate ([Cu((H3CNCH3)2C4H8)](NO3)2) • Glycinecopper(II) sulfate ([Cu(NH2CH2COOH)]SO4) • Potassium dioxalatocuprate(II) (K2[Cu(C2O4)2]) • Sodium dioxalatocuprate(II) (Na2[Cu(C2O4)2]) • Sodium dicarbonatocuprate(II) (Na2[Cu(CO3)2]) • Tetraamminecopper(II) sulfate ([Cu(NH3)4]SO4) • Tetrachlorocuprates • Tris(hydroxymethyl)methanoaminecopper(II) sulfate ([Cu(NH2C(CH2OH)3)4]SO4) |