Copper(II) sulfate

Copper(II) sulfate ;
Names:	cupric sulfate; copper vitriol; blue vitriol; bluestone; Е519 food additive PubChem: 24462; PubChem: 24463; CAS: 7758-98-7; CAS: 7758-99-8; CAS: 16448-28-5; CAS: 18939-61-2; CAS: 19086-18-1; InChI Key: ARUVKPQLZAKDPS-UHFFFAOYSA-L; InChI Key: ARUVKPQLZAKDPS-NUQVWONBAI; InChI Key: JZCCFEFSEZPSOG-UHFFFAOYSA-L;
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:	https://en.crystalls.info/w/uploads/media/9/9f/Parallelepiped.json Parallelepiped Template:Pinacoidal prismTemplate:Rhombohedron;
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

Can be bought in fertilizers store (as "blue vitriol").

Precursors

Reaction between copper(II) hydroxycarbonate, hydroxide or oxide copper (II) and sulfuric acid

Chemical equation:

2H₂SO₄ + Cu₂CO₃(OH)₂ = 2CuSO₄ + 3H₂O + CO₂↑

H₂SO₄ + Cu(OH)₂ = CuSO₄ + 2H₂O

H₂SO₄ + CuO = CuSO₄ + H₂O

For preparation of 100.00g of copper(II) sulfate

pentahydratepentahydrate
anhydrous

а 39.07g of hydroxide or 31.86g of oxide and 106.16g of 37%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:

H₂SO₄ + Cu + H₂O₂ = CuSO₄ + 2H₂O

For preparation of 100.00g of copper(II) sulfate

pentahydratepentahydrate
anhydrous

а 25.45g of copper, 454.10g of

3%3%
30%

peroxide and 106.16g of 37%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:

2H₂SO₄ + Cu = CuSO₄ + 2H₂O + SO₂↑

For preparation of 100.00g of copper(II) sulfate

pentahydratepentahydrate
anhydrous

а 25.45g of copper and 78.56g of concentratedconcentrated 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:

H₂SO₄ + Cu —electrolysis→ CuSO₄ + H₂↑

For preparation of 100.00g of copper(II) sulfate

pentahydratepentahydrate
anhydrous

а 25.45g of copper and 106.16g of 37%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:

H₂SO₄ + CuCl₂ = CuSO₄ + 2HCl↑

H₂SO₄ + Cu(CH₃COO)₂ = CuSO₄ + 2CH₃COOH↑

H₂SO₄ + Cu(NO₃)₂ = CuSO₄ + 2HNO₃↑

For preparation of 100.00g of copper(II) sulfate

pentahydratepentahydrate
anhydrous

а 68.28g of copper(II) chloride

dihydratedihydrate
anhydrous

or 79.96g of copper(II) acetate

monohydratemonohydrate
anhydrous

or 118.41g of copper(II) nitrate

hexahydratehexahydrate
anhydrous

and 39.28g of concentratedconcentrated 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.
Addition of potassium sulfate or iron(III) sulfate leads to nearly cubic crystals.
Addition of aluminum sulfate elongates it.
Addition of magnesium sulfate, zinc sulfate or sodium sulfate leads to thinner crystals.
Addition of anions other than sulfate does not influence shape.

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
Temperature	(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`

Insoluble in acetone, ethyl acetate, methyl acetate, ammonia, methylamine and benzonitrile.

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Copper compounds
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)

Sulfates
Simple	Aluminum sulfate (Al₂(SO₄)₃) • Ammonium sulfate ((NH₄)₂SO₄) • Calcium sulfate (CaSO₄) • Cadmium sulfate (CdSO₄) • Cerium(III) sulfate (Ce₂(SO₄)₃) • Cerium(IV) sulfate (Ce(SO₄)₂) • Chromium(III) sulfate (Cr₂(SO₄)₃) • Cobalt(II) sulfate (CoSO₄) • Copper(II) sulfate (CuSO₄) • Gadolinium sulfate (Gd₂(SO₄)₃) • Holmium sulfate (Ho₂(SO₄)₃) • Hydrazine sulfate (N₂H₄ · H₂SO₄) • Iron(II) sulfate (FeSO₄) • Iron(III) sulfate (Fe₂(SO₄)₃) • Lanthanum sulfate (La₂(SO₄)₃) • Lithium sulfate (Li₂SO₄) • Magnesium sulfate (MgSO₄) • Manganese(II) sulfate (MnSO₄) • Neodymium sulfate (Nd₂(SO₄)₃) • Nickel sulfate (NiSO₄) • Potassium sulfate (K₂SO₄) • Praseodymium(III) sulfate (Pr₂(SO₄)₃) • Rubidium sulfate (Rb₂SO₄) • Sodium hydrosulfate (NaHSO₄) • Sodium sulfate (Na₂SO₄) • Yttrium sulfate (Gd₂(SO₄)₃) • Zinc sulfate (ZnSO₄)
Alums	Aluminum-ammonium sulfate (NH₄Al(SO₄)₂) • Aluminum-potassium sulfate (KAl(SO₄)₂) • Chromium(III)-ammonium sulfate (NH₄Cr(SO₄)₂) • Chromium(III)-potassium sulfate (KCr(SO₄)₂) • Indium(III)-potassium sulfate (KIn(SO₄)₂) • Iron(III)-ammonium sulfate (NH₄Fe(SO₄)₂) • Iron(III)-potassium sulfate (KFe(SO₄)₂) • Vanadium(III)-ammonium sulfate (NH₄V(SO₄)₂)
Tutton's salts	Cobalt(II)-ammonium sulfate ((NH₄)₂Co(SO₄)₂) • Cobalt(II)-potassium sulfate (K₂Co(SO₄)₂) • Copper(II)-ammonium sulfate ((NH₄)₂Cu(SO₄)₂) • Copper(II)-potassium sulfate (K₂Cu(SO₄)₂) • Iron(II)-ammonium sulfate ((NH₄)₂Fe(SO₄)₂) • Iron(II)-potassium sulfate (K₂Fe(SO₄)₂) • Magnesium-ammonium sulfate ((NH₄)₂Mg(SO₄)₂) • Magnesium-potassium sulfate (K₂Mg(SO₄)₂) • Magnesium-potassium sulfate-chromate (K₂CrO₄ · MgSO₄) • Manganese(II)-ammonium sulfate ((NH₄)₂Mn(SO₄)₂) • Manganese(II)-potassium sulfate (K₂Mn(SO₄)₂) • Nickel-ammonium sulfate ((NH₄)₂Ni(SO₄)₂) • Nickel-potassium sulfate (K₂Ni(SO₄)₂) • Zinc-ammonium sulfate ((NH₄)₂Zn(SO₄)₂) • Zinc-potassium sulfate (K₂Zn(SO₄)₂) •
Double salts	Copper(II)-iron(II) sulfate ((Cu,Fe)SO₄) • Iron(II)-magnesium sulfate ((Fe,Mg)SO₄) • Lithium-potassium sulfate (KLiSO₄) • Sodium-ammonium sulfate (NaNH₄SO₄) • Zinc-sodium sulfate (Na₂Zn(SO₄)₂) •
Adducts	Triglycine sulfate ((NH₂CH₂COOH)₃ · H₂SO₄) • Glutamic acid sulfate (C₅H₉NO₄ · H₂SO₄)
Complexes	Cerium(III) sulfocerate(IV) (Ce₄[Ce(SO₄)₄]₃) • Glycinecopper(II) sulfate ([Cu(NH₂CH₂COOH)]SO₄) • Hexakarbamatzinc sulfate ([(CON₂H₄)₆Zn]SO₄) • Tetraamminecopper(II) sulfate ([Cu(NH₃)₄]SO₄) • Tris(hydroxymethil)methanoaminecopper(II) sulfate ([Cu(NH₂C(CH₂OH)₃)₄]SO₄)

Copper(II) sulfate
Names:	cupric sulfate copper vitriol blue vitriol bluestone Е519 food additive PubChem: 24462 PubChem: 24463 CAS: 7758-98-7 CAS: 7758-99-8 CAS: 16448-28-5 CAS: 18939-61-2 CAS: 19086-18-1 InChI Key: ARUVKPQLZAKDPS-UHFFFAOYSA-L InChI Key: ARUVKPQLZAKDPS-NUQVWONBAI InChI Key: JZCCFEFSEZPSOG-UHFFFAOYSA-L
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:	Parallelepiped Template:Pinacoidal prism Template:Rhombohedron
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

Copper(II) sulfate

Description

Minerals

Where to buy

Precursors

Reaction between copper(II) hydroxycarbonate, hydroxide or oxide copper (II) and sulfuric acid

Reaction between pure copper, sulfuric acid and hydrogen peroxide

Reaction between pure copper and concentrated sulfuric acid

Electrolysis of sulfuric acid solution with copped anode

Reaction between copper(II) chloride, sulfate or nitrate and excess of concentrated sulfuric acid

Influence of temperature

Influence of impurities

Influence of pH level

Storage conditions

Solubility

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