Difference between revisions of "Copper(II) sulfate"
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Copper(II) sulfate is most commonly encountered as the blue pentahydrate, but it can be dehydrated at 200˚C to form the white, powdery, anhydrous variant. At 650˚C, it will [[Thermal decomposition|decompose]] to form [[copper(II) oxide]] and [[sulfur trioxide]]. It emits an emerald green color in a [[flame test]]. The copper(II) ions in solution can complex with ammonia to form [[tetraamminecopper(II) sulfate]], which may be crystallized. Copper sulfate dissolves in concentrated [[hydrochloric acid]] to form a bright green solution of [[tetrachlorocupric acid]]. This color turns to blue when diluted. | Copper(II) sulfate is most commonly encountered as the blue pentahydrate, but it can be dehydrated at 200˚C to form the white, powdery, anhydrous variant. At 650˚C, it will [[Thermal decomposition|decompose]] to form [[copper(II) oxide]] and [[sulfur trioxide]]. It emits an emerald green color in a [[flame test]]. The copper(II) ions in solution can complex with ammonia to form [[tetraamminecopper(II) sulfate]], which may be crystallized. Copper sulfate dissolves in concentrated [[hydrochloric acid]] to form a bright green solution of [[tetrachlorocupric acid]]. This color turns to blue when diluted. | ||
| − | Metals more reactive than copper will react with copper(II) sulfate, leaving the [[sulfate]] salt of the metal and [[copper]]. Example, using [[zinc]]: | + | Metals more reactive than copper will react with copper(II) sulfate, leaving the [[sulfate]] salt of the metal and [[copper]]. Example, using [[zinc]] metal: |
: CuSO<sub>4</sub> + Zn → ZnSO<sub>4</sub> + Cu | : CuSO<sub>4</sub> + Zn → ZnSO<sub>4</sub> + Cu | ||
Revision as of 20:17, 20 March 2023
_sulfate_pentahydrate.jpg) Copper(II) sulfate pentahydrate crystal
| |
| Names | |
|---|---|
| IUPAC name
Copper(II) sulfate
| |
| Other names
Blue vitriol (pentahydrate)
Bluestone (pentahydrate) Bonattite (trihydrate mineral) Boothite (heptahydrate mineral) Chalcanthite (pentahydrate mineral) Chalcocyanite (mineral) Cupric sulfate | |
| Properties | |
| CuSO4 (anhydrous) CuSO4·5H2O (pentahydrate) | |
| Molar mass | 159.609 g/mol (anhydrous) 249.685 g/mol (pentahydrate) |
| Appearance | White solid (anhydrous) Blue solid (pentahydrate) |
| Odor | Odorless |
| Density | 3.60 g/cm3 (anhydrous) 2.286 g/cm3 (pentahydrate) |
| Melting point | anhydrous 650 °C (1,202 °F; 923 K) (decomposition) pentahydrate 110 °C (230 °F; 383 K) (decomposition) |
| Boiling point | Decomposes |
| anhydrous 14.3 g/100 ml (0 °C) 17.2 g/100 ml (10 °C) 20.5 g/100 ml (20 °C) 22.3 g/100 ml (25 °C) 24.4 g/100 ml (30 °C) 28.7 g/100 ml (40 °C) 33.7 g/100 ml (50 °C) 39.5 g/100 ml (60 °C) 55.5 g/100 ml (80 °C) 75.4 g/100 ml (100 °C) pentahydrate 23.1 g/100 ml (0 °C) 27.5 g/100 ml (10 °C) 32 g/100 ml (20 °C) 37.8 g/100 ml (30 °C) 44.6 g/100 ml (40 °C) 61.8 g/100 ml (60 °C) 83.8 g/100 ml (80 °C) 114 g/100 ml (100 °C) | |
| Solubility | Anhydrous Insoluble in ethanol Pentahydrate Insoluble in acetone, ethanol |
| Solubility in methanol | pentahydrate 1.04 g/100 ml (18 °C) |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
5 J ·mol−1·K−1 |
| Std enthalpy of
formation (ΔfH |
−769.98 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (anhydrous) Sigma-Aldrich (pentahydrate) |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
300 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Copper(I) sulfate Zinc sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Copper(II) sulfate, also known as cupric sulfate, copper sulphate or archaically blue vitriol or vitriol of Cyprus, is the chemical compound with the chemical formula CuSO4. This salt exists as a series of compounds that differ in their degree of hydration. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate (CuSO4·5H2O), the most commonly encountered salt, is bright blue and forms triclinic crystals. Copper(II) sulfate exothermically dissolves in water to give the aquo complex [Cu(H2O)6]2+, which has octahedral molecular geometry and is paramagnetic. Copper sulfate pentahydrate occurs in nature as mineral chalcantite.
Contents
Properties
Physical properties
Copper(II) sulfate is a blue crystalline solid as the pentahydrate, as it is most commonly seen, and the anhydrous form is a white to light gray powder. It has a solubility of 31.6 g/100 mL at 0˚C and 203.3 g/100 mL at 100˚C. Dissolution is slow yet exothermic, and solutions of copper(II) sulfate are dark blue.
Chemical properties
Copper(II) sulfate is most commonly encountered as the blue pentahydrate, but it can be dehydrated at 200˚C to form the white, powdery, anhydrous variant. At 650˚C, it will decompose to form copper(II) oxide and sulfur trioxide. It emits an emerald green color in a flame test. The copper(II) ions in solution can complex with ammonia to form tetraamminecopper(II) sulfate, which may be crystallized. Copper sulfate dissolves in concentrated hydrochloric acid to form a bright green solution of tetrachlorocupric acid. This color turns to blue when diluted.
Metals more reactive than copper will react with copper(II) sulfate, leaving the sulfate salt of the metal and copper. Example, using zinc metal:
- CuSO4 + Zn → ZnSO4 + Cu
The solid obtained can be treated with hydrochloric acid to get rid of excess zinc and other impurities.
Availability
Copper(II) sulfate can be found at most hardware stores as root killer for use in septic systems. These products are usually fairly pure, but require recrystallization to ensure their purity. This source, however, is suitable for use in crystal growing. It can be made from copper metal, nitric acid or hydrogen peroxide, and concentrated sulfuric acid, but this method is economically impractical if not used on an industrial scale.
Preparation
Copper(II) sulfate can also be produced by the electrolysis of sulfuric acid with a copper anode and cathode. The cathode needs to be shielded at the top and exposed at the bottom of the solution. The anode should reside at the very top. The copper(II) sulfate will form a beautiful dark blue layer at the bottom. The solution should be decanted and crystallized.
A simpler route involves reacting copper "rust", like oxide, hydroxide or carbonate with sulfuric acid. Keep adding copper oxide until all the acid has been consumed, filter the solution then recrystallize the compound from the solution.
Likewise, bubbling sulfur dioxide in an aqueous suspension of copper oxide or copper hydroxide will give copper sulfite, which will oxidize in air to copper sulfate.
Projects
- Growing crystals
- Making copper metal
- Making flash powder
- Make sulfuric acid
- Make sulfur trioxide
Handling
Safety
All copper salts, especially soluble ones, are moderately toxic. They should be stored out of reach of small children and pets. They are also toxic to the environment.
Storage
Copper sulfate hydrated can be stored in closed bottles. Anhydrous variety must be stored in sealed closed containers to prevent it from absorbing water from air.
Disposal
Copper sulfate can be disposed of by either precipitating it as the copper(II) carbonate, which is insoluble, and disposing of it as toxic waste.
Another good way is to reduce it with iron or zinc to elemental copper, that can be reused, while the resulting iron or zinc sulfate are much easier to dispose of, as they're less hazardous to the environment.
Gallery
Shielded copper cathode
Electrolytic cell for producing copper(II) sulfate
Copper(II) sulfate product, electrolytically produced
Anhydrous copper sulfate
Crystal showing the structure of the pentahydrate
Copper sulfate crystals made by the hydrogen peroxide/sulfuric acid method
A boiling solution of copper(II) sulfate prior to recrystallization
_sulfate_solution.jpg)
See also
References
- http://en.wikipedia.org/wiki/Copper(II)_sulfate
- CRC Handbook of Chemistry and Physics 66th Edition (1985-1986)
- Personal electrolytic manufacture by Arkoma
