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| Copper(II) sulfate | |
|---|---|
| General | |
| Systematic name | Copper(II) sulfate pentahydrate |
| Other names | Cupric sulfate Blue vitriol Bluestone Chalcanthite |
| Molecular formula | CuSO4·5H2O |
| Molar mass | 249.68 g/mol (pentahydrate) 159.58 g/mol (anhydrous) |
| Appearance | blue crystalline solid (pentahydrate) gray-white powder (anhydrous) |
| CAS number | * |
| EINECS number | 231-847-6 |
| Properties | |
| Density and phase | 2.284 g/cm3, solid |
| Solubility in water | 31.6 g/100 ml (0 °C) |
| Melting point | 110 °C (− 4H2O) 150 °C (− 5H2O) 650 °C decomp. |
| Structure | |
| Coordination geometry | ? |
| Crystal structure | Triclinic |
| Thermodynamic data | |
| Standard enthalpy of formation ΔfH°solid | -769.98 kJ/mol |
| Standard molar entropy S°solid | 109.05 J.K−1.mol−1 |
| Safety data | |
| EU classification | Harmful Dangerous for the environment |
| R-Phrases | , , |
| S-Phrases | , , , |
| NFPA 704 | |
| PEL-TWA | 1 mg/m³ (OSHA) |
| IDLH (NIOSH) | 100 mg/m3 |
| Flash point | non flammable |
| RTECS number | GL8800000 |
| Supplementary data page | |
| Structure and properties | n, εr, etc. |
| Thermodynamic data | Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| Related compounds | |
| Other cations | Copper(I) sulfate Nickel(II) sulfate Zinc sulfate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Chemical infobox | |
Copper(II) sulfate or copper(II) sulphate (CuSO4) is the most common copper salt, made by the action of sulfuric acid on the base copper(II) oxide. The anhydrous form is a pale green or gray-white powder, while the hydrated form is bright blue. The archaic name for copper(II) sulfate was cupric sulfate. Some common names include blue stone and blue vitriol. Like most other copper compounds, copper(II) sulfate is poisonous to humans.
Copper(II) sulfate is a desiccant. As such, it most commonly occurs in nature as copper(II) sulfate pentahydrate (CuSO4 · 5H2O). This mineral is called chalcanthite. Copper(II) sulfate decomposes before melting. The common pentahydrate form dehydrates, losing four water molecules at 110 °C and all five at 150 °C. At 650 °C copper(II) sulfate decomposes into copper(II) oxide (CuO), Sulfur dioxide (SO2) and oxygen (O2).
Uses
It can be used to plate metals with copper, as a fungicide or herbicide, or as a chemical test for water (the anhydrous form will absorb water, turning blue). Mixed with lime it is called Bordeaux mixture. It is also used, in Fehling's solution, to test for reducing sugars, which reduce the blue Cu2+aq ions to red copper(I) oxide. Still other uses include hair dyes and the processing of leather and textiles.
Copper sulfate is also used to test blood for anemia. A drop of the patient's blood is dropped into a container of copper sulfate, if it sinks within a certain time, then the patient has sufficient haemogloblin levels and is not anemic. If the blood floats or sinks too slowly, then the patient is iron-deficient and may be anemic.
In a flame test, copper ions emit a deep blue-green light, much more blue than the flame test for barium.
When heated in an open flame the crystals are dehydrated and turn grayish-white.
Copper sulfate is a commonly included chemical in childrens chemistry sets and is often used in high school crystal growing and copper plating experiments.
External links
- International Chemical Safety Card 0751 (anhydrous)
- International Chemical Safety Card 1416 (pentahydrate)
- National Pollutant Inventory - Copper and compounds fact sheet
- UNCP Copper
Copper compounds | Sulfates | Desiccants | Herbicides
Síran měďnatý | Kobber(II)sulfat | Kupfersulfat | Sulfato cúprico | Sulfate de cuivre | Réz-szulfát | Koper(II)sulfaat | 硫酸銅(II) | Koppersulfaat | Siarczan miedzi | Sulfato de cobre | Kuparisulfaatti | Сульфат меди | Сульфат міді | 硫酸铜
"Copper(II) sulfate"