Copper(II) sulfate
From Freepedia
| Copper(II) sulfate | |
|---|---|
| Image:CuSO4 5H2O.jpg | |
| General | |
| Systematic name | Copper(II) sulfate pentahydrate |
| Other names | Cupric sulfate Blue vitriol Chalcanthite |
| Molecular formula | CuSO4·5H2O |
| Molar mass | 249.68 g/mol (pentahydrate) |
| Appearance | blue crystalline solid |
| CAS number | [7758-99-8] |
| 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 | R22, R36/38, R50/53 |
| S-Phrases | S2, S22, S60, S61 |
| PEL-TWA (OSHA) | 1 mg/m3 |
| 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) Infobox disclaimer and references | |
Copper(II) sulfate, copper(II) sulphate, or blue vitriol (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 are: blue stone and blue vitriol.
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).
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). 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.
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