| Customization: | Available |
|---|---|
| CAS No.: | 7758-99-8 |
| Formula: | CuSo4.5H2O |
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| ITEMS | STANDARD | ANALYSIS RESULT |
| Appearance | Blue transparent Crystal | Blue transparent Crystal |
| CuSO4.5H2O | 96%Min | 96.5% |
| Cu | 24.5%Min | 24.6% |
| As | 0.001%Max | 0.0005% |
| Pb | 0.001%Max | 0.0008% |
| Zn | 0.02%Max | 0.012% |
| Fe | 0.05%Max | 0.02% |
| ITEMS | STANDARD | ANALYSIS RESULT |
| Appearance | Blue transparent Crystal | Blue transparent Crystal |
| CuSO4.5H2O | 98%Min | 98.8% |
| Cu | 25%Min | 25.06% |
| As | 0.001%Max | 0.0008% |
| Pb | 0.001%Max | 0.0007% |
| Fe | 0.001%Max | 0.0008% |
| H2SO4 | 0.2%Max | 0.12% |
| Water Insoluble | 0.2%Max | 0.10% |
The pentahydrate (CuSO4·5H2O), the most commonly encountered salt, is bright blue. It exothermically dissolves in water to give the aquo complex [Cu(H2O)6]2+, which has octahedral molecular geometry. The structure of the solid pentahydrate reveals a polymeric structure wherein copper is again octahedral but bound to four water ligands. The Cu(II)(H2O)4 centers are interconnected by sulfate anions to form chains. Anhydrous copper sulfate is a light grey powder.
Copper sulfate is produced industrially by treating copper metal with hot concentrated sulfuric acid or its oxides with dilute sulfuric acid. For laboratory use, copper sulfate is usually purchased. Copper sulfate can also be produced by slowly leaching low-grade copper ore in air; bacteria may be used to hasten the process.
Commercial copper sulfate is usually about 98% pure copper sulfate, and may contain traces of water. Anhydrous copper sulfate is 39.81 percent copper and 60.19 percent sulfate by mass, and in its blue, hydrous form, it is 25.47% copper, 38.47% sulfate (12.82% sulfur) and 36.06% water by mass. Four types of crystal size are provided based on its usage: large crystals (10-40 mm), small crystals (2-10 mm), snow crystals (less than 2 mm), and windswept powder (less than 0.15 mm).
Copper(II) sulfate pentahydrate decomposes before melting. It loses two water molecules upon heating at 63 °C (145 °F), followed by two more at 109 °C (228 °F) and the final water molecule at 200 °C (392 °F). Dehydration proceeds by decomposition of the tetraaquacopper(2+) moiety, two opposing aqua groups are lost to give a diaquacopper(2+) moiety. The second dehydration step occurs when the final two aqua groups are lost. Complete dehydration occurs when the final unbound water molecule is lost. At 650 °C (1,202 °F), copper(II) sulfate decomposes into copper(II) oxide (CuO) and sulfur trioxide (SO3).
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