| IUPAC name
| Other names
|Molar mass|| 264.3 g/mol (anhydrous)|
372.38 g/mol (hexahydrate)
|Appearance||Colorless deliquescent solid|
|Density|| 2.26 g/cm3 (hexahydrate)|
2.933 g/cm3 (anhydrous) (20 °C)
|Melting point|| 105–107 °C (221–225 °F; 378–380 K) (hexahydrate)|
262 °C (504 °F; 535 K) (anhydrous)
|50 g/100 ml (20 °C)|
|Solubility|| Soluble in acetonitrile, alcohols, DMSO|
Slightly soluble in glacial acetic acid
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich (hexahydrate)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Zinc perchlorate (Zn(ClO4)2) is a hygroscopic chemical compound, that may be used as oxidizer. It is more commonly encountered as its hexahydrate form, Zn(ClO4)2·6H2O.
Zinc perchlorate decomposes if heated to high temperatures and may explode if heated too strongly.
Zinc perchlorate is a hygroscopic colorless solid, soluble in water and low weight alcohols.
It is sold by chemical suppliers.
- ZnO + 2 HClO4 → Zn(ClO4)2 + H2O
- ZnCO3 + 2 HClO4 → Zn(ClO4)2 + H2O + CO2
Do not use zinc metal, as the reaction is violent.
The resulting solution is gently heated and the product is recrystallized from the concentrated solution.
Recrystallizing the salt from water yields the hexahydrate form. Anhydrous zinc perchlorate cannot be produced by heating zinc(II) perchlorate hexahydrate, since it decomposes upon heating.
One source indicates that the anhydrous form can be obtained by heating the hexahydrate with triethyl orthoformate, then drying the resulting solid under vacuum. So far this method hasn't been verified.
- Source of perchlorates
- Ignite combustible materials
Zinc perchlorate is a powerful oxidizing agent. In contact with strong acids, it will ignite organic material on contact.
Zinc perchlorate should be kept in airtight bottles, away from any combustible materials.
Can be mixed with a flammable material and ignited.
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