Zinc chloride

From Sciencemadness Wiki
Revision as of 20:11, 10 October 2015 by Mabus (Talk | contribs)

Jump to: navigation, search
Zinc chloride
Names
IUPAC name
Zinc chloride
Systematic IUPAC name
Zinc chloride
Properties
ZnCl2
Molar mass 136.315 g/mol
Appearance White deliquescent crystalline solid
Density 2.907 g/cm3
Melting point 292 °C (558 °F; 565 K)
Boiling point 756 °C (1,393 °F; 1,029 K)
4320 g/L (25 °C)
Solubility acetone, ethanol, glycerol
Hazards
Flash point None
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Zinc chloride is the name of a chemical compound with the formula ZnCl2.

Properties

Chemical

Zinc chloride is a hygroscopic compound, that will absorb water from air to form at least 5 hydrates. Heating them will result in zinc oxychloride.

Physical

Zinc chloride is an odorless, hygroscopic and even deliquescent white solid, very soluble in water and ethanol, as well as acetone and glycerol.

Availability

Zinc chloride is available as hydrated form as metal flux, though this form is not very useful.

Anhydrous zinc chloride can be purchased from chemical suppliers.

Preparation

Anhydrous zinc chloride can be prepared by reacting zinc metal with chlorine at high temperatures. The hydrated form can also be turned anhydrous by heating it in a stream of hydrogen chloride, or adding thionyl chloride.

Projects

  • Make zinc carbonate
  • Friedel–Crafts acylation catalyst
  • Make alkyl chlorides
  • Make fluorescein
  • Make smoke screens
  • Make tetrachlorozincate compounds
  • Make zinc ammonia chlorides
  • Make zinc Sorel cement
  • Dissolve cellulose
  • Fingerprint detection

Handling

Safety

Zinc chloride is a skin and respiratory irritant, especially the anhydrous form. As it hydrolyzes in water, it will release hydrochloric acid, which is corrosive. Proper protection should be worn when handling the compound.

Storage

In closed or sealed containers, especially the anhydrous form.

Disposal

Can be neutralized by mixing it with lime water.

References

Relevant Sciencemadness threads