Difference between revisions of "Zinc sulfide"
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| MeltingPt_ref = | | MeltingPt_ref = | ||
| MeltingPt_notes = (sublimes) | | MeltingPt_notes = (sublimes) | ||
| + | | Odor = Odorless (pure)<br>Rotten-eggs (impure) | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
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==Uses== | ==Uses== | ||
| − | Zinc sulfide can be used to produce [[hydrogen sulfide]] in a lab by the reaction with [[ | + | Zinc sulfide can be used to produce [[hydrogen sulfide]] in a lab by the reaction with a strong acid like [[hydrochloric acid]]. The reaction proceeds as such: |
:ZnS + 2HCl → ZnCl<sub>2</sub> + H<sub>2</sub>S | :ZnS + 2HCl → ZnCl<sub>2</sub> + H<sub>2</sub>S | ||
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[[Category:Inorganic compounds]] | [[Category:Inorganic compounds]] | ||
[[Category:Zinc compounds]] | [[Category:Zinc compounds]] | ||
| + | [[Category:Sulfur compounds]] | ||
[[Category:Sulfides]] | [[Category:Sulfides]] | ||
[[Category:Materials unstable in acidic solution]] | [[Category:Materials unstable in acidic solution]] | ||
Latest revision as of 18:57, 2 August 2018
 ZnS sample.
| |
| Names | |
|---|---|
| IUPAC name
Zinc sulfide
| |
| Other names
Albalith
Sachtolith Sphalerite Wurtzite Zinc monosulfide Zincblende | |
| Properties | |
| ZnS | |
| Molar mass | 97.474 g/mol |
| Appearance | White to yellowish solid |
| Odor | Odorless (pure) Rotten-eggs (impure) |
| Density | 4.090 g/cm3 |
| Melting point | 1,850 °C (3,360 °F; 2,120 K) (sublimes) |
| Boiling point | Sublimes |
| alpha 0.00069 g/100 ml (18 °C) beta 0.00065 g/100 ml (18 °C) | |
| Solubility | Reacts with strong acids |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
−204.6 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
2,000 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Zinc sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Zinc sulfide (or zinc sulphide) is a chemical with the chemical formula ZnS. Zinc sulfide fluoresces green, and is employed most often for its phosphorescent properties.
Contents
Properties
Chemical
Zinc sulfide can be roasted to release sulfur dioxide, leaving zinc oxide behind.
- 2 ZnS + 3 O2 → 2 ZnO + 2 SO2
Physical
Zinc sulfide is a white-yellowish solid, and it is widely used as a pigment. In its dense synthetic form, zinc sulfide can be transparent, and it is used as a window for visible optics and infrared optics. ZnS has a density of 4.090 g/cm3. It is poorly soluble in water but more soluble in acids. ZnS boils at 1,185 °C.
Availability
Zinc sulfide can be purchased from various science shops, as glowing powder.
Higher purity ZnS can be purchased from various chemical suppliers.
Preparation
Zinc sulfide is often produced by reacting zinc oxide with hydrogen sulfide, which produces zinc sulfide and water. Another method for producing the chemical is by heating a solution of zinc sulfate with sodium thiosulfate. A third way is to make a equimolar mix of zinc and sulfur powders and ignite the mix. This produces a bright green flame and impure ZnS. The impure ZnS can be purified through decantation.
Uses
Zinc sulfide can be used to produce hydrogen sulfide in a lab by the reaction with a strong acid like hydrochloric acid. The reaction proceeds as such:
- ZnS + 2HCl → ZnCl2 + H2S
Projects
- Make glowing powder
- Hydrogen sulfide production
- Sulfur dioxide generation
Handling
Safety
Zinc sulfide dust is irritant to the eyes, skin, if inhaled or ingested. In case of ingestion, it will release toxic hydrogen sulfide.
Storage
Zinc sulfide does not require special storage, although it should be kept away from any strong acid vapors, as it will release hydrogen sulfide gas on contact.
Disposal
Zinc sulfide doesn't require special disposal, though it can be neutralized with hydrogen peroxide. Avoid dumping it with acids though.
