Difference between revisions of "Zinc chloride"
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| IUPACName = Zinc chloride | | IUPACName = Zinc chloride | ||
| PIN = | | PIN = | ||
| − | | SystematicName = | + | | SystematicName = Zinc chloride |
| − | | OtherNames = | + | | OtherNames = Zinc dichloride<br>Butter of zinc |
| − | + | ||
| − | + | ||
| − | + | ||
| − | + | ||
| − | + | ||
<!-- Images --> | <!-- Images --> | ||
| ImageFile = | | ImageFile = | ||
| Line 66: | Line 61: | ||
| MeltingPt_ref = | | MeltingPt_ref = | ||
| MeltingPt_notes = | | MeltingPt_notes = | ||
| + | | Odor = Odorless | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| − | | Solubility = | + | | Solubility = 208 g/100 ml (0 °C)<br>272 g/100 ml (10 °C)<br>367 g/100 ml (20 °C)<br>408 g/100 ml (25 °C)<br>435 g/100 ml (30 °C)<br>453 g/100 ml (40 °C)<br>471 g/100 ml (50 °C)<br>495 g/100 ml (60 °C)<br>549 g/100 ml (80 °C)<br>614 g/100 ml (100 °C) |
| − | | SolubleOther = acetone, ethanol, glycerol | + | | SolubleOther = Soluble in [[acetone]], [[ethanol]], [[glycerol]] |
| − | | | + | | Solubility1 = 43.5 g/100 ml (18 °C) |
| − | | VaporPressure = | + | | Solvent1 = acetone |
| + | | Solubility2 = 100 g/100 ml (12.5 °C) | ||
| + | | Solvent2 = ethanol | ||
| + | | Solubility3 = 50 g/100 ml (15.5 °C) | ||
| + | | Solvent3 = glycerol | ||
| + | | Solubility4 = 8 g/100 ml (20 °C) | ||
| + | | Solvent4 = hydrazine | ||
| + | | Solubility5 = 2.6 g/100 ml (12.5 °C) | ||
| + | | Solvent5 = pyridine | ||
| + | | Solubility6 = 0.16 g/100 ml (0 °C) | ||
| + | | Solvent6 = sulfur dioxide | ||
| + | | VaporPressure = ~0 mmHg | ||
}} | }} | ||
| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
| Line 86: | Line 93: | ||
}} | }} | ||
| Section5 = {{Chembox Explosive | | Section5 = {{Chembox Explosive | ||
| − | | ShockSens = | + | | ShockSens = Non-explosive |
| − | | FrictionSens = | + | | FrictionSens = None |
| − | | DetonationV = | + | | DetonationV = Non-explosive |
| − | | REFactor = | + | | REFactor = Non-explosive |
}} | }} | ||
| Section6 = {{Chembox Hazards | | Section6 = {{Chembox Hazards | ||
| − | | AutoignitionPt = | + | | AutoignitionPt = None |
| − | | ExploLimits = | + | | ExploLimits = None |
| − | | ExternalMSDS = | + | | ExternalMSDS = [https://www.docdroid.net/s3rxRW2/zinc-chloride-sa.pdf.html Sigma-Aldrich] (anhydrous) |
| − | | FlashPt = | + | | FlashPt = None |
| − | | LD50 = | + | | LD50 = 350 mg/kg (rat, oral) |
| LC50 = | | LC50 = | ||
| − | | MainHazards = | + | | MainHazards = Irritant<br>Corrosive |
| NFPA-F = | | NFPA-F = | ||
| NFPA-H = | | NFPA-H = | ||
| Line 109: | Line 116: | ||
| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = | + | | OtherCompounds = [[Zinc acetate]] |
}} | }} | ||
}} | }} | ||
| − | '''Zinc chloride''' is the name of a chemical compound with the formula ZnCl<sub>2</sub>. | + | '''Zinc chloride''' is the name of a chemical compound with the formula '''ZnCl<sub>2</sub>'''. |
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Zinc chloride is a hygroscopic compound, that will absorb water from air to form at least 5 hydrates. Heating | + | Zinc chloride is a hygroscopic compound, that will absorb water from air to form at least 5 hydrates. Heating zinc chloride hydrate and aqueous solutions of zinc chloride will decompose them, resulting in zinc oxychlorides and HCl. |
===Physical=== | ===Physical=== | ||
| − | Zinc chloride is an odorless, hygroscopic and even deliquescent white solid, very soluble in water and ethanol, as well as acetone and glycerol. | + | Zinc chloride is an odorless, hygroscopic and even deliquescent white solid, very soluble in [[water]] and [[ethanol]], as well as [[acetone]] and [[glycerol]]. It will also dissolve in [[hydrochloric acid]]. |
==Availability== | ==Availability== | ||
| Line 125: | Line 132: | ||
Anhydrous zinc chloride can be purchased from chemical suppliers. | Anhydrous zinc chloride can be purchased from chemical suppliers. | ||
| + | |||
| + | Zinc chloride can be found in nature in the form of ''simonkolleite'' (zinc chloride hydroxide monohydrate). | ||
==Preparation== | ==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]]. | + | 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]], then boiling off the resulting liquid. |
==Projects== | ==Projects== | ||
| Line 133: | Line 142: | ||
*Friedel–Crafts acylation catalyst | *Friedel–Crafts acylation catalyst | ||
*Make alkyl chlorides | *Make alkyl chlorides | ||
| − | *Make fluorescein | + | *Make [[fluorescein]] |
*Make smoke screens | *Make smoke screens | ||
*Make tetrachlorozincate compounds | *Make tetrachlorozincate compounds | ||
*Make zinc ammonia chlorides | *Make zinc ammonia chlorides | ||
*Make zinc Sorel cement | *Make zinc Sorel cement | ||
| − | *Dissolve cellulose | + | *Dissolve [[cellulose]] |
*Fingerprint detection | *Fingerprint detection | ||
| Line 146: | Line 155: | ||
===Storage=== | ===Storage=== | ||
| − | + | Zinc chloride should be kept in closed or sealed containers, especially the anhydrous form. A drybox or desiccator can also be used, though water will slowly get inside the container. For storage of very pure zinc chloride, a Schlenk flask should be used. | |
===Disposal=== | ===Disposal=== | ||
| − | Can be neutralized by mixing it with lime water. | + | Can be neutralized by mixing it with lime water, then poured down the drain or dumped in trash. |
==References== | ==References== | ||
| Line 155: | Line 164: | ||
===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=41278 Recrystallizing Zinc Chloride] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=41278 Recrystallizing Zinc Chloride] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=32902 Anhydrous Zinc Chloride Attempted Synthesis] | ||
[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
Latest revision as of 21:40, 8 August 2020
| Names | |
|---|---|
| IUPAC name
Zinc chloride
| |
| Systematic IUPAC name
Zinc chloride | |
| Other names
Zinc dichloride
Butter of zinc | |
| Properties | |
| ZnCl2 | |
| Molar mass | 136.315 g/mol |
| Appearance | White deliquescent crystalline solid |
| Odor | Odorless |
| Density | 2.907 g/cm3 |
| Melting point | 292 °C (558 °F; 565 K) |
| Boiling point | 756 °C (1,393 °F; 1,029 K) |
| 208 g/100 ml (0 °C) 272 g/100 ml (10 °C) 367 g/100 ml (20 °C) 408 g/100 ml (25 °C) 435 g/100 ml (30 °C) 453 g/100 ml (40 °C) 471 g/100 ml (50 °C) 495 g/100 ml (60 °C) 549 g/100 ml (80 °C) 614 g/100 ml (100 °C) | |
| Solubility | Soluble in acetone, ethanol, glycerol |
| Solubility in acetone | 43.5 g/100 ml (18 °C) |
| Solubility in ethanol | 100 g/100 ml (12.5 °C) |
| Solubility in glycerol | 50 g/100 ml (15.5 °C) |
| Solubility in hydrazine | 8 g/100 ml (20 °C) |
| Solubility in pyridine | 2.6 g/100 ml (12.5 °C) |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (anhydrous) |
| Flash point | None |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
350 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Zinc acetate |
| 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.
Contents
Properties
Chemical
Zinc chloride is a hygroscopic compound, that will absorb water from air to form at least 5 hydrates. Heating zinc chloride hydrate and aqueous solutions of zinc chloride will decompose them, resulting in zinc oxychlorides and HCl.
Physical
Zinc chloride is an odorless, hygroscopic and even deliquescent white solid, very soluble in water and ethanol, as well as acetone and glycerol. It will also dissolve in hydrochloric acid.
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.
Zinc chloride can be found in nature in the form of simonkolleite (zinc chloride hydroxide monohydrate).
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, then boiling off the resulting liquid.
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
Zinc chloride should be kept in closed or sealed containers, especially the anhydrous form. A drybox or desiccator can also be used, though water will slowly get inside the container. For storage of very pure zinc chloride, a Schlenk flask should be used.
Disposal
Can be neutralized by mixing it with lime water, then poured down the drain or dumped in trash.
