Difference between revisions of "Cobalt(II) chloride"

From Sciencemadness Wiki
Jump to: navigation, search
(Created page with "'''Cobalt(II) chloride''' is a colorful compound with the formula CoCl<sub>2</sub>. Three hydrates of cobalt chloride exist, anydrous, dihydrate, and hexahydrate. All three hy...")
 
m (Fixed typos.)
 
(10 intermediate revisions by 2 users not shown)
Line 1: Line 1:
−
'''Cobalt(II) chloride''' is a colorful compound with the formula CoCl<sub>2</sub>. Three hydrates of cobalt chloride exist, anydrous, dihydrate, and hexahydrate. All three hydrates are hygroscopic, with the anhydrous a light blue color, and the di and heptahydrate violet. All three are useful reagents which are commonly used as starting points for reactions involving cobalt.
+
{{distinguish|phosgene}}
 +
{{Chembox
 +
| Name = Cobalt(II) chloride
 +
| Reference =
 +
| IUPACName =
 +
| PIN =
 +
| SystematicName =
 +
| OtherNames = Cobalt dichloride<br>Cobaltous chloride<br>Muriate of cobalt
 +
<!-- Images -->
 +
| ImageFile = GoodCoClII.jpg
 +
| ImageSize = 300
 +
| ImageAlt =
 +
| ImageName =
 +
| ImageCaption = Anhydrous cobalt chloride.
 +
| ImageFile1 =
 +
| ImageSize1 =
 +
| ImageAlt1 =
 +
| ImageName1 =
 +
| ImageFile2 =
 +
| ImageSize2 =
 +
| ImageAlt2 =
 +
| ImageName2 =
 +
| ImageFile3 =
 +
| ImageSize3 =
 +
| ImageAlt3 =
 +
| ImageName3 =
 +
| ImageFileL1 =
 +
| ImageSizeL1 =
 +
| ImageAltL1 =
 +
| ImageNameL1 =
 +
| ImageFileR1 =
 +
| ImageSizeR1 =
 +
| ImageAltR1 =
 +
| ImageNameR1 =
 +
| ImageFileL2 =
 +
| ImageSizeL2 =
 +
| ImageAltL2 =
 +
| ImageNameL2 =
 +
| ImageFileR2 =
 +
| ImageSizeR2 =
 +
| ImageAltR2 =
 +
| ImageNameR2 =
 +
<!-- Sections -->
 +
| Section1 = {{Chembox Identifiers
 +
| 3DMet =
 +
| Abbreviations =
 +
| SMILES = Cl[Co]Cl
 +
  }}
 +
| Section2 = {{Chembox Properties
 +
| AtmosphericOHRateConstant =
 +
| Appearance = Blue crystals (anhydrous)<br>Violet-blue (dihydrate)<br>Rose-red crystals (hexahydrate)
 +
| BoilingPt =
 +
| BoilingPtC =
 +
| BoilingPt_ref =
 +
| BoilingPt_notes =
 +
| Density = 3.356 g/cm<sup>3</sup> (anhydrous)<br>2.477 g/cm<sup>3</sup> (dihydrate)<br>1.924 g/cm<sup>3</sup> (hexahydrate)
 +
| Formula = CoCl<sub>2</sub>
 +
| HenryConstant =
 +
| LogP =
 +
| MolarMass = 129.839 g/mol (anhydrous)<br>165.87 g/mol (dihydrate)<br>237.93 g/mol (hexahydrate)
 +
| MeltingPt =
 +
| MeltingPtC =
 +
| MeltingPt_ref =
 +
| MeltingPt_notes = ''anhydrous''<br>735 °C (1,355 °F; 1,008 K)<hr>''monohydrate''<br>140 °C (284 °F; 413 K)<hr>''dihydrate''<br>100 °C (212 °F; 373 K)<hr>''hexahydrate''<br>86 °C (187 °F; 359 K)
 +
| Odor = Odorless
 +
| pKa =
 +
| pKb =
 +
| Solubility = 43.6 g/100 ml (0 °C)<br>45 g/100 ml (7 °C)<br>52.9 g/100 ml (20 °C)<br>105 g/100 ml (96 °C)
 +
| SolubleOther = Soluble in [[ethanol]], [[glycerol]], [[pyridine]]
 +
| Solubility1 = 8.6 g/100 ml
 +
| Solvent1 = acetone
 +
| Solubility2 = 38.5 g/100 ml
 +
| Solvent2 = methanol
 +
| VaporPressure =
 +
  }}
 +
| Section3 = {{Chembox Structure
 +
| Coordination = Hexagonal (anhydrous)<br>Monoclinic (dihydrate)<br>Octahedral (hexahydrate)
 +
| CrystalStruct =
 +
| MolShape =
 +
  }}
 +
| Section4 = {{Chembox Thermochemistry
 +
| DeltaGf =
 +
| DeltaHc =
 +
| DeltaHf =
 +
| Entropy =
 +
| HeatCapacity =
 +
  }}
 +
| Section5 = {{Chembox Explosive
 +
| ShockSens =
 +
| FrictionSens =
 +
| DetonationV =
 +
| REFactor =
 +
  }}
 +
| Section6 = {{Chembox Hazards
 +
| AutoignitionPt = Non-flammable
 +
| ExploLimits =
 +
| ExternalMSDS = [https://www.docdroid.net/sqcM7iy/cobaltii-chloride-anhydrous-sa.pdf.html Sigma-Aldrich] (anhydrous)<br>[https://www.docdroid.net/xUSW2ht/cobaltii-chloride-hexahydrate-sa.pdf.html Sigma-Aldrich] (hexahydrate)
 +
| FlashPt = Non-flammable
 +
| LD50 = 766 mg/kg (rat)
 +
| LC50 =
 +
| MainHazards =
 +
| NFPA-F =
 +
| NFPA-H =
 +
| NFPA-R =
 +
| NFPA-S =
 +
  }}
 +
| Section7 = {{Chembox Related
 +
| OtherAnions =
 +
| OtherCations =
 +
| OtherFunction =
 +
| OtherFunction_label =
 +
| OtherCompounds =
 +
  }}
 +
}}
 +
'''Cobalt(II) chloride''' is a colorful compound with the formula '''CoCl<sub>2</sub>'''. Three hydrates of cobalt chloride exist, anhydrous, dihydrate, and hexahydrate. All three hydrates are hygroscopic, with the anhydrous a light blue color, and the di and heptahydrate violet. All three are useful reagents which are commonly used as starting points for reactions involving cobalt.
  
 
==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
 +
In the presence of [[ammonia]] or amines, cobalt(II) is readily oxidized by atmospheric oxygen to give a variety of cobalt(III) complexes, such as hexamminecobalt(III) chloride:
  
−
===Physical===
+
:4 CoCl<sub>2</sub>•6H<sub>2</sub>O + 4 NH<sub>4</sub>Cl + 20 NH<sub>3</sub> + O<sub>2</sub> → 4 [Co(NH<sub>3</sub>)<sub>6</sub>]Cl<sub>3</sub> + 26 H<sub>2</sub>O
−
Molecular formula: CoCl<sub>2</sub>
+
  
−
Melting point: 735 °C (anhydrous), 100 °C (dihydrate), 86 °C (hexahydrate)
+
CoCl<sub>2</sub> will react with [[sodium hypochlorite]], to form [[cobalt (III) oxide]].
  
−
Boiling point: 1049 °C
+
===Physical===
−
 
+
[[File:AnhydrousCoCl.jpg|thumb|right|Cobalt(II) chloride in solution.]]
−
Molar mass: 129.839 g/mol (anhydrous), 165.87 g/mol (dihydrate), 237.93 g/mol (hexahydrate)
+
Cobalt(II) chloride is a salt that is blue when anhydrous and pink-purple when hydrated. The compound melts at 735 °C (anhydrous), 100 °C (dihydrate), 86 °C (hexahydrate). It boils at 1049 °C. CoCl<sub>2</sub> is soluble in water (52.9 g/100 mL at 20 °C) methanol (38.5 g/100 mL), and slightly soluble in acetone, diethyl ether. The density for the three forms is 3.356 g/cm<sup>3</sup> (anhydrous), 2.477 g/cm<sup>3</sup> (dihydrate), 1.924 g/cm<sup>3</sup> (heptahydrate).
−
 
+
−
Density: 3.356 g/cm (anhydrous), 2.477 g/cm (dihydrate), 1.924 g/cm (heptahydrate)
+
−
 
+
−
Solubility in water: 52.9 g/100 mL (20 °C)
+
−
 
+
−
[[File:AnhydrousCoCl.jpg|thumb|left|Cobalt(II) chloride in solution.]]
+
  
 
==Preparation==
 
==Preparation==
−
Cobalt chloride heptahydrate can be synthesized by reacting two moles of hydrochloric acid with one mole of cobalt chloride. Add a small amount of acid and then stir the mixture before adding another small portion, as the CO2 created can cause the mixture to overflow. Usually there will be a layer of unreacted cobalt carbonate/other contaminants which must be filter out using either vacuum or gravity filtration if order to receive a pure product.
+
Cobalt chloride heptahydrate can be synthesized by reacting two moles of hydrochloric acid with one mole of cobalt carbonate. Add a small amount of acid and then stir the mixture before adding another small portion, as the CO2 created can cause the mixture to overflow. Usually, there will be a layer of unreacted cobalt carbonate/other contaminants that must be filtered out using either vacuum or gravity filtration in order to receive a pure product.
  
−
:CoCO<sub>3</sub> + 2 HCl → CoCl<sub>2</sub> + CO<sub>2</sub>+ H<sub>2</sub>O
+
: CoCO<sub>3</sub> + 2 HCl → CoCl<sub>2</sub> + CO<sub>2</sub>+ H<sub>2</sub>O
  
 
By heating this solution to dryness a light blue powder will be formed which is anhydrous cobalt chloride.
 
By heating this solution to dryness a light blue powder will be formed which is anhydrous cobalt chloride.
Line 29: Line 137:
  
 
==Availability==
 
==Availability==
−
[[File:GoodCoClII.jpg|thumb|left|308px|Anhydrous cobalt chloride.]]
+
Cobalt(II) chloride can be purchased from chemical suppliers, both as a solid and as a solution.
  
−
[[Cobalt carbonate]] can be purchased from pottery stores and 30% [[Hydrochloric acid]] can be bought at hardware stores.
+
It can also be found in some types of colored silica gel, though the amount is small.
 +
 
 +
Cobalt(II) chloride, along with other cobalt(II) compounds is classified as "Substance of very high concern" in the EU and its sale is regulated.
  
 
==Projects==
 
==Projects==
−
Cobalt chloride is the starting point of many interesting reactions such as [[Hexamminecobalt (III) chloride]] and [[Potassium cobaltinitrite]]. Combined with a solution of [[Sodium hypochlorite]], it precipitates [[Cobalt(III) Oxide]].
+
*Cobalt chloride can be used for the synthesis of many complexes, such as [[Hexamminecobalt (III) chloride]] and [[Potassium cobaltinitrite]].
 +
*Invisible ink
 +
*Electroplating cobalt metal
 +
*Water indicator, especially in desiccants
 +
*Make cobalt coordination complexes
  
 
==Handling==
 
==Handling==
 
===Safety===
 
===Safety===
−
Ld50(for rats): 80mg/kg'
+
Cobalt dichloride is a strong allergen, with a LD<sub>50</sub> of 80 mg/kg (rats).
  
 
Eye and hand protection should be worn while handling this compound.
 
Eye and hand protection should be worn while handling this compound.
  
 
===Storage===
 
===Storage===
−
Cobalt chloride should be stored in an air tight container to counter its strong hygroscopic nature.
+
Cobalt(II) chloride should be stored in an airtight container or bag to counter its strong hygroscopic nature.
  
 
===Disposal===
 
===Disposal===
−
 
+
Cobalt dichloride should be converted to an insoluble form before disposal.
  
 
==References==
 
==References==
 
<references />
 
<references />
 
*http://i.imgur.com/XjuOnB1.gif
 
*http://i.imgur.com/XjuOnB1.gif
 +
 
===Relevant Sciencemadness threads===
 
===Relevant Sciencemadness threads===
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=6064 Cobalt Chloride]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=6064 Cobalt Chloride]
 +
 +
[[Category:Chemical compounds]]
 
[[Category:Inorganic compounds]]
 
[[Category:Inorganic compounds]]
−
[[Category:Chemical compounds]]
+
[[Category:Cobalt compounds]]
 +
[[Category:Chlorides]]
 
[[Category:Easily prepared chemicals]]
 
[[Category:Easily prepared chemicals]]
−
[[Category:Chlorides]]
 
−
[[Category:Cobalt compounds]]
 

Latest revision as of 00:04, 9 August 2020

Not to be confused with phosgene.
Cobalt(II) chloride
GoodCoClII.jpg
Anhydrous cobalt chloride.
Names
Other names
Cobalt dichloride
Cobaltous chloride
Muriate of cobalt
Identifiers
Jmol-3D images Image
Properties
CoCl2
Molar mass 129.839 g/mol (anhydrous)
165.87 g/mol (dihydrate)
237.93 g/mol (hexahydrate)
Appearance Blue crystals (anhydrous)
Violet-blue (dihydrate)
Rose-red crystals (hexahydrate)
Odor Odorless
Density 3.356 g/cm3 (anhydrous)
2.477 g/cm3 (dihydrate)
1.924 g/cm3 (hexahydrate)
Melting point anhydrous
735 °C (1,355 °F; 1,008 K)
monohydrate
140 °C (284 °F; 413 K)
dihydrate
100 °C (212 °F; 373 K)
hexahydrate
86 °C (187 °F; 359 K)
43.6 g/100 ml (0 °C)
45 g/100 ml (7 °C)
52.9 g/100 ml (20 °C)
105 g/100 ml (96 °C)
Solubility Soluble in ethanol, glycerol, pyridine
Solubility in acetone 8.6 g/100 ml
Solubility in methanol 38.5 g/100 ml
Hazards
Safety data sheet Sigma-Aldrich (anhydrous)
Sigma-Aldrich (hexahydrate)
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
766 mg/kg (rat)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Cobalt(II) chloride is a colorful compound with the formula CoCl2. Three hydrates of cobalt chloride exist, anhydrous, dihydrate, and hexahydrate. All three hydrates are hygroscopic, with the anhydrous a light blue color, and the di and heptahydrate violet. All three are useful reagents which are commonly used as starting points for reactions involving cobalt.

Properties

Chemical

In the presence of ammonia or amines, cobalt(II) is readily oxidized by atmospheric oxygen to give a variety of cobalt(III) complexes, such as hexamminecobalt(III) chloride:

4 CoCl2•6H2O + 4 NH4Cl + 20 NH3 + O2 → 4 [Co(NH3)6]Cl3 + 26 H2O

CoCl2 will react with sodium hypochlorite, to form cobalt (III) oxide.

Physical

Cobalt(II) chloride in solution.

Cobalt(II) chloride is a salt that is blue when anhydrous and pink-purple when hydrated. The compound melts at 735 °C (anhydrous), 100 °C (dihydrate), 86 °C (hexahydrate). It boils at 1049 °C. CoCl2 is soluble in water (52.9 g/100 mL at 20 °C) methanol (38.5 g/100 mL), and slightly soluble in acetone, diethyl ether. The density for the three forms is 3.356 g/cm3 (anhydrous), 2.477 g/cm3 (dihydrate), 1.924 g/cm3 (heptahydrate).

Preparation

Cobalt chloride heptahydrate can be synthesized by reacting two moles of hydrochloric acid with one mole of cobalt carbonate. Add a small amount of acid and then stir the mixture before adding another small portion, as the CO2 created can cause the mixture to overflow. Usually, there will be a layer of unreacted cobalt carbonate/other contaminants that must be filtered out using either vacuum or gravity filtration in order to receive a pure product.

CoCO3 + 2 HCl → CoCl2 + CO2+ H2O

By heating this solution to dryness a light blue powder will be formed which is anhydrous cobalt chloride.

If heptahydrate crystals are desired the solution may be dried in a desiccator.

Availability

Cobalt(II) chloride can be purchased from chemical suppliers, both as a solid and as a solution.

It can also be found in some types of colored silica gel, though the amount is small.

Cobalt(II) chloride, along with other cobalt(II) compounds is classified as "Substance of very high concern" in the EU and its sale is regulated.

Projects

Handling

Safety

Cobalt dichloride is a strong allergen, with a LD50 of 80 mg/kg (rats).

Eye and hand protection should be worn while handling this compound.

Storage

Cobalt(II) chloride should be stored in an airtight container or bag to counter its strong hygroscopic nature.

Disposal

Cobalt dichloride should be converted to an insoluble form before disposal.

References

Relevant Sciencemadness threads

Retrieved from "https://www.sciencemadness.org/smwiki/index.php?title=Cobalt(II)_chloride&oldid=13172"