Difference between revisions of "Calcium chloride"

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'''Calcium chloride''' is a salt of [[calcium]] and [[chlorine]]. It's mainly used in amateur chemistry as a [[desiccant]], because it is extremely hygroscopic and doesn't decompose when heated to dryness.
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{{Chembox
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| Name = Calcium chloride
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| Reference =
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| IUPACName = Calcium chloride
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| PIN =
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| SystematicName =
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| OtherNames = Calcium(II) chloride<br>Calcium dichloride<br>E509
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| ImageFile = Calcium_chloride_anhydrous.jpg
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| ImageCaption = Anhydrous calcium chloride
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| Section1 = {{Chembox Identifiers
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| 3DMet =
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| Abbreviations =
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| SMILES =
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  }}
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| Section2 = {{Chembox Properties
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| AtmosphericOHRateConstant =
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| Appearance = White hygroscopic solid
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| BoilingPt =
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| BoilingPtC = 1935
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| BoilingPt_ref =
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| BoilingPt_notes =
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| Density = 2.15 g/cm<sup>3</sup> (anhydrous)<br> 2.24 g/cm<sup>3</sup> (monohydrate)<br> 1.85 g/cm<sup>3</sup> (dihydrate)<br> 1.83 g/cm<sup>3</sup> (tetrahydrate)<br> 1.71 g/cm<sup>3</sup> (hexahydrate)
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| Formula = CaCl<sub>2</sub>
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| HenryConstant =
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| LogP =
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| MolarMass =
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| MeltingPt =
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| MeltingPtC = 775
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| MeltingPt_ref =
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| MeltingPt_notes = (anhydrous)
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| Odor = Odorless
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| pKa = 8–9 (anhydrous)<br>6.5–8.0 (hexahydrate)
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| pKb =
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| Solubility = ''Anhydrous''<br>74.5 g/100 ml (20 °C)<br>''Hexahydrate''<br>49.4 g/100 ml (−25 °C)<br>59.5 g/100 mL (0 °C)<br>65 g/100 ml (10 °C)<br>81.1 g/100 ml (25 °C)<br>102.2 g/100 ml (30.2 °C)<br>''α-Tetrahydrate''<br>90.8 g/100 ml (20 °C)<br>114.4 g/100 ml (40 °C)<br>'Dihydrate''<br>134.5 g/100 ml (60 °C)<br>152.4 g/100 ml (100 °C)
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| SolubleOther = Soluble in glacial [[acetic acid]], [[alcohol]]s<br>Insoluble in liq. [[ammonia]], [[dimethyl sulfoxide|DMSO]], [[ethyl acetate]]
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| Solubility1 = 18.3 g/100 g (0 °C)<br> 25.8 g/100 g (20 °C)<br> 35.3 g/100 g (40 °C)<br> 56.2 g/100 g (70 °C)
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| Solvent1 = ethanol
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| Solubility2 = 21.8 g/100 g (0 °C)<br> 29.2 g/100 g (20 °C)<br> 38.5 g/100 g (40 °C)
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| Solvent2 = methanol
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| Solubility3 = 0.01 g/100 g (20 °C)
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| Solvent3 = acetone
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| Solubility4 = 1.66 g/100 g
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| Solvent4 = pyridine
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| VaporPressure =
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  }}
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| Section3 = {{Chembox Structure
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| Coordination = [[Octahedral]] (Ca<sup>2+</sup>, anhydrous)
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| CrystalStruct = Orthorhombic (rutile, anhydrous), oP6<br>Tetragonal (anhydrous, > 217 °C), oP6<br>Trigonal (hexahydrate)
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| MolShape =
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  }}
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| Section4 = {{Chembox Thermochemistry
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| DeltaGf = −748.81 kJ/mol
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| DeltaHc =
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| DeltaHf = −795.42 kJ/mol (anhydrous)<br>−1110.98 kJ/mol (monohydrate)<br>−1403.98 kJ/mol (dihydrate)<br>−2009.99 kJ/mol (tetrahydrate)<br>−2608.01 kJ/mol (hexahydrate)
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| Entropy = 108.4 J·mol<sup>-1</sup>·K<sup>-1</sup>
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| HeatCapacity = 72.89 J·mol<sup>-1</sup>·K<sup>-1</sup> (anhydrous)<br>106.23  J·mol<sup>-1</sup>·K<sup>-1</sup> (monohydrate)<br>172.92 J·mol<sup>-1</sup>·K<sup>-1</sup> (dihydrate)<br> 251.17 J·mol<sup>-1</sup>·K<sup>-1</sup> (tetrahydrate)<br>300.7 J·mol<sup>-1</sup>·K<sup>-1</sup> (hexahydrate)
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  }}
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| Section5 = {{Chembox Explosive
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| ShockSens =
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| FrictionSens =
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| DetonationV =
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| REFactor =
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  }}
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| Section6 = {{Chembox Hazards
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| AutoignitionPt = Non-flammable
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| ExploLimits = Non-flammable
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| ExternalMSDS = [https://www.docdroid.net/LsGPrKt/calcium-chloride-anhydrous-sa.pdf.html Sigma-Aldrich]
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| FlashPt = Non-flammable
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| LD50 = 1,000 mg/kg (rats, oral)
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| LC50 =
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| MainHazards = Irritant
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| NFPA-F =
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| NFPA-H =
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| NFPA-R =
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| NFPA-S =
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| Section7 = {{Chembox Related
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| OtherAnions =
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| OtherCations =
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| OtherFunction =
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| OtherFunction_label =
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| OtherCompounds = [[Magnesium chloride]]<br>[[Strontium chloride]]<br>[[Barium chloride]]
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  }}
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}}
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'''Calcium chloride''' ('''CaCl<sub>2</sub>''') is a salt of [[calcium]] and [[chlorine]]. It's mainly used in amateur chemistry as a [[desiccant]], because it is extremely hygroscopic and doesn't (significantly) decompose when heated to dryness.
  
 
==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
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Calcium chloride serves as a source of calcium ions for reactions. Because [[calcium carbonate]] and sulfate are more or less insoluble, calcium chloride can be used to produce any metal chloride by introduction of a soluble sulfate or carbonate to its solutions.
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Calcium chloride serves as a source of calcium ions for reactions. Because [[calcium carbonate]] and [[calcium sulfate|sulfate]] are more or less insoluble, calcium chloride can be used to produce any metal chloride by introduction of a soluble sulfate or carbonate to its solutions.
  
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Molten calcium chloride can be electrolyzed to yield calcium metal and chlorine gas:
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: CaCl<sub>2</sub> + MSO<sub>4</sub> → MCl + CaSO<sub>4</sub>
  
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:CaCl<sub>2(l)</sub> → Ca<sub>(s)</sub> + Cl<sub>2(g)</sub>
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Molten calcium chloride can be electrolyzed to yield [[calcium]] metal and [[chlorine]] gas:
 +
 
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: CaCl<sub>2(l)</sub> → Ca<sub>(s)</sub> + Cl<sub>2(g)</sub>
  
 
===Physical===
 
===Physical===
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==Preparation==
 
==Preparation==
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Calcium chloride can be obtained by the reaction of [[calcium hydroxide]] or [[calcium carbonate]] and [[hydrochloric acid]]. If these compounds are hard to come by, clean white limestone, seashells, or well-cleaned egg shells can be dissolved in hydrochloric acid, and the solute filtered. Calcium carbonate is then reprecipitated by addition of [[sodium carbonate]] or [[sodium bicarbonate]], and finally dissolved in hydrochloric acid and filtered again. It is highly recommended that it is prepared strictly from a pure calcium salt though, as this process is time-consuming, costly, and fails to remove magnesium or iron impurities.
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Calcium chloride can be obtained by the reaction of [[calcium hydroxide]] or [[calcium carbonate]] and [[hydrochloric acid]].
 +
 
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: Ca(OH)<sub>2</sub> + 2 HCl → CaCl<sub>2</sub> + 2 H<sub>2</sub>O
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 +
: CaCO<sub>3</sub> + 2 HCl → CaCl<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub>
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 +
If these compounds are hard to come by, clean white limestone, seashells, or well-cleaned egg shells can be dissolved in hydrochloric acid, and the solute filtered. Calcium carbonate is then reprecipitated by addition of [[sodium carbonate]] or [[sodium bicarbonate]], and finally dissolved in hydrochloric acid and filtered again. It is highly recommended that it is prepared strictly from a pure calcium salt though, as this process is time-consuming, costly, and fails to remove magnesium or iron impurities.
  
 
==Projects==
 
==Projects==
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* Electrolysis of molten, anhydrous calcium chloride to produce [[calcium|calcium metal]].
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* Dry solvents
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* Make ammonium chloride
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* Building a homemade [[desiccator]]
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* Building a homemade [[dessicator]]
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* Make a dry box
 
* Make a dry box
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* Remove alcohols from esters (from the reaction product of esterifications)
 +
* Electrolysis of molten, anhydrous calcium chloride to produce [[calcium]] metal
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* Make [[ammonium chloride]]
  
 
==Handling==
 
==Handling==
 
===Safety===
 
===Safety===
 
Anhydrous calcium chloride can be an irritant due to its strong desiccating properties. Otherwise, it is only minimally toxic.
 
Anhydrous calcium chloride can be an irritant due to its strong desiccating properties. Otherwise, it is only minimally toxic.
 +
 +
If large amounts of it are ingested, it may lead to vomiting, as large amounts of saline solution are irritating to the digestive track.
  
 
===Storage===
 
===Storage===
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===Disposal===
 
===Disposal===
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No special disposal is required. Calcium chloride is non-toxic to the environment, and it's even used as anti-icing during the winter.
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No special disposal is required. Calcium chloride is non-toxic to the environment, and it's even used as anti-icing during the winter. Avoid dumping large amounts of it into fields, as most plants tend to be chloride-sensitive.
  
 
==References==
 
==References==
 
<references/>
 
<references/>
 
===Relevant Sciencemadness threads===
 
===Relevant Sciencemadness threads===
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=155091 Calcium chloride recrystallization]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=34110 Making Calcium Chloride,and anhydrous]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=59880 OTC Calcium Chloride - Good for Drying]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=61108 Drying calcium chloride]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=155804 Drying CaCl2?]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=61416 Gah, I ruined my calcium chloride, how did it happen?]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=16145 calcium chloride from calcium carbonate (using a chloride salt)]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=63030 Why not use calcium chloride to supply calcium for nutrients?]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=157046 CaCl2 trap on vacuum pump?]
  
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[[Category:Chemical compounds]]
 +
[[Category:Inorganic compounds]]
 
[[Category:Calcium compounds]]
 
[[Category:Calcium compounds]]
 
[[Category:Chlorides]]
 
[[Category:Chlorides]]
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[[Category:Neutral salts]]
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[[Category:Desiccants]]
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[[Category:Readily available chemicals]]
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[[Category:Halides]]
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[[Category:Irritants]]

Latest revision as of 21:01, 22 March 2021

Calcium chloride
Calcium chloride anhydrous.jpg
Anhydrous calcium chloride
Names
IUPAC name
Calcium chloride
Other names
Calcium(II) chloride
Calcium dichloride
E509
Properties
CaCl2
Appearance White hygroscopic solid
Odor Odorless
Density 2.15 g/cm3 (anhydrous)
2.24 g/cm3 (monohydrate)
1.85 g/cm3 (dihydrate)
1.83 g/cm3 (tetrahydrate)
1.71 g/cm3 (hexahydrate)
Melting point 775 °C (1,427 °F; 1,048 K) (anhydrous)
Boiling point 1,935 °C (3,515 °F; 2,208 K)
Anhydrous
74.5 g/100 ml (20 °C)
Hexahydrate
49.4 g/100 ml (−25 °C)
59.5 g/100 mL (0 °C)
65 g/100 ml (10 °C)
81.1 g/100 ml (25 °C)
102.2 g/100 ml (30.2 °C)
α-Tetrahydrate
90.8 g/100 ml (20 °C)
114.4 g/100 ml (40 °C)
'Dihydrate
134.5 g/100 ml (60 °C)
152.4 g/100 ml (100 °C)
Solubility Soluble in glacial acetic acid, alcohols
Insoluble in liq. ammonia, DMSO, ethyl acetate
Solubility in ethanol 18.3 g/100 g (0 °C)
25.8 g/100 g (20 °C)
35.3 g/100 g (40 °C)
56.2 g/100 g (70 °C)
Solubility in methanol 21.8 g/100 g (0 °C)
29.2 g/100 g (20 °C)
38.5 g/100 g (40 °C)
Solubility in acetone 0.01 g/100 g (20 °C)
Solubility in pyridine 1.66 g/100 g
Acidity (pKa) 8–9 (anhydrous)
6.5–8.0 (hexahydrate)
Thermochemistry
108.4 J·mol-1·K-1
−795.42 kJ/mol (anhydrous)
−1110.98 kJ/mol (monohydrate)
−1403.98 kJ/mol (dihydrate)
−2009.99 kJ/mol (tetrahydrate)
−2608.01 kJ/mol (hexahydrate)
Hazards
Safety data sheet Sigma-Aldrich
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1,000 mg/kg (rats, oral)
Related compounds
Related compounds
 Magnesium chloride
Strontium chloride
Barium chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Calcium chloride (CaCl2) is a salt of calcium and chlorine. It's mainly used in amateur chemistry as a desiccant, because it is extremely hygroscopic and doesn't (significantly) decompose when heated to dryness.

Properties

Chemical

Calcium chloride serves as a source of calcium ions for reactions. Because calcium carbonate and sulfate are more or less insoluble, calcium chloride can be used to produce any metal chloride by introduction of a soluble sulfate or carbonate to its solutions.

CaCl2 + MSO4 → MCl + CaSO4

Molten calcium chloride can be electrolyzed to yield calcium metal and chlorine gas:

CaCl2(l) → Ca(s) + Cl2(g)

Physical

Calcium chloride is white, solid at room temperature. The anhydrous salt is very hygroscopic, it will quickly absorb water from the air to form a solution, a property known as deliquescence. Anhydrous calcium chloride must be stored in a very dry environment.

Availability

Calcium chloride can be cheaply purchased at hardware stores, stored in desiccator bags, that contain the anhydrous form. Some road salts are another source, and can be obtained in large quantities, though these products may also contain other chlorides or impurities. The anhydrous form can be produced by strongly heating the hydrate. Often, the dried calcium chloride will harden into a solid mass, that takes time to break, during which it will rapidly absorb water from air as it cools.

Preparation

Calcium chloride can be obtained by the reaction of calcium hydroxide or calcium carbonate and hydrochloric acid.

Ca(OH)2 + 2 HCl → CaCl2 + 2 H2O
CaCO3 + 2 HCl → CaCl2 + H2O + CO2

If these compounds are hard to come by, clean white limestone, seashells, or well-cleaned egg shells can be dissolved in hydrochloric acid, and the solute filtered. Calcium carbonate is then reprecipitated by addition of sodium carbonate or sodium bicarbonate, and finally dissolved in hydrochloric acid and filtered again. It is highly recommended that it is prepared strictly from a pure calcium salt though, as this process is time-consuming, costly, and fails to remove magnesium or iron impurities.

Projects

  • Dry solvents
  • Building a homemade desiccator
  • Make a dry box
  • Remove alcohols from esters (from the reaction product of esterifications)
  • Electrolysis of molten, anhydrous calcium chloride to produce calcium metal
  • Make ammonium chloride

Handling

Safety

Anhydrous calcium chloride can be an irritant due to its strong desiccating properties. Otherwise, it is only minimally toxic.

If large amounts of it are ingested, it may lead to vomiting, as large amounts of saline solution are irritating to the digestive track.

Storage

Calcium chloride should be stored in sealed containers or bags, as it is extremely hygroscopic. Zipper bags are also good to store anhydrous CaCl2.

Disposal

No special disposal is required. Calcium chloride is non-toxic to the environment, and it's even used as anti-icing during the winter. Avoid dumping large amounts of it into fields, as most plants tend to be chloride-sensitive.

References

Relevant Sciencemadness threads

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