Difference between revisions of "Barium perchlorate"

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| 3DMet =  
 
| 3DMet =  
 
| Abbreviations =  
 
| Abbreviations =  
−
| SMILES =  
+
| SMILES = [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Ba+2]
 
   }}
 
   }}
 
| Section2 = {{Chembox Properties
 
| Section2 = {{Chembox Properties
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| BoilingPtC =  
 
| BoilingPtC =  
 
| BoilingPt_ref =  
 
| BoilingPt_ref =  
−
| BoilingPt_notes =  
+
| BoilingPt_notes = Decomposes
−
| Density = 3.2 g/cm<sup>3</sup>
+
| Density = 3.2 g/cm<sup>3</sup> (20 °C)
−
| Formula = Ba(ClO<sub>4</sub>)<sub>2</sub>
+
| Formula = BaCl<sub>2</sub>O<sub>8</sub><br>Ba(ClO<sub>4</sub>)<sub>2</sub>
 
| HenryConstant =  
 
| HenryConstant =  
 
| LogP =  
 
| LogP =  
 
| MolarMass = 336.228 g/mol
 
| MolarMass = 336.228 g/mol
 
| MeltingPt =  
 
| MeltingPt =  
−
| MeltingPtC = 505
+
| MeltingPtC = 470-505
 
| MeltingPt_ref =  
 
| MeltingPt_ref =  
 
| MeltingPt_notes =  
 
| MeltingPt_notes =  
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| pKa =  
 
| pKa =  
 
| pKb =  
 
| pKb =  
−
| Solubility = 66.48 g/100 ml (25 °C)
+
| Solubility = 198 g/100 ml (25 °C)<ref name="nekrasov">Nekrasov B.V. Fundamentals of General Chemistry. - T.1. - M.: Chemistry, 1973 (Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973)</ref>
−
| SolubleOther =  
+
| SolubleOther = Soluble in [[acetone]], [[ethanol]]<br>Insoluble in [[diethyl ether]]
−
| Solvent =  
+
| Solubility1 = 125 g/100 ml (25 °C)<ref name="nekrasov" />
 +
| Solvent1 = acetone
 +
| Solubility2 = 67.2 g/100 ml<ref>Handbook of experimental data on the solubility of salt systems. - T. 4. - L .: GNTIHL, 1963 pp. 2694 (Справочник экспериментальных данных по растворимости солевых систем. - Т. 4. - Л.: ГНТИХЛ, 1963 pp. 2694)</ref>
 +
| Solvent2 = ammonia
 +
| Solubility3 = 58.2 g/100 ml (20 °C)<ref name="seidell">Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940</ref>
 +
| Solvent3 = butanol
 +
| Solubility4 = 125 g/100 ml (25 °C)<ref name="nekrasov" />
 +
| Solvent4 = ethanol
 +
| Solubility5 = 56.2 g/100 ml (20 °C)<ref name="seidell" />
 +
| Solvent5 = isobutanol
 +
| Solubility6 = 217 g/100 ml (20 °C)<ref name="seidell" />
 +
| Solvent6 = methanol
 +
| Solubility7 = 75.7 g/100 ml (20 °C)<ref name="seidell" />
 +
| Solvent7 = propanol
 
| VaporPressure = ~0 mmHg
 
| VaporPressure = ~0 mmHg
 
   }}
 
   }}
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| DeltaGf =  
 
| DeltaGf =  
 
| DeltaHc =  
 
| DeltaHc =  
−
| DeltaHf =  
+
| DeltaHf = -774 kJ/mol
−
| Entropy =  
+
| Entropy = 251 J·mol<sup>-1</sup>·K<sup>-1</sup>
 
| HeatCapacity =  
 
| HeatCapacity =  
 
   }}
 
   }}
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===Chemical===
 
===Chemical===
 
Barium perchlorate decomposes when heated to high temperatures to liberate oxygen.
 
Barium perchlorate decomposes when heated to high temperatures to liberate oxygen.
 +
 +
Addition of conc. sulfuric acid will produce anhydrous [[perchloric acid]]. The resulting [[barium sulfate]] is insoluble in solvents, thus the perchloric acid can be purified by simply filtering the product.
 +
 +
: H<sub>2</sub>SO<sub>4</sub> + Ba(ClO<sub>4</sub>)<sub>2</sub> → 2 HClO<sub>4</sub> + BaSO<sub>4</sub> ↓
  
 
===Physical===
 
===Physical===
Line 123: Line 140:
  
 
==Preparation==
 
==Preparation==
−
Can be prepared by reacting [[perchloric acid]] with barium oxide, hydroxide or carbonate. The resulting barium perchlorate solution is then concentrated and cooled to recrystallize the salt.
+
Can be prepared by reacting [[perchloric acid]] with [[barium oxide]], hydroxide or [[barium carbonate|carbonate]]. The resulting barium perchlorate solution is then concentrated and cooled to recrystallize the salt.
 +
 
 +
: 2 HClO<sub>4</sub> + BaO → Ba(ClO<sub>4</sub>)<sub>2</sub> + H<sub>2</sub>O
 +
: 2 HClO<sub>4</sub> + Ba(OH)<sub>2</sub> → Ba(ClO<sub>4</sub>)<sub>2</sub> + 2 H<sub>2</sub>O
 +
: 2 HClO<sub>4</sub> + BaCO<sub>3</sub> → Ba(ClO<sub>4</sub>)<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub>
  
 
Another route involves the reaction between [[barium chloride]] and [[silver perchlorate]].
 
Another route involves the reaction between [[barium chloride]] and [[silver perchlorate]].
 +
 +
: BaCl<sub>2</sub> + 2 AgClO<sub>4</sub> → Ba(ClO<sub>4</sub>)<sub>2</sub> + 2 AgCl ↓
  
 
==Projects==
 
==Projects==
 
*Make flash powder
 
*Make flash powder
 
*Make concentrated perchloric acid
 
*Make concentrated perchloric acid
 +
*Make transition metal perchlorates
  
 
==Handling==
 
==Handling==
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===Disposal===
 
===Disposal===
−
Barium perchlorate, like other perchlorates can be reduced with elemental [[iron]] in the absence of air under UV light to [[barium chloride]], which in term can be precipitated to [[barium sulfate]], which has low toxicity and can be safely disposed of.
+
Barium perchlorate, like other perchlorates, can be reduced with elemental [[iron]] in the absence of air under UV light to [[barium chloride]], which in term can be precipitated to [[barium sulfate]], which has low toxicity and can be safely disposed of.
  
 
==References==
 
==References==

Latest revision as of 19:36, 9 September 2023

Barium perchlorate
Names
IUPAC name
Barium perchlorate
Other names
Barium diperchlorate
Perchloric acid, barium salt
Identifiers
Jmol-3D images Image
Properties
BaCl2O8
Ba(ClO4)2
Molar mass 336.228 g/mol
Appearance White solid
Odor Odorless
Density 3.2 g/cm3 (20 °C)
Melting point 470–505 °C (878–941 °F; 743–778 K)
Boiling point Decomposes
198 g/100 ml (25 °C)[1]
Solubility Soluble in acetone, ethanol
Insoluble in diethyl ether
Solubility in acetone 125 g/100 ml (25 °C)[1]
Solubility in ammonia 67.2 g/100 ml[2]
Solubility in butanol 58.2 g/100 ml (20 °C)[3]
Solubility in ethanol 125 g/100 ml (25 °C)[1]
Solubility in isobutanol 56.2 g/100 ml (20 °C)[3]
Vapor pressure ~0 mmHg
Thermochemistry
251 J·mol-1·K-1
-774 kJ/mol
Hazards
Safety data sheet Sigma-Aldrich
Related compounds
Related compounds
 Barium chloride
Barium chlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Barium perchlorate (Ba(ClO4)2) is a powerful oxidizing agent, mainly used in pyrotechnics.

Properties

Chemical

Barium perchlorate decomposes when heated to high temperatures to liberate oxygen.

Addition of conc. sulfuric acid will produce anhydrous perchloric acid. The resulting barium sulfate is insoluble in solvents, thus the perchloric acid can be purified by simply filtering the product.

H2SO4 + Ba(ClO4)2 → 2 HClO4 + BaSO4 ↓

Physical

Barium perchlorate is a white solid, soluble in water.

Availability

Some fireworks may contain barium perchlorate.

Barium perchlorate can be bought from chemical suppliers.

Preparation

Can be prepared by reacting perchloric acid with barium oxide, hydroxide or carbonate. The resulting barium perchlorate solution is then concentrated and cooled to recrystallize the salt.

2 HClO4 + BaO → Ba(ClO4)2 + H2O
2 HClO4 + Ba(OH)2 → Ba(ClO4)2 + 2 H2O
2 HClO4 + BaCO3 → Ba(ClO4)2 + H2O + CO2

Another route involves the reaction between barium chloride and silver perchlorate.

BaCl2 + 2 AgClO4 → Ba(ClO4)2 + 2 AgCl ↓

Projects

  • Make flash powder
  • Make concentrated perchloric acid
  • Make transition metal perchlorates

Handling

Safety

Barium perchlorate is a strong oxidizer and also toxic if ingested.

Storage

In closed bottles, away from combustible materials.

Disposal

Barium perchlorate, like other perchlorates, can be reduced with elemental iron in the absence of air under UV light to barium chloride, which in term can be precipitated to barium sulfate, which has low toxicity and can be safely disposed of.

References

  1. ↑ 1.0 1.1 1.2 Nekrasov B.V. Fundamentals of General Chemistry. - T.1. - M.: Chemistry, 1973 (Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973)
  2. ↑ Handbook of experimental data on the solubility of salt systems. - T. 4. - L .: GNTIHL, 1963 pp. 2694 (Справочник экспериментальных данных по растворимости солевых систем. - Т. 4. - Л.: ГНТИХЛ, 1963 pp. 2694)
  3. ↑ 3.0 3.1 3.2 3.3 Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940

Relevant Sciencemadness threads

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