Hydronium perchlorate
| |||
Names | |||
---|---|---|---|
Other names
| |||
Identifiers | |||
CAS Number |
| ||
3D model (JSmol) |
| ||
ChemSpider |
| ||
PubChem CID |
| ||
InChI
| |||
| |||
Properties | |||
Chemical formula | [H3O]ClO4 | ||
Molar mass | 118.47 g·mol−1 | ||
Appearance | Colorless solid | ||
Density | 1.96 g/cm3 | ||
Melting point | 45 °C (113 °F; 318 K) | ||
Structure[1] | |||
Crystal structure | Orthorhombic | ||
Space group | Pnma | ||
a = 9.2343 Å, b = 5.8178 Å, c = 7.4606 Å | |||
Related compounds | |||
Other anions | Hydronium chloride | ||
Other cations | Perchloric acid | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references |
Hydronium perchlorate is an inorganic chemical compound with the chemical formula [H3O]ClO4. It is an unusual salt due to it being a solid and stable hydronium salt. It consists of hydronium cations [H3O]+ and perchlorate anions ClO−4.
Production
Hydronium perchlorate is produced by the reaction of anhydrous perchloric acid and water in a 1:1 molar ratio:[2]
- HClO4 + H2O → [H3O]+ClO−4
A more analytically reliable method was reported using the macrocyclic Schiff base of sodium 2,6-diformyl-4-methylphenolate and 2,6-diformyl-4-methylphenol as a chelating agent to sequester Cu(II): transmetallation of the macrocycle with copper(II) perchlorate yielded colorless crystals of hydronium perchlorate.[1]
It can also be produced by the reaction of anhydrous nitric acid and perchloric acid.[3][clarification needed]
References
- ^ a b Azhar A Rahman; Anwar Usman; Suchada Chantrapromma; Hoong-Kun Fun (2003). "Redetermination of hydronium perchlorate at 193 and 293 K". Acta Crystallographica C. 59 (Pt 9): i92-4. Bibcode:2003AcCrC..59I..92R. doi:10.1107/s0108270103010461. PMID 12944636.
- ^ C. E. Nordman (1962). "The crystal structure of hydronium perchlorate at -80°C". Acta Crystallographica. 15 (1): 18–23. Bibcode:1962AcCry..15...18N. doi:10.1107/S0365110X62000055.
- ^ Kenneth Schofield (1980). "3". Aromatic nitration. Cambridge University Press. p. 30. ISBN 9780521233620.
- v
- t
- e
- Ag4O4
- Al2O3
- AmO2
- Am2O3
- As2O3
- As2O5
- Au2O3
- B2O3
- BaO
- BeO
- Bi2O3
- BiO2
- Bi2O5
- BrO2
- Br2O3
- Br2O5
- Br
3O
8 - CO
- CO2
- C3O2
- CaO
- CaO2
- CdO
- CeO2
- Ce3O4
- Ce2O3
- ClO2
- Cl2O
- Cl2O2
- Cl2O3
- Cl2O4
- Cl2O6
- Cl2O7
- CoO
- Co2O3
- Co3O4
- CrO3
- Cr2O3
- Cr2O5
- Cr5O12
- CsO2
- Cs2O3
- CuO
- Dy2O3
- Er2O3
- Eu2O3
- FeO
- Fe2O3
- Fe3O4
- Ga2O
- Ga2O3
- GeO
- GeO2
- H2O
- 2H2O
- 3H2O
- H218O
- H2O2
- HfO2
- HgO
- Hg2O
- Ho2O3
- IO
- I2O4
- I2O5
- I2O6
- I4O9
- In2O3
- IrO2
- KO2
- K2O2
- La2O3
- Li2O
- Li2O2
- Lu2O3
- MgO
- Mg2O3
- MnO
- MnO2
- Mn2O3
- Mn2O7
- MoO2
- MoO3
- Mo2O3
- NO
- NO2
- N2O
- N2O3
- N2O4
- N2O5
- NaO2
- Na2O
- Na2O2
- NbO
- NbO2
- Nd2O3
- O2F
- OF
- OF2
- O2F2
- O3F2
- O4F2
- O5F2
- O6F2
- O2PtF6
- more...