Rubidium perchlorate
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Names | |
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IUPAC name Rubidium perchlorate | |
Other names Perchloric acid rubidium salt, Rubidium chlorate(VII), Rubidii perchloras (lat.) | |
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ECHA InfoCard | 100.033.476 ![]() |
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InChI
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Properties | |
Chemical formula | RbClO4 |
Molar mass | 184.918 g/mol |
Appearance | Colorless crystals |
Density | 2.878 g/cm3 2.71 g/cm3 over 279 °C |
Melting point | 281 °C (538 °F; 554 K) |
Boiling point | 600 °C (1,112 °F; 873 K) (decomposes) |
Solubility in water | see chart |
Solubility product (Ksp) | 3×10−3[2] |
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GHS labelling: | |
Pictograms | ![]() ![]() |
Warning | |
Hazard statements | H272, H302, H315, H319, H332, H335 |
Precautionary statements | P210, P220, P221, P261, P264, P270, P271, P280, P301+P312, P302+P352, P304+P312, P304+P340, P305+P351+P338, P312, P321, P330, P332+P313, P337+P313, P362, P370+P378, P403+P233, P405, P501 |
NFPA 704 (fire diamond) | ![]() 2 0 0 OX |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). ![]() ![]() ![]() Infobox references |
Chemical compound
Rubidium perchlorate, RbClO4, is the perchlorate of rubidium. It is an oxidizing agent, as are all perchlorates.
Preparation and properties
Rubidium perchlorate can be obtained through the careful heating of a rubidium chlorate solution, leading to a disproportionation reaction with the release of oxygen gas:[3]
- 2 RbClO3 → RbClO4 + RbCl + O2
When heated, it decomposes into the chloride and oxygen:[4]
- RbClO4 → RbCl + 2 O2
It has two polymorphs. Below 279 °C, it crystallizes in orthorhombic crystal system with lattice constants a = 0.927 nm, b = 0.581 nm, c = 0.753 nm. Over 279 °C, it has a cubic structure with lattice constant a = 0.770 nm.[1]
Table of solubility in water:[1]
Temperature (°C) | 0 | 8.5 | 14 | 20 | 25 | 50 | 70 | 99 |
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Solubility (g / 100 ml) | 1.09 | 0.59 | 0.767 | 0.999 | 1.30 | 3.442 | 6.72 | 17.39 |
References
- ^ a b c F. Brezina, J. Mollin, R. Pastorek, Z. Sindelar. Chemicke tabulky anorganickych sloucenin (Chemical tables of inorganic compounds). SNTL, 1986.
- ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–189. ISBN 1138561630.
- ^ Abegg, R.; Auerbach, F. (1908). Handbuch der anorganischen Chemie. Vol. 2. S. Hirzel. p. 431.
- ^ d' Ans, Jean; Lax, Ellen (1997). Taschenbuch für Chemiker und Physiker. 3. Elemente, anorganische Verbindungen und Materialien, Minerale. Vol. 3 (4th ed.). Berlin: Springer. p. 686. ISBN 3-540-60035-3. OCLC 312750698.
External links
- MSDS at Science Lab