| Names | |
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Other names
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.033.583 |
| EC Number |
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| PdSO4 | |
| Molar mass | 202.48 g/mol |
| Appearance | Red-brown solid (anhydrous) |
| Density | 4.2 g/cm3[1] |
| Melting point | 525 °C (977 °F; 798 K)[1] (decomposition) |
| Hydrolysis[2] | |
| Solubility | Soluble in conc. sulfuric acid[2] |
| Structure[1] | |
| Monoclinic | |
| C2/c | |
a = 7.84 Å, b = 5.18 Å, c = 7.91 Å α = 90°, β = 95.6°, γ = 90°
| |
| Thermochemistry | |
Std molar
entropy (S⦵298) |
97.5 J/(mol·K) |
Std enthalpy of
formation (ΔfH⦵298) |
-672.4 kJ/mol |
| Hazards | |
| GHS labelling: | |
 
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| Danger | |
| H302, H314 | |
| P260, P264, P270, P280, P301+P317, P301+P330+P331, P302+P361+P354, P304+P340, P305+P354+P338, P316, P321, P330, P363, P405, P501 | |
| Related compounds | |
Other cations
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Nickel(II) sulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Palladium(II) sulfate is an inorganic chemical compound with the formula PdSO4. It is a hygroscopic red-brown solid that forms the dihydrate, PdSO4·2H2O.[1]
Preparation and properties[edit]
Palladium(II) sulfate is produced by the reaction of palladium metal with a mixture of nitric acid and sulfuric acid. It can also be produced by the reaction of palladium(II) sulfide and oxygen in dimethylformamide.[1][3][4][5]
When anhydrous palladium(II) sulfate absorbs moisture from the air, it forms a greenish-brown dihydrate. The anhydrous form can be regenerated by the heating of the dihydrate at 202 °C.[1][4]
Anhydrous palladium(II) sulfate decomposes to palladium(II) oxide at 525 °C releasing sulfur trioxide:[1]
- PdSO4 → PdO + SO3
References[edit]
- ^ a b c d e f g Thomas Dahmen; Pia Rittner; Silke Böger-Seidl; Reginald Gruehn (1994). "Beiträge zum thermischen Verhalten von Sulfaten XIV. Zum thermischen Verhalten von PdSO4 · 2H2O und PdSO4 · 0.75H2O sowie zur Struktur von M-PdSO4" [Contributions to the thermal behavior of sulfates XIV. On the thermal behavior of PdSO4 · 2H2O and PdSO4 · 0.75H2O as well as the structure of M-PdSO4]. Journal of Alloys and Compounds (in German). 216 (1): 11–19. doi:10.1016/0925-8388(94)91034-0.
- ^ a b Georg Brauer: Handbuch der präparativen anorganischen Chemie. 3., umgearb. Auflage. Band III. Enke, Stuttgart 1981, ISBN 3-432-87823-0, p. 1731
- ^ Turki Alkathiri; Kai Xu; Bao Yue Zhang; Muhammad Waqas Khan; Azmira Jannat; Nitu Syed; Ahmed F. M. Almutairi; Nam Ha; Manal M. Y. A. Alsaif; Naresha Pillai; Zhong Li; Torben Daeneke; Jian Zhen Ou (2022). "2D Palladium Sulphate for Visible-Light-Driven Optoelectronic Reversible Gas Sensing at Room Temperature". Small Science. 2 (3). doi:10.1002/smsc.202100097.
- ^ a b R. Eskenazi; J. Raskovan; R. Levitus (1966). "Sulphato complexes of palladium (II)". Journal of Inorganic and Nuclear Chemistry. 28 (2): 521–526. doi:10.1016/0022-1902(66)80333-0.
- ^ W. Manchot; A. Waldmüller (1926). "Zur Kenntnis der Metall-Nitroso-Verbindungen: Über Stickoxyd-Verbindungen des Palladiums" [For knowledge of metal-nitroso compounds: About nitrogen oxide compounds of palladium]. Berichte der Deutschen Chemischen Gesellschaft (in German). 59 (9): 2363–2366. doi:10.1002/cber.19260590931.