Chemistry:Palladium(II) sulfate
From HandWiki
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3D model (JSmol)
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| Properties | |
| PdSO4 | |
| Molar mass | 202.48 g/mo |
| 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°
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| Thermochemistry | |
Std molar
entropy (S |
97.5 J/(mol·K) |
Std enthalpy of
formation (ΔfH⦵298) |
-672.4 kJ/mol |
| Hazards | |
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| GHS Signal word | Danger |
| H302, H314 | |
| P260, P264, P270, P280, P301+317Script error: No such module "Preview warning".Category:GHS errors, P301+330+331, P302+361+354Script error: No such module "Preview warning".Category:GHS errors, P304+340, P305+354+338Script error: No such module "Preview warning".Category:GHS errors, P316Script error: No such module "Preview warning".Category:GHS errors, 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). | |
| Infobox references | |
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
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
- ↑ 1.0 1.1 1.2 1.3 1.4 1.5 1.6 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" (in de). Journal of Alloys and Compounds 216 (1): 11–19. doi:10.1016/0925-8388(94)91034-0.
- ↑ 2.0 2.1 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 et al. (2022). "2D Palladium Sulphate for Visible-Light-Driven Optoelectronic Reversible Gas Sensing at Room Temperature" (in en). Small Science 2 (3). doi:10.1002/smsc.202100097.
- ↑ 4.0 4.1 R. Eskenazi; J. Raskovan; R. Levitus (1966). "Sulphato complexes of palladium (II)" (in en). 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" (in de). Berichte der Deutschen Chemischen Gesellschaft 59 (9): 2363–2366. doi:10.1002/cber.19260590931.
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