Gallium(III) sulfate
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3D model (JSmol)
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CompTox Dashboard (EPA)
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| Properties | |
| Ga2(SO4)3 | |
| Molar mass | 445.7 g/mol |
| Appearance | White solid[1] |
| Density | 3.86 g/cm3[2] |
| Melting point | 749 °C (1,380 °F; 1,022 K)[3] (decomposes) |
| Slightly soluble[2] | |
| Hazards | |
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| GHS Signal word | Warning |
GHS hazard statements
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H315, H319, H335 |
| P302+352, P305+351+338 | |
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Other cations
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Aluminium sulfate, Indium(III) 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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Gallium(III) sulfate refers to the chemical compound with the formula Ga2(SO4)3, or its hydrates Ga2(SO4)3·xH2O. Gallium metal dissolves in sulfuric acid to form solutions containing [Ga(OH2)6]3+ and SO42− ions. The octadecahydrate Ga2(SO4)3·18H2O crystallises from these solutions at room temperature. This hydrate loses water in stages when heated, forming the anhydrate Ga2(SO4)3 above 150 °C[4] and completely above 310 °C.[1] Anhydrous Ga2(SO4)3 is isostructural with iron(III) sulfate, crystallizing in the rhombohedral space group R3.[5]
Preparation[]
Gallium(III) sulfate is prepared from the reaction of hydroxygallium diacetate and sulfuric acid. The two reactants were mixed at 90 °C and left for 2 days which produced the octadecahydrate. Then, it was dried in a vacuum for 2 hours which created the extremely hygroscopic anhydrous form. The overall reaction is below:
- 2Ga(CH3COO)2OH + 3H2SO4 → Ga2(SO4)3 + 4CH3COOH + 2H2O
After the production, it was confirmed to be the simple salt, Ga2(SO4)3, by x-ray diffraction.[1]
Properties[]
When heated over 749°C, gallium sulfate gives off sulfur trioxide, yielding gallium(III) oxide.[3] A gallium sulfate solution in water mixed with zinc sulfate can precipitate ZnGa2O4.[6]
Derivatives[]
Basic gallium sulfate is known with the formula (H3O)Ga3(SO4)2(OH)6.[3]
Double gallium sulfates are known with composition NaGa3(SO4)2(OH)6, KGa3(SO4)2(OH)6, RbGa3(SO4)2(OH)6, NH4Ga3(SO4)2(OH)6. These are isostructural with jarosite and alunite, and these minerals can have gallium substituted for iron or aluminium.[3] Organic base double gallium sulfates can contain different core structures, these can be chains of [Ga(SO4)3]3-, [Ga(OH)(SO4)2]2- or [Ga(H2O)2(SO4)2]− or sheets of [Ga(H2O)2(SO4)2]− units.[7]
| formula | mw | crystal system |
space group |
unit cell Å | volume | density | properties | reference | |
|---|---|---|---|---|---|---|---|---|---|
| (H3O)Ga3(SO4)2(OH)6 | R3m | a=7.18 c=17.17 z=1.5 | 766 | [8] | |||||
| Ga4(OH)10SO4 | [9] | ||||||||
| NH4Ga3(SO4)2(OH)6 | [7] | ||||||||
| trisodium gallium sulfate | Na3Ga(SO4)3 | tetragonal | a = 9.451 c = 7.097 | [10] | |||||
| NaGa3(SO4)2(OH)6 | [7] | ||||||||
| KGa3(SO4)2(OH)6 | [7] | ||||||||
| RbGa3(SO4)2(OH)6 | [7] | ||||||||
| Caesium gallium sulfate dodecahydrate | CsGa(SO4)2•12H2O | cubic | Pa3 | Z=4 | 2.127 | refractive index=1.461 | [11] | ||
| dimethylammonium gallium sulfate hexahydrate | (CH3)2NH2Ga(SO4)2·6H2O | ferroeelastic | [12][13] | ||||||
| guanidinium gallium sulfate | [C(NH2)3]Ga(SO4)2·6H2O | hexagonal | P31m | a=11.82 c=9.13 | ferroelectric | [14] | |||
| Ethylenediammonium acid gallium sulfate | [C2H10N2][H3O][Ga(SO4)3] | [7] | |||||||
| Ethylenediammonium basic gallium sulfate | [C2H10N2][Ga(OH)(SO4)2]·H2O | [7] | |||||||
| Tetramethylenediammonium gallium sulfate | [C4H14N2][Ga(H2O)2(SO4)2]2 | [7] | |||||||
| Hexamethylenediammonium gallium sulfate | [C6H18N2][Ga(H2O)2(SO4)2]2 | [7] |
References[]
- ^ Jump up to: a b c V.Yu. Proydakova; S.V. Kuznetsov; V.V. Voronov; P.P. Fedorov. "СИНТЕЗ СУЛЬФАТА ГАЛЛИЯ" [SYNTHESIS OF GALLIUM SULFATE]. Fine Chemical Technologies (in Russian). doi:10.32362/2410-6593-2017-12-3-52-57.
- ^ Jump up to: a b "Gallium(III) sulfate hydrate". Alfa Aesar. Alfa Aesar. Retrieved 11 May 2021.
- ^ Jump up to: a b c d Rudolph, Wolfram W.; Schmidt, Peer (July 2011). "Studies on synthetic galloalunites AGa3(SO4)2(OH)6: Synthesis, thermal analysis, and X-ray characterization". Thermochimica Acta. 521 (1–2): 112–120. CiteSeerX 10.1.1.881.3389. doi:10.1016/j.tca.2011.04.013.
- ^ A. J. Downs, ed. (2012). Chemistry of Aluminium, Gallium, Indium and Thallium. Springer. p. 153. ISBN 9789401049603.
- ^ Krause, M.; Gruehn, R. (1995). "Contributions on the thermal behaviour of sulphates XVII.1 Single crystal structure refinements of In2(SO4)3 and Ga2(SO4)3". Z. Kristallogr. 210 (6): 427–431. doi:10.1524/zkri.1995.210.6.427.
- ^ Hirano, Masanori; Okumura, Shiro; Hasegawa, Yasunori; Inagaki, Michio (October 2002). "Direct Precipitation of Spinel-Type Zn(Fe, Ga)2O4 Solid Solutions from Aqueous Solutions at 90°C: Influence of Iron Valence of Starting Salt on Their Crystallite Growth". Journal of Solid State Chemistry. 168 (1): 5–10. Bibcode:2002JSSCh.168....5H. doi:10.1006/jssc.2002.9662.
- ^ Jump up to: a b c d e f g h i Kaufman, Elizabeth A.; Zeller, Matthias; Norquist, Alexander J. (2010-10-06). "A Slow Leak Synthetic Route to Organically Templated Gallium Sulfates". Crystal Growth & Design. 10 (10): 4656–4661. doi:10.1021/cg1009412. ISSN 1528-7483.
- ^ Kydon, D. W.; Pintar, M.; Petch, H. E. (1968-06-15). "NMR Evidence of H 3 O + Ions in Gallium Sulfate". The Journal of Chemical Physics. 48 (12): 5348–5351. Bibcode:1968JChPh..48.5348K. doi:10.1063/1.1668226. ISSN 0021-9606.
- ^ Kang, Bong Kyun; Lim, Hyeong Dae; Mang, Sung Ryul; Song, Keun Man; Jung, Mong Kwon; Kim, Sang-Woo; Yoon, Dae Ho (2015-01-20). "Synthesis and Characterization of Monodispersed β-Ga 2 O 3 Nanospheres via Morphology Controlled Ga 4 (OH) 10 SO 4 Precursors". Langmuir. 31 (2): 833–838. doi:10.1021/la504209f. ISSN 0743-7463.
- ^ Fedorov, P. P.; Proidakova, V. Yu.; Kuznetsov, S. V.; Voronov, V. V. (November 2017). "Phase equilibria in systems of gallium sulfate with lithium or sodium sulfate". Russian Journal of Inorganic Chemistry. 62 (11): 1508–1513. doi:10.1134/S0036023617110067. ISSN 0036-0236. S2CID 103985885.
- ^ Howard E. Swanson, Nancy T. Gilfrich, Marlene I. Cook, Roger Stinchfield, and Paul C. Parks (1 April 1959). "Standard X-ray Diffraction Powder Patterns" (PDF).CS1 maint: multiple names: authors list (link)
- ^ Yasuda, Naohiko; Kaneda, Akio; Czapla, Zbigniew (March 1999). "Pressure effects in dimethylammonium gallium sulfate (DMAGaS)". Ferroelectrics. 223 (1): 71–78. doi:10.1080/00150199908260555. ISSN 0015-0193.
- ^ Völkel, G; Böttcher, R; Michel, D; Czapla, Z; Banys, J (2005-07-20). "Dimethylammonium gallium sulfate hexahydrate and dimethylammonium aluminium sulfate hexahydrate—members of a crystal family with exceptional commensurate/incommensurate phase sequences". Journal of Physics: Condensed Matter. 17 (28): 4511–4529. Bibcode:2005JPCM...17.4511V. doi:10.1088/0953-8984/17/28/010. ISSN 0953-8984.
- ^ Geller, S.; Booth, D.P. (1959-01-01). "The crystal structure of guanidinium gallium sulfate hexahydrate, [C(NH2)3]Ga(SO4)2·6H2O". Zeitschrift für Kristallographie - Crystalline Materials. 111 (1–6). doi:10.1524/zkri.1959.111.16.117. ISSN 2196-7105. S2CID 201840778.
- Gallium compounds
- Sulfates
- Catalysts