Chemistry:Gallium(III) sulfate
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3D model (JSmol)
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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 | 680 °C (1,256 °F; 953 K)[1] (decomposes) |
| Slightly soluble[2] | |
| Hazards | |
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| GHS Signal word | Warning |
| H315, H319, H335 | |
| P302+352, P305+351+338 | |
| NFPA 704 (fire diamond) | |
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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, a salt, 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[3] and completely above 310 °C.[1] Anhydrous Ga2(SO4)3 is isostructural with iron(III) sulfate, crystallizing in the rhombohedral space group R3.[4]
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 680 °C, gallium sulfate gives off sulfur trioxide, yielding gallium(III) oxide.[1] A gallium sulfate solution in water mixed with zinc sulfate can precipitate ZnGa2O4.[5]
Derivatives
Basic gallium sulfate is known with the formula (H3O)Ga3(SO4)2(OH)6.[6]
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 compounds are isostructural with jarosite and alunite. Jarosite and alunite can contain a small amount of gallium substituted for iron or aluminium.[6] 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
- ↑ 1.0 1.1 1.2 1.3 1.4 V.Yu. Proydakova; S.V. Kuznetsov; V.V. Voronov; P.P. Fedorov (2017). "СИНТЕЗ СУЛЬФАТА ГАЛЛИЯ" (in Russian). Fine Chemical Technologies 12 (3): 52–57. doi:10.32362/2410-6593-2017-12-3-52-57.
- ↑ 2.0 2.1 "Gallium(III) sulfate hydrate". https://www.alfa.com/en/catalog/011152/.
- ↑ 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. Bibcode: 1995ZK....210..427K.
- ↑ 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" (in en). Journal of Solid State Chemistry 168 (1): 5–10. doi:10.1006/jssc.2002.9662. Bibcode: 2002JSSCh.168....5H. https://linkinghub.elsevier.com/retrieve/pii/S0022459602996623.
- ↑ 6.0 6.1 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. doi:10.1016/j.tca.2011.04.013.
- ↑ 7.0 7.1 7.2 7.3 7.4 7.5 7.6 7.7 7.8 Kaufman, Elizabeth A.; Zeller, Matthias; Norquist, Alexander J. (2010-10-06). "A Slow Leak Synthetic Route to Organically Templated Gallium Sulfates" (in en). Crystal Growth & Design 10 (10): 4656–4661. doi:10.1021/cg1009412. ISSN 1528-7483. https://pubs.acs.org/doi/10.1021/cg1009412.
- ↑ Kydon, D. W.; Pintar, M.; Petch, H. E. (1968-06-15). "NMR Evidence of H 3 O + Ions in Gallium Sulfate" (in en). The Journal of Chemical Physics 48 (12): 5348–5351. doi:10.1063/1.1668226. ISSN 0021-9606. Bibcode: 1968JChPh..48.5348K. http://aip.scitation.org/doi/10.1063/1.1668226.
- ↑ 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" (in en). Langmuir 31 (2): 833–838. doi:10.1021/la504209f. ISSN 0743-7463. PMID 25539482. https://pubs.acs.org/doi/10.1021/la504209f.
- ↑ 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" (in en). Russian Journal of Inorganic Chemistry 62 (11): 1508–1513. doi:10.1134/S0036023617110067. ISSN 0036-0236. http://link.springer.com/10.1134/S0036023617110067.
- ↑ Howard E. Swanson, Nancy T. Gilfrich, Marlene I. Cook, Roger Stinchfield, and Paul C. Parks (1 April 1959). "Standard X-ray Diffraction Powder Patterns". https://nvlpubs.nist.gov/nistpubs/Legacy/circ/nbscircular539v8.pdf.
- ↑ Yasuda, Naohiko; Kaneda, Akio; Czapla, Zbigniew (March 1999). "Pressure effects in dimethylammonium gallium sulfate (DMAGaS)" (in en). Ferroelectrics 223 (1): 71–78. doi:10.1080/00150199908260555. ISSN 0015-0193. Bibcode: 1999Fer...223...71Y. http://www.tandfonline.com/doi/abs/10.1080/00150199908260555.
- ↑ 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. doi:10.1088/0953-8984/17/28/010. ISSN 0953-8984. Bibcode: 2005JPCM...17.4511V. https://iopscience.iop.org/article/10.1088/0953-8984/17/28/010.
- ↑ Geller, S.; Booth, D.P. (1959-01-01). "The crystal structure of guanidinium gallium sulfate hexahydrate, [C(NH2)3Ga(SO4)2·6H2O"]. Zeitschrift für Kristallographie - Crystalline Materials 111 (1–6): 117–128. doi:10.1524/zkri.1959.111.16.117. ISSN 2196-7105. https://www.degruyter.com/document/doi/10.1524/zkri.1959.111.16.117/html.
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