I am trying to dissolve antimony trichloride in 0.1 M HCl or DI water at concentrations as low as 2 mM but it is not dissolving. I am having the same problem with another antimony compound potassium antimony tartrate, which is also not dissolving. Does anyone have an idea how to dissolve these compounds?
According to everything I've ready SbCl3 should be readily soluble in water or HCl Antimony Potassium tartrate has very low solubility though. Try heating your solutions to speed the process.
it Is better to take hot acid instead of normal temperature, and try the procedure
Antimony trichloride (SbCl3) readily hydrolyzes in water or aq. solutions. It is hygroscopic, so that it can uptake moisture from humid air, while also converting to hydrolyzed products, such as antimony oxychloride (SbOCl): SbCl3 + H2O ⇌ SbOCl + 2 HCl. The last may possibly precipitate as a pasty sediment and/or convert itself to tetra-antimony dichloride pentoxide, Sb4O5Cl2, which can possibly precipitate (white) and/or crystallize from solution. Also Sb3+ can hydrolyze in aq. sol.: Sb3+ + 6 H2O ⇌ Sb(OH)3 +3 H3O+, having Sb(OH)2+ and Sb(OH)2+ as intermediate species. Also the SbCl2+ and SbCl2+ species occur. By adding excess chloride to the solution, chloroantimonate(III) anions tend to form from SbCl3, as it behaves as a Lewis acid, namely: SbCl4-, SbCl52-, SbCl63-. Such species can also undergo hydrolysis (e.g.): SbCl4- + 3 H2O ⇌ SbOCl + 2 H3O+ + 3 Cl-. Moreover, SbO+ (from dissociation of SbOCl) also hydrolyzes: SbO+ + 3 H2O ⇌ Sb(OH)3 + H3O+.
Solubility of antimony trichloride (SbCl3) in either water or aq. hydrochloric acid can be found at: A. Seidell,"Solubilities of Inorganic and Organic Compounds", 2nd ed., Van Nostrand Comp., New York, 1919, p. 88.
İ have SbO Cl . Can İ transform it To İnCl3 by dissolution in HCl an use it for deposition of InSb nanowires ?
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