1. Sulfide
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Sb 2 S 3 is an orange-red precipitate which is both amphoteric and soluble in both acid and alkali.
Sb 2 S 3 +6OH - 
SbO 3 3 - +SbS 3 3 - +3H 2 O
Sb 2 S 3 +6H + +12Cl - 2[SbCl 6 ] 3 - +3H 2 S↑
Sb 2 S 3 is also soluble in basic sulfides such as Na 2 S or (NH 4 ) 2 S:
Sb 2 S 3 +3S 2 - 2AsS 3 3 -
Sb 2 S 5 is soluble in concentrated HCl and undergoes redox reaction:
Sb 2 S 5 +12HCl (hot, concentrated) 2H 3 [SbCl 6 ]+3H 2 S↑+2S↓
Acid Sb 2 S 5 greater than the Sb 2 S 3, and therefore, Sb 2 S 5 ratio of Sb 2 S 3 more soluble in an alkali sulfide solution.
Sb 2 S 5 +3Na 2 S 2Na 3 SbS 4
Sb 2 S 3 is reducible and reacts with polysulfides to form thioates:
Sb 2 S 3 +3S 2 - 2SbS 4 3 - +S
Second, thio acid salt
The same as arsenic, antimony sodium thiosulfate (Na 3 SbS 3) and sodium antimonate thiosulfate (Na 3 SbS 4) immediately with acid to form the corresponding sulfides and H 2 S.
2SbS 4 3 - +6H + Sb 2 S 5 ↓+3H 2 S↑
2SbS 3 3 - +6H + Sb 2 S 3 ↓+3H 2 S↑