WS₂ is not soluble in molten alkali in the traditional sense but reacts with it, decomposing into soluble products. In molten sodium hydroxide (NaOH) at 500-600°C, WS₂ transforms into sodium tungstate (Na₂WO₄) and sodium sulfide (Na₂S): WS₂ + 4NaOH + 2O₂ → Na₂WO₄ + Na₂S + 2H₂O. Both products dissolve in the melt, effectively breaking down WS₂, though this is a chemical reaction, not solubility of intact WS₂.
The reaction requires heat and oxygen (from air or the melt), as molten NaOH alone is less reactive. Tests with WS₂ powder in NaOH at 550°C show complete conversion within hours, with the melt turning clear upon cooling and dilution, confirmed by detecting WO₄²⁻ and S²⁻ ions. Compared to room-temperature NaOH (no reaction), the molten state’s high energy overcomes WS₂’s stability. Potassium hydroxide (KOH) yields similar results (e.g., K₂WO₄).
This reactivity contrasts with WS₂’s inertness in water or dilute bases, highlighting temperature’s role. MoS₂ behaves similarly, forming molybdates, though WS₂’s higher thermal stability delays reaction onset. In applications, this limits WS₂’s use in high-temperature alkaline environments unless shielded, but it enables processes like alkali fusion for tungsten recovery.
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