As discussed in the lab intro, a low concentration of sulfide is needed to precipitate group II ions. This is because the group Il sulfides are much less soluble than group III sulfides. Prove this by calculating the molar solubility of SnS₂(Sn¹+ is a group II ion) and A12S3 (A1³+ is a group III ion). The Ksp values are given below. Type your answers in the boxes below. SnS₂ Ksp = 1 x 10-46 Al2 S3 Ksp = 4.0 x 10-14 Solubility of SnS₂ is Solubility of A12 S3 is M M
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![**Educational Exercise: Solubility of Sulfides**
As discussed in the lab introduction, a low concentration of sulfide is needed to precipitate group II ions. This is because group II sulfides are much less soluble than group III sulfides. Prove this by calculating the molar solubility of SnS₂ (Sn⁴⁺ is a group II ion) and Al₂S₃ (Al³⁺ is a group III ion). The Kₛₚ values are given below. Type your answers in the boxes provided.
**Chemical Equations and Solubility Products:**
- SnS₂ \(K_{sp} = 1 \times 10^{-46}\)
- Al₂S₃ \(K_{sp} = 4.0 \times 10^{-14}\)
**Calculate the Solubility:**
- Solubility of SnS₂ is: [_______] M
- Solubility of Al₂S₃ is: [_______] M
Use these values to understand the differences in solubility between group II and group III sulfides.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F00982369-4b63-4fd7-a0c5-99df656ce3de%2F0a6530f7-e7cf-42e5-930c-2b185944f9a1%2Fs94w5k_processed.png&w=3840&q=75)
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