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Chapter 15

Chapter 15. 2. Dr. Ayesha Mohy-ud-din. Solubility Equilibria 01. Solubility Product: is the product of the molar concentrations of constituent ions and provides a measure of a compound’s solubility. MX 2 ( s ) æ M 2+ ( aq ) + 2 X – ( aq ) K sp = [M 2+ ][X – ] 2.

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Chapter 15

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  1. Chapter 15 2 Dr. Ayesha Mohy-ud-din

  2. Solubility Equilibria 01 • Solubility Product: is the product of the molar concentrations of constituent ions and provides a measure of a compound’s solubility. MX2(s) æ M2+(aq) + 2 X–(aq) Ksp = [M2+][X–]2

  3. Al(OH)3 1.8 x 10–33 BaCO3 8.1 x 10–9 BaF2 1.7 x 10–6 BaSO4 1.1 x 10–10 Bi2S3 1.6 x 10–72 CdS 8.0 x 10–28 CaCO3 8.7 x 10–9 CaF2 4.0 x 10–11 Ca(OH)2 8.0 x 10–6 Ca3(PO4)2 1.2 x 10–26 Cr(OH)3 3.0 x 10–29 CoS 4.0 x 10–21 CuBr 4.2 x 10–8 Solubility Equilibria 02 CuI 5.1 x 10–12 Cu(OH)2 2.2 x 10–20 CuS 6.0 x 10–37 Fe(OH)2 1.6 x 10–14 Fe(OH)3 1.1 x 10–36 FeS 6.0 x 10–19 PbCO3 3.3 x 10–14 PbCl2 2.4 x 10–4 PbCrO4 2.0 x 10–14 PbF2 4.1 x 10–8 PbI2 1.4 x 10–8 PbS 3.4 x 10–28 MgCO3 4.0 x 10–5 Mg(OH)2 1.2 x 10–11 MnS 3.0 x 10–14 Hg2Cl2 3.5 x 10–18 HgS 4.0 x 10–54 NiS 1.4 x 10–24 AgBr 7.7 x 10–13 Ag2CO3 8.1 x 10–12 AgCl 1.6 x 10–10 Ag2SO4 1.4 x 10–5 Ag2S 6.0 x 10–51 SrCO3 1.6 x 10–9 SrSO4 3.8 x 10–7 SnS 1.0 x 10–26 Zn(OH)2 1.8 x 10–14 ZnS 3.0 x 10–23

  4. Solubility Equilibria 04 • Ion Product (IP): solubility equivalent of the reaction quotient. It is used to determine whether a precipitate will form. IP < Ksp UnsaturatedIP = Ksp SaturatedIP > Ksp Supersaturated; precipitate forms.

  5. The Common-Ion Effect and Solubility 01 • The solubility product (Ksp) is an equilibrium constant; precipitation will occur when the ion product exceeds the Ksp for a compound. • If AgNO3 is added to saturated AgCl, the increase in [Ag+] will cause AgCl to precipitate. IP = [Ag+]0 [Cl–]0 > Ksp

  6. The Common-Ion Effect and Solubility 02

  7. The Common-Ion Effect and Solubility 03

  8. Qualitative Analysis Scheme

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