Lecture 16

# Lecture 16 - 8.8 Solubility Equilibria Solubility Product...

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Unformatted text preview: 8.8 Solubility Equilibria Solubility Product, Ksp: - Equilibrium constant for ions in saturated aqueous solution. e.g., For Mg(OH)2 (s) ⇔ Mg2+ (aq) + 2OH- (aq) Ksp = [Mg2+][OH-]2 = 1.8 x 10-11 What is the solubility of Mg(OH)2 in water, in mol/L and g/L? 1.7 x 10-4M; 9.6 mg/L What is the molar solubility of Mg(OH)2 in 0.010M NaOH? 1.8 x 10-7M What is the molar solubility of Mg(OH)2 in buffer of pH = 9.0 ? 1.8 x 10-1M What is the molar solubility of Mg(OH)2 in buffer of pH = 5.0 ? 1.8 x 107M ?? 1 Precipitation • Criteria for Precipitation: Compute the Ion Product (reaction quotient), Qsp For PbI2 (s) ⇔ Pb2+ (aq) + 2I- (aq) Ksp = 7.1 x 10-9 If 3 drops of 0.20M KI are added to 100.0mL of 0.010 M Pb(NO3)2, will a precipitate form? Note: 1 drop = 0.05mL 0.05ml lL 0.20M KI 1 mol I − moles I = 3 drops x x x x = 3x10 −5 mol I − drop 1000mL L mol KI − [I-]= 3 x 10-5mol/0.100L = 3 x 10-4M [Pb2+] = 0.010M Qsp = [Pb2+][I-]2 = (0.010)(3 x 10-4)2 = 9 x 10-10 < Ksp Precipitation will not occur 2 3 Titrations of Polyprotic Acids, e.g., H3PO4 Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8; Ka3 = 4.8 x 10-13 4 Titrations of Polyprotic Acids, e.g., H3PO4 Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8; Ka3 = 4.8 x 10-13 5 Problem 69: Titration of Na2CO3 with HCl a) Identify major species in solution at points A-F b) For the titration of 25.00 mL of 0.1000 M Na2CO3 with 0.1000M HCl, 6 calculate the pH at ponts A-E. B and D are halfway points to equivalence ...
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Lecture 16 - 8.8 Solubility Equilibria Solubility Product...

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