Chem208_Lecture_19_Color - Today: Solubility Equilibria...

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Unformatted text preview: Today: Solubility Equilibria Complexation Equilibria Chapter 18–1, 2, 3, 5, 7, 8 Chapter 24–8, 9 PS8 due by 2:00 Fri, 4/4 Exam II: Tuesday, 4/8 7:30-9:00 Room Assignments are shown on today’s handout Review Session schedule will be announced on Thursday 1 Sample Problems • In a saturated solution of Mg(OH)2, [Mg2+] is found to be 2.56 x 10–3 M; [OH–] is found to be 4.68 x 10–5 M. Calculate Ksp for Mg(OH)2. • What is the molar solubility (moles/liter) of Mg(OH)2 in pure water? • What is the pH of a saturated solution of Mg(OH)2 formed by adding excess Mg(OH)2(s) to water? • Which is more soluble, Mg(OH)2 or AgCl (Ksp = 1.80 x 10–10 for AgCl)? 2 • Should a precipitate form when equal volumes of 5.0 x 10–3 M Mg2+ [ie, MgCl2(aq)] and 5.0 x 10-3 M OH– [ie, NaOH(aq)] are mixed together? • What is the molar solubility of Mg(OH)2(s) in a solution containing 1.00 x 10–2 M NaOH(aq)? • Why does Mg(OH)2 dissolve in acidic solution? • Calculate the molar solubility of Mg(OH)2(s) in 1.0 M NH4Cl(aq). Kb = 1.8 x 10–5 for NH3(aq). The reaction of interest is: Mg(OH)2(s) + 2 NH4+(aq) ⇔ Mg2+(aq) + 2 NH3(aq) + 2 H2O(l) 3 ...
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Chem208_Lecture_19_Color - Today: Solubility Equilibria...

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