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Solubility Lesson 8 Titrations & Max Ion Concentration

Solubility Lesson 8 Titrations & Max Ion Concentration. Review Questions 1. Mg(OH) 2 will have the greatest solubility in: Mg(OH) 2 ⇌ Mg 2+ + 2OH - A. NaOH B. Mg(NO 3 ) 2 C. H 2 O . OH - lowers solubility. Mg 2+ lowers solubility. No effect solubility. D. AgNO 3.

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Solubility Lesson 8 Titrations & Max Ion Concentration

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  1. Solubility Lesson 8 Titrations & Max Ion Concentration

  2. Review Questions 1. Mg(OH)2 will have the greatest solubility in: Mg(OH)2 ⇌ Mg2+ + 2OH- A. NaOH B. Mg(NO3)2 C. H2O OH- lowers solubility Mg2+ lowers solubility No effect solubility D. AgNO3 Ag+ increases solubility by reacting with OH-

  3. Review Questions 2. Mg(OH)2 will have the lowest solubility in: Mg(OH)2 ⇌ Mg2+ + 2OH- A. 1.0 M NaNO3 B. 1.0 M NaOH No effect 1.0 M OH- lowers solubility C. 1.0 M Sr(OH)2 2.0 M OH- lowers solubility more remember:Sr(OH)2  Sr2+ + 2OH- 1.0 M 1.0 M 2.0 M

  4. Review Questions 3. PbCl2 will have the lowest solubility in: PbCl2 ⇌ Pb2+ + 2Cl- A. 1.0 M NaCl B. 1.0 M MgCl2 C. 1.0 M AlCl3 1.0 M Cl- 2.0 M Cl- 3.0 M Cl- D. 2.0 M CaCl2 4.0 M Cl-

  5. Maximum Ion Concentration 0.100 M BrO3- 4. What is the maximum [Ag+]possible in a 0.100MNaBrO3 without forming a precipitate@ 25 0C. [Ag+] AgBrO3(s)⇌ Ag+ + BrO3- 0.100 M Ksp = [Ag+][BrO3-] What is the molarity of [Ag+] just before it precipitates? 5.3 x 10-5 = [Ag+][0.100] [Ag+] =5.3 x 10-4 M

  6. 5. Calculate the maximumnumber of gramsof AgNO3 that will dissolve 100.0 mL of0.200M AlCl3without forming a precipitate @ 25 0C. AgCl(s)⇌ Ag+ + Cl- 0.600 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [Ag+][0.600] [Ag+]= 3.0 x 10-10 M 0.1000 L AgNO3 x 3.0 x 10-10 moles x 169.9 g = 5.1 x 10-9 g 1 L 1 mole

  7. 6. In a titration 3.61 mLof0.0200MNaI is required to completely precipitate all of the lead II ions in 10.0 mLof saturatedPbCl2solution. Calculate the [Pb2+]. Pb2+ + 2I- PbI2 0.0100 L 0.00361 L 0.0200 M ? M x 0.0200 mol x 1 mol Pb2+ 0.00361 L I- 2 mol I- 1L [Pb2+] = 0.0100 L =0.00361 M

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