1. Solubility Lesson 8 Titrations & Max Ion Concentration

2. Review Questions 1.Mg(OH) 2 will have the greatest solubility in: A.NaOH B.Mg(NO 3 ) 2 C.H 2 O D.AgNO 3

3. 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 D.AgNO 3

4. Review Questions 1.Mg(OH) 2 will have the greatest solubility in: Mg(OH) 2 ⇌ Mg 2+ +2OH - A.NaOHNa + lowers solubility B.Mg(NO 3 ) 2 Mg 2+ lowers solubility C.H 2 ONo effect solubility D.AgNO 3 Ag + increases solubility by reacting with OH -

5. Review Questions 1.Mg(OH) 2 will have the greatest solubility in: Mg(OH) 2 ⇌ Mg 2+ +2OH - A.NaOHNa + lowers solubility B.Mg(NO 3 ) 2 Mg 2+ lowers solubility C.H 2 ONo effect solubility D.AgNO 3 Ag + increases solubility by reacting with OH -

6. Review Questions 2.Mg(OH) 2 will have the greatest solubility in: A.1.0 M NaNO 3 B.NaOH C.Sr(OH) 2

7. Review Questions 2.Mg(OH) 2 will have the greatest solubility in: Mg(OH) 2 ⇌ Mg 2+ +2OH - A.1.0 M NaNO 3 B.1.0 M NaOH C.Sr(OH) 2

8. Review Questions 2.Mg(OH) 2 will have the greatest solubility in: Mg(OH) 2 ⇌ Mg 2+ +2OH - A.1.0 M NaNO 3 No effect B.1.0 M NaOH1.0 M OH - lowers solubility C.Sr(OH) 2 2.0 M OH - lowers solubility more

9. Review Questions 2.Mg(OH) 2 will have the greatest solubility in: Mg(OH) 2 ⇌ Mg 2+ +2OH - A.1.0 M NaNO 3 No effect B.1.0 M NaOH1.0 M OH - lowers solubility C.Sr(OH) 2 2.0 M OH - lowers solubility more remember: Sr(OH) 2  Sr 2+ + 2OH - 1.0 M1.0 M2.0 M

10. Review Questions 3.PbCl 2 will have the greatest solubility in: PbCl 2 ⇌ Pb 2+ +2Cl - A.1.0 M NaCl B.1.0 M MgCl 2 C.1.0 M AlCl 3 D.2.0 M CaCl 2

11. Review Questions 3.PbCl 2 will have the greatest solubility in: PbCl 2 ⇌ Pb 2+ +2Cl - A.1.0 M NaCl1.0 M Cl - B.1.0 M MgCl 2 C.1.0 M AlCl 3 D.2.0 M CaCl 2

12. Review Questions 3.PbCl 2 will have the greatest solubility in: PbCl 2 ⇌ Pb 2+ +2Cl - A.1.0 M NaCl1.0 M Cl - B.1.0 M MgCl 2 2.0 M Cl - C.1.0 M AlCl 3 D.2.0 M CaCl 2

13. Review Questions 3.PbCl 2 will have the greatest solubility in: PbCl 2 ⇌ Pb 2+ +2Cl - A.1.0 M NaCl1.0 M Cl - B.1.0 M MgCl 2 2.0 M Cl - C.1.0 M AlCl 3 3.0 M Cl - D.2.0 M CaCl 2

14. Review Questions 3.PbCl 2 will have the greatest solubility in: PbCl 2 ⇌ Pb 2+ +2Cl - A.1.0 M NaCl1.0 M Cl - B.1.0 M MgCl 2 2.0 M Cl - C.1.0 M AlCl 3 3.0 M Cl - D.2.0 M CaCl 2 4.0 M Cl -

15. 1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl 2 solution. Calculate the [Pb 2+ ]. Pb 2+ +2I -  PbI 2(s) Equation 0.0100 L0.00361 LData ? M0.0200 M [Pb 2+ ]=

16. 1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl 2 solution. Calculate the [Pb 2+ ]. Pb 2+ +2I -  PbI 2(s) Equation 0.0100 L0.00361 LData ? M0.0200 M [Pb 2+ ]=0.00361 L I -

17. 1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl 2 solution. Calculate the [Pb 2+ ]. Pb 2+ +2I -  PbI 2(s) Equation 0.0100 L0.00361 LData ? M0.0200 M [Pb 2+ ]=0.00361 L I - x 0.0200 mol 1L

18. 1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl 2 solution. Calculate the [Pb 2+ ]. Pb 2+ +2I -  PbI 2(s) Equation 0.0100 L0.00361 LData ? M0.0200 M [Pb 2+ ]=0.00361 L I - x 0.0200 mol x 1 mol Pb 2+ 1L 2 mol I -

19. 1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl 2 solution. Calculate the [Pb 2+ ]. Pb 2+ +2I -  PbI 2(s) Equation 0.0100 L0.00361 LData ? M0.0200 M [Pb 2+ ]=0.00361 L I - x 0.0200 mol x 1 mol Pb 2+ 1L 2 mol I - 0.0100 L

20. 1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl 2 solution. Calculate the [Pb 2+ ]. Pb 2+ +2I -  PbI 2(s) Equation 0.0100 L0.00361 LData ? M0.0200 M [Pb 2+ ]=0.00361 L I - x 0.0200 mol x 1 mol Pb 2+ 1L 2 mol I - 0.0100 L =0.00361 M

21. 2. Determine the Ksp for PbCl 2 from the results of the last question. PbCl 2(s) ⇌ Pb 2+ +2Cl - ss2s Ksp=[Pb 2+ ][Cl - ] 2 Ksp=[s][2s] 2 Ksp=4s 3 Ksp=4(0.00361) 3 Ksp=1.88 x 10 -7

22. Maximum Ion Concentration 1. The maximum concentration of [AgBrO 3 ] is lower in a solution of NaBrO 3 than it would be in pure water. This is because the solution already has BrO 3 - present. What is the maximum [Ag + ] possible in a 0.100M NaBrO 3 solution? 0.100 M BrO 3 - [AgBrO 3 ] What molarity of [AgBrO 3 ] is possible before it precipitates? AgBrO 3(s) ⇌ Ag + +BrO 3 - 0.100 M Ksp=[Ag + ][BrO 3 - ] 5.3 x 10 -5 =[Ag + ][0.100] [Ag + ]=[AgBrO 3 ]=5.3 x 10 -4 M

23. 2. Calculate the maximum number of grams of AgNO 3 that will dissolve 100.0 mL of 0.200M AlCl 3 without forming a precipitate. 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

24. 2. Calculate the maximum number of grams of AgNO 3 that will dissolve 100.0 mL of 0.200M AlCl 3 without forming a precipitate. 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 AgNO 3

25. 2. Calculate the maximum number of grams of AgNO 3 that will dissolve 100.0 mL of 0.200M AlCl 3 without forming a precipitate. 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 AgNO 3 x 3.0 x 10 -10 moles 1 L

26. 2. Calculate the maximum number of grams of AgNO 3 that will dissolve 100.0 mL of 0.200M AlCl 3 without forming a precipitate. 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 AgNO 3 x 3.0 x 10 -10 moles x 169.9 g 1 L 1 mole

27. 2. Calculate the maximum number of grams of AgNO 3 that will dissolve 100.0 mL of 0.200M AlCl 3 without forming a precipitate. 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 AgNO 3 x 3.0 x 10 -10 moles x 169.9 g = 5.1 x 10 -9 g 1 L 1 mole