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Solubility Lesson 8 Review Notes

Solubility Lesson 8 Review Notes. Adding a Crystal to a Saturated Solution  Consider the saturated solution. Ag +. Cl -. Adding a Crystal to a Saturated Solution Note that the solution is saturated -. Ag +. Cl -. Adding a Crystal to a Saturated Solution

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Solubility Lesson 8 Review Notes

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  1. Solubility Lesson 8 Review Notes

  2. Adding a Crystal to a Saturated Solution  Consider the saturated solution Ag+ Cl-

  3. Adding a Crystal to a Saturated Solution Note that the solution is saturated- Ag+ Cl-

  4. Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max Ag+ Cl-

  5. Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizingequals the rate of dissolving. Ag+ Cl-

  6. Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizingequals the rate of dissolving. More solid AgCl is added to the saturated solution above. Ag+ Cl-

  7. Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizingequals the rate of dissolving. More solid AgCl is added to the saturated solution above. Ag+ Cl-

  8. Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizingequals the rate of dissolving. More solid AgCl is added to the saturated solution above. Ag+ Cl-

  9. Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizingequals the rate of dissolving. More solid AgCl is added to the saturated solution above. The solution is full already so the ion concentrations remain constant! Ag+ Cl-

  10. Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizingequals the rate of dissolving. More solid AgCl is added to the saturated solution above. The solution is full already so the ion concentrations remain constant! The new solid dissolves at a greater rate, however crystallizes at an equally greater rate so there is no net change in ion concentration! Ag+ Cl-

  11. Describe the change in each of the followingwhen more solid AgCl is added to a saturated solution. 1. [Ag+]

  12. Describe the change in each of the followingwhen more solid AgCl is added to a saturated solution. 1. [Ag+]Constant 2. [Cl-]

  13. Describe the change in each of the followingwhen more solid AgCl is added to a saturated solution. 1. [Ag+]Constant 2. [Cl-]Constant 3. Rate of dissolving

  14. Describe the change in each of the followingwhen more solid AgCl is added to a saturated solution. 1. [Ag+]Constant 2. [Cl-]Constant 3. Rate of dissolvingIncreases 4. Rate of crystallizing

  15. Describe the change in each of the followingwhen more solid AgCl is added to a saturated solution. 1. [Ag+]Constant 2. [Cl-]Constant 3. Rate of dissolvingIncreases 4. Rate of crystallizingIncreases Replay the last frame if you don't get this!

  16. 5. The ions in hard water are Mg2+ and Ca2+ Na2CO3 can be added to water to remove these ions 6. Calculate the total ion concentration of 1.0 M AlCl3 AlCl3 Al3+ + 3Cl- 1.0 M 1.0 M 3.0 M Total 4.0 M 7. What is the solubility of CaC2O4? Not on page 4 On page 5 Must be low! They all are!

  17. 8. The solubility is 7.1 x 10-5 M. The compound is A. CaSO4 B. CaCO3 Ksp = s2 = 5.0 x 10-9 B 9. A solution of AgNO3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first? A. NaCl B. NaIO3

  18. 10. The solubility is 7.1 x 10-5 M. The compound is A. CaSO4 B. CaCO3 Ksp = s2 = 5.0 x 10-9 B 11. A solution of AgNO3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first? A. NaCl ksp = 1.8 x 10-10 B. NaIO3 ksp = 3.2 x 10-8

  19. 12. The solubility is 7.1 x 10-5 M. The compound is A. CaSO4 B. CaCO3 Ksp = s2 = 5.0 x 10-9 B 13. A solution of AgNO3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first? A. NaClksp = 1.8 x 10-10 smaller B. NaIO3 ksp = 3.2 x 10-8

  20. 14. Small amounts of AgNO3 are added to three solutions that have the same concentration. If only one solution does not form a precipitate, which one is it ? A. NaCl B. NaIO3 C. NaBr

  21. 14. Small amounts of AgNO3 are added to three solutions that have the same concentration. If only one solution does not form a precipitate, which one is it ? A. NaCl ksp = 1.8 x 10-10 B. NaIO3 ksp = 3.2 x 10-8 C. NaBr ksp = 5.4 x 10-8

  22. 14. Small amounts of AgNO3 are added to three solutions that have the same concentration. If only one solution does not form a precipitate, which one is it ? A. NaCl ksp = 1.8 x 10-10 B. NaIO3ksp = 3.2 x 10-8 C. NaBr ksp = 5.4 x 10-8

  23. 14. Which solution has the greatest conductivity? A. 1.0 M AgCl B. 1.0 M CaCO3 C. 1.0 M AlCl3 D. 1.0 M CaCl2

  24. 14. Which solution has the greatest conductivity? A. 1.0 M AgCl low B. 1.0 M CaCO3 low C. 1.0 M AlCl3 high D. 1.0 M CaCl2 high

  25. 14. Which solution has the greatest conductivity? A. 1.0 M AgCl low B. 1.0 M CaCO3 low C. 1.0 M AlCl3 high AlCl3 Al3+ + 3Cl- D. 1.0 M CaCl2 high CaCl2 Al3+ + 2Cl-

  26. 15. Which solution has the greatest conductivity? A. 1.0 M AgCl low B. 1.0 M CaCO3 low C. 1.0 M AlCl3high AlCl3 Al3+ + 3Cl- D. 1.0 M CaCl2 high CaCl2 Ca2+ + 2Cl- 4 ions versus 3

  27. 16. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. AgCl(s)⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s) Ba2+ + 2Cl- 9.0 x 10-10 M

  28. 15. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. AgCl(s)⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s)⇄ Ba2+ + 2Cl- 4.5 x 10-10 M9.0 x 10-10 M

  29. 15. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. . AgCl(s)⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s)⇄ Ba2+ + 2Cl- 4.5 x 10-10 M9.0 x 10-10 M 0.50 L

  30. 15. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. AgCl(s)⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s)⇄ Ba2+ + 2Cl- 4.5 x 10-10 M9.0 x 10-10 M 0.50 L x 4.5 x 10-10mole 1 L

  31. 15. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. AgCl(s)⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s)⇄ Ba2+ + 2Cl- 4.5 x 10-10 M9.0 x 10-10 M 0.50 L x 4.5 x 10-10mole x 208.3 g 1 L 1 mole

  32. 15. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. AgCl(s)⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s)⇄ Ba2+ + 2Cl- 4.5 x 10-10 M9.0 x 10-10 M 0.50 L x 4.5 x 10-10mole x 208.3 g = 4.7 x 10-8 g 1 L 1 mole

  33. 16. In an experiment to determine the solubility of BaF2, 500 mL of the saturated solution was heated in an evaporating dish to remove the water. The evaporating dish and residue were heated two more times to ensure all of the water had been driven off. Volume of saturated solution 500.0 mL Mass of evaporating dish 72.540 g Mass of evaporating dish & BaF2 after first heating 73.500 g Mass of evaporating dish & BaF2 after second heating 72.855 g Mass of evaporating dish & BaF2 after third heating 72.855 g Use this data to calculate the Ksp for BaF2.

  34. [BaF2] = s = (72.855 - 72.540)g x 1 mole 175.3 g 0.500 L s = 0.0035938 M BaF2(s)⇄ Ba2+ + 2F- s s 2s Ksp = [Ba2+][F-]2 Ksp = [s][2s]2 Ksp = 4s3 Ksp = 4(0.0035938)3 Ksp = 1.86 x 10-7 Homework web review 1 practice test 1 and 2

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