Solubility Lesson 8 Review Notes

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

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

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

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

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

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

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

Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizing equals 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! Cl - Ag +

Adding a Crystal to a Saturated Solution Note that the solution is saturated- filled to the max and the rate of crystallizing equals 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! Cl - Ag +

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

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

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

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

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

5.The ions in hard water are Mg 2+ and Ca 2+ Na 2 CO 3 can be added to water to remove these ions 6.Calculate the total ion concentration of 1.0 M AlCl 3 AlCl 3  Al Cl M1.0 M3.0 M Total4.0 M 7.What is the solubility of CaC 2 O 4 ? Not on page 4 On page 5Must be low! They all are!

8.The solubility is 7.1 x M. The compound is A.CaSO 4 B.CaCO 3 Ksp = s 2 =5.0 x B 9.A solution of AgNO 3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first? A.NaCl B.NaIO 3

10.The solubility is 7.1 x M. The compound is A.CaSO 4 B.CaCO 3 Ksp = s 2 =5.0 x B 11.A solution of AgNO 3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first? A.NaClksp = 1.8 x B.NaIO 3 ksp = 3.2 x 10 -8

12.The solubility is 7.1 x M. The compound is A.CaSO 4 B.CaCO 3 Ksp = s 2 =5.0 x B 13.A solution of AgNO 3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first? A.NaClksp = 1.8 x smaller B.NaIO 3 ksp = 3.2 x 10 -8

14.Small amounts of AgNO 3 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.NaIO 3 C.NaBr

14.Small amounts of AgNO 3 are added to three solutions that have the same concentration. If only one solution does not form a precipitate, which one is it ? A.NaClksp = 1.8 x B.NaIO 3 ksp = 3.2 x C.NaBrksp = 5.4 x 10 -8

14.Small amounts of AgNO 3 are added to three solutions that have the same concentration. If only one solution does not form a precipitate, which one is it ? A.NaClksp = 1.8 x B.NaIO 3 ksp = 3.2 x C.NaBrksp = 5.4 x 10 -8

14.Which solution has the greatest conductivity? A.1.0 M AgCl B.1.0 M CaCO 3 C.1.0 M AlCl 3 D.1.0 M CaCl 2

14.Which solution has the greatest conductivity? A.1.0 M AgCllow B.1.0 M CaCO 3 low C.1.0 M AlCl 3 high D.1.0 M CaCl 2 high

14.Which solution has the greatest conductivity? A.1.0 M AgCllow B.1.0 M CaCO 3 low C.1.0 M AlCl 3 highAlCl 3  Al Cl - D.1.0 M CaCl 2 highCaCl 2  Al Cl -

15.Which solution has the greatest conductivity? A.1.0 M AgCllow B.1.0 M CaCO 3 low C.1.0 M AlCl 3 highAlCl 3  Al Cl - D.1.0 M CaCl 2 highCaCl 2  Ca Cl - 4 ions versus 3

16.Calculate the maximum number of grams BaCl 2 that will dissolve in 0.50 L of 0.20 M AgNO 3 solution. AgCl (s) ⇄ Ag + + Cl M Ksp=[Ag + ][Cl - ] 1.8 x = [0.20][Cl - ] [Cl - ] =9.0 x M BaCl 2(s)  Ba Cl x M

15.Calculate the maximum number of grams BaCl 2 that will dissolve in 0.50 L of 0.20 M AgNO 3 solution. AgCl (s) ⇄ Ag + + Cl M Ksp=[Ag + ][Cl - ] 1.8 x = [0.20][Cl - ] [Cl - ] =9.0 x M BaCl 2(s) ⇄ Ba Cl x M9.0 x M

15.Calculate the maximum number of grams BaCl 2 that will dissolve in 0.50 L of 0.20 M AgNO 3 solution.. AgCl (s) ⇄ Ag + + Cl M Ksp=[Ag + ][Cl - ] 1.8 x = [0.20][Cl - ] [Cl - ] =9.0 x M BaCl 2(s) ⇄ Ba Cl x M9.0 x M 0.50 L

15.Calculate the maximum number of grams BaCl 2 that will dissolve in 0.50 L of 0.20 M AgNO 3 solution. AgCl (s) ⇄ Ag + + Cl M Ksp=[Ag + ][Cl - ] 1.8 x = [0.20][Cl - ] [Cl - ] =9.0 x M BaCl 2(s) ⇄ Ba Cl x M9.0 x M 0.50 L x 4.5 x mole 1 L

15.Calculate the maximum number of grams BaCl 2 that will dissolve in 0.50 L of 0.20 M AgNO 3 solution. AgCl (s) ⇄ Ag + + Cl M Ksp=[Ag + ][Cl - ] 1.8 x = [0.20][Cl - ] [Cl - ] =9.0 x M BaCl 2(s) ⇄ Ba Cl x M9.0 x M 0.50 L x 4.5 x molex g 1 L 1 mole

15.Calculate the maximum number of grams BaCl 2 that will dissolve in 0.50 L of 0.20 M AgNO 3 solution. AgCl (s) ⇄ Ag + + Cl M Ksp=[Ag + ][Cl - ] 1.8 x = [0.20][Cl - ] [Cl - ] =9.0 x M BaCl 2(s) ⇄ Ba Cl x M9.0 x M 0.50 L x 4.5 x molex g = 4.7 x g 1 L 1 mole

16.In an experiment to determine the solubility of BaF 2, 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 solution500.0 mL Mass of evaporating dish g Mass of evaporating dish & BaF 2 after first heating g Mass of evaporating dish & BaF 2 after second heating g Mass of evaporating dish & BaF 2 after third heating g Use this data to calculate the K sp for BaF 2.

[BaF 2 ] = s = ( )gx1 mole g L s= M BaF 2(s) ⇄ Ba F - ss2s Ksp=[Ba 2+ ][F - ] 2 Ksp=[s][2s] 2 Ksp=4s 3 Ksp=4( ) 3 Ksp=1.86 x Homeworkweb review 1 practice test 1 and 2