SolubilityLesson 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 dissolving Increases 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 dissolving Increases 4. Rate of crystallizing Increases

Replay the last frame if you don't get this!

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 4On page 5 Must be low! They all are!

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

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

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. NaCl ksp = 1.8 x 10-10 smaller

B. NaIO3 ksp = 3.2 x 10-8

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

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

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

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

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

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-

15. 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 Ca2+ + 2Cl-

4 ions versus 3

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

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 M 9.0 x 10-10 M

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 M 9.0 x 10-10 M

0.50 L

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 M 9.0 x 10-10 M

0.50 L x 4.5 x 10-10 mole1 L

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 M 9.0 x 10-10 M

0.50 L x 4.5 x 10-10 mole x 208.3 g 1 L 1 mole

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 M 9.0 x 10-10 M

0.50 L x 4.5 x 10-10 mole x 208.3 g = 4.7 x 10-8 g1 L 1 mole

 

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.

[BaF2] = s = (72.855 - 72.540)g x 1 mole175.3 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 1practice test 1 and 2