solubility lesson 8 review notes
Post on 15-Jan-2016
77 Views
Preview:
DESCRIPTION
TRANSCRIPT
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
top related