1. Solubility
Lesson 8
Review Notes

2. Adding a Solid to a Saturated Solution
Consider the saturated solution- the rate of crystallizing equals the rate of dissolving
More solid AgCl is added
The solution is full so the ion concentrations remain constant
Ag+
Cl-
The rate of dissolving and rate of crystallizing both increase by the same amount.

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

4. 5. The ions in hard water are Mg2+ and Ca2+
Na2CO3 can be added to water to remove these ions

5. 6. Calculate the total ion concentration of 1.0 M AlCl3
AlCl3  Al Cl-
1.0 M 1.0 M 3.0 M
Total 4.0 M

6. 7. What is the molar solubility of CaC2O4?
Ksp = s2
2.3 x = s2
4.8 x M

7. 8. The solubility is 7.1 x 10-5 M. The compound is:
A. CaSO4
Ksp = s2
= x 10-9
B. CaCO3

8. 9. A solution of AgNO3 is added slowly to each of the following 0.10 M solutions. Which forms a precipitate first?
A. NaCl
ksp = x
B. NaIO3
ksp = x 10-8

9. 10. Small amounts of AgNO3 are added to three solutions. One solution
a precipitate, which one is it?
does not form
A. NaCl
ksp = x
B. NaIO3
ksp = x 10-8
C. NaBr
ksp = x

10. 11. Which solution has the greatest conductivity?
A. 1.0 M NaCl
B. 1.0 M CaCO3
D. 1.0 M CaCl2
1.0 M M = M
C. 1.0 M AlCl3
 Al Cl-
 Ca Cl-
1.0 M M = M

11. 12. 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 = [0.20][Cl-]
[Cl-] = x M
BaCl2(s) ⇄ Ba Cl-
4.5 x M
9.0 x M
0.50 L
x x mole
x g
= x g
1 L
1 mole