1. Solubility
Lesson 8
Titrations &
Max Ion Concentration

2. Review Questions
1. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2 ⇌ Mg OH-
A. NaOH
B. Mg(NO3)2
C. H2O
OH- lowers solubility
Mg2+ lowers solubility
No effect solubility
D. AgNO3
Ag+ increases solubility by reacting with OH-

3. Review Questions
2. Mg(OH)2 will have the lowest solubility in:
Mg(OH)2 ⇌ Mg OH-
A. 1.0 M NaNO3
B. 1.0 M NaOH
No effect
1.0 M OH- lowers solubility
C M Sr(OH)2
2.0 M OH- lowers solubility more
remember: Sr(OH)  Sr OH-
1.0 M 1.0 M 2.0 M

4. Review Questions 3. PbCl2 will have the lowest solubility in:
PbCl2 ⇌ Pb Cl-
A. 1.0 M NaCl
B. 1.0 M MgCl2
C. 1.0 M AlCl3
1.0 M Cl-
2.0 M Cl-
3.0 M Cl-
D. 2.0 M CaCl2
4.0 M Cl-

5. Maximum Ion Concentration
4. What is the maximum [Ag+] possible in a 0.100M NaBrO3 without forming a 25 0C.
[Ag+]
0.100 M BrO3-
AgBrO3(s) ⇌ Ag BrO3-
0.100 M
Ksp = [Ag+][BrO3-]
What is the molarity of [Ag+] just before it precipitates?
5.3 x = [Ag+][0.100]
[Ag+] = x M

6. 5. Calculate the maximum number of grams of AgNO3 that will
5. Calculate the maximum number of grams of AgNO3 that will dissolve mL of 0.200M AlCl3 without forming a 25 0C.
AgCl(s) ⇌ Ag+ + Cl-
0.600 M
Ksp = [Ag+][Cl-]
1.8 x = [Ag+][0.600]
[Ag+] = 3.0 x M
L AgNO3
x x moles
x g
= x g
1 L
1 mole

7. 6. In a titration 3.61 mL of M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl2 solution. Calculate the [Pb2+].
Pb I-  PbI2 L L
? M M
L I-
x mol
x 1 mol Pb2+ 1L
2 mol I-
[Pb2+] = L
= M