Solubility Lesson 8 Titrations & Max Ion Concentration
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Transcript of Solubility Lesson 8 Titrations & Max Ion Concentration
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SolubilityLesson 8
Titrations &Max Ion Concentration
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Review Questions
1. Mg(OH)2 will have the greatest solubility in:
A. NaOH
B. Mg(NO3)2
C. H2O
D. AgNO3
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Review Questions
1. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2 ⇌ Mg2+ + 2OH-
A. NaOH
B. Mg(NO3)2
C. H2O
D. AgNO3
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Review Questions
1. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2 ⇌ Mg2+ + 2OH-
A. NaOH Na+ lowers solubility
B. Mg(NO3)2 Mg2+ lowers solubility
C. H2O No effect solubility
D. AgNO3Ag+ increases solubility by reacting with OH-
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Review Questions
1. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2 ⇌ Mg2+ + 2OH-
A. NaOH Na+ lowers solubility
B. Mg(NO3)2 Mg2+ lowers solubility
C. H2O No effect solubility
D. AgNO3 Ag+ increases solubility by reacting with OH-
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Review Questions
2. Mg(OH)2 will have the greatest solubility in:
A. 1.0 M NaNO3
B. NaOH
C. Sr(OH)2
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Review Questions
2. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2 ⇌ Mg2+ + 2OH-
A. 1.0 M NaNO3
B. 1.0 M NaOH
C. Sr(OH)2
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Review Questions
2. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2 ⇌ Mg2+ + 2OH-
A. 1.0 M NaNO3 No effect
B. 1.0 M NaOH 1.0 M OH- lowers solubility
C. Sr(OH)2 2.0 M OH- lowers solubility more
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Review Questions
2. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2 ⇌ Mg2+ + 2OH-
A. 1.0 M NaNO3 No effect
B. 1.0 M NaOH 1.0 M OH- lowers solubility
C. Sr(OH)2 2.0 M OH- lowers solubility more
remember: Sr(OH)2 Sr2+ + 2OH-
1.0 M 1.0 M 2.0 M
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Review Questions
3. PbCl2 will have the greatest solubility in:
PbCl2 ⇌ Pb2+ + 2Cl-
A. 1.0 M NaCl
B. 1.0 M MgCl2
C. 1.0 M AlCl3
D. 2.0 M CaCl2
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Review Questions
3. PbCl2 will have the greatest solubility in:
PbCl2 ⇌ Pb2+ + 2Cl-
A. 1.0 M NaCl 1.0 M Cl-
B. 1.0 M MgCl2
C. 1.0 M AlCl3
D. 2.0 M CaCl2
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Review Questions
3. PbCl2 will have the greatest solubility in:
PbCl2 ⇌ Pb2+ + 2Cl-
A. 1.0 M NaCl 1.0 M Cl-
B. 1.0 M MgCl2 2.0 M Cl-
C. 1.0 M AlCl3
D. 2.0 M CaCl2
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Review Questions
3. PbCl2 will have the greatest solubility in:
PbCl2 ⇌ Pb2+ + 2Cl-
A. 1.0 M NaCl 1.0 M Cl-
B. 1.0 M MgCl2 2.0 M Cl-
C. 1.0 M AlCl3 3.0 M Cl-
D. 2.0 M CaCl2
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Review Questions
3. PbCl2 will have the greatest solubility in:
PbCl2 ⇌ Pb2+ + 2Cl-
A. 1.0 M NaCl 1.0 M Cl-
B. 1.0 M MgCl2 2.0 M Cl-
C. 1.0 M AlCl3 3.0 M Cl-
D. 2.0 M CaCl2 4.0 M Cl-
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1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl2 solution. Calculate the [Pb2+].
Pb2+ + 2I- PbI2(s) Equation
0.0100 L 0.00361 L Data? M 0.0200 M
[Pb2+] =
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1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl2 solution. Calculate the [Pb2+].
Pb2+ + 2I- PbI2(s) Equation
0.0100 L 0.00361 L Data? M 0.0200 M
[Pb2+] = 0.00361 L I-
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1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl2 solution. Calculate the [Pb2+].
Pb2+ + 2I- PbI2(s) Equation
0.0100 L 0.00361 L Data? M 0.0200 M
[Pb2+] = 0.00361 L I- x 0.0200 mol 1L
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1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl2 solution. Calculate the [Pb2+].
Pb2+ + 2I- PbI2(s) Equation
0.0100 L 0.00361 L Data? M 0.0200 M
[Pb2+] = 0.00361 L I- x 0.0200 mol x 1 mol Pb2+
1L 2 mol I-
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1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl2 solution. Calculate the [Pb2+].
Pb2+ + 2I- PbI2(s) Equation
0.0100 L 0.00361 L Data? M 0.0200 M
[Pb2+] = 0.00361 L I- x 0.0200 mol x 1 mol Pb2+
1L 2 mol I-
0.0100 L
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1. In a titration 3.61 mL of 0.0200M NaI is required to completely precipitate all of the lead II ions in 10.0 mL of saturated PbCl2 solution. Calculate the [Pb2+].
Pb2+ + 2I- PbI2(s) Equation
0.0100 L 0.00361 L Data? M 0.0200 M
[Pb2+] = 0.00361 L I- x 0.0200 mol x 1 mol Pb2+
1L 2 mol I-
0.0100 L
= 0.00361 M
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2. Determine the Ksp for PbCl2 from the results of the last
question.
PbCl2(s) ⇌ Pb2+ + 2Cl-
s s 2s
Ksp = [Pb2+][Cl-]2
Ksp = [s][2s] 2
Ksp = 4s3
Ksp = 4(0.00361)3
Ksp = 1.88 x 10-7
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Maximum Ion Concentration 1. The maximum concentration of [AgBrO3] is lower in a solution of NaBrO3 than it would be in pure water. This is
because the solution already has BrO3- present. What is the
maximum [Ag+] possible in a 0.100M NaBrO3 solution?
0.100 M BrO3-
[AgBrO3]
What molarity of [AgBrO3] is possible before it precipitates?
AgBrO3(s) ⇌ Ag+ + BrO3-
0.100 MKsp = [Ag+][BrO3
-]5.3 x 10-5 = [Ag+][0.100]
[Ag+] = [AgBrO3] = 5.3 x 10-4 M
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2. Calculate the maximum number of grams of AgNO3 that will dissolve 100.0 mL of 0.200M AlCl3 without forming a
precipitate.
AgCl(s) ⇌ Ag+ + Cl-
0.600 MKsp = [Ag+][Cl-]
1.8 x 10-10 = [Ag+][0.600]
[Ag+] = 3.0 x 10-10 M
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2. Calculate the maximum number of grams of AgNO3 that will dissolve 100.0 mL of 0.200M AlCl3 without forming a
precipitate.
AgCl(s) ⇌ Ag+ + Cl-
0.600 MKsp = [Ag+][Cl-]
1.8 x 10-10 = [Ag+][0.600]
[Ag+] = 3.0 x 10-10 M
0.1000 L AgNO3
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2. Calculate the maximum number of grams of AgNO3 that will dissolve 100.0 mL of 0.200M AlCl3 without forming a
precipitate.
AgCl(s) ⇌ Ag+ + Cl-
0.600 MKsp = [Ag+][Cl-]
1.8 x 10-10 = [Ag+][0.600]
[Ag+] = 3.0 x 10-10 M
0.1000 L AgNO3 x 3.0 x 10-10 moles 1 L
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2. Calculate the maximum number of grams of AgNO3 that will dissolve 100.0 mL of 0.200M AlCl3 without forming a
precipitate.
AgCl(s) ⇌ Ag+ + Cl-
0.600 MKsp = [Ag+][Cl-]
1.8 x 10-10 = [Ag+][0.600]
[Ag+] = 3.0 x 10-10 M
0.1000 L AgNO3 x 3.0 x 10-10 moles x 169.9 g 1 L 1 mole
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2. Calculate the maximum number of grams of AgNO3 that will dissolve 100.0 mL of 0.200M AlCl3 without forming a
precipitate.
AgCl(s) ⇌ Ag+ + Cl-
0.600 MKsp = [Ag+][Cl-]
1.8 x 10-10 = [Ag+][0.600]
[Ag+] = 3.0 x 10-10 M
0.1000 L AgNO3 x 3.0 x 10-10 moles x 169.9 g = 5.1 x 10-9 g 1 L 1 mole