SolubilityLesson 8

Titrations &Max Ion Concentration

Review Questions

1. Mg(OH)2 will have the greatest solubility in:

A. NaOH

B. Mg(NO3)2

C. H2O

D. AgNO3

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

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-

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-

Review Questions

2. Mg(OH)2 will have the greatest solubility in:

A. 1.0 M NaNO3

B. NaOH

C. Sr(OH)2

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

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

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

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

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

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

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

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-

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+] =

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-

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

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-

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

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

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

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

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

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

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

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

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