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Lesson 4 Calculating Molar Solubility From Ksp. 1.Calculate the molar solubility @ 25 o C for BaCrO 4 in units of g/L BaCrO 4(s) ⇌ Ba 2+ +CrO 4 2- sss Ksp=[Ba 2+ ][CrO 4 2- ] Ksp= s 2 from page 5 1.2 x 10 -10 = s 2 s= 1.1 x 10 -5 M

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Lesson 4 Calculating Molar Solubility From Ksp

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Lesson 4

Calculating

Molar Solubility

From Ksp


1.Calculate the molar solubility @ 25oC for BaCrO4 in units of g/L

BaCrO4(s)⇌Ba2++CrO42-

sss

Ksp=[Ba2+][CrO42-]

Ksp=s2

from page 51.2 x 10-10=s2

s=1.1 x 10-5 M

note that solubility units are M!

1.1 x 10-5 mole x 253.3 g = 0.0028 g/L

L 1 mole


2.Calculate the molar solubility @ 25oC for Cu(IO3)2 in units

of g/L

Cu(IO3)2⇌Cu2++2IO3-

ss2s

Ksp=[Cu2+][IO3-]2

Ksp=[s][2s]2

Ksp=4s3

6.9 x 10-8=4s3

s=2.6 x 10-3 M

note sig figs are 2 like the Ksp!


2.584 x 10-3moles

L


2.584 x 10-3moles x 413.2 g

L 1 mole


2.584 x 10-3moles x 413.2 g=1.1 g/L

L 1 mole


3.Calculate the molar solubility @ 25oC for Fe(OH)3. Calculate the mass required to prepare 2.0 L of the above saturated solution.

Fe(OH)3⇌Fe3++3OH-

ss3s

Ksp=[Fe3+][OH-]3

Ksp=[s][3s]3

2.6 x 10-39=27s4

s=9.906 x 10-11 M

2.0 L


3.Calculate the molar solubility @ 25oC for Fe(OH)3. Calculate the mass required to prepare 2.0 L of the above solution.

Fe(OH)3⇌Fe3++3OH-

ss3s

Ksp=[Fe3+][OH-]3

Ksp=[s][3s]3

2.6 x 10-39=27s4

s=9.906 x 10-11 M

2.0 L x 9.906 x 10-11moles

1 L


3.Calculate the molar solubility @ 25oC for Fe(OH)3. Calculate the mass required to prepare 2.0 L of the above solution.

Fe(OH)3⇌Fe3++3OH-

ss3s

Ksp=[Fe3+][OH-]3

Ksp=[s][3s]3

2.6 x 10-39=27s4

s=9.906 x 10-11 M

2.0 L x 9.906 x 10-11moles x 106.8 g

1 L mole


3.Calculate the molar solubility @ 25oC for Fe(OH)3. Calculate the mass required to prepare 2.0 L of the above solution.

Fe(OH)3⇌Fe3++3OH-

ss3s

Ksp=[Fe3+][OH-]3

Ksp=[s][3s]3

2.6 x 10-39=27s4

s=9.906 x 10-11 M

2.0 L x 9.906 x 10-11moles x 106.8 g = 2.1 x 10-8 g

1 L mole


The size of the Ksp is related to the solubility of the ionic compound. For salts that are comparable (AB versus AB), the larger the Ksp of the salt, the greater is its solubility.

4.Indicate the solid with the greatest solubility.

PbSO4

ZnS

AgCl

BeS


The size of the Ksp is related to the solubility of the ionic compound. For salts that are comparable (AB versus AB), the larger the Ksp of the salt, the greater is its solubility.

4.Indicate the solid with the greatest solubility.

PbSO4start on page 4

ZnS

AgCl

BeS


The size of the Ksp is related to the solubility of the ionic compound. For salts that are comparable (AB versus AB), the larger the Ksp of the salt, the greater is its solubility.

4.Indicate the solid with the greatest solubility.

PbSO4lowstart on page 4

ZnS

AgCl

BeS


The size of the Ksp is related to the solubility of the ionic compound. For salts that are comparable (AB versus AB), the larger the Ksp of the salt, the greater is its solubility.

4.Indicate the solid with the greatest solubility.

PbSO4lowstart on page 4

ZnSlow

AgCl

BeS


The size of the Ksp is related to the solubility of the ionic compound. For salts that are comparable (AB versus AB), the larger the Ksp of the salt, the greater is its solubility.

4.Indicate the solid with the greatest solubility.

PbSO4lowstart on page 4

ZnSlow

AgCllow

BeS


The size of the Ksp is related to the solubility of the ionic compound. For salts that are comparable (AB versus AB), the larger the Ksp of the salt, the greater is its solubility.

4.Indicate the solid with the greatest solubility.

PbSO4lowstart on page 4

ZnSlow

AgCllow

BeShigh


5.Indicate the solid with the least solubility.

PbSO4

ZnS

AgCl

BeS


5.Indicate the solid with the least solubility.

PbSO4lowstart on page 4

ZnSlow

AgCllow

BeShigh


5.Indicate the solid with the least solubility.

PbSO4lowstart on page 4

ZnSlowuse page 5 if required

AgCllow

BeShigh


5.Indicate the solid with the least solubility.

PbSO4low1.8 x 10-8start on page 4

ZnSlowuse page 5 if required

AgCllow

BeShigh


5.Indicate the solid with the least solubility.

PbSO4low1.8 x 10-8start on page 4

ZnSlow2.0 x 10-25use page 5 if required

AgCllow

BeShigh


5.Indicate the solid with the least solubility.

PbSO4low1.8 x 10-8start on page 4

ZnSlow2.0 x 10-25use page 5 if required

AgCllow1.8 x 10-10

BeShigh


5.Indicate the solid with the least solubility.

PbSO4low1.8 x 10-8start on page 4

ZnSlow2.0 x 10-25use page 5 if required

AgCllow1.8 x 10-10

BeShigh


6.How many of the following salts could produce a solution with a concentration more than 0.10 M?

Greater than 0.10 M means high solubility!

FeSO4

ZnSO4

Al2(SO4)3

Na2SO4


6.How many of the following salts could produce a solution with a concentration more than 0.10 M?

Greater than 0.10 M means high solubility!

FeSO4high

ZnSO4

Al2(SO4)3

Na2SO4


6.How many of the following salts could produce a solution with a concentration more than 0.10 M?

Greater than 0.10 M means high solubility!

FeSO4high

ZnSO4high

Al2(SO4)3

Na2SO4


6.How many of the following salts could produce a solution with a concentration more than 0.10 M?

Greater than 0.10 M means high solubility!

FeSO4high

ZnSO4high

Al2(SO4)3high

Na2SO4


6.How many of the following salts could produce a solution with a concentration more than 0.10 M?

Greater than 0.10 M means high solubility!

FeSO4high

ZnSO4high

Al2(SO4)3high

Na2SO4high


6.How many of the following salts could produce a solution with a concentration more than 0.10 M?

Greater than 0.10 M means high solubility!

FeSO4high

ZnSO4high

Al2(SO4)3high

Na2SO4highfour!


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]=


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles

1 L


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +1Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.Ksp


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.KspBa(OH)2⇌Ba2++2OH-


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.KspBa(OH)2⇌Ba2++2OH-

ss2s


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.KspBa(OH)2⇌Ba2++2OH-

ss2s

Ksp = [Ba2+][OH-]2


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.KspBa(OH)2⇌Ba2++2OH-

ss2s

Ksp = [Ba2+][OH-]2 = [s][2s]2


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.KspBa(OH)2⇌Ba2++2OH-

ss2s

Ksp = [Ba2+][OH-]2 = [s][2s]2 = 4s3


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.KspBa(OH)2⇌Ba2++2OH-

ss2s

Ksp = [Ba2+][OH-]2 = [s][2s]2 = 4s3

= 4(0.1091)3


7.40.00 mL of a saturated Ba(OH)2 solution is neutralized by adding 29.10 mL of 0.300 M HCl. Calculate the Ksp for Ba(OH)2.

A.Titration2HCl +Ba(OH)2

0.02910 L0.04000 L

0.300 M? M

[Ba(OH)2]= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2

1 L 2 moles HCl

0.0400 L

s=0.1091 M

B.KspBa(OH)2⇌Ba2++2OH-

ss2s

Ksp = [Ba2+][OH-]2 = [s][2s]2 = 4s3

= 4(0.1091)3 = 5.20 x 10-3


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