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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- s s s 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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slide1

Lesson 4

Calculating

Molar Solubility

From Ksp

slide2

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

BaCrO4(s)⇌ Ba2+ + CrO42-

s s s

Ksp = [Ba2+][CrO42-]

Ksp = s2

from page 5 1.2 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

slide3

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

of g/L

Cu(IO3)2 ⇌ Cu2+ + 2IO3-

s s 2s

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!

slide7

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-

s s 3s

Ksp = [Fe3+][OH-]3

Ksp = [s][3s]3

2.6 x 10-39 = 27s4

s = 9.906 x 10-11 M

2.0 L

slide8

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-

s s 3s

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

slide9

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-

s s 3s

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

slide10

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-

s s 3s

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

slide11

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

slide12

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 start on page 4

ZnS

AgCl

BeS

slide13

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 low start on page 4

ZnS

AgCl

BeS

slide14

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 low start on page 4

ZnS low

AgCl

BeS

slide15

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 low start on page 4

ZnS low

AgCl low

BeS

slide16

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 low start on page 4

ZnS low

AgCl low

BeShigh

slide18

5. Indicate the solid with the least solubility.

PbSO4low start on page 4

ZnS low

AgCl low

BeShigh

slide19

5. Indicate the solid with the least solubility.

PbSO4low start on page 4

ZnS low use page 5 if required

AgCl low

BeShigh

slide20

5. Indicate the solid with the least solubility.

PbSO4low 1.8 x 10-8 start on page 4

ZnS low use page 5 if required

AgCl low

BeShigh

slide21

5. Indicate the solid with the least solubility.

PbSO4low 1.8 x 10-8 start on page 4

ZnS low 2.0 x 10-25use page 5 if required

AgCl low

BeShigh

slide22

5. Indicate the solid with the least solubility.

PbSO4low 1.8 x 10-8 start on page 4

ZnS low 2.0 x 10-25use page 5 if required

AgCl low 1.8 x 10-10

BeShigh

slide23

5. Indicate the solid with the least solubility.

PbSO4low 1.8 x 10-8 start on page 4

ZnS low 2.0 x 10-25use page 5 if required

AgCl low 1.8 x 10-10

BeShigh

slide24

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

slide25

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 high

ZnSO4

Al2(SO4)3

Na2SO4

slide26

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 high

ZnSO4 high

Al2(SO4)3

Na2SO4

slide27

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 high

ZnSO4 high

Al2(SO4)3 high

Na2SO4

slide28

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 high

ZnSO4 high

Al2(SO4)3 high

Na2SO4high

slide29

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 high

ZnSO4 high

Al2(SO4)3 high

Na2SO4high four!

slide30

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.

slide31

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. Titration 2HCl + Ba(OH)2

slide32

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 L

0.300 M? M

slide33

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 L

0.300 M? M

[Ba(OH)2] =

slide34

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 L

0.300 M? M

[Ba(OH)2] = 0.02910 L HCl

slide35

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 L

0.300 M? M

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

1 L

slide36

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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

slide37

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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

slide38

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. Titration 2HCl + 1Ba(OH)2

0.02910 L 0.04000 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

slide39

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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

slide40

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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 Ba(OH)2⇌ Ba2+ + 2OH-

slide41

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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 Ba(OH)2⇌ Ba2+ + 2OH-

s s 2s

slide42

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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 Ba(OH)2⇌ Ba2+ + 2OH-

s s 2s

Ksp = [Ba2+][OH-]2

slide43

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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 Ba(OH)2⇌ Ba2+ + 2OH-

s s 2s

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

slide44

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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 Ba(OH)2⇌ Ba2+ + 2OH-

s s 2s

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

slide45

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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 Ba(OH)2⇌ Ba2+ + 2OH-

s s 2s

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

= 4(0.1091)3

slide46

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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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 Ba(OH)2⇌ Ba2+ + 2OH-

s s 2s

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

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