Lesson 4 Calculating Molar Solubility From Ksp

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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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Lesson 4

Calculating

Molar Solubility

From Ksp

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

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!

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

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

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

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

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.

PbSO4 start 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.

PbSO4 low start 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.

PbSO4 low start on page 4

ZnS low

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.

PbSO4 low start on page 4

ZnS low

AgCl low

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.

PbSO4 low start on page 4

ZnS low

AgCl low

BeShigh

5. Indicate the solid with the least solubility.

PbSO4low start on page 4

ZnS low

AgCl low

BeShigh

5. Indicate the solid with the least solubility.

PbSO4low start on page 4

ZnS low use page 5 if required

AgCl low

BeShigh

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

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

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

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

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!

FeSO4 high

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!

FeSO4 high

ZnSO4 high

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!

FeSO4 high

ZnSO4 high

Al2(SO4)3 high

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!

FeSO4 high

ZnSO4 high

Al2(SO4)3 high

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!

FeSO4 high

ZnSO4 high

Al2(SO4)3 high

Na2SO4high four!

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. Titration 2HCl + 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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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. Titration 2HCl + Ba(OH)2

0.02910 L 0.04000 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. 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

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

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

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

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

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-

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

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

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

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

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

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