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# Lesson 4 Calculating Molar Solubility From Ksp - PowerPoint PPT Presentation

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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Calculating

Molar Solubility

From Ksp

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

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!

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-

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

PbSO4

ZnS

AgCl

BeS

PbSO4low start on page 4

ZnS low

AgCl low

BeShigh

PbSO4low start on page 4

ZnS low use page 5 if required

AgCl low

BeShigh

PbSO4low 1.8 x 10-8 start on page 4

ZnS low use page 5 if required

AgCl low

BeShigh

PbSO4low 1.8 x 10-8 start on page 4

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

AgCl low

BeShigh

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

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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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 with a concentration more than 0.10 M? 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