Post on 13-Jan-2016
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Lesson 4Calculating
Molar Solubility From Ksp
1. Calculate the molar solubility @ 25oC for BaCrO4 in units of
g/L
BaCrO4(s) ⇌ Ba2+ + CrO42-
s s sKsp = [Ba2+][CrO4
2-]
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 10-3 moles L
2.584 x 10-3 moles x 413.2 gL 1 mole
2.584 x 10-3 moles x 413.2 g = 1.1 g/LL 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 10-11 moles 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 10-11 moles 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 10-11 moles 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
BeS high
5. Indicate the solid with the least solubility.
PbSO4
ZnS
AgCl
BeS
5. Indicate the solid with the least solubility.
PbSO4 low start on page 4
ZnS low
AgCl low
BeS high
5. Indicate the solid with the least solubility.
PbSO4 low start on page 4
ZnS low use page 5 if required
AgCl low
BeS high
5. Indicate the solid with the least solubility.
PbSO4 low 1.8 x 10-8 start on page 4
ZnS low use page 5 if required
AgCl low
BeS high
5. Indicate the solid with the least solubility.
PbSO4 low 1.8 x 10-8 start on page 4
ZnS low 2.0 x 10-25 use page 5 if required
AgCl low
BeS high
5. Indicate the solid with the least solubility.
PbSO4 low 1.8 x 10-8 start on page 4
ZnS low 2.0 x 10-25 use page 5 if required
AgCl low 1.8 x 10-10
BeS high
5. Indicate the solid with the least solubility.
PbSO4 low 1.8 x 10-8 start on page 4
ZnS low 2.0 x 10-25 use page 5 if required
AgCl low 1.8 x 10-10
BeS high
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
Na2SO4 high
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 high 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 L0.300 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 2sKsp = [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 L0.300 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 2sKsp = [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 L0.300 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 2sKsp = [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 L0.300 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 2sKsp = [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 L0.300 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 2sKsp = [Ba2+][OH-]2 = [s][2s]2 = 4s3
= 4(0.1091)3 = 5.20 x 10-3