Transcript Document

Lesson 4
Calculating
Molar Solubility
From Ksp
1.
Calculate the molar solubility @ 25oC for BaCrO4 in units of
g/L
from page 5
BaCrO4(s)
s
Ksp =
⇌
Ksp
s2
=
Ba2+ +
s
[Ba2+][CrO42-]
1.2 x 10-10
=
s
1.1 x 10-5 M
=
s2
note that solubility units are M!
1.1 x 10-5 mole
L
x
253.3 g
1 mole
=
0.0028 g/L
CrO42s
2.
Calculate the molar solubility @ 25oC for Cu(IO3)2 in units
of g/L
Cu(IO3)2
⇌
s
Cu2+
+
s
Ksp
=
[Cu2+][IO3-]2
Ksp
=
[s][2s]2
Ksp
=
4s3
=
4s3
=
2.6 x 10-3 M
6.9 x 10-8
s
2IO3-
2s
note sig figs are 2 like the Ksp!
2.584 x 10-3 moles
L
2.584 x 10-3 moles
L
x
413.2 g
1 mole
2.584 x 10-3 moles
L
x
413.2 g
1 mole
=
1.1 g/L
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
⇌
s
+
s
3OH3s
Ksp
=
[Fe3+][OH-]3
Ksp
=
[s][3s]3
2.6 x 10-39
=
27s4
=
9.906 x 10-11 M
s
2.0 L
Fe3+
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
⇌
s
Fe3+
+
s
3OH-
3s
Ksp
=
[Fe3+][OH-]3
Ksp
=
[s][3s]3
2.6 x 10-39
=
27s4
=
9.906 x 10-11 M
s
2.0 L x 9.906 x 10-11 moles
1L
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
⇌
s
Fe3+
+
s
3OH-
3s
Ksp
=
[Fe3+][OH-]3
Ksp
=
[s][3s]3
2.6 x 10-39
=
27s4
=
9.906 x 10-11 M
s
2.0 L x 9.906 x 10-11 moles x 106.8 g
1L
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
⇌
s
Fe3+
+
s
3OH-
3s
Ksp
=
[Fe3+][OH-]3
Ksp
=
[s][3s]3
2.6 x 10-39
=
27s4
=
9.906 x 10-11 M
s
2.0 L x 9.906 x 10-11 moles x 106.8 g
1L
mole
= 2.1 x 10-8 g
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
ZnS
AgCl
BeS
start on page 4
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
low
start on page 4
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
ZnS
low
AgCl
BeS
start on page 4
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
ZnS
low
AgCl
low
BeS
start on page 4
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
ZnS
low
AgCl
low
BeS
high
start on page 4
5.
Indicate the solid with the least solubility.
PbSO4
ZnS
AgCl
BeS
5.
Indicate the solid with the least solubility.
PbSO4
low
ZnS
low
AgCl
low
BeS
high
start on page 4
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
ZnS
low
AgCl
low
BeS
high
1.8 x 10-8
start on page 4
use page 5 if required
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
ZnSO4
Al2(SO4)3
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
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
+
0.02910 L
0.300 M
Ba(OH)2
0.04000 L
?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
+
0.02910 L
0.300 M
[Ba(OH)2]
=
Ba(OH)2
0.04000 L
?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
+
0.02910 L
0.300 M
[Ba(OH)2]
= 0.02910 L HCl
Ba(OH)2
0.04000 L
?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
+
0.02910 L
0.300 M
[Ba(OH)2]
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles
1L
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
+
0.02910 L
0.300 M
[Ba(OH)2]
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
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
+
0.02910 L
0.300 M
[Ba(OH)2]
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
1Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
0.1091 M
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
0.1091 M
Ba(OH)2
s
⇌
Ba2+
s
+
2OH2s
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
0.1091 M
Ba(OH)2
s
= [Ba2+][OH-]2
⇌
Ba2+
s
+
2OH2s
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
0.1091 M
Ba(OH)2
⇌
s
= [Ba2+][OH-]2
= [s][2s]2
Ksp
Ba2+
s
+
2OH2s
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
0.1091 M
Ba(OH)2
⇌
Ba2+
s
s
= [Ba2+][OH-]2
= [s][2s]2 = 4s3
Ksp
+
2OH2s
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
0.1091 M
Ba(OH)2
⇌
Ba2+
s
s
= [Ba2+][OH-]2
= [s][2s]2 = 4s3
Ksp
= 4(0.1091)3
+
2OH2s
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
+
0.02910 L
0.300 M
[Ba(OH)2]
s
B.
Ksp
Ba(OH)2
0.04000 L
?M
= 0.02910 L HCl x 0.300 moles x 1 mole Ba(OH)2
1L
2 moles HCl
0.0400 L
=
0.1091 M
Ba(OH)2
⇌
Ba2+
s
s
= [Ba2+][OH-]2
= [s][2s]2 = 4s3
Ksp
= 4(0.1091)3
= 5.20 x 10-3
+
2OH2s