The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K s p for each of the slightly soluble solids indicated: (a) AgBr : [ Ag + ] = 5.7 × 10 − 7 M , [ Br − ] = 5.7 × 10 − 7 M (b) CaCO 3 : [ Ca 2 + ] = 5.3 × 10 − 3 M , [ CO 3 2 − ] = 9.0 × 10 − 7 M (c) PbF 2 : [ Pb 2 + ] = 2.1 × 10 − 3 M , [ F − ] = 4.2 × 10 − 3 M (d) Ag 2 CrO 4 : [ Ag + ] = 5.3 × 10 − 5 M , 3.2 × 10 − 3 M (e) InF 3 : [ In 3 + ] = 2.3 × 10 − 3 M , [ F − ] = 7.0 × 10 − 3 M
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K s p for each of the slightly soluble solids indicated: (a) AgBr : [ Ag + ] = 5.7 × 10 − 7 M , [ Br − ] = 5.7 × 10 − 7 M (b) CaCO 3 : [ Ca 2 + ] = 5.3 × 10 − 3 M , [ CO 3 2 − ] = 9.0 × 10 − 7 M (c) PbF 2 : [ Pb 2 + ] = 2.1 × 10 − 3 M , [ F − ] = 4.2 × 10 − 3 M (d) Ag 2 CrO 4 : [ Ag + ] = 5.3 × 10 − 5 M , 3.2 × 10 − 3 M (e) InF 3 : [ In 3 + ] = 2.3 × 10 − 3 M , [ F − ] = 7.0 × 10 − 3 M
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:
(a)
AgBr
:
[
Ag
+
]
=
5.7
×
10
−
7
M
,
[
Br
−
]
=
5.7
×
10
−
7
M
(b)
CaCO
3
:
[
Ca
2
+
]
=
5.3
×
10
−
3
M
,
[
CO
3
2
−
]
=
9.0
×
10
−
7
M
(c)
PbF
2
:
[
Pb
2
+
]
=
2.1
×
10
−
3
M
,
[
F
−
]
=
4.2
×
10
−
3
M
(d)
Ag
2
CrO
4
:
[
Ag
+
]
=
5.3
×
10
−
5
M
,
3.2
×
10
−
3
M
(e)
InF
3
:
[
In
3
+
]
=
2.3
×
10
−
3
M
,
[
F
−
]
=
7.0
×
10
−
3
M
The solubility equilibrium of iron(II) hydroxide is expressed as: Fe(OH)2 (s) ⇌ Fe2+(aq) + 2OH−(aq)
(A) Calculate the molar solubility of iron(II) hydroxide, Fe(OH)2, given that its Ksp is 12.0×10-16.
(B) Calculate the molar solubility of Fe(OH)2 in a 0.40 M solution of NaOH(aq).
show all of your work including the ICE Tables .
A buffer solution was prepared that contained 0.60 M hydrogen fluoride, HF (Ka = 7.2 x
104) and 1.00M potassium fluoride, KF. The total volume was 250 mL.
(a) What ions and molecules are present in the solution? List them in order of decreasing
concentration:
Decreasing order of Concentration
(b) What is the pH of the buffer solution described above?
(c) What is the pH of 100. mL of the buffer solution if you add 100. x 10-3 g of NaOH? Assume
negligible change in volume. (USEFUL INFORMATION: MM NaOH = 39.997 g mol-1)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell