Calculate the concentration of Pb 2+ in each of the following. a. a saturated solution of Pb(OH) 2 , K sp = 1.2 × 10 −15 b. a saturated solution of Pb(OH) 2 buffered at pH = 13.00 c. Ethylenediaminetetraacetate (EDTA 4− ) is used as a complexing agent in chemical analysis and has the following structure: Solutions of EDTA 4− are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The reaction of EDTA 4− with Pb 2+ is Pb 2 + ( a q ) + E D T A 4 − ( a q ) ⇌ P b E D T A 2 − ( a q ) K = 1.1 × 10 18 Consider a solution with 0.010 mole of Pb(NO 3 ) 2 added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na 4 .EDTA. Does Pb(OH) 2 precipitate from this solution?
Calculate the concentration of Pb 2+ in each of the following. a. a saturated solution of Pb(OH) 2 , K sp = 1.2 × 10 −15 b. a saturated solution of Pb(OH) 2 buffered at pH = 13.00 c. Ethylenediaminetetraacetate (EDTA 4− ) is used as a complexing agent in chemical analysis and has the following structure: Solutions of EDTA 4− are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The reaction of EDTA 4− with Pb 2+ is Pb 2 + ( a q ) + E D T A 4 − ( a q ) ⇌ P b E D T A 2 − ( a q ) K = 1.1 × 10 18 Consider a solution with 0.010 mole of Pb(NO 3 ) 2 added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na 4 .EDTA. Does Pb(OH) 2 precipitate from this solution?
Solution Summary: The author explains that the concentration of PbText2+ is to be calculated in each of the given cases.
Calculate the concentration of Pb2+ in each of the following.
a. a saturated solution of Pb(OH)2, Ksp = 1.2 × 10−15
b. a saturated solution of Pb(OH)2 buffered at pH = 13.00
c. Ethylenediaminetetraacetate (EDTA4−) is used as a complexing agent in chemical analysis and has the following structure:
Solutions of EDTA4− are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The reaction of EDTA4− with Pb2+ is
Pb
2
+
(
a
q
)
+
E
D
T
A
4
−
(
a
q
)
⇌
P
b
E
D
T
A
2
−
(
a
q
)
K
=
1.1
×
10
18
Consider a solution with 0.010 mole of Pb(NO3)2 added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na4.EDTA. Does Pb(OH)2 precipitate from this solution?
a. The change in the Gibbs energy of a certain constant pressure process is found to fit the expression:
AG-85.1 J mol −1 +36.5 J mol ¹K-1 × T
A. Calculate the value of AS for the process.
B. Next, use the Gibbs-Helmholtz equation:
(a(AG/T))
ΔΗ
-
T2
to calculate the value of AH for the process.
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