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 chemistry graduate student is given 450. mL of a 0.50M methylamine (CH, NH,) solution. Methylamine is a weak base with K=4.4 x 10. What mass of
CH,NH, Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.96?
%3D
You may assume that the volume of the solution doesn't change when the CH,NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round it to
2 significant digits.
Explanation
Check
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1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?
A chemistry graduate student is given 500. mL of a 0.40M ammonia (NH,) solution. Ammonia is a weak base with
- 5
K=1.8 x 10 °. What mass of NH,Cl should the student dissolve in the NH, solution to turn it into a buffer with
9.
pH = 8.99?
You may assume that the volume of the solution doesn't change when the NH,Cl is dissolved in it. Be sure your answer has
4
a unit symbol, and round it to 2 significant digits.
x10
Principles of Chemistry: A Molecular Approach (3rd Edition)
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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