Question
In: Chemistry
A solution contains 0.036 M0.036 M Ag+Ag+ and 0.013 M0.013 M Pb2+.Pb2+. If you add Cl−,Cl−,...
A solution contains 0.036 M0.036 M Ag+Ag+ and 0.013 M0.013 M Pb2+.Pb2+. If you add Cl−,Cl−, AgClAgCl and PbCl2PbCl2 will begin to precipitate.
What is the concentration of Cl−Cl− required, in molarity, when AgClAgCl precipitation begins?
concentration of Cl−=Cl−=
M
What is the concentration of Cl−Cl− required, in molarity when AgClAgCl precipitation is 99.99% complete?
concentration of Cl−=Cl−=
M
What is the concentration of Cl−Cl− required, in molarity when PbCl2PbCl2 precipitation begins?
concentration of Cl−=Cl−=
M
What is the concentration of Cl−Cl− required, in molarity when PbCl2PbCl2 precipitation is 99.99% complete?
concentration of Cl−=Cl−=
M
Finally, give the Cl−Cl− concentration range in which Ag+Ag+ can be completely separated from Pb2+Pb2+ by precipitation.
Give the lowest Cl−Cl− concentration for the separation of Ag+Ag+ from Pb2+.Pb2+.
concentration of Cl−=Cl−=
M
Give the highest Cl−Cl− concentration for the separation of Ag+Ag+ from Pb2+.Pb2+.
concentration of Cl−=Cl−=
M
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
A solution contains 0.028 M Ag and 0.032 M Pb2 . If you add Cl–, AgCl...
A solution contains 0.028 M Ag and 0.032 M Pb2 . If you add Cl–,
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of Cl– required, in molarity, when:
A. AgCl precipitation begins?
B. AgCl precipitation is 99.99% complete?
C. PbCl2 precipitation begins?
D. PbCl2 precipitation is 99.99% complete?
Finally, give the concentration range of Cl– for the complete
precipitation of Ag and Pb2 .
E. Concentration of Cl– at the start of precipitation:
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A solution contains 0.041 M Ag and 0.047 M Pb2 . If you add Cl–, AgCl...
A solution contains 0.041 M Ag and 0.047 M Pb2 . If you add Cl–,
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A solution contains 0.040 M Hg22 and 0.032 M Pb2 . If you add
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B. Hg2Cl2 precipitation is 99.99% complete?
C. PbCl2 precipitation begins?
D. PbCl2 precipitation is 99.99% complete?
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A solution contains 0.026 M Hg2+2 and 0.019 M Pb2+. If you add Cl−, Hg2Cl2 and PbCl2...
A solution contains 0.026 M Hg2+2 and 0.019 M Pb2+.
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A) What is the concentration of Cl− required, in molarity, when
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B) What is the concentration of Cl− required, in molarity, when
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C) What is the concentration of Cl− required, in molarity, when
PbCl2 precipitation begins?
D) What is the concentration of Cl− required, in molarity, when
PbCl2 precipitation is 99.99% complete?...
A solution contains 0.040 M Hg2^2+ and 0.015 M Pb^2+ . If you add Cl–, Hg2Cl2...
A solution contains 0.040 M Hg2^2+ and 0.015 M Pb^2+ . If you
add Cl–, Hg2Cl2 and PbCl2 will begin to precipitate. What is the
concentration of Cl– required, in molarity, when
A. Hg2Cl2 precipitation begins?
B. Hg2Cl2 precipitation is 99.99% complete?
C. PbCl2 precipitation begins?
D. PbCl2 precipitation is 99.99% complete?
Finally, give the concentration range of Cl– for the complete
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A solution contains 0.0110 M Pb2 (aq) and 0.0110 M Sr2 (aq). If we add SO42–(aq),...
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Ca3(PO4)2
When the second cation just starts to precipitate, what
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1). A solution contains 0.0490 M Ca2+ and 0.0980 M Ag+. If solid Na3PO4 is added...
1). A solution contains 0.0490 M Ca2+ and 0.0980 M
Ag+. If solid Na3PO4 is added to
this mixture, which of the phosphate species would precipitate out
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(a). Ca3(PO4)2
(b). Ag3PO4
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precipitate, what percentage of the first cation remains in
solution?
percentage = ?%
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