Why is lead(II) present in two groups of cation analysis? [closed]
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Well, I found that lead cation $ce{Pb^2+}$ is present in both group 1 and group 2 of cation analysis. But why?
inorganic-chemistry analytical-chemistry
edited Jan 29 at 15:00
andselisk
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asked Jan 29 at 14:17
GarimaGarima
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closed as unclear what you're asking by Jon Custer, aventurin, Mithoron, Tyberius, airhuff Jan 29 at 20:11
Please clarify your specific problem or add additional details to highlight exactly what you need. As it's currently written, it’s hard to tell exactly what you're asking. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
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$begingroup$
Well, I found that lead cation $ce{Pb^2+}$ is present in both group 1 and group 2 of cation analysis. But why?
inorganic-chemistry analytical-chemistry
edited Jan 29 at 15:00
andselisk
17.7k656117
asked Jan 29 at 14:17
GarimaGarima
123
$endgroup$
closed as unclear what you're asking by Jon Custer, aventurin, Mithoron, Tyberius, airhuff Jan 29 at 20:11
Please clarify your specific problem or add additional details to highlight exactly what you need. As it's currently written, it’s hard to tell exactly what you're asking. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
add a comment |
$begingroup$
Well, I found that lead cation $ce{Pb^2+}$ is present in both group 1 and group 2 of cation analysis. But why?
inorganic-chemistry analytical-chemistry
edited Jan 29 at 15:00
andselisk
17.7k656117
asked Jan 29 at 14:17
GarimaGarima
123
$endgroup$
Well, I found that lead cation $ce{Pb^2+}$ is present in both group 1 and group 2 of cation analysis. But why?
inorganic-chemistry analytical-chemistry
inorganic-chemistry analytical-chemistry
edited Jan 29 at 15:00
andselisk
17.7k656117
asked Jan 29 at 14:17
GarimaGarima
123
edited Jan 29 at 15:00
andselisk
17.7k656117
asked Jan 29 at 14:17
GarimaGarima
123
edited Jan 29 at 15:00
andselisk
17.7k656117
edited Jan 29 at 15:00
andselisk
17.7k656117
edited Jan 29 at 15:00
andselisk
17.7k656117
17.7k656117
asked Jan 29 at 14:17
GarimaGarima
123
asked Jan 29 at 14:17
GarimaGarima
123
asked Jan 29 at 14:17
GarimaGarima
123
123
closed as unclear what you're asking by Jon Custer, aventurin, Mithoron, Tyberius, airhuff Jan 29 at 20:11
Please clarify your specific problem or add additional details to highlight exactly what you need. As it's currently written, it’s hard to tell exactly what you're asking. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
closed as unclear what you're asking by Jon Custer, aventurin, Mithoron, Tyberius, airhuff Jan 29 at 20:11
Please clarify your specific problem or add additional details to highlight exactly what you need. As it's currently written, it’s hard to tell exactly what you're asking. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
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1 Answer
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Simply because lead(II) fits both analytical groups:
- it forms lead(II) chloride $ce{PbCl2}$, a poor soluble chloride, which puts it in the 1st group;
- it also forms lead(II) sulfide $ce{PbS}$, insoluble in water and diluted acids, which also puts it in the 2nd group.
One reason for putting lead in both groups is that the chloride is somewhat of a borderline case in terms of being insoluble enough to appear in Group I. Group II represents a more complicated analysis but is more sensitive for lead.
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
$endgroup$
2
$begingroup$
Lead (II) chloride has enough solubility so it could slip through the cracks in Group I. Group II where the sulfide is precipitated is more sensitive.
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– Oscar Lanzi
Jan 29 at 15:46
1
$begingroup$
@OscarLanzi You are right, probably it would be worth adding that there are no sharp margins between these 6 groups and various sources add or remove cations from one group to another arbitrarily.
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– andselisk
Jan 29 at 15:49
add a comment |
1 Answer
1
active
oldest
votes
1 Answer
1
active
oldest
votes
active
oldest
votes
active
oldest
votes
$begingroup$
Simply because lead(II) fits both analytical groups:
- it forms lead(II) chloride $ce{PbCl2}$, a poor soluble chloride, which puts it in the 1st group;
- it also forms lead(II) sulfide $ce{PbS}$, insoluble in water and diluted acids, which also puts it in the 2nd group.
One reason for putting lead in both groups is that the chloride is somewhat of a borderline case in terms of being insoluble enough to appear in Group I. Group II represents a more complicated analysis but is more sensitive for lead.
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
$endgroup$
2
$begingroup$
Lead (II) chloride has enough solubility so it could slip through the cracks in Group I. Group II where the sulfide is precipitated is more sensitive.
$endgroup$
– Oscar Lanzi
Jan 29 at 15:46
1
$begingroup$
@OscarLanzi You are right, probably it would be worth adding that there are no sharp margins between these 6 groups and various sources add or remove cations from one group to another arbitrarily.
$endgroup$
– andselisk
Jan 29 at 15:49
add a comment |
$begingroup$
Simply because lead(II) fits both analytical groups:
- it forms lead(II) chloride $ce{PbCl2}$, a poor soluble chloride, which puts it in the 1st group;
- it also forms lead(II) sulfide $ce{PbS}$, insoluble in water and diluted acids, which also puts it in the 2nd group.
One reason for putting lead in both groups is that the chloride is somewhat of a borderline case in terms of being insoluble enough to appear in Group I. Group II represents a more complicated analysis but is more sensitive for lead.
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
$endgroup$
2
$begingroup$
Lead (II) chloride has enough solubility so it could slip through the cracks in Group I. Group II where the sulfide is precipitated is more sensitive.
$endgroup$
– Oscar Lanzi
Jan 29 at 15:46
1
$begingroup$
@OscarLanzi You are right, probably it would be worth adding that there are no sharp margins between these 6 groups and various sources add or remove cations from one group to another arbitrarily.
$endgroup$
– andselisk
Jan 29 at 15:49
add a comment |
$begingroup$
Simply because lead(II) fits both analytical groups:
- it forms lead(II) chloride $ce{PbCl2}$, a poor soluble chloride, which puts it in the 1st group;
- it also forms lead(II) sulfide $ce{PbS}$, insoluble in water and diluted acids, which also puts it in the 2nd group.
One reason for putting lead in both groups is that the chloride is somewhat of a borderline case in terms of being insoluble enough to appear in Group I. Group II represents a more complicated analysis but is more sensitive for lead.
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
$endgroup$
Simply because lead(II) fits both analytical groups:
- it forms lead(II) chloride $ce{PbCl2}$, a poor soluble chloride, which puts it in the 1st group;
- it also forms lead(II) sulfide $ce{PbS}$, insoluble in water and diluted acids, which also puts it in the 2nd group.
One reason for putting lead in both groups is that the chloride is somewhat of a borderline case in terms of being insoluble enough to appear in Group I. Group II represents a more complicated analysis but is more sensitive for lead.
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
edited Jan 29 at 16:03
Oscar Lanzi
15.7k12648
15.7k12648
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
answered Jan 29 at 14:59
andseliskandselisk
17.7k656117
17.7k656117
2
$begingroup$
Lead (II) chloride has enough solubility so it could slip through the cracks in Group I. Group II where the sulfide is precipitated is more sensitive.
$endgroup$
– Oscar Lanzi
Jan 29 at 15:46
1
$begingroup$
@OscarLanzi You are right, probably it would be worth adding that there are no sharp margins between these 6 groups and various sources add or remove cations from one group to another arbitrarily.
$endgroup$
– andselisk
Jan 29 at 15:49
add a comment |
2
$begingroup$
Lead (II) chloride has enough solubility so it could slip through the cracks in Group I. Group II where the sulfide is precipitated is more sensitive.
$endgroup$
– Oscar Lanzi
Jan 29 at 15:46
1
$begingroup$
@OscarLanzi You are right, probably it would be worth adding that there are no sharp margins between these 6 groups and various sources add or remove cations from one group to another arbitrarily.
$endgroup$
– andselisk
Jan 29 at 15:49
2
2
$begingroup$
Lead (II) chloride has enough solubility so it could slip through the cracks in Group I. Group II where the sulfide is precipitated is more sensitive.
$endgroup$
– Oscar Lanzi
Jan 29 at 15:46
$begingroup$
Lead (II) chloride has enough solubility so it could slip through the cracks in Group I. Group II where the sulfide is precipitated is more sensitive.
$endgroup$
– Oscar Lanzi
Jan 29 at 15:46
1
1
$begingroup$
@OscarLanzi You are right, probably it would be worth adding that there are no sharp margins between these 6 groups and various sources add or remove cations from one group to another arbitrarily.
$endgroup$
– andselisk
Jan 29 at 15:49
$begingroup$
@OscarLanzi You are right, probably it would be worth adding that there are no sharp margins between these 6 groups and various sources add or remove cations from one group to another arbitrarily.
$endgroup$
– andselisk
Jan 29 at 15:49
add a comment |
