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| how do you precipitate the group II cations? |
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| what is the source of S2- (sulfide ion) that we use to precipitate the group II cations? |
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| what is the difference between HCl and H2S re: their behaviors in water? |
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| HCl is very soluble; H2S is very INsoluble. |
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| what might happen if the group II solution is too acidic before adding H2S? |
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Definition
| sulfide ion concentration might be too low to precipitate all the group II cations |
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| the reason that cadmium sulfide dissolves in 3M HCl is |
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Definition
| the Cl- and the Cd2+ form a complex ion which enables the CdS <--> Cd2+ + S2- equilibrium to move forward |
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Term
a group II sulfide that is soluble in a strong base is: ______
by what process does it dissolve? |
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Definition
SnS2
- dissolves by complex ion formation |
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| how can you tell whether a solid is Bi2S3 or CdS? |
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| observe - Bi2S3 is black; CdS is yellow-orange. |
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| how do you tell whether a solid is CuS or Bi2S3? |
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Definition
| dissolve in HNO3. CuS will be blue. |
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| net ionic equation: tin(IV) nitrite is treated with H2S |
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Definition
| Sn4+(aq)+2S2-(aq) --> SnS2(s) |
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| net ionic equation: excess ammonia reacts with copper(II) ion solution |
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Definition
| Cu2+ + 4NH3 <--> Cu[(NH3)4]2+ |
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| net ionic equation: bismuth sulfide dissolves in nitric acid solution |
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Definition
| Bi2S3(s) + 2NO3- + 8H3O --> 3S(s) + 2NO + 12H2O +2Bi3+ |
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| the net ionic equations of Cd2+, Cu2+, Bi3+, and Sn4+ reacting with H2S |
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Definition
Cd2+ + S2- --> CdS (s)
Cu2+ + S2- --> CuS (s)
Bi3+ + S2- --> Bi2S3 (s)
Sn4+ + S2- --> SnS2(s)
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