Which anion could be used to selectively remove silver ions?

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Discussion Overview

The discussion centers on identifying which anion—Cl, SO4, or CO3—could be used to selectively remove silver ions from a solution. Participants explore the implications of precipitate formation and the selectivity of the anions in the context of other potential cations present in the solution.

Discussion Character

  • Exploratory, Technical explanation, Debate/contested

Main Points Raised

  • One participant questions the presence of other cations in the solution, suggesting that the chosen anion must not precipitate those ions alongside silver.
  • Another participant raises the consideration of the molar concentration of Ag+ in the saturated solution for each potential precipitate, implying that this could influence the effectiveness of the anion.
  • Reference is made to solubility rules, indicating that transition metals are generally insoluble unless paired with a soluble anion, although this is reiterated without additional context.
  • A participant seeks clarification on what constitutes "soluble" anions, indicating a need for further exploration of the definitions involved.

Areas of Agreement / Disagreement

Participants express differing views on the criteria for selecting an anion, particularly regarding the presence of other cations and the implications of solubility rules. The discussion remains unresolved with multiple competing considerations.

Contextual Notes

There are limitations regarding the assumptions about the solution's composition and the specific definitions of solubility that are not fully addressed.

HHH
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The question is, which anion could be used to selectively remove silver ions from solution? The options are Cl, SO4, or CO3.

All 3 of them form precipitates, but is there any that is better than the others?
 
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Do you know what other cations are present in the solution? If you're trying to selectively precipitate silver ions, it is important that the salt you add does not also precipitate other ions.
 
Another thing to consider: for which of the three potential precipitates molar concentration of Ag+ in the saturated solution is the lowest?
 
Check your solubility rules and that should guide you. Transition metals are generally insoluble unless paired with another anion which is soluble.
 
brake4country said:
Transition metals are generally insoluble unless paired with another anion which is soluble.

And what are "soluble" anions?
 

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