- ANO
- BCl
- CSCN
- DCN
View written solutionFree
Correct answer: B, C, D
- Identify the equilibrium
The given equilibrium is the disproportionation of cuprous ion:
We are asked: in aqueous medium at , this equilibrium shifts towards the left in the presence of which ions.
Shifting left means stabilizing relative to .
- Use the idea of complex formation
If a ligand forms a stable complex with , then is removed from free solution and becomes more stable. By Le Chatelier's principle, this will oppose disproportionation and shift equilibrium to the left.
If a ligand instead stabilizes more strongly, the equilibrium would shift to the right.
So we examine which ligands preferentially stabilize .
- Nature of and
- is a soft acid.
- is relatively harder than .
According to HSAB principle:
- Soft ligands stabilize strongly.
- Hard ligands are less favorable for .
Now check each ligand.
- Option A:
is a weakly coordinating, relatively hard oxygen-donor ligand. It does not strongly stabilize .
So it does not shift the equilibrium to the left.
A is incorrect.
- Option B:
forms complexes such as with and helps stabilize cuprous ion in solution.
Thus becomes more stable, so the equilibrium shifts left.
B is correct.
- Option C:
is a soft/polarizable ligand and stabilizes effectively through complex formation.
Hence the equilibrium shifts towards the left.
C is correct.
- Option D:
forms very stable cuprous cyanide complexes such as , strongly stabilizing .
Therefore disproportionation is suppressed and equilibrium shifts left.
D is correct.
- Final derived answer
The ions that shift
towards the left are:
So the correct options are:
- Comparison with stored correct answer
Stored correct answer:
My derived answer:
They match.
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