A white prccipirarc of A g C l dissolves in cxcess of (J) NFI3(Aq) (II) Na2 S2 O3 (III) NaCN (a

step 1 As we know that the white precipitate of silver chloride dissolved in excess of ammonia, hypo so

A white prccipirarc of A g C l dissolves in cxcess of (J)...

A white prccipirarc of $A g C l$ dissolves in cxcess of
(J) $\mathrm{NFI}_{3}(\mathrm{Aq})$
(II) $\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}$
(III) $\mathrm{NaCN}$
(a) I only
(b) IJ J only
(c) I, II and III
(d) I and II

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Key Concepts

Complex Ion Formation

This concept involves the formation of complex ions when a metal ion binds with one or more ligands. In many cases, sparingly soluble salts can dissolve in solutions that provide ligands capable of forming stable complexes with the metal ion, effectively reducing the concentration of the free metal ion and shifting the equilibrium toward dissolution.

Solubility Equilibria

Solubility equilibria govern the balance between an insoluble salt and its ions in solution. When a complexing agent is added, it reacts with one of the ions, lowering its concentration and thereby shifting the equilibrium to dissolve more of the salt. This principle underlies the increased solubility of many slightly soluble compounds in the presence of appropriate ligands.

Coordination Chemistry

Coordination chemistry studies the structures and properties of complexes formed between metal ions and ligands. The nature of the ligands, such as ammonia, thiosulfate, or cyanide, and their ability to coordinate to a metal ion, plays a critical role in the stability and solubility of the resulting complex. This field explains why certain reagents can dissolve otherwise insoluble compounds by forming strongly bound complexes.

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