Which of the following will dissolve in excess of ammonia?

A g I

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A g B r

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A g C l

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N o n e o f t h e s e

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Solution

The correct option is C $A g C l$
Silver(I) chloride (AgCl), a white precipitate is insoluble in acids. It is very thermodynamically stable in ammonia solution. The $K_{s p}$ value of AgCl is very less. Despite the fact that silver chloride has a minuscule $K_{s p}$ value, some free ions are present in the solution. Addition of an excess of concentrated ammonia solution effectively consumes this free silver ion as ammonia, a good electron-pair donor ligand, combines with silver ion.

The reaction is as given below:

$A g C l + N H_{3} \to [A g (N H_{3})_{2}] + C l^{-}$

Hence, the correct option is (C).

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A g C l, A g B r, A g I, A g F

[I^{-}] = [B r^{-}] = [C l^{-}] = 0.2 M

A g C l

A g B r

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S a l t K_{s p} (m o l L^{- 1})^{2}

A g C l 1.8 \times 10^{- 10}

A g B r 5 \times 10^{- 13}

A g I 8.3 \times 10^{- 17}

K_{s p} (A g C l) > K_{s p} (A g B r) > K_{s p} (A g I)

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