The precipitate of AgCI dissolves in an excess of `NH_(3)` , KCN and `Na_(2)S_(2)O_(3)` solution respectively, producing complex ions represented by the following chemical formulae

Options

A. `[Ag (NH_(3))_(2)]^(+)` , `[Ag (CN)_(2)]^(-)` and `[Ag (S_(2)O_(3))_(2)]^(3-)`
B. `Ag . 2NH_(3)` , Ag . KCN and AgCI . `S_(2)O_(3)`
C. `[Ag (NH_(3))_(2)]^(2+)` , `[Ag (CN)_(2)]^(2-)` and `[Ag (S_(2)O_(3))_(2)]^(3-)`
D. `[Ag (NH_(3))_(2)]^(+)` , `[Ag (CN)_(2)]^(2-)` and `[Ag (S_(2)O_(3))_(2)]^(3-)`

Answer

A

Explanation

AgCl dissolves in dilute ammonia solution to give the dimmine silver (l) ion:
`AgCI (s) + 2NH_(3) (aq) rarr [Ag(NH_(3))_(2)]^(+) (aq) + Cl^(-) (aq)`
All the silver halides (including iodide) dissolve in thiosulphate and cyanide solutions giving thiosulphato and dicyano complexes of silver (l).
`Ag^(+) + 2S_(2) O_(3)^(2-) rarr [Ag(S_(2)O_(3))_(2)]^(3-)`

`Ag^(+) + 2CN^(-) rarr [Ag(CN)_(2)]^(-)`
`underset("Dicyanoargentate(l)ion")([N-=C-AgC-=N]^(-))`