what must be the concentration of aqueous of `NH_(3)` which must be added to a solution containing `4xx10^(-3)M Ag^(+)` and `0.001M NaCl` to prevent t

Question

what must be the concentration of aqueous of `NH_(3)` which must be added to a solution containing `4xx10^(-3)M Ag^(+)` and `0.001M NaCl` to prevent t

what must be the concentration of aqueous of `NH_(3)` which must be added to a solution containing `4xx10^(-3)M Ag^(+)` and `0.001M NaCl` to prevent the precipitaion of `AgCl`.

Monjur Alahi

4 views

2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

Silver ion concentration which can be allowed to remain in the solutions
`1.8xx10^(-10)=[Ag^(+)][CI^(-)]`
`[Ag^(+)]=(1.8xx10^(-10))/(0.01)=1.8xx10^(-7)M`
This quantity is so small that almost all the `Ag^(+)` ion will be consumed by `NH(3)` in complex formation.
`{:(,Ag^(+)+,2NH_(3)hArr,[Ag(NH_(3))_(2),]^(+),K=(10^(8))/(6)),(t=0,4xx10^(-3),b,0,),(at eq,1.8xx10^(-7),(b-8xx10^(-3)),4xx10^(-3),):}`