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When a metal rod $M$ is dipped into an aqueous colourless concentrated solution of compound $\mathrm{N}$, the solution turns light blue. Addition of aqueous $\mathrm{NaCl}$ to the blue solution gives a white precipitate $\mathrm{O}$. Addition of aqueous $\mathrm{NH}_3$ dissolves $\mathrm{O}$ and gives an intense blue solution.Question:
The final solution contains
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When a metal rod $M$ is dipped into an aqueous colourless concentrated solution of compound $\mathrm{N}$, the solution turns light blue. Addition of aqueous $\mathrm{NaCl}$ to the blue solution gives a white precipitate $\mathrm{O}$. Addition of aqueous $\mathrm{NH}_3$ dissolves $\mathrm{O}$ and gives an intense blue solution.Question:
The final solution contains
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$\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+}$and $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_4\right]^{2+}$
$\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+}$and $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_4\right]^{2+}$
Since in the beginning, concentrated $\mathrm{AgNO}_3$ solution was taken, some $\mathrm{AgNO}_3$ remain in solution which gives white precipitate of $\mathrm{AgCl}$ on addition of $\mathrm{NaCl}$. The precipitate finally dissolve in ammonia and $\mathrm{Cu}^{2+}$ present in solution also forms complex with ammonia as
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