Question

Consider the following isomers.
(i) $\left[Pt\right(N{H}_3{)}_{4}C{l}_2]B{r}_2$
(ii) $\left[Pt\right(N{H}_3{)}_{4}B{r}_2]C{l}_2$
(iii) $\left[Co\right(N{H}_3{)}_{4}C{l}_2]N{O}_2$
Which of the following observation is correct?

• A. (i) will give a pale yellow and (ii) will give a white precipitate with $AgN{O}_3$ solution.
• B. (iii) will give a white precipitate with $AgN{O}_3$ solution.
• C. (i),(ii) and (iii) will give white precipitate with $AgN{O}_3$ solution.
• D. None of the above isomers will give white precipitate with $AgN{O}_3$ solution.

Answer 1

Answer: (A)

(i) will give a pale yellow and (ii) will give a white precipitate with $AgN{O}_3$ solution.

(i) $\left[Pt\right(N{H}_3{)}_{4}C{l}_2]B{r}_2$ will dissociate in aqueous solution to produce $\left[Pt\right(N{H}_3{)}_{4}C{l}_2{]}^{2+}$ ions and bromide ions. Bromide ions reacts with silver nitrate ($AgN{O}_3$) to form pale yellow precipitate of silver bromide ($AgBr$).(ii) $\left[Pt\right(N{H}_3{)}_{4}B{r}_2]C{l}_2$ will dissociate in aqueous solution to produce $\left[Pt\right(N{H}_3{)}_{4}B{r}_2{]}^{2+}$ ions and chloride ions. Chloride ions reacts with silver nitrate to form white precipitate of silver chloride ($AgCl$).

(iii) $\left[Co\right(N{H}_3{)}_{4}C{l}_2]N{O}_2$ will dissociate in aqueous solution to produce $\left[Co\right(N{H}_3{)}_{4}C{l}_2{]}^{+}$ ions and nitrite ($N{O}_2^{-}$) ions. Nitirte ions do not form precipitate with silver nitrate.