Consider the following equilibrium
\(\mathrm{AgCl}\downarrow + 2\mathrm{NH_3} \rightleftharpoons [\mathrm{Ag(NH_3)_2}]^+ + \mathrm{Cl^-}\)
White precipitate of AgCl appears on adding which of the following?
\(\mathrm{AgCl}\downarrow + 2\mathrm{NH_3} \rightleftharpoons [\mathrm{Ag(NH_3)_2}]^+ + \mathrm{Cl^-}\)
White precipitate of AgCl appears on adding which of the following?
Show Hint
- \(\mathrm{NH_3}\)
- aqueous \(\mathrm{NaCl}\)
- aqueous \(\mathrm{HNO_3}\)
- aqueous \(\mathrm{NH_4Cl}\)
The Correct Option is C
Solution and Explanation
Adding \(\mathrm{NH_3}\) shifts it right (dissolves AgCl) - not (1).
\(\mathrm{HNO_3}\) reacts with free ammonia: \(\mathrm{NH_3} + \mathrm{H^+} \rightarrow \mathrm{NH_4^+}\). Removal of \(\mathrm{NH_3}\) shifts the equilibrium left, the complex decomposes and white AgCl precipitates.
This is the standard test: acidifying an ammoniacal silver chloride solution with nitric acid reprecipitates AgCl.
Answer: (3) aqueous HNO3
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