A solution \(X\), on mixing with \(AgNO _{3}\) solution, gives a white precipitate soluble in \(NH _{3}\). A solution \(Y\) when added to \(X\), also gives a white precipitate which is soluble on boiling. Solution \(Y\) contains
A. \(Ag ^{+}\) B. \(Pb ^{2+}\) C. \(Pb ^{4+}\) D. \(Zn ^{2+}\)
Correct Answer: B
Explanation
This is the test for chloride \(( Cl -)\).cidified \(AgNO _{3}\) solution is added to the test solution. A white precipitate of \(AgCl\), which is soluble in ammonia solution, indicates the presence of the ion. \(Ag _{(a q)}^{+}+ Cl _{(a) p)}^{-} \rightarrow AgCl _{(1)}\) \(AgCl _{( s )}+ NH _{3(20)} \rightleftharpoons\left[ Ag \left( NH _{3}\right)_{2}\right]+ Cl\) Therefore, \(X\) contains \(Cl\). When solution \(Y\) is added to \(X\), it gives a white precipitate which is soluble on boiling. This is characteristic of \(PbCl _{2}\) and so \(Y\) must contain \(Pb ^{2}\)
