Answer:
Since, (X)
dissolves in \[NaOH\]solution and gives a white precipitate which dissolves in
excess of \[NaOH\]form soluble complex. (X) must be aluminium metal and (A)
must be aluminium hydroxide, \[Al{{(OH)}_{3}}\].
\[Al{{(OH)}_{3}}\]dissolves in excess of \[NaOH\]form (B)
which is sodium tetrahydroxoaluminate White ppt.
\[Al+2NaOH+2{{H}_{2}}O\to 2NaAl{{O}_{2}}+3{{H}_{2}}\]
\[NaAl{{O}_{2}}+2{{H}_{2}}O\rightleftharpoons
\underset{\begin{smallmatrix}
(A) \\
White\,ppt.
\end{smallmatrix}}{\mathop{Al{{(OH)}_{3}}}}\,+NaOH\]
\[Al{{(OH)}_{3}}+NaOH\to
\underset{\text{Soluble}\,\text{complex}}{\mathop{Na[Al{{(OH)}_{4}}]}}\,\]
(A) dissolves in dilute \[HCl\] to form \[AlC{{l}_{3}}\]
(C)
\[Al{{(OH)}_{3}}+3HCl\to
\underset{(C)}{\mathop{AlC{{l}_{3}}}}\,+3{{H}_{2}}O\]
(A) when heated strongly forms \[A{{l}_{2}}{{O}_{3}}\]which
is used for the extraction of aluminium metal.
\[2Al{{(OH)}_{3}}\xrightarrow{Heat}\underset{(D)}{\mathop{A{{l}_{2}}{{O}_{3}}}}\,+3{{H}_{2}}O\]
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