Question:
Consider the following reactions
\[
Al(s)+HCl(aq)\rightarrow X+A\uparrow
\]
\[
Al(s)+NaOH(aq)\rightarrow Y+B\uparrow
\]
Which of the following is are correct?
I. Y is water soluble
II. X is not soluble in water
III. Both A and B are same
Consider the following reactions
\[
Al(s)+HCl(aq)\rightarrow X+A\uparrow
\]
\[
Al(s)+NaOH(aq)\rightarrow Y+B\uparrow
\]
Which of the following is are correct?
I. Y is water soluble
II. X is not soluble in water
III. Both A and B are same
Show Hint
Aluminium is amphoteric:
\[
Al + Acid \rightarrow Salt + H_2
\]
\[
Al + Base \rightarrow Aluminate + H_2
\]
Updated On: Jun 17, 2026
- I only
- I, III only
- II, III only
- I, II, III
Show Solution
Verified By Collegedunia
The Correct Option is B
Solution and Explanation
Concept:
Aluminium is amphoteric and reacts with both acids and bases.
Step 1: Reaction with hydrochloric acid.
\[ 2Al+6HCl \rightarrow 2AlCl_3+3H_2 \] Thus, \[ X=AlCl_3 \] and \[ A=H_2 \] Since aluminium chloride is soluble in water, statement II is false.
Step 2: Reaction with sodium hydroxide.
\[ 2Al+2NaOH+6H_2O \rightarrow 2Na[Al(OH)_4]+3H_2 \] Thus, \[ Y=Na[Al(OH)_4] \] which is soluble in water. Therefore statement I is true.
Step 3: Compare gases A and B.
Both reactions evolve \[ H_2 \] Hence statement III is also true.
Step 4: Final conclusion.
Statements I and III are correct. \[ \boxed{\text{I and III only}} \]
Step 1: Reaction with hydrochloric acid.
\[ 2Al+6HCl \rightarrow 2AlCl_3+3H_2 \] Thus, \[ X=AlCl_3 \] and \[ A=H_2 \] Since aluminium chloride is soluble in water, statement II is false.
Step 2: Reaction with sodium hydroxide.
\[ 2Al+2NaOH+6H_2O \rightarrow 2Na[Al(OH)_4]+3H_2 \] Thus, \[ Y=Na[Al(OH)_4] \] which is soluble in water. Therefore statement I is true.
Step 3: Compare gases A and B.
Both reactions evolve \[ H_2 \] Hence statement III is also true.
Step 4: Final conclusion.
Statements I and III are correct. \[ \boxed{\text{I and III only}} \]
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