Question

The dissolution of \[Al{(OH)_3}\] by a solution of NaOH results in the formation of:
A. \[{[Al{({H_2}O)_4}{(OH)_2}]^ + }\]
B. \[[Al{({H_2}O)_3}{(OH)_3}]\]
C. \[{[Al{({H_2}O)_2}{(OH)_4}]^ - }\]
D. \[[Al{({H_2}O)_6}{(OH)_3}]\]

Answer 1

Hint: In order to solve this question, we need to first identify the nature of both the reactants. The product that is formed is always dependent on the nature of the reactants and the conditions under which the reaction is carried out.

Complete Step-by-Step answer:
Before proceeding to the final chemical equation, let us first understand the reactants that are being used.
 \[Al{(OH)_3}\] is also commonly known as aluminium hydroxide. This compound is amphoteric in nature, which means that this compound exhibits both acidic as well as basic properties. Aluminium hydroxide is obtained from a mineral known as gibbsite.
NaOH on the other hand is known as Sodium hydroxide or caustic soda. It is a very strong base and exists in the form of a white solid.
When we dissolute Aluminium hydroxide in a solution of sodium hydroxide, the corresponding chemical reaction is as follows:
 \[Al{(OH)_3} + NaOH \to {[Al{({H_2}O)_2}{(OH)_4}]^ - }\]
Hence, the product obtained by dissolution of \[Al{(OH)_3}\] by a solution of NaOH is \[{[Al{({H_2}O)_2}{(OH)_4}]^ - }\] . The chemical name of this compound is diaqua tetrahydroxoaluminate ion.

Hence, Option C is the correct option

Note: Generally, the dissolution of \[Al{(OH)_3}\] by a solution of NaOH results in the formation of a compound named sodium aluminate and water. But the difference in the conditions in which the reactions are carried out result in the different results.