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Chapter 34: Problem 18

Action of caustic soda on \(\mathrm{Al}(\mathrm{OH})_{3}\) gives a compound having formula (a) \(\mathrm{Al}_{2}(\mathrm{OH})_{4}\) (b) \(\mathrm{Na}_{3} \mathrm{AlO}_{3}\) (c) \(\mathrm{Na}_{2} \mathrm{Al}(\mathrm{OH})_{4}\) (d) \(\mathrm{NaAlO}_{2}\)

Short Answer

Expert verified
(c) \( \mathrm{Na}_{2} \mathrm{Al}(\mathrm{OH})_{4} \)

Step by step solution

01

Understand the Reactants

Caustic soda is the common name for sodium hydroxide (aOH]). The compound l(OH)_{3}] represents aluminum hydroxide.
02

Analyze the Reaction

When l(OH)_{3}] reacts with aOH], it forms a compound known as sodium aluminate. Aluminum hydroxide, being amphoteric, reacts with a base like sodium hydroxide.
03

Determine the Product Formula

The reaction between l(OH)_{3}] and excess aOH] forms a_{2}Al(OH)_{4}]. This is because the hydroxide ions from aOH] convert l(OH)_{3}] into aluminate ion, resulting in sodium aluminate.
04

Match with Provided Options

Among the options provided, a_{2}Al(OH)_{4}] corresponds to option (c). This is consistent with the reaction of aluminum hydroxide with an excess of caustic soda.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sodium Hydroxide
Sodium hydroxide, often referred to as caustic soda, is a widely used chemical compound. Its chemical formula is \( \text{NaOH} \), and it appears as a white solid. This compound is known for its strong alkaline properties. It easily dissolves in water to form a strongly basic solution. This makes it a powerful cleaning agent and a necessary reagent in several chemical processes.

Here are a few key points about sodium hydroxide:
  • It is a strong base and fully dissociates in water to form hydroxide ions \( \text{(OH}^- \text{)} \).
  • It has a high solubility in water, meaning that it can readily produce a solution when mixed.
  • Common uses include cleaning, manufacturing of soap, and various chemical preparations.
Sodium Aluminate
When sodium hydroxide reacts with aluminum hydroxide, a compound called sodium aluminate is formed. Its common formula is \( \text{Na}_2\text{Al(OH)}_4 \). This particular reaction highlights the nature of aluminum hydroxide reacting with bases, a process known as forming aluminates.

Here are crucial aspects of sodium aluminate:
  • It typically appears as a crystalline solid.
  • It involves the displacement of the hydroxide from sodium hydroxide with the aluminate ion.
  • This formation is due to the reaction of a strong base with an amphoteric compound.
These factors make sodium aluminate a valuable compound in water treatment and the paper industry. It acts as a coagulant, helping in the removal of impurities from water.
Amphoteric Nature
The term "amphoteric" refers to a substance's ability to react with both acids and bases. Aluminum hydroxide, \( \text{Al(OH)}_3 \), is a classic example of an amphoteric compound. This means it can react with both acids and bases, forming different products depending on the nature of the reactant.

Important points about amphoteric substances include:
  • They have dual chemical behavior, characterized by their ability to act either as acids or bases depending on the surrounding environment.
  • When reacting with an acid, \( \text{Al(OH)}_3 \) will typically form a salt and water.
  • When reacting with a base, it forms compounds like sodium aluminate, as in the discussed reaction with sodium hydroxide.
Understanding this nature helps recognize the unique place these substances hold in chemistry, highlighting their versatility in different chemical reactions.

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Most popular questions from this chapter

Which of the following reagents is used to identify acetic acid? (a) Tollen's reagent (b) Neutral \(\mathrm{FeCl}_{3}\) solution (c) Ceric ammonium nitrate (d) \(\mathrm{NaOH}\) and \(\mathrm{I}_{2}\)

Which of the following compounds is not colored yellow? (a) \(\mathrm{Zn}_{2}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (b) \(\mathrm{K}_{3}\left[\mathrm{Co}\left(\mathrm{NO}_{2}\right)_{6}\right]\) (c) \(\left(\mathrm{NH}_{4}\right)_{3}\left[\mathrm{AS}\left(\mathrm{Mo}_{3} \mathrm{O}_{10}\right)_{4}\right]\) (d) \(\mathrm{BaCrO}_{4}\)

Amount of oxalic acid present in a solution can be determined by its titration with \(\mathrm{KMnO}_{4}\) solution in the presence of \(\mathrm{H}_{2} \mathrm{SO}_{4} .\) The titration gives unsatisfactory result when carried out in the presence of \(\mathrm{HCl}\), because of (a) Gets oxidized by oxalic acid to chlorine (b) Furnishes \(\mathrm{H}^{+}\)ions in addition to those from oxalic acid (c) Reduces permanganate to \(\mathrm{Mn}^{2+}\) (d) Oxidises oxalic acid to carbon dioxide and water

Three separate samples of a solution of single salt gave these results. One formed a white precipitate with excess ammonia solution, one formed a white precipitate with dil. \(\mathrm{NaCl}\) and one formed a black precipitate with \(\mathrm{H}_{2} \mathrm{~S} .\) The salt could be (a) \(\mathrm{AgNO}_{3}\) (b) \(\mathrm{MnSO}_{4}\) (c) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) (d) \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}\)

A certain pale-green substance, \(X\) becomes dark brown on adding \(\mathrm{NaNO}_{2}\) in presence of dil. \(\mathrm{H}_{2} \mathrm{SO}_{4}\). its aqueous solution gives precipitates with (i) \(\mathrm{BaCl}_{2}\) and (ii) \(\mathrm{NaOH}\) in separate tests. The latter \(\mathrm{NaOH}\) in separate tests. The latter precipitate, Y, gradually changes colour from green to brown, on exposure to air. Identify X here? (a) \(\mathrm{NiSO}_{4}\) (b) \(\mathrm{FeSO}_{4}\) (c) \(\mathrm{ZnSO}_{4}\) (d) \(\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)
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