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Chapter 10: Problem 84

Which of the following is only acidic in nature? (a) \(\mathrm{B}(\mathrm{OH})_{3}\) (b) \(\mathrm{Al}(\mathrm{OH})_{3}\) (c) \(\mathrm{Be}(\mathrm{OH})_{2}\) (d) \(\mathrm{Mg}(\mathrm{OH})_{2}\)

Short Answer

Expert verified
The correct answer is (a) \(\mathrm{B} (\mathrm{OH})_3\).

Step by step solution

01

Understanding the Nature of Hydroxides

Hydroxide compounds can exhibit acidic, basic, or amphoteric behavior. Acidic hydroxides are Lewis acids and release protons, whereas basic ones can accept protons. Amphoteric hydroxides can act either as acids or bases depending on the environment.
02

Analyze the Options

Let's identify the nature of each compound: - (a) \(\mathrm{B} (\mathrm{OH})_3\) is known to be acidic. - (b) \(\mathrm{Al} (\mathrm{OH})_3\) is amphoteric, meaning it can behave as both an acid and a base.- (c) \(\mathrm{Be} (\mathrm{OH})_2\) is also amphoteric.- (d) \(\mathrm{Mg} (\mathrm{OH})_2\) is basic.
03

Identifying the Correct Answer

From the analysis in Step 2, only \(\mathrm{B} (\mathrm{OH})_3\) behaves purely as an acidic compound, while others show either basic or amphoteric characteristics.

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Key Concepts

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

Lewis acids
Lewis acids are molecules or ions that can accept an electron pair from a Lewis base. This makes them electron pair acceptors, which is distinct from the traditional Br酶nsted-Lowry definition where acids donate protons. Understanding Lewis acids helps us identify substances that can participate in complex chemical reactions.
  • For example, \(\mathrm{B} (\mathrm{OH})_3\) is a classic Lewis acid. It can accept an electron pair because it lacks a complete set of valence electrons and is electron deficient. It accepts electrons from molecules that can donate a pair, typically in reactions like hydrolysis, leading to acidic solutions.
The Lewis acid behavior of \(\mathrm{B} (\mathrm{OH})_3\) makes it exclusively acidic compared to some other compounds which can exhibit multiple behaviors depending on the conditions.
Amphoteric hydroxides
Amphoteric hydroxides possess an intriguing ability to act as both acids and bases, depending on the chemical environment. This dual behavior happens because they can either donate or accept protons, or even donate or accept electron pairs, similar to the concept of Lewis acids and bases.Consider \(\mathrm{Al} (\mathrm{OH})_3\) and \(\mathrm{Be} (\mathrm{OH})_2\):
  • \(\mathrm{Al} (\mathrm{OH})_3\) will act as a base when reacting with strong acids but will behave as an acid in the presence of strong bases. This occurs because the molecule can donate hydroxide ions to acids or accept hydrogen ions in basic conditions.
  • Likewise, \(\mathrm{Be} (\mathrm{OH})_2\) will show similar versatile behavior in different environments. This dual nature makes them valuable in chemical reactions where a change in pH or environment can completely change their behavior.
Such properties also make them essential in various industrial and chemical processes.
Basic hydroxides
Basic hydroxides, such as \(\mathrm{Mg} (\mathrm{OH})_2\), feature the opposite characteristics of acidic hydroxides. These hydroxides are capable of accepting protons, which makes them bases in the Br酶nsted-Lowry sense. This property allows them to neutralize acids effectively. Here's how these basic hydroxides behave:
  • For example, \(\mathrm{Mg} (\mathrm{OH})_2\) commonly acts as a weak base. In an aqueous environment, it can dissociate to form magnesium ions and hydroxide ions, the latter of which can readily combine with hydrogen ions to form water, effectively reducing the acidity of solutions.This is why magnesium hydroxide is widely used as an antacid to relieve indigestion by neutralizing stomach acids.
Understanding the base character of substances like \(\mathrm{Mg} (\mathrm{OH})_2\) is crucial in applications ranging from medicine to industrial processing.

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Most popular questions from this chapter

Which of the following is an electron deficient compound? (a) \(\mathrm{NaCl}\) (b) \(\mathrm{B}_{2} \mathrm{H}_{6}\) (c) \(\mathrm{KCl}\) (d) \(\mathrm{NaH}\)

Boric acid is polymeric due to (a) Its geometry (b) Its presence of hydrogen bonds (c) Its acidic nature (d) Its monobasic nature

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The incorrect statement regarding Aluminium \& Thallium: (1) Tl is more electropositive than Al. (2) \(\mathrm{Al}\) is more electropositive than Thallium. (3) \(\mathrm{Tl}^{+3}\) is more stable than \(\mathrm{Al}^{+}\). (4) \(\mathrm{Tl}^{+3}\) is a powerful reducing agent. (a) \(1,2,3\) (b) \(1,3,4\) (c) \(2,3,4\) (d) 1,4

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