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Chapter 7: Problem 27

The ionization constant of a base is \(\frac{1}{10} .\) The base is described as (1) Normal base (2) Strong basc (3) Weak base (4) None of these

Short Answer

Expert verified
Option (3) Weak base

Step by step solution

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01

- Understanding the ionization constant

The ionization constant (also known as the base dissociation constant) is a measure of the strength of a base in solution. It tells us how well the base dissociates into its ions in water.
02

- Analyze the given value

In this problem, the ionization constant of the base is given as \(\frac{1}{10}\) which is equal to 0.1.
03

- Determine the strength of the base

A strong base typically has a high ionization constant, close to 1 or above. A weak base has a low ionization constant, usually much less than 1. Given that 0.1 is much less than 1, this base is considered weak.
04

- Choose the correct option

Based on the information, the base with an ionization constant of 0.1 is classified as a weak base. Therefore, the correct option is (3) Weak base.

Key Concepts

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

base dissociation constant
The base dissociation constant (often represented as Kb) helps us understand how well a base ionizes in water. When a base dissolves in water, it splits into ions. The base dissociation constant measures the extent of this ionization.

For example, when ammonia (NH\textsubscript{3}) dissolves in water, it partially turns into ammonium (\text{NH\textsubscript{4}\textsuperscript{+}}) and hydroxide ions (\text{OH\textsuperscript{-}}). The formula for the base dissociation constant is:

\[ K_b = \frac{[\text{products}]}{[\text{reactants}]} \]
Replacing 'products' and 'reactants' with the actual concentrations, for ammonia it would be:

\[ K_b = \frac{[\text{NH\textsubscript{4}\textsuperscript{+}}] [\text{OH\textsuperscript{-}}]}{[\text{NH\textsubscript{3}}]} \]
A high Kb value indicates a strong base, as it ionizes completely in water. Conversely, a low Kb value shows a weak base, meaning only a small fraction of the base ionizes in water.
acid-base strength
Understanding the strength of acids and bases is crucial for their identification and use. For bases, the strength is determined by their ionization in water.

  • Strong Bases: These are bases that ionize almost completely in water. They have a high Kb value, often close to or greater than 1.
  • Weak Bases: These bases only partially ionize in water. They have a much lower Kb value, usually significantly less than 1.

Why does this matter? Strong bases, like sodium hydroxide (NaOH), are very effective at increasing the pH of solutions. They can be used in processes requiring high pH levels.

Weak bases, such as ammonia (NH3), are less aggressive but very useful when a milder effect is needed. It's essential to know whether a base is strong or weak before using it in chemical reactions or processes.
weak base
A weak base is a substance that only partially ionizes in water. This means that, even when a weak base is present in water, only a small percentage of its molecules dissociate to form ions. The rest of the base exists in its original form.

Common examples of weak bases include:
  • Ammonia (NH3)
  • Pyridine (C5H5N)
  • Ammonium Hydroxide (NH4OH)

Weak bases have a relatively low Kb value, indicating their limited ionization. For instance, the Kb for ammonia is approximately 1.8 x 10^-5, which is much less than 1, showing it is a weak base.

When solving problems involving weak bases, always consider the ionization constant. Combined with the concentration of the base, this will help determine the degree of ionization and the resulting pH of the solution.

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Most popular questions from this chapter

The phenomenon of interaction of anions and cations furnished by clectrolyte with \(\mathrm{II}^{+}\) and OIT - ions of water to producc acidic nature or alkalinity is known as hydrolysis. In hydrolysis(1) The \(\mathrm{pH}\) may either increase or decrease (2) All the salts (except those made up with strong acid and base) undergo hydrolysis (3) The variation of \(\mathrm{pH}\) depends upon the nature of salt as well as on the temperature (4) All

Which of the following statements is wrong? (1) for an acid buffer solution the \(\mathrm{pH}\) can be increased by inereasing the concentration of salt (2) for a basic buffer solution the pH can increased by decreasing the concentration of base(3) buffer capacity of a buffer solution is maximum when the ratio of salt/acid or base is 1 (4) the number of moles of acid or base required by one litre of buffer solution to alter its \(\mathrm{pH}\) by one unit is called buffer efficiency

Which cquilibrium can be described as Lcwis acid basc reaction but not Bronsted acid basc reaction? (1) \(\mathrm{H}_{2} \mathrm{O}+\mathrm{CH}_{3} \mathrm{COOH} \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3} \mathrm{COO}^{-}\) (2) \(2 \mathrm{NH}_{3}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{NH}_{4}^{+}+\mathrm{SO}_{4}^{2-}\) (3) \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{NH}_{3} \rightarrow \mathrm{CH}_{3} \mathrm{COONH}_{4}\) (4) \(\left[\mathrm{Cu}\left(\mathrm{II}_{2} \mathrm{O}\right)_{4}\right]^{21}+4 \mathrm{NII}_{3} \rightarrow\left[\mathrm{Cu}\left(\mathrm{NII}_{3}\right)_{4}\right]^{2}+4 \mathrm{II}_{2} \mathrm{O}\)

Sodium carbonate cannot be used in place of ammonium carbonate for the identification of the fifth group radicals. This is because the (1) sodium ions will interfere in the detection of the fifth group radicals (2) concentration of carbonate ions is very low (3) sodium will react with acidic radicals (4) magnesium will be precipitated

The equilibrium constant for the formation of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) from the elements is extremely large and that for the formation of \(\mathrm{NO}(\mathrm{g})\) from its elements is very small. This implies that (1) \(\mathrm{H}_{2} \mathrm{O}\) has a tendency to decompose into its elements. (2) NO has low tendency to decompose into its elements. (3) NO has appreciable tendency to decompose into its elements. (4) NO cannot be produced from direct reaction between nitrogen and oxygen.
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