Weak Bases

Weak bases are basic compounds that when dissolved in liquids do not entirely break down into their constituent ions. As a result, when the weak base is dissolved in a solution, some of it dissociates into hydroxide anions and the corresponding conjugate acid, while the rest stays undissociated inside the solution.

Ionization of a weak base is a form of equilibrium process in which a chemical equilibrium between the concentration of the undissociated base and its constituent ions is achieved inside the solution (the conjugate acid and the hydroxide anion). It’s vital to remember that a weak base’s conjugate acid is usually always a weak acid. Similarly, the conjugate base of a weak acid will act as a weak base.

When a weak base is dissolved in water, the following type of equilibrium arises:

B + H₂O ⇌ BH⁺ + OH^–

A lone pair of electrons in the basic molecule absorbs a proton from the water molecule in this equilibrium process, resulting in the creation of a hydroxide ion. The weaker the base, the greater the concentration of the equilibrium to the left. Similarly, the stronger the base, the higher the equilibrium concentration to the right.

Examples of Weak Bases

Some Examples of the Weak Bases are,

• Ammonia (NH₃)
• Trimethylamine (N(CH₃)₃)
• Pyridine (C₅H₅N)

Summary of Strong and Weak Bases

• The base that ionizes completely in an aqueous solution are called the Strong Base.
• The base that ionizes partially in an aqueous solution are called the Weak Base.
• Conjugate base of a strong acid is a weak base.
• Conjugate base of a weak acid is a strong base.

Read More,

• Acid, Base and Salts
• Chemical Indicator
• Neutralization Reaction

The citric acid in fruits like oranges and lemons, tartaric acid in tamarind, malic acid in apples, lactic acid in milk and milk products, and hydrochloric acid in gastric juices are just a few examples of acids and bases found in nature. Many bases, such as lime water, can also be found. Many of these acids are used in our daily lives, such as vinegar or acetic acid in the kitchen, boric acid in laundry, baking soda in cooking, washing soda in cleaning, and so on.

Many acids and bases that we do not use in our daily lives are utilised in laboratories and industries, such as HCl, H₂SO₄, and NaOH, KOH, among others. The neutralisation process results in the creation of salt and water when these acids and bases are mixed in the proper quantities.