Properties of Bases

Did you know that most items we use are basic? Everything, from the soap to our toothbrush, is basic. When these basic products contact our body, they cause an alkalising reaction. Some properties of bases are common, like the bitter taste. They are also slippery. Furthermore, as bases are made up of charged particles, they conduct electricity when dissolved in water. 

In this article, you will learn more about the general properties of bases.

What are bases?

Based on chemical definitions, a base is any molecule or ion that takes protons. The OH- ion is considered to be a base. Alkali is the word used to describe dissolved bases in water when present in solution. If you take a sodium hydroxide (NaOH) solution in water, you will see that the ions Na+ and OH– separate after they have dissolved. As a result, alkali hydroxide (OH–) is present in the solution, making the solution a base.

Types of Bases:

Acidity, concentration, and degree of ionisation are three factors that may differentiate between different types of bases.

Based on their acidity, the following types of bases exist:

A base’s acidity is defined by the number of hydroxyl ions in the solution. Based on their acidity, bases are categorised into three groups: acid, basic, and essential acid.

1. Monoacidic Base.
2. Diacidic Base.
3. Triacidic Base.

• Monoacidic bases contain just one hydroxyl ion and interact with only one hydrogen ion. They are also known as monoacidic bases. NaOH, KOH, and other mono acidic bases are such compounds.

• Diacidic: A base containing two hydroxyl ions that interact with two hydrogen ions is a di acidic base. Ca(OH)2 & Mg(OH)2  are di acidic base compounds.

• Inorganic triacidic base is an acid-containing three hydroxyl ions and three hydrogen ions in equal proportion. Al(OH)3, Fe(OH)2, and other triacidic bases are examples of such compounds.

Types of bases classified according to their degree of ionisation include:

Bases in solution may be classified according to the degree of ionisation. It is often referred to as “basic strength.” When dissolved in water, it releases a small number of hydroxyl ions into the solution. Two kinds of bases may be distinguished based on their degree of ionisation.

Bases that are strong and bases that are weak:

Strong: A strong base dissociates completely or significantly when exposed to water. Consider the examples of NaOH, KOH, and other similar compounds.

Weak: A weak base is one that either does not dissolve completely or only dissociates to a very small degree when exposed to water. Example: NH4OH and several similar compounds

What are the physical properties of bases?

• Bases have a bitter taste. 
• Your skin becomes sticky after touching a base because bases react with proteins. As bases have a greater potential for reacting with proteins in our skin, they are more lethal than acids. 
• Bases turn the red litmus paper blue.

What are the chemical properties of bases?

• Bases react with metals in a variety of ways.
  Alkalis (soluble in water) react with the metal, resulting in sodium chloride forming hydrogen gas. For example, zinc reacts with sodium hydroxide in a variety of ways.

NaOH (aq) + Zn(S) → Na2ZnO2 + H2(g)

• Non-metal oxides react with bases to form salt and water, both beneficial. As an illustration, consider the interaction between carbon dioxide and lime water (calcium hydroxide).   

CO2 + Ca(OH)2 → CaCO3 + H2O

• Reactions between bases and water
  A hydroxide ion is released from an aqueous solution when a base is present. Following is a general representation of the reaction between a base (B) and water, which results in the formation of a conjugate acid (BH+) and a conjugate base (OH):

B(aq) + H2O(l) ⇌ BH+(aq) + OH–(aq)

• Acids and bases react to produce water and salt during a neutralisation reaction. Chemically, the anion of acid “HY” is symbolised by the letter “Y.” To simplify, we may write this equation as HY + XOH = HOH + XY, where ‘X’ stands for an anion of base “XOH,” and “XY” stands for the product salt.

Acid + Base → Salt + Water

6HNO3(aq) + Fe2O3(s) → 2Fe(NO3)3(aq) + 3H2O(l)

Common applications of bases

Bases are found in various objects, not just in scientific laboratories. From food to pharmaceuticals to cleaning supplies, bases are found in several items that we come across in our daily lives. 

• Many products are made using sodium hydroxides, such as soaps, textiles, paper, and medications.
• Bases are used as a laboratory reagent in producing synthetic fibres and dyes.
• Bases are used when the soil’s acidity is reduced due to the whitewashing method.

Conclusion

Bases in solution may be classified according to the degree of ionisation. It is often referred to as “basic strength.” When dissolved in water, it releases a small number of hydroxyl ions into the solution. Two kinds of bases may be distinguished based on their degree of ionisation. Your skin becomes sticky after touching a base because bases react with proteins. As bases have a greater potential for reacting with proteins in our skin, they are more lethal than acids.