Write the main difference between an acid and a base. With the help of suitable examples explain the term neutralization and formation of (i) acidic, (basic) and neutral salts.

The main difference between an acid and a base lies in their chemical properties and behavior in solution:

Acid:

Acids are substances that donate protons (H⁺ ions) when dissolved in water.
Examples of acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and citric acid (found in citrus fruits).
Base:

Bases are substances that accept protons (H⁺ ions) or donate hydroxide ions (OH⁻) when dissolved in water.
Examples of bases include sodium hydroxide (NaOH), potassium hydroxide (KOH), and ammonia (NH3).
Neutralization:
Neutralization is a chemical reaction between an acid and a base that results in the formation of water and a salt. The reaction can be represented as follows:

acid + base → salt + water

During neutralization, the H⁺ ions from the acid combine with the OH⁻ ions from the base to form water, while the remaining ions combine to form a salt.

Formation of Salts:

Acidic Salts:

Acidic salts are formed when a strong acid reacts with a weak base.
For example, if sulfuric acid (H2SO4) reacts with ammonia (NH3), the resulting salt ammonium sulfate (NH4)2SO4 is acidic in nature.
Basic Salts:

Basic salts are formed when a strong base reacts with a weak acid.
For example, if sodium hydroxide (NaOH) reacts with acetic acid (CH3COOH), the resulting salt sodium acetate (CH3COONa) is basic in nature.
Neutral Salts:

Neutral salts are formed when a strong acid reacts with a strong base or when a weak acid reacts with a weak base.
For example, the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) forms the neutral salt sodium chloride (NaCl), commonly known as table salt.
In summary, the key differences between acids and bases lie in their ability to donate or accept protons. Neutralization reactions occur when acids and bases react to form water and a salt, and the nature of the resulting salt (acidic, basic, or neutral) depends on the strengths of the acid and base involved in the reaction.