Question

On the basis of ionization explain classification of acids and bases with suitable examples. Classify acids/bases on the basis of amount of water present in the solution.

Short answer

Question: What are the primary factors in classifying acids and bases based on their ionization, and provide examples for each type of acid and base. Answer: The primary factors in classifying acids and bases based on their ionization are their ionization extent (strong or weak) and concentration of water present (dilute or concentrated). Strong acids (e.g. hydrochloric acid, sulfuric acid, nitric acid) and bases (e.g. potassium hydroxide, sodium hydroxide, calcium hydroxide) ionize completely in water, while weak acids (e.g. acetic acid, hydrofluoric acid, carbonic acid) and bases (e.g. ammonia, water, pyridine) ionize partially. Dilute solutions have a low concentration of the acid/base and high amount of water, while concentrated solutions have a high concentration of the acid/base and low amount of water. This classification applies to both strong and weak acids/bases.

Step-by-step solution

Definition of Acids and Bases

Acids are substances that donate protons (H+ ions) to a solution. In contrast, bases are substances that accept protons (H+ ions) from a solution. The process of donating or accepting protons is called ionization.

Strong Acids and Bases

Strong acids and bases are substances that completely ionize in water, meaning they dissociate into ions 100% when dissolved in water. In other words, a strong acid will donate all of its H+ ions, and a strong base will accept all available H+ ions. Examples of strong acids: hydrochloric acid (HCl), sulfuric acid (H2SO4), nitric acid (HNO3). Examples of strong bases: potassium hydroxide (KOH), sodium hydroxide (NaOH), calcium hydroxide (Ca(OH)2).

Weak Acids and Bases

Weak acids and bases are substances that do not ionize completely in water. They only partially dissociate into ions when dissolved in water, meaning only a portion of their molecules will release H+ ions (for weak acids) or accept H+ ions (for weak bases). Examples of weak acids: acetic acid (CH3COOH), hydrofluoric acid (HF), carbonic acid (H2CO3). Examples of weak bases: ammonia (NH3), water (H2O), pyridine (C5H5N).

Classification Based on Water Concentration: Dilute and Concentrated Solutions

Dilute acids or bases have a low concentration of the acid/base in the solution, meaning there is a high amount of water present. On the other hand, concentrated acids or bases have a high concentration of the acid/base, and a low amount of water present. It is important to note that this classification is independent of whether an acid or base is strong or weak. A strong acid or base can be diluted by adding more water, and a weak acid or base can be concentrated by removing water. For example, both concentrated hydrochloric acid (strong acid) and concentrated acetic acid (weak acid) are classified as concentrated solutions due to their high concentrations of the respective acids and low amounts of water. Similarly, both dilute potassium hydroxide (strong base) and dilute ammonia (weak base) are classified as dilute solutions due to their low concentrations of the respective bases and high amounts of water.