Lecture Notes: Acidity and Basicity

Introduction

• Discussion on acidity and basicity.
• Comparison of organic and inorganic acids.

Discussion on Acidity

Definition of Acidity

• Acid means it donates hydrogen ions (H⁺).
• The strength of an acid indicates its ability to donate hydrogen ions.

Strong and Weak Acids

• Strong acids completely dissociate.
• Weak acids partially dissociate.

Measuring Acidity

• Dissociation constant (Kₐ) is used to measure acid strength.
• A higher value of Kₐ means a stronger acid.
• pKₐ = -log(Kₐ) is used to find the pKₐ value.
• A lower pKₐ value means a stronger acid.

Chemical Reactions

• Strong acids are more reactive.
• Reactions of weak acids are more reversible.

Comparison of Acidity

Inorganic and Organic Acids

• Inorganic acids are stronger compared to organic acids.

Comparison of Various Acids

• Comparison of inorganic acids like hydrochloric acid (HCl), sulfuric acid (H₂SO₄).
• Comparison of organic acids like acetic acid.

Effect of Electronegativity

• Elements with higher electronegativity form stronger acids.

Discussion on Basicity

Identification of Base

• Base means it increases OH⁻ ions or accepts H⁺ ions.

Application of Basicity

• The role of nitrogen's lone pair in basicity is significant.

Special Tips from Guest Lecture

• How to use pKₐ for comparison of acidity and basicity.
• Examples given to understand chemical reactions.

Conclusion

• Understanding the basic principles of acidity and basicity through chemical reactions and the role of electronegativity is important.
• Understanding the properties of each element and molecule helps in comprehending their acidity and basicity.