ASRJC 2025 H2 Chem Acid-Base Equilibria Notes

2025 JC2 H2 Chemistry of Aqueous Solutions: Acid–base Equilibria (Student) 2025/ASRJC/Chemistry 1 ANDERSON SERANGOON JUNIOR COLLEGE JC2 H2 CHEMISTRY ACID–BASE EQUILIBRIA CONTENT AND SECTION Remarks 1 Theories of Acids & Bases Lecture 1 (SDL) 13 Jan 2025 1.1 : Arrhenius Theory of Acids & Bases 1.2 : Brønsted–Lowry Theory of Acids & Bases 1.3 : Lewis Theory of Acids & Bases 2. The pH Scale 3. The Ionic Product of Water (Kw) 4. Strengths of Acids & Bases 4.1 : Calculations involving a Strong Acid or Strong Alkali Lecture 2 4.2 : Weak Acids & Weak Bases (A) Strength of Acids and Bases & Dissociation Constants (B) Calculations involving a Weak Acid or Weak Alkali 4.3 : Complementary Strengths of a Conjugate Acid–Base Pair 5 Salt Solutions Lecture 3 5.1 : Salt Hydrolysis 5.2 : Calculation of pH of salt solution 6 Buffer Solutions 6.1 : Types of Buffer Solutions 6.2 : How a Buffer System Controls pH 6.3 : Calculating pH of Buffer Solutions 6.4 : Buffer Capacity and Buffer Range 6.5 : Importance & Uses of Buffer Solutions Lecture 1 (SDL) 13 Jan 2025 7 Acid–Base Titration Lecture 4 7.1 : Indicators 7.2 : Titration Curves (A) Strong acid – strong base (SA–SB) titration (B) Weak acid – strong base (WA–SB) titration (C) Strong acid – weak base (SA–WB) titration Lecture 5 (D) Weak acid – weak base (WA–WB) titration Examples of titration curves (E) Titration involving polybasic acids Summary – how to use the last 2 pages of the notes

2025 JC2 H2 Chemistry of Aqueous Solutions: Acid–base Equilibria (Student) 2025/ASRJC/Chemistry 2 Content Map Content (i) Acid dissociation constants, Ka and the use of pKa (ii) Base dissociation constants, Kb and the use of pKb (iii) The ionic product of water, Kw (iv) pH: choice of pH indicators (v) Buffer solutions Learning Outcomes Students should be able to: (a) explain qualitatively the differences in behaviour between strong and weak acids and bases in terms of the extent of dissociation (b) explain the terms pH; Ka; pKa; Kb; pKb; Kw and apply them in calculations, including the relationship Kw = KaKb (c) calculate [H+(aq)] and pH values for strong acids, weak monobasic (monoprotic) acids, strong bases, and weak monoacidic bases [Calculations involving weak acids/bases will not require solving of quadratic equations] (d) describe the changes in pH during acid–base titrations and explain these changes in terms of the strengths of the acids and bases (e) explain the choice of suitable indicators for acid–base titrations, given appropriate data (f) (i) explain how buffer solutions control pH (ii) describe and explain their uses, including the role of H2CO3/HCO3– in controlling pH in blood (g) calculate the pH of buffer solutions, given appropriate data References 1. Chemistry for Advanced Level, Cann and Hughes, Murray 2. C