7.0 I O N I C E Q U I L I B R I A
Subtopic | Learning Outcome At the end of this subtopic, Y O U ..!!! as KMS PDT student should be able to : |
7.1 Acids and bases | a) Define acid and base according to the Arrhenius, Bronsted-Lowry and Lewis theories. b) Define and identify conjugate acid and conjugate base according to Bronsted-Lowry theory. c) Define strong acid and strong base, weak acid and weak base. d) Write the expressions of dissociation constants, Ka and Kb weak acid and weak base. e) Relate the strength of a weak acid and a weak base to the respective dissociation constants, Ka and Kb. f) Relate Ka, Kb to pKa and pKb, g) Define pH and pOH. h) Relate pH and pOH to the ionic product of water, Kw at 25oC. i) Calculate the pH values of a strong acid and strong base. j) Perform calculations involving pH, dissociation constant, initial concentration, equilibrium concentration and the degree of dissociation, α. |
7.2 Salts (no calculation) | a) Explain salt hydrolysis and write hydrolysis equation for the salt formed from the reaction between: i. strong acid and strong base ii. strong acid and weak base iii. weak acid and strong base b) Classify the salts as neutral, acidic or basic. |
7.3 Buffer | a) Define buffer solution. b) Describe the preparation of buffer solution c) Explain qualitatively how a buffer solution controls its pH. d) Derive the Henderson-Hasselbalch equation. (HHEq) pH = pKa + log [conjugate base] [weak acid ] pOH = pKb + log [conjugate acid] [weak base ] e) Calculate the pH of buffer solutions. f) Calculate the pH of solution when small amount of strong acid or strong base is added to buffer solution |
7.4 Acid – base titrations | a) Describe the titration process and distinguish between the end point and equivalence point. b) Perform calculations involving titrations between a strong acid and a strong base c) Sketch and interpret the variation of pH against titre value for titrations between i. strong acid-strong base ii. strong acid-weak base iii. weak acid-strong base d) Identify suitable indicators for acid-base titrations. |
7.5 Solubility equilibria | a) Define solubility, molar solubility and solubility product, Ksp. b) Calculate Ksp from concentrations of ions and vice versa. c) Predict the possibility of precipitation of slightly soluble ionic compounds by comparing the values of ion-product, Q to Ksp. d) Define and explain the common ion effect (CIE) e) Perform calculations related to common ion effect. |
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