Solve Kc/Kp equilibrium expressions, pH buffer equations, and Ksp precipitation problems accurately for NEET & JEE.
Equilibrium explores reversible chemical systems and ionic dissociation in aqueous solutions. Mastering Law of Mass Action, Le Chatelier's Principle, pH calculations, and Solubility Product (Ksp) guarantees scoring success.
Chemical Equilibrium: Kc and Kp relationship: Kp = Kc (RT)^(Delta n). Le Chatelier's Principle predicts system response to stress: Increasing reactant concentration shifts equilibrium forward; increasing pressure shifts toward fewer gas moles; increasing temperature shifts endothermic reactions forward.
Ionic Equilibrium & pH: Kw = [H+][OH-] = 10^-14 at 298 K. pH = -log[H+]. Buffer Solutions resist pH changes: Acidic buffer (Weak acid + its salt, e.g., CH3COOH + CH3COONa) follows Henderson-Hasselbalch equation: pH = pKa + log ([Salt] / [Acid]).
Solubility Product (Ksp): Governs dissolution of sparingly soluble salts. Precipitation occurs whenever ionic product (Qsp) exceeds solubility product (Ksp). Dr. Aarzoo Saini provides step-by-step buffer and Ksp numerical practice at We-Gyaan Classes.
Key Takeaways for Students
- Relate Kp and Kc using Kp = Kc (RT)^(Delta n).
- Predict equilibrium shifts under concentration, pressure, and temperature stress using Le Chatelier's Principle.
- Calculate acidic and basic buffer pH using Henderson-Hasselbalch equations.
- Compare Qsp with Ksp to determine precipitation conditions.
Authored by Dr. Aarzoo Saini
Founder & Lead Educator at We-Gyaan Classes Roorkee, with over 20 years of teaching excellence in Science and Chemistry for Board Exams, NEET, JEE, and CUET.