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 What is Ionic Equilibrium?* Ionic equilibrium refers to the state of balance between ions in a solution. It's a dynamic equilibrium, meaning that the rates of forward and reverse reactions are equal, and the concentrations of the ions remain constant. This concept is crucial in understanding various chemical and biological processes. *Types of Ionic Equilibria* 1. *Strong Electrolytes*: Strong electrolytes completely dissociate into ions in solution, resulting in a high concentration of ions. Examples include sodium chloride (NaCl) and hydrochloric acid (HCl). 2. *Weak Electrolytes*: Weak electrolytes partially dissociate into ions in solution, resulting in a lower concentration of ions. Examples include acetic acid (CH3COOH) and ammonia (NH3). *Factors Affecting Ionic Equilibrium* 1. *Concentration*: Changing the concentration of ions can shift the equilibrium. According to Le Chatelier's principle, increasing the concentration of one ion can cause the equilibrium to shift in...

🧪 Class 11 Chemistry: Chemical Equilibrium Explained for Students 🔷 What is Chemical Equilibrium? Chemical equilibrium is a state in a reversible reaction where the rate of the forward reaction equals the rate of the backward reaction. ➡️ At this point, the concentrations of reactants and products remain constant (not necessarily equal, just constant). In this Haber process, the reaction can proceed in both directions. When equilibrium is reached, ammonia is formed at the same rate it's decomposed. --- 🔷 Characteristics of Equilibrium 1. Dynamic Nature: Reactions are still happening — but at equal rates. 2. No Change in Concentration: Amount of reactants/products stays constant. 3. Can Be Achieved from Either Side: Whether you start with reactants or products, equilibrium will be reached. 4. Occurs in Closed Systems: No exchange of matter with surroundings. --- 🔷 Types of Equilibrium 1. Physical Equilibrium: Involves physical processes. Example: Water ⇌ Vapor 2. Chemical Equili...