Author Capstone Axis

Solubility Equilibria of Sparingly Soluble Salts 💧 Salt Solubility Basics Salts dissolve differently in water! Their solubility depends on: 🔋 Lattice enthalpy (ion-ion attraction in solid) 💦 Solvation enthalpy (ion-water attraction, always releases energy!) For dissolving: Solvation enthalpy > Lattice enthalpy. Polar solvents (like water) help this! 📊 Solubility Categories Category Solubility Examples Soluble > […]

Understanding Redox Reactions: The Classic View 🔥 Oxidation = Gaining Oxygen or Electronegative Elements Originally, oxidation meant adding oxygen to a substance. Examples: \(2 \text{Mg} \, (\text{s}) + \, \text{O}_2 \, (\text{g}) \rightarrow 2 \text{MgO} \, (\text{s})\) \(\text{S} \, (\text{s}) + \, \text{O}_2 \, (\text{g}) \rightarrow \, \text{SO}_2 \, (\text{g})\) \(\text{CH}_4 (\text{g}) + 2\text{O}_2 (\text{g})

Hydrolysis of Salts & pH Salts can interact with water (hydrolysis!), changing the solution’s pH: 👉 Weak acid + Strong base salt (e.g., CH3COONa): CH3COO– + H2O ⇌ CH3COOH + OH– → pH > 7 (Alkaline) 👉 Strong acid + Weak base salt (e.g., NH4Cl): NH4+ + H2O ⇌ NH4OH + H+ → pH <

Acids and Bases: Ionization & Properties ⚗️ Lewis Acids and Bases Lewis Acid: Accepts an electron pair (e.g., BF3, AlCl3) Lewis Base: Donates an electron pair (e.g., NH3, OH–, H2O) Example reaction: \[ \text{BF}_3 + \text{NH}_3 \rightarrow \text{BF}_3:\text{NH}_3 \] Here, BF3 (no proton!) acts as the acid. 💪 Strong vs. Weak Acids/Bases Strong Acids: Fully

Effect of Temperature on Equilibrium 🔥🧊 Temperature changes shift equilibrium! For example: Reaction: \(\ce{[Co(H2O)6]^{3+} (aq) + 4Cl^{-} (aq) \rightleftharpoons [CoCl4]^{2-} (aq) + 6H2O(l)}\) Pink ⇄ Blue At room temperature: mixture is blue 🔵 (more \(\ce{[CoCl4]^{2-}}\)). When cooled: mixture turns pink 💖 (more \(\ce{[Co(H2O)6]^{3+}}\)). Effect of Catalysts ⚡ Catalysts speed up reactions but don’t change equilibrium:

Acids, Bases, and Salts Acids, bases, and salts are everywhere in nature! 🍋 For example: Hydrochloric acid (HCl) in your stomach helps digestion. Vinegar contains acetic acid. Lemon juice has citric acid, and tamarind has tartaric acid. Properties of Acids & Bases Acids taste sour, turn blue litmus → red, and release H₂ gas with

Relationship Between Equilibrium Constant (K), Reaction Quotient (Q), and Gibbs Energy (G) 1. What Gibbs Energy Tells Us 🔥 If ΔG is negative → Reaction is spontaneous! It moves forward. ⏩ If ΔG is positive → Reaction is not spontaneous. It prefers the reverse direction. ⏪ If ΔG = 0 → Reaction is at equilibrium.

Factors Affecting Chemical Equilibrium 🔥 Key NEET Concepts Le Chatelier’s Principle applications ΔG° = -RT ln K relationship Pressure effects on gas equilibria Temperature vs. equilibrium constant Catalyst role in equilibrium ⚖️ Le Chatelier’s Principle When equilibrium is disturbed, the system counteracts the change: Added reactant? → Reaction consumes it (shifts forward) Removed product? →

Applications of Equilibrium Constants Key Features of Equilibrium Constants 🔑 Only works when reactant/product concentrations stop changing (at equilibrium!). Value does NOT depend on starting concentrations. Depends on temperature 🌡️ – one unique K per reaction at a given temp. For reverse reaction: Kreverse = 1/Kforward. If you multiply the reaction by a number (n),

Equilibrium Constants: Kc and Kp For any reaction at equilibrium: 🎯 Kc: Uses molar concentrations (mol/L) 🎯 Kp: Uses partial pressures (for gases) General reaction: \[ aA + bB \rightleftharpoons cC + dD \] \[ K_c = \frac{[C]^c [D]^d}{[A]^a [B]^b}, \quad K_p = \frac{(p_C)^c (p_D)^d}{(p_A)^a (p_B)^b} \] Relationship between Kp and Kc \[ K_p =