Ionic Equilibrium Class 12 Notes Pdf Download _best_ | Bonus Inside

Substances that ionize almost completely (e.g., HCl, NaOH, NaCl).

Buffers are solutions that resist a change in pH when small amounts of acid or base are added. ionic equilibrium class 12 notes pdf download

[Click Here to Download Ionic Equilibrium Class 12 Notes PDF] Substances that ionize almost completely (e

Acids are electron-pair acceptors (electrophiles); Bases are electron-pair donors (nucleophiles). 4. The pH Scale and Self-Ionization of Water Water acts as both an acid and a base (amphoteric). Ionic Product of Water ( Kwcap K sub w ): At 298K, pH Calculation: Relationship: (at 25°C). 5. Buffer Solutions pH Calculation: Relationship: (at 25°C).

Weak base + its salt with a strong acid (e.g., NH4OHcap N cap H sub 4 cap O cap H NH4Clcap N cap H sub 4 cap C l Equation: 6. Salt Hydrolysis When salts dissolve in water, they can affect the pH: Strong Acid + Strong Base: Neutral (pH = 7). Strong Acid + Weak Base: Acidic (pH < 7). Weak Acid + Strong Base: Basic (pH > 7). 7. Solubility Product ( Kspcap K sub s p end-sub For a sparingly soluble salt like AgClcap A g cap C l

Substances that ionize only partially, establishing an equilibrium between the ions and the undissociated molecules (e.g., CH3COOHcap C cap H sub 3 cap C cap O cap O cap H NH4OHcap N cap H sub 4 cap O cap H 2. Ostwald’s Dilution Law For a weak electrolyte ABcap A cap B , the degree of dissociation ( ) increases with dilution. Formula: is very small, This law is only applicable to weak electrolytes. 3. Acids and Bases: The Three Theories Arrhenius Theory: Acids give H+cap H raised to the positive power ions; Bases give OH−cap O cap H raised to the negative power Bronsted-Lowry Theory: Acids are proton ( H+cap H raised to the positive power