Ionic Equilibrium

Chemical reactions mostly take place in solutions. Solution chemistry plays a very significant role in chemistry. All chemical substances are made up of either polar units (called ions) or non-polar units. The activity of these entities is more evident and pronounced in solution. The behaviour of these substances depends upon their nature and conditions of the medium in which they are added. It is therefore necessary to understand the principles that govern their behaviour in solution.

This type of equilibrium is observed in substances that undergo ionization easily, or in polar substances in which ionization can be induced. Ionic and polar substances are more easily soluble in polar solvents because of the ease of ionization taking place in the solvent medium. With the dissolution of ionic and polar substances in the solvent, these solutions become rich in mobile charge carriers (ions) and thus can conduct electricity. Substances, which are capable of conducting electricity are called as electrolytes while those substances which are non-conducting are called as non-electrolytes.

Topic

Sub - Topics

Ionic Equilibrium

Types of Electrolytes | Ostwald s Dilution Law-Part1 Common ION Effect-Part1 | Acids and Bases-Part1 Lewis Concept of Acids and Bases | Solubility Product-Part1 | Applications of Solubility Product-Part1 | Periodic Variations of Acidic and Basic Properties | Relative Strength of Acids and Bases-Part1 | Ionic Product of Water-Part1 | Hydrogen Ion Concentration pH Scale-Part1 | pH OF Weak Acids and Bases-Part1 | Relationship-Solubility and Solubility Product-Part1 Acid-Base Neutralization-Part1 | Salt Hydrolysis | Salt of Strong Acid and Weak Base-Part1 | Salt of Weak acid and Strong Base | Salt of Weak Acid and Weak Base | Hydrolysis of Amphiprotic Anion-Part1 | Buffer Solutions-Part1 | Buffer Capacity-Part1 | Hendersons Equation | Theory of Indicators


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