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FAQs on Advanced Level MCQs Question Bank - Ionic Equilibrium - JEE

1. What is Ionic Equilibrium?
Ans. Ionic Equilibrium refers to the equilibrium established between the ions in a solution. It occurs when a soluble ionic compound dissolves in water and dissociates into its constituent ions. This equilibrium involves the balance between the forward reaction of ionization and the reverse reaction of recombination.
2. How is Ionic Equilibrium different from Chemical Equilibrium?
Ans. Ionic Equilibrium specifically deals with the equilibrium between ions in a solution, while Chemical Equilibrium refers to the equilibrium between reactants and products in a chemical reaction. Ionic Equilibrium focuses on the dissociation and recombination of ions, whereas Chemical Equilibrium considers all species involved in a reaction.
3. What factors affect Ionic Equilibrium?
Ans. Several factors influence Ionic Equilibrium. These include temperature, concentration of ions, presence of common ions, pH of the solution, and nature of the solvent. Temperature affects the equilibrium constant, while concentration and common ions influence the degree of ionization. pH and solvent properties affect the solubility of ionic compounds.
4. How does pH affect Ionic Equilibrium?
Ans. The pH of a solution plays a significant role in Ionic Equilibrium. pH is a measure of the concentration of hydrogen ions in a solution. In acidic solutions, with a lower pH, the equilibrium shifts towards the dissociation of weak acids and the hydrolysis of weak bases. In basic solutions, with a higher pH, the equilibrium shifts towards the ionization of weak bases and the hydrolysis of weak acids.
5. What is the importance of Ionic Equilibrium in chemical reactions?
Ans. Ionic Equilibrium is crucial in understanding and predicting the behavior of chemical reactions. It helps determine the extent of ionization and the concentration of ions in a solution, which affects the reaction's rate and equilibrium position. Ionic Equilibrium also aids in analyzing acid-base reactions, solubility of salts, buffer solutions, and the pH of solutions.
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