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FAQs on Ionic Equilibrium & Chemical equilibrium - Additional Documents & Tests for IIT JAM

1. What is meant by ionic equilibrium?
Ans. Ionic equilibrium refers to the state in which the concentrations of ionic species in a solution remain constant with time. It occurs when the rate of formation of ions is equal to the rate of recombination of ions. In simple terms, it is the balance between the dissociation and association of ions in a solution.
2. How is chemical equilibrium different from ionic equilibrium?
Ans. Chemical equilibrium refers to the state in which the concentrations of all reactants and products in a chemical reaction remain constant with time. It occurs when the rate of the forward reaction is equal to the rate of the reverse reaction. On the other hand, ionic equilibrium specifically deals with the equilibrium between ions in a solution, where the concentrations of the ions remain constant with time.
3. What factors affect the ionic equilibrium in a solution?
Ans. Several factors can affect the ionic equilibrium in a solution. Some of the key factors include temperature, pressure (for systems involving gases), concentration of ions, presence of a catalyst, and the nature of the solvent. Changes in these factors can shift the equilibrium position and alter the concentrations of ions in the solution.
4. How can we calculate the equilibrium constant for an ionic equilibrium?
Ans. The equilibrium constant, denoted by K, is a measure of the extent of an ionic equilibrium. It can be calculated by dividing the concentration of the products raised to their stoichiometric coefficients by the concentration of the reactants raised to their stoichiometric coefficients. The equilibrium constant expression can be derived from the balanced chemical equation representing the ionic equilibrium.
5. Can you provide an example of an ionic equilibrium and explain its significance?
Ans. One example of an ionic equilibrium is the dissociation of a weak acid in water. For instance, acetic acid (CH3COOH) partially dissociates into hydronium ions (H3O+) and acetate ions (CH3COO-) in water. This equilibrium is represented by the chemical equation CH3COOH ⇌ H3O+ + CH3COO-. The significance of this ionic equilibrium lies in understanding the behavior of weak acids and their ability to donate protons in a solution. The equilibrium constant for this reaction, known as the acid dissociation constant (Ka), provides valuable information about the strength of the acid and its degree of dissociation.
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