Ionic Equilibrium Jee Advanced Questions
JEE Advanced Practice Problems
Ionic Equilibrium Jee Advanced Questions
Ionic Equilibrium refers to the balance between the cations (positively charged ions) and anions (negatively charged ions) present in a solution. In this state, the concentration of ions remains constant, and there is an equal rate of dissociation of ions from their respective compounds and recombination to form neutral compounds. Jee Advanced Questions related to ionic equilibrium focus on the concepts of acid-base reactions, ionization, dissociation, equilibrium constant, pH, and related calculations. Understanding these concepts is crucial for solving complex questions and problems in chemistry and is also essential for understanding the behavior of ionic compounds in various solutions.
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1 - What is meant by ionic equilibrium?
Ionic equilibrium refers to the state in which the concentration of ions in a solution remains constant over time, due to an equal rate of dissociation and association of ions. It is a dynamic equilibrium between the dissolved ions and the undissolved solid.
2) What is the role of a salt bridge in maintaining ionic equilibrium?
A salt bridge is a device used to connect the two half cells of an electrochemical cell. It allows for the flow of ions between the two half cells, preventing any buildup of charge and maintaining electrical neutrality. This helps to maintain the ionic equilibrium by allowing for the continuous movement of ions.
3) What is the difference between a strong acid/base and a weak acid/base in terms of their dissociation in water?
Strong acids and bases completely dissociate in water, meaning all the molecules break apart into their respective ions. On the other hand, weak acids and bases only partially dissociate, resulting in a mixture of undissociated molecules and ions in the solution.
4) How does the pH of a solution change when a strong acid is added to it?
When a strong acid is added to a solution, it increases the concentration of H+ ions, causing the pH to decrease. This is because a strong acid completely dissociates, leading to a higher concentration of H+ ions, which makes the solution more acidic.
5) What is the relationship between the dissociation constant (Kd) and the strength of an acid or base?
The dissociation constant (Kd) is a measure of the extent to which an acid or base dissociates in water. A higher Kd value indicates a stronger acid or base, as it means a higher concentration of ions are present in the solution.
6) How does the addition of a common ion affect the solubility of a slightly soluble salt?
The addition of a common ion, one that is already present in the solution, decreases the solubility of a slightly soluble salt. This is because the common ion shifts the equilibrium towards the undissolved solid, reducing the concentration of ions in the solution.
7) Explain the concept of buffer solutions.
Buffer solutions are solutions that resist changes in pH when either an acid or base is added to them. They are made up of a weak acid or base and its conjugate salt, which can absorb or release H+ ions to maintain the pH of the solution.
8) How does the pH of a buffer solution change when a strong acid or base is added to it?
The pH of a buffer solution remains relatively constant when a strong acid or base is added to it, as the buffer components can absorb or release H+ ions to neutralize the added acid or base and maintain the pH.
9) What is the principle of Le Chatelier's principle?
Le Chatelier's principle states that when a system at equilibrium is subjected to a change, it will shift its equilibrium position to counteract that change and maintain the equilibrium.
10) Explain the effect of temperature on the solubility of salts.
In general, an increase in temperature increases the solubility of salts. This is because the energy of the particles increases, making them more likely to overcome the attractive forces holding them together and dissolve in the solvent.
11) What is a common ion effect?
The common ion effect states that the presence of a common ion in a solution containing a slightly soluble salt decreases the solubility of the salt. This occurs because the common ion shifts the equilibrium towards the undissolved solid, reducing the concentration of ions in the solution.
12) How does pH affect the dissociation of a weak acid or base?
The pH of a solution affects the dissociation of a weak acid or base. A higher pH (more basic) favors the dissociation of a weak acid, while a lower pH (more acidic) favors the dissociation of a weak base.
13) What is the difference between electrolytes and non electrolytes?
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Electrolytes are substances that dissociate into ions in water, while non electrolytes do not dissociate and remain as intact molecules. Electrolytes can conduct electricity, while non electrolytes cannot.
14) Explain the concept of solubility product.
Solubility product (Ksp) is a measure of the amount of a slightly soluble salt that will dissolve in water to form a saturated solution at a given temperature. It represents the product of the concentrations of ions in the solution at equilibrium.
15) How does the addition of a strong electrolyte affect the solubility of a slightly soluble salt?
The addition of a strong electrolyte has no effect on the solubility of a slightly soluble salt. This is because strong electrolytes are completely dissociated in solution, so they do not impact the equilibrium between the dissolved ions and the undissolved solid.
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