NEET > Chemistry Class 11 > Ionic Equilibrium in One Shot (NCERT)
Ionic Equilibrium in One Shot (NCERT) Video Lecture - Chemistry Class 11 - NEET
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FAQs on Ionic Equilibrium in One Shot (NCERT) Video Lecture - Chemistry Class 11 - NEET
| 1. What is ionic equilibrium? |  |
Ans. Ionic equilibrium refers to the state of balance between the ions and the undissociated molecules in a solution. It occurs when the rate of ionization of a substance is equal to the rate of recombination of ions, resulting in a constant concentration of ions in the solution.
| 2. How is ionic equilibrium established in a solution? | |
Ans. Ionic equilibrium is established in a solution when a soluble ionic compound dissolves in water, and the ions separate from each other. The positive and negative ions are then surrounded by water molecules, forming a hydrated ion. This process is called ionization or dissociation.
| 3. What factors affect the degree of ionization in a solution? | |
Ans. The degree of ionization in a solution is influenced by several factors, including temperature, concentration, nature of the solvent, and presence of common ions. Higher temperatures generally increase the degree of ionization, while higher concentrations and the presence of common ions tend to decrease it.
| 4. How can we calculate the degree of ionization? | |
Ans. The degree of ionization (α) can be calculated using the formula: α = (n / c) × 100, where n is the concentration of the ions after dissociation and c is the initial concentration of the electrolyte. The degree of ionization is expressed as a percentage.
| 5. What is the relationship between ionic equilibrium and acid-base reactions? | |
Ans. Ionic equilibrium plays a crucial role in acid-base reactions. Acids and bases are substances that undergo ionization in aqueous solutions. The dissociation of an acid produces hydrogen ions (H+) while the dissociation of a base produces hydroxide ions (OH-). The equilibrium between the ions and the undissociated molecules determines the strength of the acid or base and the pH of the solution.
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