NEET > Chemistry Class 11 > Common Ion Effect in the Ionization of Acids & Bases
Common Ion Effect in the Ionization of Acids & Bases Video Lecture - Chemistry Class 11 - NEET
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FAQs on Common Ion Effect in the Ionization of Acids & Bases Video Lecture - Chemistry Class 11 - NEET
| 1. What is the common ion effect in the ionization of acids and bases? |  |
Ans. The common ion effect refers to the phenomenon where the presence of a common ion in a solution reduces the degree of ionization of an acid or a base. This occurs because the common ion, which is already present in the solution due to another compound, suppresses the dissociation of the acid or base, leading to a decrease in the concentration of the ionized species.
| 2. How does the common ion effect affect the pH of a solution? | |
Ans. The common ion effect can affect the pH of a solution by shifting the equilibrium of the acid-base reaction. When a common ion is added to a solution containing a weak acid or base, the equilibrium is shifted towards the side with fewer ions, reducing the concentration of hydrogen ions (in the case of an acid) or hydroxide ions (in the case of a base). This results in a decrease in the pH of the solution.
| 3. Can you give an example of the common ion effect in practice? | |
Ans. One example of the common ion effect is the addition of sodium acetate (CH3COONa) to a solution of acetic acid (CH3COOH). Acetic acid is a weak acid that partially ionizes in water to produce acetate ions (CH3COO-) and hydrogen ions (H+). When sodium acetate, which also contains acetate ions, is added to the solution, the common ion (acetate ion) reduces the ionization of acetic acid, resulting in a lower concentration of hydrogen ions and a decrease in the acidity of the solution.
| 4. How does the common ion effect impact the solubility of salts? | |
Ans. The common ion effect can impact the solubility of salts by reducing their solubility in a solution. When a salt is dissolved in a solution that already contains one of its ions as a common ion, the equilibrium of the dissolution reaction is shifted towards the undissociated form of the salt. This decrease in the concentration of the dissociated ions leads to a decrease in the solubility of the salt in the solution.
| 5. Is the common ion effect reversible? | |
Ans. Yes, the common ion effect is reversible. If the common ion is removed from the solution, the equilibrium of the acid-base reaction or the dissolution reaction can shift back towards the side with more ions, resulting in an increase in the degree of ionization or solubility, respectively. Removing the common ion allows the system to reach a new equilibrium without the suppressing effect, restoring the original pH or solubility.
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