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| 1. What is the concept of ionic equilibrium? |  |
Ans. Ionic equilibrium refers to a state where the concentration of ions in a solution remains constant over time. It occurs when the rate of dissociation of the ionic compound is equal to the rate of recombination, resulting in a dynamic equilibrium. This concept is often studied in the context of acid-base reactions and solubility of salts in water.
| 2. How is ionic equilibrium relevant to the IIT JAM exam? | |
Ans. Ionic equilibrium is an important topic in the IIT JAM exam, particularly in the Physical Chemistry section. Questions related to acid-base equilibria, solubility product, pH calculations, and buffer solutions are frequently asked. A solid understanding of ionic equilibrium is crucial for scoring well in this exam.
| 3. What are some common applications of ionic equilibrium in real life? | |
Ans. Ionic equilibrium has several practical applications in various fields. Some examples include understanding the pH balance in our body, determining the effectiveness of antacids in neutralizing stomach acid, designing buffer solutions in chemical laboratories, analyzing water quality, and developing corrosion-resistant materials.
| 4. How can one calculate the pH of a solution in an ionic equilibrium? | |
Ans. The pH of a solution in an ionic equilibrium can be determined using the concentration of hydrogen ions (H+) or hydroxide ions (OH-) present in the solution. For acidic solutions, pH is calculated using the formula pH = -log[H+]. For basic solutions, pOH is calculated using the formula pOH = -log[OH-], and pH can be obtained by subtracting pOH from 14.
| 5. What is the significance of the solubility product (Ksp) in ionic equilibrium? | |
Ans. The solubility product (Ksp) is a measure of the extent to which a sparingly soluble salt dissolves in water. It plays a crucial role in predicting the formation of precipitates and determining the solubility of salts. By comparing the value of Ksp with the ion concentrations in a solution, one can determine whether a precipitate will form or not. This concept is important in fields such as pharmaceuticals, environmental chemistry, and industrial processes.
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Dec 23, 2024 Last updated |
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