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Solubility Product Constant Video Lecture | Chemistry Class 11 - NEET

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FAQs on Solubility Product Constant Video Lecture - Chemistry Class 11 - NEET

1. What is the solubility product constant?
The solubility product constant (Ksp) is a mathematical expression that represents the equilibrium between a solid compound and its dissolved ions in a solution. It is a measure of the extent to which a compound can dissolve in a solvent, and it is specific to each compound.
2. How is the solubility product constant calculated?
The solubility product constant is calculated by multiplying the concentrations of the ions raised to their respective stoichiometric coefficients in the balanced chemical equation for the dissociation of the compound. For example, for the compound AB2, if it dissociates into A+ and 2B-, the solubility product constant would be [A+][B-]^2.
3. What factors affect the solubility product constant?
The solubility product constant is primarily affected by temperature. In general, as the temperature increases, the solubility of most compounds also increases, leading to a higher solubility product constant. Additionally, the solubility product constant can also be influenced by the presence of other ions in the solution, pH, and the nature of the solvent.
4. What is the significance of the solubility product constant?
The solubility product constant is a fundamental concept in chemistry as it helps in predicting the solubility of compounds and understanding their behavior in solution. It is particularly useful in fields such as pharmaceuticals, environmental chemistry, and chemical analysis, where the solubility of compounds plays a crucial role.
5. How is the solubility product constant used in determining the solubility of a compound?
By knowing the solubility product constant and the concentrations of the ions in a solution, one can calculate the solubility of a compound. If the ion concentrations exceed the solubility product constant, the compound is considered to be supersaturated and will likely precipitate. Conversely, if the ion concentrations are below the solubility product constant, the compound is considered to be undersaturated and will continue to dissolve.
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