The solubility product constant (Ksp) is an equilibrium constant for a solid dissolving into its ions in an aqueous solution. It provides valuable insight into the solubility of ionic compounds and predicts whether a precipitate will form under specific conditions.
| Concept | Description |
| Saturated Solution | A state where the dissolved ionic compound is in equilibrium with the undissolved solid. |
| Dynamic Equilibrium | The state where the dissolution and precipitation of a solid occur at the same rate. |
| Factors Affecting Solubility | Includes lattice enthalpy, solvation enthalpy, pH, and temperature. |
| Common Ion Effect | The presence of a common ion reduces the solubility of a salt. |
| Temperature | Solubility varies with temperature, which must be specified when reporting Ksp values. |
Key Equations and Examples
| Compound | Reaction | Ksp Expression |
| Barium Sulfate | BaSO4 ↔ Ba2+ + SO42- | Ksp = [Ba2+][SO42-] |
| Calcium Chloride | CaCl2 ↔ Ca2+ + 2Cl- | Ksp = [Ca2+][Cl-]2 |
| Magnesium Fluoride | MgF2 ↔ Mg2+ + 2F- | Ksp = [Mg2+][F-]2 |
Several factors influence solubility, including:
Understanding Ksp is crucial for NEET aspirants. It is frequently tested in the form of conceptual and numerical questions. Reliable resources like Infinity Learn provide notes and practice questions following CBSE and NCERT guidelines to help students excel.
| Question | Answer |
| What affects Ksp? | Factors include the common ion effect, ion-pair formation, and ionic strength of the solution. |
| How is Ksp for calcium chloride calculated? | CaCl2 ↔ Ca2+ + 2Cl-, Ksp = [Ca2+][Cl-]2. |
| How is Ksp for magnesium fluoride calculated? | MgF2 ↔ Mg2+ + 2F-, Ksp = [Mg2+][F-]2. |
The entire amount of a chemical that can be dissolved in a solvent at equilibrium is referred to as solubility. The solubility product constant, across the other hand, is an equilibrium constant that sends details on the equilibrium between solid solute and its fragmented constituent ions across the solution.
The solubility product constant (Ksp) helps predict the solubility of ionic compounds in water. It also determines whether a precipitate will form when two solutions are mixed and provides insights into the equilibrium state of saturated solutions.
The common ion effect decreases the solubility of an ionic compound in a solution that already contains one of its ions. This occurs because the presence of the common ion shifts the equilibrium towards the undissolved form, reducing the dissolution.
To calculate solubility, set up the equilibrium expression using Ksp. Then, substitute the concentrations of the ions in terms of the solubility () and solve the equation to find the solubility in moles per liter.