Mastering the Solubility Product Constant (Ksp)
In the science category, the Solubility Product Constant (Ksp) is the equilibrium constant for a solid substance dissolving in an aqueous solution. This chemistry solver allows you to calculate the molar solubility (s) of various ionic compounds—sparingly soluble salts—based on their specific crystal structure and dissociation patterns.
Understanding Ksp is vital for predicting whether a precipitate will form when two solutions are mixed. It is a cornerstone of qualitative analysis and industrial processes like water softening and mineral extraction.
Salt Types and Solubility Formulas
The relationship between Ksp and molar solubility depends on the stoichiometry of the salt. This science solver supports the following common configurations:
| Salt Type | Example | Ksp Formula |
|---|---|---|
| AB | AgCl, BaO | Ksp = s² |
| AB2 or A2B | PbCl², Ag²CrO² | Ksp = 4s³ |
| AB3 | Al(OH)³ | Ksp = 27s&sup4; |
| A2B3 | Ca³(PO²)² | Ksp = 108s&sup5; |
Chemical Equilibrium Principles
The solubility product represents the point at which a solution is saturated. If the Ion Product (Q) exceeds the Ksp value, a precipitate will form until equilibrium is restored. This science solver automates the complex root calculations required for high-order salts.
Reference Ksp values can be found in the NIST Chemistry WebBook or the Royal Society of Chemistry data sheets.
Chemistry FAQ
What is the common ion effect?
The solubility of a salt decreases significantly if one of its constituent ions is already present in the solution. This is a direct application of Le Chatelier's principle and is accounted for in advanced professional chemistry solvers.