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Solubility Product Constant Equation (1:1 salt):
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The solubility product constant (Ksp) is the equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the product of the concentrations of the ions in a saturated solution, each raised to the power of its stoichiometric coefficient.
The calculator uses the solubility product constant equation for 1:1 salts:
Where:
Explanation: For a 1:1 salt (like AgCl), the dissolution equation is AB(s) ⇌ A⁺(aq) + B⁻(aq), so Ksp = [A⁺][B⁻] = s × s = s².
Details: The solubility product constant is crucial for predicting precipitation reactions, determining solubility limits, and understanding the behavior of sparingly soluble salts in various chemical and environmental contexts.
Tips: Enter the solubility value in mol/L. The value must be a positive number greater than zero.
Q1: What does Ksp tell us about solubility?
A: A smaller Ksp value indicates lower solubility, while a larger Ksp value indicates higher solubility of the compound.
Q2: How does temperature affect Ksp?
A: Ksp values are temperature-dependent. For most salts, solubility increases with temperature, so Ksp increases with temperature.
Q3: Can Ksp be used for all types of salts?
A: The equation Ksp = s² applies specifically to 1:1 salts. For other stoichiometries (like 1:2 or 2:3 salts), different equations are used.
Q4: What are common examples of 1:1 salts?
A: Common 1:1 salts include AgCl, AgBr, BaSO₄, and PbSO₄, where one cation combines with one anion.
Q5: How is Ksp used in predicting precipitation?
A: By comparing the ion product (Q) with Ksp, we can predict if precipitation will occur: if Q > Ksp, precipitation occurs; if Q < Ksp, no precipitation occurs.