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Solubility, Molar Solubility, and Solubility Product

Description: 22192.png
KSP = [Ay+] × [Bx]y (since A, By is a pure solid)
KSP = xx × yy × s(x + y)
  • When the ionic product of a salt in solution is equal to its solubility product, the solution is saturated and the undissociated salt remains in equilibrium with its ions in the solution.
  • When the ionic product of a salt in solution is less than the solubility product, the solution is unsaturated and the solution contains only ions and no undissociated salt.
  • When the ionic product is greater than the solubility product, the excess ions in solution combine and gets precipitated. So when the product of the concentrations of the constituent ions raised to appropriate powers exceeds the solubility product of the salt, the salt will be precipitated.




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