Casey Naor

The solubility product constant is the equilibrium constant for the dissolution of a solid substance into an aqueous solution. It is denoted by the symbol Ksp.

Solubility is defined as a property of a substance called solute to get dissolved in a solvent in order to form a solution. The solubility of ionic compounds (which dissociate to form cations and anions) in water varies to a great deal. Some compounds are highly soluble and may even absorb moisture from the atmosphere, whereas others are highly insoluble.

Solubility depends on a number of parameters, amongst which the lattice enthalpy of salt and solvation enthalpy of ions in the solution are of most importance.

Salts are classified on the basis of their solubility in the following table.

Suppose barium sulphate along with its saturated aqueous solution is taken. The following equation represents the equilibrium set up between the undissolved solids and ions:

\(\begin{array}{l}BaSO_4 \overset{saturated ~solution ~in~ water}{\rightleftharpoons}  Ba^{2+} (aq) + SO_4^{-} (aq)\end{array} \)

The equilibrium constant in the above case is:

In the case of pure solid substances, the concentration remains constant, and so we can say:

Here Ksp is known as the solubility product constant. This further tells us that solid barium sulphate when in equilibrium with its saturated solution, the product of concentrations of ions of both barium and sulphate is equal to the solubility product constant.

We now have a brief idea about the solubility of a compound and the factors affecting it. For any further query on this topic, call the mentor support team at BYJU’S.

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