**Determination of solubility of sparingly soluble salts:**

Conductance measurement can be used for measurements of solubility of slightly soluble substances like BaSO_{4}, PbSO_{4}, AgCl etc. The method is based on the difference in the conductance of the ions of the salts. For the purpose a saturated solution of the salt is prepared in conductivity water and allowed to stand until almost all the insoluble fraction settles down. The clear solution from the top is taken and its conductance is measured in a conductance cell. The cell is thoroughly washed and filled with the same conductivity water and the conductance of the water measured in the same cell. The observed conductance is then converted to specific conductance. The conductance of water is then subtracted from the conductance of the solution. The value so obtained is the conductance due to the salt.

The molar conductance (Λ_{m}) of a saturated solution as given by equation-

**Λ _{m} = (κ x 1000)/c**

where κ is the specific conductance and ‘c’ is the concentration of the solution in mol L^{-1}. Since the salt is sparingly soluble, the solution is very dilute and Λ_{m} may be considered to be equal to Λ^{0}_{m }i.e.. the molar conductance at infinite dilution. The value of Λ^{0}_{m} tor AgCl can be found by applying Kohlrausch’s law of independent ionic migration. According to this law, Λ^{0}_{m(AgCl)} = λ^{0}_{ag} + λ^{0}_{Cl}. Substituting Λ^{0}_{m} in above equation ‘c’ can be calculated provided κ is known. This will give the value of ‘c’ in mol L^{-1 }from which the solubility in gL^{-1} may be calculated.