Solubility of solids depends on nature and temprature of solute and solvent. Solubility is very important in a chemistry laboratory as it helps to determine the correct solution for a particular problem.
Lead Carbonate is not soluble in water at normal temperatures ( 20oC and pressure of 1 bar). Under these conditions it may form as a crystalline PbCO3 or Pb(CO3)22-. It is slightly soluble in carbon dioxide solution, acetic acid and dilute nitric acid.
It is yellow crystalline substance with Moh’s hardness of 3 to 3.5 and density of 6.60 g/cm3. Decomposes in boiling water at 315oC to form the basic carbonate 2PbCO3*Pb(OH)2, which loses its water of crystallization at 160oC.
Reaction with concentrated acetic acid gives anhydrous lead(II) acetate. It also combines with boric acid to form lead metaborate, which has an approximate composition of Pb(BO2)2*H2O.
Solubility of Pb carbonate varies depending on the concentration of the lead metal in water, as well as on the pH of the water. When free chlorine, OCl* or HOCl are present in the water, alkalinity increases, and leads to a slowing of lead dissolution. This is because oxidizing acids and ions are insoluble in alkaline conditions, while hydroxide ions are more soluble.