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Explain the factors affecting solubility of salts in solution. |
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Answer» Solution :The solubility of ionic solids in water differs to a great extent. Some of the ionic solids like `CaF_2` are so soluble that they are hygroscopic in nature and absorb even water from the atmosphere on the other extreme there are substances which have so little solubility , like LiF (lithium fluoride ) , that these are regarded of insoluble . There are some ionic solids which have solubility in between these extreme cases. The solubility depends on a number of feeling. (i)Lattice enthalpy of the SALT. (ii) Solvation enthalpy of ions in the solution . (i)Lattice enthalpy : Lattice enthalpy is the AMOUNT of energy required to break one no. of solid salt into its ions.Greater the lattice enthalpy , more will be the energy required to break the lattice of the salt . (ii)Solvation enthalpy : Solvation enthalpy is the amount of energy RELEASED when one mole ofa solid salt gets dissolved in a solvent the for a salt to dissolve in a solvent, the STRONG forces of attraction between its ions (i.e. lattice enthalpy ) must be overcome by the ion- solvent INTERACTION. Therefore a salt will be soluble in a solvent only when solvation enthalpy is more than lattice enthalpy . It solvation enthalpy is less than lattice enthalpy , the salt will be insoluble . |
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