Question

Substances with high lattice energies tend to be less soluble than substances with low lattice energies. On that basis predict the relative aqueous solubility at 20 °C, from highest to lowest, of the following ionic compounds: Ce2(SO4)3, K2SO4, KBr, NaCl.

Answer 1

Answer:

KBr > NaCl  > $K_{2}SO_{4}$ > $Ce_{2}(SO_{4})_{3}$  

Explanation:

Generally, the higher the lattice energy of the substance, the lower the solubility of the substance. The lattice energy of KBr is the lowest, follow by that NaCl and that of $K_{2}SO_{4}$ while that of  $K_{2}SO_{4}$ is the highest. Based on the relationship between the lattice energy and solubility, the solubility of the substances ranging from the highest to lowest is KBr > NaCl  > $K_{2}SO_{4}$ > $Ce_{2}(SO_{4})_{3}$.