Problem: Ce2(SO4)3 becomes less soluble in water as temperature increases because it has a negative entropy of solvation. Most other salts become more soluble in water with increasing temperature because their entropy of solvation is positive. Which explanation best describes this discrepancy? a) The bond strength of Ce2(SO4)3 is very strong, which leads to an increase in the order of the system during the reaction. b) The highly charged Ce3+ and SO42- ions become surrounded by a uniquely ordered sphere of water molecules, which increases the order of the system. c) The solid structure of Ce2(SO4)3 lacks a highly ordered crystal structure thereby leading to a decrease in the order of the system during the reaction.  d) The ions Ce3+ and SO42- repel water molecules, which leads to a decrease in the order of the system during the reaction. e) There is no explanation for this phenomenon. 

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Ce2(SO4)3 becomes less soluble in water as temperature increases because it has a negative entropy of solvation. Most other salts become more soluble in water with increasing temperature because their entropy of solvation is positive. Which explanation best describes this discrepancy?

a) The bond strength of Ce2(SO4)3 is very strong, which leads to an increase in the order of the system during the reaction.

b) The highly charged Ce3+ and SO42- ions become surrounded by a uniquely ordered sphere of water molecules, which increases the order of the system.

c) The solid structure of Ce2(SO4)3 lacks a highly ordered crystal structure thereby leading to a decrease in the order of the system during the reaction. 

d) The ions Ce3+ and SO42- repel water molecules, which leads to a decrease in the order of the system during the reaction.

e) There is no explanation for this phenomenon. 

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