This is very similar to problem 1. The dissociation of the CsCl salt into solvated ions in solution is an endothermic process (deltaH > 0). Therefore it takes up heat. However, it is strongly favored entropically because the ions are dispersed randomly in solution. In this case, T x deltaS is greater than deltaH so the reaction is spontaneous even though it is endothermic. Thus, the beaker gets cold.