Based on Le Chatelier's principle, what is the predicted effect on solubility of CaCl when a saturated solution?

When two opposing processes are in equilibrium, their rates of occurrence are equal.

Assume, for instance, that you add enough salt to a beaker filled with 100 mL of water such that no more salt will dissolve and that some salt is visible at the bottom of the beaker in the solid state. Individual Na+ and Cl− ions may alternate between the dissolved and solid states; the two processes depicted below are occurring simultaneously and at an equal rate.

Cl−(aq) + Na+(aq) -> NaCl(s) AND Cl−(aq) + Na+(aq) -> NaCl(s)

Visit https://tutor.hix.ai to try out the simulation.

As time passes, you will see some of the ions leave the salt crystal (solid NaCl) and other ions that were free in solution bond onto the crystal. Use the salt shaker to add salt until you see some of the Na and Cl ions remain bonded together.

According to Le Chatelier's principle, increasing the temperature will decrease the solubility of CaCl2 in a saturated solution.