What does the solubility product constant (K_sp) represent in the context of an ionic compound?

Given the molar solubility of calcium fluoride (CaF₂) is 2.14 x 10^-4 M, calculate its K_sp.

How does an increase in temperature generally affect the K_sp of an endothermic dissolution reaction?

If the concentration of ions in a solution is increased, how does this affect the reaction quotient (Q) and the equilibrium state?

Combine your understanding of solubility and K_sp to explain why calcium carbonate (CaCO₃) is less soluble in seawater compared to freshwater.