What does an increase in the concentration of ions in a solution indicate regarding Qs?

The correct understanding rests on the concept of the solubility product constant (Qs), which is the equilibrium constant that relates to the solubility of ionic compounds in solution. When the concentration of ions in a solution increases, it directly influences the reaction quotient (Q), which is similar to Qs but can vary as conditions change.

As more ions are added to the solution, the value of Q reflects their increased concentrations. This eventual increase in Q indicates that the system is moving toward a new equilibrium state, depending on whether the solution is supersaturated or not. If the increase in ion concentration pushes Q beyond the value of Qs, it can lead to precipitation, as the system attempts to re-establish equilibrium.

Therefore, the correct answer is that Qs increases when the concentration of ions in a solution rises, due to the relationship that exists between the concentrations of reactants and products in terms of solubility and precipitation in an equilibrium system.