Which of the following conditions will lead to precipitation in a solution when comparing the solubility product constant (Ksp) and the reaction quotient (Q)?

• A. Q > Ksp
• B. Q = 0
• C. Q = Ksp
• D. Q < Ksp

Answer: (A)

Verified step by step guidance

1. Understand the concept of the solubility product constant (Ksp), which is the equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the level at which a solute dissolves in solution.
2. Learn about the reaction quotient (Q), which is calculated in the same way as Ksp but for a system that is not at equilibrium. It helps predict the direction in which a reaction will proceed to reach equilibrium.
3. To determine if a precipitate will form, compare the values of Q and Ksp. If Q is greater than Ksp, the solution is supersaturated, and precipitation will occur as the system shifts to reach equilibrium.
4. If Q equals Ksp, the system is at equilibrium, and no precipitation will occur because the solution is saturated.
5. If Q is less than Ksp, the solution is unsaturated, and no precipitation will occur because more solute can dissolve in the solution.