Which comparison is used to understand the beginning of precipitation?
Answer and explanation
Correct answer: Comparison of ionic product and solubility product
For a sparingly soluble salt, calculate Q from the current concentrations of its ions and compare it with Ksp. If Q is below Ksp, the solution is unsaturated; if Q equals Ksp, it is saturated; and if Q exceeds Ksp, the excess ions tend to form a precipitate until equilibrium is restored. This comparison directly tests the precipitation condition, unlike colour, smell or container height.
Frequently asked questions
What is the correct answer to this question?
Comparison of ionic product and solubility product
Why is this the correct answer?
For a sparingly soluble salt, calculate Q from the current concentrations of its ions and compare it with Ksp. If Q is below Ksp, the solution is unsaturated; if Q equals Ksp, it is saturated; and if Q exceeds Ksp, the excess ions tend to form a precipitate until equilibrium is restored. This comparison directly tests the precipitation condition, unlike colour, smell or container height.
Which subject and chapter does this question cover?
This is a Class 11 Chemistry question. Chapter: Equilibrium. Topic: Solubility product and common ion effect.
