If ionic product is equal to solubility product, what type of solution is it?
Answer and explanation
Correct answer: Saturated
The equality Q = Ksp means that the ion concentrations satisfy the solubility-product equilibrium condition. The solution is saturated with respect to the salt: it contains the maximum equilibrium amount of dissolved ions at the stated temperature. No net precipitation is required at that instant, although undissolved solid may coexist with the solution. Q less than Ksp is unsaturated and Q greater than Ksp favours precipitation.
Frequently asked questions
What is the correct answer to this question?
Saturated
Why is this the correct answer?
The equality Q = Ksp means that the ion concentrations satisfy the solubility-product equilibrium condition. The solution is saturated with respect to the salt: it contains the maximum equilibrium amount of dissolved ions at the stated temperature. No net precipitation is required at that instant, although undissolved solid may coexist with the solution. Q less than Ksp is unsaturated and Q greater than Ksp favours precipitation.
Which subject and chapter does this question cover?
This is a Class 11 Chemistry question. Chapter: Equilibrium. Topic: Solubility product and common ion effect.
