Under which condition will precipitation of an insoluble salt occurring from mixing two electrolyte solutions strictly take place?
Answer and explanation
Correct answer: B. When the ionic product quotient (Qsp) strictly exceeds the solubility product constant (Ksp): Qsp > Ksp
- If : the solution is unsaturated, and no precipitate forms;
- If : the solution is saturated, and dynamic equilibrium exists with no net precipitation;
- If : the solution is supersaturated, and precipitation occurs until the remaining ionic concentrations satisfy .
- If : the solution is saturated, and dynamic equilibrium exists with no net precipitation;
- If : the solution is supersaturated, and precipitation occurs until the remaining ionic concentrations satisfy .
- Step 1: In solution chemistry, the ionic product ( or ) is calculated using the initial concentrations of participating ions in solution immediately upon mixing.
- Step 2: represents the maximum equilibrium product of ionic concentrations in a saturated solution at that temperature.
- Step 3: Three cases exist:
Answer
When the ionic product quotient (Qsp) strictly exceeds the solubility product constant (Ksp): Qsp > Ksp
Why not the others: 'Qsp < Ksp' describes an unsaturated solution where all ions remain dissolved; 'Qsp = Ksp' describes an exact saturation threshold without precipitation; 'When temperature is at absolute zero' is physically impossible in aqueous liquid solutions.
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