What happens when the ionic product is greater than the solubility product?

If solubility product is greater than the ionic product then, the solution is unsaturated and no precipitate will form by the addition of more solute. When Ksp< ionic product: If solubility product is less than the ionic product then the solution is super saturated and the excess of solute will precipitate immediately.

What is the relationship between the ion product and the solubility product constant when a precipitate forms?

Explanation: 1) If Solubility product is larger than the ionic product then no precipitate will form on adding more solute because unsaturated solution is formed. 2) If Solubility product is smaller than the ionic product then excess solute will precipitate out because of the formation of super saturated solution.

What happens when QSP is greater than KSP?

Ï Qsp must equal to or greater than Ksp for precipitation to occur. If Qsp < Ksp, then the reaction proceeds toward products. (i.e. to the right, ˆˆ no precipitation) If Qsp > Ksp, then the reaction proceeds to form reactants. If Qsp = Ksp, then the system reaches equilibrium.

What is the difference between ionic product and solubility product?

Both ionic product and solubility product represent the product of the concentrations of the ions in the solution. On the other hand, the term solubility product is applied only to a saturated solution in which there exists a dynamic equilibrium between the undissolved salt and the ions present in solution.

When the ionic product of a solution is equal to its solubility product then the solution will be?

When it is equal to the solubility product for the salt, the system is at equilibrium. Now imagine what happens when a few crystals of NaCl are added to a saturated solution of AgCl in water. There are two sources of the chloride ion in this solution.

When the ionic product of a solution exceeds the solubility product the solution becomes?

super saturated and precipitation of salts occur.

What happens when Q equals KSP?

If Q > Ksp, a precipitate will form. Note that precipitation may not happen immediately if Q is equal to or greater than Ksp. A solution could be supersaturated for some time until precipitation occurs. Fractional precipitation is a technique that separates ions from solution based on their different solubilities.

When two solutions are mixed a precipitate forms is QSP greater than less than or equal to KSP explain?

When QSP is greater than KSP, the solution is oversaturated. So it’s exceeded the limit of what can dissolve, and therefore you can imagine some lead two plus ions combining with some sulfate ions to form a precipitate. Therefore, when QSP is greater than KSP, a precipitate will form.